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Chemistry
Energy & Matter In Chemical Change
469
Chemistry
10th Grade
10/22/2012
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Term
Physical Or Chemical Property :

Boiling Point
 Definition
Physical Property
Term
Physical Or Chemical Property :

Condensation Point
 Definition
Physical Property
Term
Physical Or Chemical Property :

Melting Point
 Definition
Physical Property
Term
Physical Or Chemical Property :

Freezing Point
 Definition
Physical Property
Term
Physical Or Chemical Property :

Malleability
 Definition
Physical Property
Term
Physical Or Chemical Property :

Ductility
 Definition
Physical Property
Term
Physical Or Chemical Property :

Colour
 Definition
Physical Property
Term
Physical Or Chemical Property :

State
 Definition
Physical Property
Term
Physical Or Chemical Property :

Solubility
 Definition
Physical Property
Term
Physical Or Chemical Property :

Crystal Formation
 Definition
Physical Property
Term
Physical Or Chemical Property :

Conductivity
 Definition
Physical Property
Term
Physical Or Chemical Property :

Magnetism
 Definition
Physical Property
Term
Physical Or Chemical Property :

Ability To Burn
 Definition
Chemical Property
Term
Physical Or Chemical Property :

Flash Point
 Definition
Chemical Property
Term
Physical Or Chemical Property :

Behavior In Air
 Definition
Chemical Property
Term
Physical Or Chemical Property :

Reaction With Water
 Definition
Chemical Property
Term
Physical Or Chemical Property :

Reaction With Acids
 Definition
Chemical Property
Term
Physical Or Chemical Property :

Reaction To Heat.
 Definition
Chemical Property
Term
Physical Or Chemical Property :

Reaction to Red & Blue Litmus.
 Definition
Chemical Property
Term
The observe a chemical property you must see a ___________ _______ .
 Definition
Chemical Change
Term
During a chemical reaction, energy is always __________ or _________.
 Definition
During a chemical reaction, energy is always absorbed or released.
Term
During a chemical reaction, __________ is always __________ or _________.
 Definition
During a chemical reaction, energy is always absorbed or released.
Term
What was Aristotle's theory on matter ?
 Definition
That all mater was composed of fire, earth, water and air.
Term
What was Democritus's theory on matter?
 Definition
Matter was made up of tiny particles, that could not be divided into smaller pieces.
Term
Democritus called modern day atoms, _____, meaning ___________.
 Definition
Democritus called modern day atoms, Atomos, meaning Invisible.
Term
__________ was better known and more respected than __________ so although _________'s theory on matter was closer to our theory today, people believed ________'s theory for about 2000 years after __________ & ___________'s theories were brought up in ____BC.
 Definition
Aristotle was better known and more respected than Democritus so although Democritus's theory on matter was closer to our theory today, people believed Aristotle's theory for about 2000 years after Democritus & Aristotle's theories were brought up in 400BC.
Term
Aristotle & Democritus were ________ _____________.
 Definition
Aristotle & Democritus were Greek Philosophers.
Term
Alchemy = Combination of ________ & _________.
 Definition
Alchemy = Combination of Science & Magic.
Term
Mercury was discover through ________ .
 Definition
Mercury was discover through Alchemy.
Term
_______ measured relationships between volume and pressure of gas.
 Definition
Robert Boyle measured relationships between volume and pressure of gas.
Term
Robert Boyle measured relationships between _________ and ___________ of gas.
 Definition
Robert Boyle measured relationships between volume and pressure of gas.
Term
Robert Boyle lived from _____ to _____.
 Definition
Robert Boyle lived from 1627 to 1691.
Term
Antoine Lavoisier lived from _____ to _____.
 Definition
Antoine Lavoisier lived from 1743 to 1794.
Term
Antoine Lavoisier measured the _____ of the substances that _______ together and the substance _______ in many_______ _________.
 Definition
Antoine Lavoisier measured the masses of the substances that reacted together and the substance produced in many chemical reactions.
Term
_________ _________ measured the masses of the substances that reacted together and the substance produced in many chemical reactions.
 Definition
Antoine Lavoisier measured the masses of the substances that reacted together and the substance produced in many chemical reactions.
Term
_________ _________ discovered that mass is neither produced nor lost during a chemical reaction (Law of Conservation of Mass).
 Definition
Antoine Lavoisier discovered that mass is neither produced nor lost during a chemical reaction (Law of Conservation of Mass).
Term
Antoine Lavoisier discovered that mass is neither _________ nor _____ during a ________ __________ (Law of Conservation of Mass).
 Definition
Antoine Lavoisier discovered that mass is neither produced nor lost during a chemical reaction (Law of Conservation of Mass).
Term
Antoine Lavoisier discovered that mass is neither produced nor lost during a chemical reaction (Law ___ ____________ ___ _____).
 Definition
Antoine Lavoisier discovered that mass is neither produced nor lost during a chemical reaction (Law of Conservation of Mass).
Term
Antoine Lavoisier was a ________ ___________.
 Definition
Antoine Lavoisier was a French scientist.
Term
The works of _______, _________, ________ & ______ illustrate the role of evidence in the development of the model of the atom.
 Definition
The works of Dalton, Thomson, Rutherford, and Bohr illustrate the role of evidence in the development of the model of the atom.
Term
The works of Dalton, Thomson, Rutherford, and Bohr illustrate the role of evidence in the ______________ ____ ____ ________ ___ ____ _______.
 Definition
The works of Dalton, Thomson, Rutherford, and Bohr illustrate the role of evidence in the development of the model of the atom.
Term
John Dalton lived from _____ - _____.
 Definition
John Dalton lived from 1766-1844.
Term
John Dalton was an ________ ________ & ________.
 Definition
John Dalton was an English Chemist & Physicist.
Term
John Dalton based his model of the atom on experiments he did in _____________ _______ .
 Definition
John Dalton based his model of the atom on experiments he did in combining elements.
Term
John Dalton imagined all atoms were like_____ _____, but they had different _________, like ____, _____, and ________.
 Definition
John Dalton imagined all atoms were like small spheres, but they had different properties like size, mass and colour.
Term
One part of _____ _______ explanation on matter is that all matter is made of small, indivisible particles.
 Definition
One part of John Daltons explanation on matter is that all matter is made of small, indivisible particles.
Term
One part of _____ _______ explanation on matter is that all the atoms of an element are identical in properties such as size and mass.
 Definition
One part of John Daltons explanation on matter is that all the atoms of an element are identical in properties such as size and mass.
Term
One part of _____ _______ explanation on matter is that atoms of different elements have different properties.
 Definition
One part of John Daltons explanation on matter is that atoms of different elements have different properties.
Term
One part of _____ _______ explanation on matter is that atoms of different elements can combine in specific fixed ratios to form new substances.
 Definition
One part of John Daltons explanation on matter is that atoms of different elements can combine in specific fixed ratios to form new substances.
Term
JJ Thomson lived from _____ - _____ .
 Definition
JJ Thomson lived from 1856-1940.
Term
JJ Thomson's theories suggested that _____ of different ________ contained ________ particles that were _________.
 Definition
JJ Thomson's theories suggested that atoms of different elements contained smaller particles that were identical.
Term
JJ Thomson's model stated that all _____ are made of smaller _________ particles put together in different combinations to make the different ________.
 Definition
JJ Thomson's model stated that all atoms are made of smaller subatomic particles put together in different combinations to make the different elements.
Term
Ernest Rutherford lived from _____ - _____.
 Definition
Ernest Rutherford lived from 1871-1937.
Term
___ ________ & ______ _______ worked together in England.
 Definition
JJ Thomson & Ernest Rutherford worked together in England.
Term
Ernest Rutherford did research at _______ University in Montreal.
 Definition
Ernest Rutherford did research at McGill University in Montreal.
Term
Ernest Rutherford performed an experiment that lead to the discovery of the ________ of the _____.
 Definition
Ernest Rutherford performed an experiment that lead to the discovery of the nucleus of the atom.
Term
_______ ___________ performed an experiment that lead to the discovery of the nucleus of the atom.
 Definition
Ernest Rutherford performed an experiment that lead to the discovery of the nucleus of the atom.
Term
_______ ___________ came up with the bowling ball, tissue paper reference.
 Definition
Ernest Rutherford came up with the bowling ball, tissue paper reference.
Term
__________ received the Noble Prize in Chemistry in 1908.
 Definition
Rutherford received the Noble Prize in Chemistry in 1908.
Term
Rutherford received the Noble Prize in Chemistry in _____ .
 Definition
Rutherford received the Noble Prize in Chemistry in 1908.
Term
Neils Bohr lived from ____ - ____ .
 Definition
Neils Bohr lived from 1885-1962.
Term
Neils Bohr was a ______ _______.
 Definition
Neils Bohr was a Danish Physicist.
Term
Neils Bohr worked under __________.
 Definition
Neils Bohr worked under Rutherford.
Term
Neils Bohr's experiments partly explained why the _________ charged electrons do not merge with the __________ charged nucleus. Why is this ?
 Definition
Neils Bohr's experiments partly explained why the negatively charged electrons do not merge with the positively charged nucleus. This is because electrons can not fall below the lowest energy level.
Term
An ________ can not fall into a _____ under normal circumstances.
 Definition
An electron can not fall into a nucleus under normal circumstances.
Term
Todays model of the atom is based on a theory called ________ __________.
 Definition
Todays model of the atom is based on a theory called Quantum Mechanics.
Term
Our current model of an atom can change in the future as scientists learn more about ___ ______ and ____________ _______.
 Definition
Our current model of an atom can change in the future as scientists learn more about the atom and subatomic particles.
Term
There are ____ elements.
 Definition
There are 113 elements.
Term
___ naturally occurring elements.
 Definition
90 naturally occurring elements.
Term
___ synthetic elements.
 Definition
25 synthetic elements.
Term
All the elements can be divided into 3 groups; ______, _______, _________.
 Definition
All the elements can be divided into 3 groups; metals, non-metals & metalloids.
Term
Most elements are ______.
 Definition
Most elements are metals.
Term
Metals are ________ and _______.
 Definition
Metals are malleable and ductile.
Term
___ elements are non-metals.
 Definition
17 elements are non-metals.
Term
Some metalloids conduct electricity, but _____ ____ _____ .
 Definition
Some metalloids conduct electricity, but not very well.
Term
An atom is about _____ in diameter.
 Definition
An atom is about 10^-10 in diameter.
Term
The three kinds of subatomic particles are; _________, ________ & ________.
 Definition
The three kinds of subatomic particles are; electrons, protons & neutrons.
Term
Electrons are __________ charged particles.
 Definition
Electrons are negatively charged particles.
Term
Protones are __________ charged particles.
 Definition
Protons are positively charged particles.
Term
Neutrons are __________ charged particles.
 Definition
Neutrons are neutral particles.
Term
Protons & Neutrons are gathered together in the _______.
 Definition
Protons & Neutrons are gathered together in the nucleus.
Term
________ & ________ are gathered together in the nucleus.
 Definition
Protons & Neutrons are gathered together in the nucleus.
Term
Protons & Neutrons account for more than ____% of the total mass of an atom.
 Definition
Protons & Neutrons account for more than 99.9% of the total mass of an atom.
Term
________ & ________ account for more than 99.9% of the total mass of an atom.
 Definition
Protons & Neutrons account for more than 99.9% of the total mass of an atom.
Term
Electrons account for over ____% of an atom.
 Definition
Electrons account for over 99.9% of an atom.
Term
________ account for over 99.9% volume of an atom.
 Definition
Electrons account for over 99.9% volume of an atom.
Term
The number of electrons that can exist in the different energy levels varies.
 Definition
Term
The number of electrons that can exist in the different energy levels (doesn't vary/varies).
 Definition
The number of electrons that can exist in the different energy levels varies.
Term
The lowest energy level is the one (closest to/farthest from) the nucleus.
 Definition
The lowest energy level is the one closest to the nucleus.
Term
An energy level can be _____, _____ ______ or ________ _____.
 Definition
An energy level can be empty, partly filled or completely filled.
Term
_______ & ________ are attracted to each other because they have different charges. This means that ____ can not collapse.
 Definition
Electrons & Protons are attracted to each other because they have different charges. This means that atoms can not collapse.
Term
The atomic number of a element indicates the number of _____ it has .
 Definition
The atomic number of a element indicates the number of protons it has.
Term
The elements in a period are arranged according to ________ ______ _______.
 Definition
The elements in a period are arranged according to increasing atomic number.
Term
As you move from left to right in a period, each element has one more _______ in its atom.
 Definition
As you move from left to right in a period, each element has one more protons in its atom.
Term
To help distinguish between the isotopes of an element, each isotope is given a number called the ____ _______.
 Definition
To help distinguish between the isotopes of an element, each isotope is given a number called the mass number.
Term
The mass number is an integer equal to the total number of ______ & ________ in the ________ of an atom.
 Definition
The mass number is an integer equal to the total number of protons & neutrons in the nucleus of an atom.
Term
Why aren't electrons included in mass number?
 Definition
Electrons aren't included in mass number because their mass is too small.
Term
You can determine the number of neutrons in an atom by __________ the atomic number from the _____ number.
 Definition
You can determine the number of neutrons in an atom by subtracting the atomic number from the mass number.
Term
_____________
ELEMENT SYMBOL.
_____________.
 Definition
mass number
ELEMENT SYMBOL
atomic number.
Term
The atomic molar mass is the average mass of that specific _________.
 Definition
The atomic molar mass is the average mass of that specific isotope.
Term
Isotopes of the same element (do/do not) have the same mass.
 Definition
Isotopes of the same element do not have the same mass.
Term
In general, atoms are neutral, so the number of________ in an atom equals the number of _________.
 Definition
In general, atoms are neutral, so the number of electrons in an atom equals the number of protons.
Term
Why don't isotopes of the same element have the same mass?
 Definition
Because each isotope has a different number of neutrons in its nucleus.
Term
The process of gaining or losing electrons is called __________.
 Definition
The process of gaining or losing electrons is called ionization.
Term
The result of ionization is the formation of an ____.
 Definition
The result of ionization is the formation of an ion.
Term
An ion is an __________ charged atom or group of atoms.
 Definition
At ion is an electrically charged atom or group of atoms.
Term
Positively charged ions are called ______.
 Definition
Positively charged ions are called cations.
Term
Most cations form when metal atoms _____ ________. When a cation is forming, the ____ ________ usually move to another atom. Electrons are _________ charged. When they leave an atom, the ion that remains is positively charged because it now has more _________ than _________.
 Definition
Most cations form when metal atoms lose electrons. When a cation is forming the lost electrons usually move to another atom. Electrons are negatively charged. When they leave an atom, the ion that remains is positively charged because it now has more protons than electrons.
Term
An ions ______ is sometimes shown as a superscript after the atomic symbol.
 Definition
An ions charge is sometimes shown as a superscript after the atomic symbol.
Term
Negatively charged ions are called ______.
 Definition
Negatively charged ions are called anions. (THINK ONIONS).
Term
Most anions from when non-metals ____ _(#)_ ________.
 Definition
Most anions from when non-metals gain two electrons.
Term
Most ion formation takes place when ______ & _________ form ionic compounds.
 Definition
Most ion formation takes place when metals & non-metals form ionic compounds.
Term
Most ion formation takes place when metals & non-metals form _____ __________.
 Definition
Most ion formation takes place when metals & non-metals form ionic compounds.
Term
Metal atoms tend to form cations by losing electrons to non-metals, which form ______.
 Definition
Metal atoms tend to form cations by losing electrons to non-metals, which form anions.
Term
Atoms gain or lose electrons so that they have the same number of electrons as the nearest _____ ____. This makes them more ______.
 Definition
Atoms gain or lose electrons so that they have the same number or electrons as the nearest noble gas. This makes them more stable.
Term
In chemistry, becoming more stable means becoming less _______.
 Definition
In chemistry, becoming more stable means becoming less reactive.
Term
The elements in the same group or family on the periodic table have similar _______ & ________ ________. One of these properties is reactivity.
 Definition
The elements in the same group or family on the periodic table have similar physical & chemical properties. One of these properties is reactivity.
Term
An element reactivity is related to the number of _______ in its outer energy level.
 Definition
An element reactivity is related to the number of electrons in its outer energy level.
Term
Elements are most stable when they have _______ outer energy levels.
 Definition
Elements are most stable when they have filled outer energy levels.
Term
The process of gaining or losing electrons is called __________.
 Definition
The process of gaining or losing electrons is called ionization.
Term
The result of ionization is the formation of an ____.
 Definition
The result of ionization is the formation of an ion.
Term
An ion is an __________ charged atom or group of atoms.
 Definition
At ion is an electrically charged atom or group of atoms.
Term
Positively charged ions are called ______.
 Definition
Positively charged ions are called cations.
Term
Most cations form when metal atoms _____ ________. When a cation is forming, the ____ ________ usually move to another atom. Electrons are _________ charged. When they leave an atom, the ion that remains is positively charged because it now has more _________ than _________.
 Definition
Most cations form when metal atoms lose electrons. When a cation is forming, the lost electrons usually move to another atom. Electrons are negatively charged. When they leave an atom, the ion that remains is positively charged because it now has more protons than electrons.
Term
An ions ______ is sometimes shown as a superscript after the atomic symbol.
 Definition
An ions charge is sometimes shown as a superscript after the atomic symbol.
Term
Negatively charged ions are called ______.
 Definition
Negatively charged ions are called anions. (THINK ONIONS).
Term
Most anions from when non-metals ____ _(#)_ ________.
 Definition
Most anions from when non-metals gain two electrons.
Term
Most ion formation takes place when ______ & _________ form ionic compounds.
 Definition
Most ion formation takes place when metals & non-metals form ionic compounds.
Term
Most ion formation takes place when metals & non-metals form _____ __________.
 Definition
Most ion formation takes place when metals & non-metals form ionic compounds.
Term
Metal atoms tend to form cations by losing electrons to non-metals, which form ______.
 Definition
Metal atoms tend to form cations by losing electrons to non-metals, which form anions.
Term
Atoms gain or lose electrons so that they have the same number of electrons as the nearest _____ ____. This makes them more ______.
 Definition
Atoms gain or lose electrons so that they have the same number or electrons as the nearest noble gas. This makes them more stable.
Term
In chemistry, becoming more stable means becoming less _______.
 Definition
In chemistry, becoming more stable means becoming less reactive.
Term
Recall the elements in the same group or family on the periodic table have similar _______ & ________ ________. One of these properties is reactivity.
 Definition
Recall the elements in the same group or family on the periodic table have similar physical & chemical properties. One of these properties is reactivity.
Term
An element reactivity is related to the number of _______ in its outer energy level.
 Definition
An element reactivity is related to the number of electrons in its outer energy level.
Term
Elements are most stable when they have _______ outer energy levels.
 Definition
Elements are most stable when they have filled outer energy levels.
Term
Noble gases are very _____.
 Definition
Noble gases are very stable.
Term
Noble gases neither gain nor lose _______.
 Definition
Noble gases neither gain nor lose electrons.
Term
Elements become more stable when they have the same number of electrons in their outer energy level as the nearest _______ _____ does.
 Definition
Elements become more stable when they have the same number of electrons in their outer energy level as the nearest noble gas does.
Term
The electrons in the outer energy level are called _______ _______.
 Definition
The electrons in the outer energy level are called valence electrons.
Term
The tendency to gain or lose electrons is sometimes called _________.
 Definition
The tendency to gain or lose electrons is sometimes called valency.
Term
The term _______ _______ is commonly used to describe the number of electrons an element can gain or lose to combine with other elements.
 Definition
The term valence number is commonly used to describe the number of electrons an element can gain or lose to combine with other elements.
Term
Elements in the same family have the same number of _________ electrons. This results in similar chemical properties.
 Definition
Elements in the same family have the same number of valence electrons. This results in similar chemical properties.
Term
From left to right across a period, atoms gain one ________ _________ (and one proton) with each new element.
 Definition
From left to right across a period, atoms gain one valence electron (and one proton) with each new element.
Term
Within a period, electrons are always added to the same _______ level.
 Definition
Within a period, electrons are always added to the same energy level.
Term
An element in the second period has electrons in ___ energy levels, and an element in the third period has electrons in ____ energy levels.
 Definition
An element in the second period has electrons two energy levels, and an element in the third energy level has electrons in three energy levels.
Term
The period number indicates the number of _______ ______ ____.
 Definition
The period number indicates the number of occupied energy levels.
Term
Another way to understand the patterns by which atoms gain or lose electrons is to look at their ______ ______.
 Definition
Another way to understand the patterns by which atoms gain or lose electrons is to look at theirs energy levels.
Term
All of the _____ _____ have filled energy levels.
 Definition
All of the noble gases have filled energy levels.
Term
Atoms tend to gain or lose _______ so that they end up with completely ______ energy levels.
 Definition
Atoms tend to gain or lose electrons so that they end up with completely filled energy levels.
Term
What is another name for the Octet Rule ?
 Definition
The Rule of Eight.
Term
What is another name for The Rule of Eight ?
 Definition
The Octet Rule
Term
The ______ _____ states that atoms bond in such a way as to have eight electrons in their valence energy level.
 Definition
The Octet Rule states that atoms bond in such a way as to have eight electrons in their valence energy level.
Term
The Octet Rule states that atoms bond in such a way as to have eight electrons in their ________ _______ ______.
 Definition
The Octet Rule states that atoms bond in such a way as to have eight electrons in their valence energy level.
Term
The Octet Rule is just another way of saying that atoms tend to be stable with ____ outer energy levels.
 Definition
The Octet Rule is just another way of saying that atoms tend to be stable with full outer energy levels.
Term
The ______ ____ is just another way of saying that atoms tend to be stable with full outer energy levels.
 Definition
The Octet Rule is just another way of saying that atoms tend to be stable with full outer energy levels.
Term
You can figure out an element's ______ or _______ by looking for the octet.
 Definition
You can figure out an element's charge or valence by looking for the octet.
Term
You can figure out an element's charge or valence by looking for the _____.
 Definition
You can figure out an element's charge or valence by looking for the octet.
Term
The exceptions of the octet rule are _______, _________ & _________. They each need only two ________ in their valence energy levels because their nearest noble gas, helium, has two electrons.
 Definition
The exceptions of the octet rule are hydrogen, lithium & beryllium. They each need only two electrons in their valence energy levels because their nearest noble gas, helium, has two electrons.
Term
The exceptions of the octet rule are hydrogen, lithium & beryllium. They each need only two electrons in their valence energy levels because their nearest noble gas, _______, has two electrons.
 Definition
The exceptions of the octet rule are hydrogen, lithium & beryllium. They each need only two electrons in their valence energy levels because their nearest noble gas, helium, has two electrons.
Term
All metals tend to lose electrons to become more stable, but it is difficult for atoms to lose more than about _____ electrons. This is because every time an electron is lost, the remaining electrons are held more closely by the _______. Predicting the number of electrons transition metals will lose is difficult.
 Definition
All metals tend to lose electrons to become more stable, but it is difficult for atoms to lose more than about three electrons. This is because every time an electron is lost, the remaining electrons are held more closely by the nucleus. Predicting the number of electrons transition metals will lose is difficult.
Term
When consulting the period table for the ion charge of an element, the ______ charge is the most common.
 Definition
When consulting the period table for the ion charge of an element, the first charge is the most common.
Term
Who is responsible for naming compounds?
 Definition
The International Union of Pure and Applied Chemistry.
Term
What does IUPAC stand for?
 Definition
The International Union of Pure and Applied Chemistry.
Term
_____ is used for electrical messaging in our bodies. Salt conducts the electrical signals in our nerves because it forms ____.
 Definition
Salt is used for electrical messaging in our bodies. Salt conducts the electrical signals in our nerves because it forms ions.
Term
Salt belongs to a class of substances called ____ _______.
 Definition
Salt belongs to a class of substances called ionic compounds.
Term
Ionic compounds form when ________ transfer from one atom to another.
 Definition
Ionic compounds form when electrons transfer form one atom to another.
Term
The two kinds of ions group together in an organized array called ______ _______.
 Definition
The two kinds of ions group together in an organized array called crystal lattice.
Term
The most stable atoms have ____ ______ _____ ______.
 Definition
The most stable atoms have full outer energy levels.
Term
When sodium transfers an electron to ______, sodium's energy level is now full. When _______ receives the electron, its outer energy level is also now full. This type of bonding in called _____ bonding.
 Definition
When sodium transfers an electron to chlorine, sodium's energy level is now full. When chlorine receives the electron, its out energy level is also now full. This type of bonding is called ionic bonding.
Term
Ionic bonds form between atoms of _____ and _________.
 Definition
Ionic bonds form between atoms of metals and non-metals.
Term
Ionic compounds are all _____ at room temperature.
 Definition
Ionic compounds are all solid at room temperature.
Term
Ionic compounds tend to ______ in water, although some do so better than others.
 Definition
Ionic compounds tend to dissolve in water, although some do so better than others.
Term
Solutions of ionic compounds always _______ _________.
 Definition
Solutions of ionic compounds always conduct electricity.
Term
All names of ionic compounds have ___ parts, because all ionic compounds are made from ___ parts.
 Definition
All names of ionic compounds have two parts, because all ionic compounds are made from two parts.
Term
Every ionic compound is made up of a ____ (positive) and an ______ (negative).
 Definition
Every ionic compound is made up of a cation (positive) and an anion (negative).
Term
The naming rule of ionic compounds is;
1) Name the ____ first by using the element's name. (Usually a metal ion).
2) Name the _____ second by using the first part of the element's name and changing the last part to "-ide." (The anion is usually a non-metal ion.)

Ex. Sodium+Chlorine = ________ _______.
 Definition
The naming rule of ionic compounds is;
1) Name the cation first by using the element's name. (Usually a metal ion).
2) Name the anion second by using the first part of the element's name and changing the last part to "-ide." (The anion is usually a non-metal ion.)

Ex. Sodium + Chlorine = Sodium Chloride.
Term
The formula of an ionic compound contains element symbols that identify each type of ___ present. In some formulas, the symbols are followed by subscript numbers that indicate the ratio of ions in the compound.
 Definition
The formula of an ionic compound contains element symbols that identify each type of ion present. In some formulas, the symbols are followed by subscript numbers that indicate the ratio of ions in the compound.
Term
The _______ ____ is the smallest amount of a substance with the composition shown by the chemical formula. It consists of cations and anions in the smallest whole-number ratio that results in a neutral unit in the crystal lattice of a compound. If there are no subscripts, assume that the compound has ___ cation and ___ anion.
 Definition
The formula unit is the smallest amount of a substance with the composition shown by the chemical formula. It consists of cations and anions in the smallest whole-number ratio that results in a neutral unit in the crystal lattice of a compound. If there are no subscripts, assume that the compound has one cation and one anion.
Term
All ionic compounds are composed of an _____ number of positive and negative charges. Meaning the total charge of the ______ must equal the total charge of the _____.
 Definition
All ionic compounds are composed of an even number of positive and negative charges. Meaning the total charge of the anions must equal the total charge of the cations.
Term
In some compounds the cation has a charge of 1+ and the anion has a charge of 1-. Why does this happen?

Ex. Na^+ + Cl^- = NaCl.
 Definition
This happens because there has been a transfer of electrons between the atoms.

Ex. Na^+ + Cl^- = NaCl.
Term
Al^3+ + Cl ^- =AlCl^^3

What is the Al:Cl Ratio ?
 Definition
Al^3+ + Cl ^- =AlCl^^3

The Al:Cl ratio is 1:3 because you need 3 atoms of Aluminum for 1 atom of Chloride.
Term
The method of lowest common multiple is another way of determining the correct formula for an _____ _______.

1) Find the lowest common multiple of the charges for the two ions.
2) Divide by the combining capacity of one ion to get the correct subscript for that ion.
3) Repeat the process for the other ion.
This process ensures that the number of positive charges is equal to the number of negative charges, so the formula unit is electrically neutral.
 Definition
The method of lowest common multiple is another way of determining the correct formula for an ionic compound.

1) Find the lowest common multiple of the charges for the two ions.
2) Divide by the combining capacity of one ion to get the correct subscript for that ion.
3) Repeat the process for the other ion.
This process ensures that the number of positive charges is equal to the number of negative charges, so the formula unit is electrically neutral.
Term
Steps for writing formulas for Ionic Compounds.

1) Identify the ___ & their ______.
2) Determine the total ______ needed to balance.
3) Note the ratio of _____:______.
4) Use subscript to write the formula if needed.
 Definition
Steps for writing formulas for Ionic Compounds.

1) Identify the ions & their charges.
2) Determine the total charges needed to balance.
3) Note the ratio of cations to anions.
4) Use subscripts to write the formula, if needed.
Term
TRUE or FALSE.
Some metals have more than one stable ion.
 Definition
TRUE.
Term
Elements with more than one stable ion are called ___________ elements.
 Definition
Elements with more than one stable ion are called multivalent elements.
Term
Ionic compounds containing multivalent elements must have _____ ________ in their names to indicate which ion is forming that compound. They are written in brackets after the element to indicate the charge.

Ex. Chromium is multivalent, so chromium(III) sulfide indicates that Cr^3+ ion forms that compound.
 Definition
Ionic compounds containing multivalent elements must have Roman numerals in their names to indicate which ion is forming that compound. They are written in brackets after the element to indicate the charge.

Ex. Chromium is multivalent, so chromium(III) sulfide indicates that Cr^3+ ion forms that compound.
Term
Why aren't Roman Numerals used in formulas ?
 Definition
Because you can figure out the charge on the ion by looking at the formula.
Term
You can use the ______ charge to find the _______ charge when the cation is __________.
 Definition
You can use the anions charge to find the cations charge when the cation is multivalent.
Term
The Roman numeral is needed only if the metal element is __________.
 Definition
The Roman numeral is need only if the metal element is multivalent.
Term
The ________ _____ will tell you if an element is multivalent.
 Definition
The Periodic Table will tell you if an element is multivalent.
Term
Some ions are made up of several non-metallic ______ joined together. These are called ____________ _____.
 Definition
Some ions are made up of several non-metallic atoms joined together. These are called polyatomic ions.
Term
Poly means ____.
 Definition
Poly means many.
Term
Polyatomic Ions usually move through chemical reactions _______.
 Definition
Polyatomic Ions usually move through chemical reaction intact.
Term
The correct way to show polyatomic ions is by writing the formula with its ___ ______.
 Definition
The correct way to show polyatomic ions is by writting the formula with its ion charge.
Term
What are the two most common suffixes used in naming polyatomic ions ?
 Definition
"-ate" and "ite".
Term
____ means more oxygen atoms are part of the ion.
 Definition
"-ate" means more oxygen atoms are part of the ion.
Term
____ means less oxygen atoms are part of the ion.
 Definition
"-ite" means less oxygen atoms are part of the ion.
Term
Naming Compounds Containing Polyatomic Ions.

1) Name the _______.
2) Name the _______.
3) You do not need to change the ending of a polyatomic ion's name.
 Definition
Naming Compounds Containing Polyatomic Ions.

1) Name the cation.
2) Name the anion.
3) You do not need to change the ending of a polyatomic ion's name.
Term
Methane is the chemical name for _________ ____.
 Definition
Methane is the chemical name for natural gas.
Term
A _________ forms when two or more non-mettalic atoms bond together. It can be made up of atoms of different elements or of atoms of all the same element.
 Definition
A molecule forms when two or more non-mettalic atoms bond together. It can be made up of atoms of different elements or of atoms of all the same element.
Term
The formula unit of an ______ ________, represents a ratio of ions in a crystal lattice.
 Definition
The formula unit of an ionic compound, represents a ratio of ions in a crystal lattice.
Term
TRUE OR FALSE

A formula is an independent unit.
 Definition
FALSE

A formula is not an independent unit, it is just one part of a crystal lattice.
Term
_________ are independent units made up of fixed numbers of atoms bonded together.
 Definition
Molecules are independent units made up of fixed numbers of atoms bonded together.
Term
Molecular substances can be solid, liquid or gas at room temperature, unlike _____ _________.
 Definition
Molecular substances can be solid, liquid or gas at room temperature, unlike ionic compounds.
Term
In general are molecular substances good conductors of electricity ?
 Definition
No, molecular substances tend to be poor conductors of electricity, even in solution.
Term
In general, do molecular substances tend to dissolve in water well ?
 Definition
No, many molecular substances do not dissolve in water well.
Term
The atoms in a molecule are joined together by ________ _____.
 Definition
The atoms in a molecule are joined together by covalent bonds.
Term
How do covalent bonds form ?
 Definition
Covalent bonds form when atoms share electrons.
Term
Each pair of shared _________ forms one covalent bond.
 Definition
Each pair of shared electrons forms one covalent bond.
Term
Are atoms transferred from one atom to another in covalent bonds ?
 Definition
No.
Term
Are atoms transferred from one atom to another in ionic bonds ?
 Definition
Yes.
Term
Nitrogen is known as a _________ ______ because it forms molecules made up of only one type of atom. Its molecules are _________.
 Definition
Nitrogen iss known as a molecular element because it forms molecules made up of only one type of atom. Its molecules are diatomic.
Term
________ means that each molecule is composed of only two atoms.
 Definition
Diatomic means that each molecule is composed of only two atoms.
Term
TRUE OR FALSE

Some elements form polyatomic molecules.
 Definition
TRUE

Some elements form polyatomic molecules.
Term
Monatomic, Diatomic or Polyatomic ?

C
 Definition
Monatomic
Term
Monatomic, Diatomic or Polyatomic ?

Noble Gases
 Definition
Monatomic
Term
Monatomic, Diatomic or Polyatomic ?

All metals.
 Definition
Monatomic
Term
Monatomic, Diatomic or Polyatomic ?

H₂
 Definition
Diatomic
Term
Monatomic, Diatomic or Polyatomic ?

N₂
 Definition
Diatomic
Term
Monatomic, Diatomic or Polyatomic ?

O₂
 Definition
Diatomic
Term
Monatomic, Diatomic or Polyatomic ?

F₂
 Definition
Diatomic
Term
Monatomic, Diatomic or Polyatomic ?

Cl₂
 Definition
Diatomic
Term
Monatomic, Diatomic or Polyatomic ?

Br₂
 Definition
Diatomic
Term
Monatomic, Diatomic or Polyatomic ?

I₂
 Definition
Diatomic
Term
Monatomic, Diatomic or Polyatomic ?

O₃
 Definition
Polyatomic
Term
Monatomic, Diatomic or Polyatomic ?

P₄
 Definition
Polyatomic
Term
Monatomic, Diatomic or Polyatomic ?

S₈
 Definition
Polyatomic
Term
What number does this prefix stand for ?

mono
 Definition
1
Term
What number does this prefix stand for ?

di
 Definition
2
Term
What number does this prefix stand for ?

tri
 Definition
3
Term
What number does this prefix stand for ?

tetra
 Definition
4
Term
What number does this prefix stand for ?

penta
 Definition
5
Term
What number does this prefix stand for ?

hexa
 Definition
6
Term
What number does this prefix stand for ?

hepta
 Definition
7
Term
What number does this prefix stand for ?

octa
 Definition
8
Term
What number does this prefix stand for ?

ennea (nona)
 Definition
9
Term
What number does this prefix stand for ?

deca
 Definition
10
Term
A binary compound contains ___ elements.
 Definition
A binary compound contains two elements.
Term
TRUE OR FALSE

All binary compounds contain hydrogen.
 Definition
FALSE

Some binary compounds contain hydrogen, and some do not.
Term
For molecules, Greek prefixes are used to indicate how many ______ of each ________ are present in the compound.
 Definition
For molecules, Greek prefixes are used to indicate how many atoms of each element are present in the compound.
Term
Any compound that does not have a metal or an ammonium ion in its formula is ________.
 Definition
Any compound that does not have a metal or an ammonium ion in its formula is molecular.
Term
Format for naming binary molecular compounds not containing hydrogen is :

_______ + first element followed by prefix + second element ending in "-ide".
 Definition
Format for naming binary molecular compounds not containing hydrogen is :

prefix + first element followed by prefix + second element ending in "-ide".
Term
Format for naming binary molecular compounds not containing hydrogen is :

prefix + ______ _______ _______ ___ _______ + second element ending in "-ide".
 Definition
Format for naming binary molecular compounds not containing hydrogen is :

prefix + first element followed by prefix + second element ending in "-ide".
Term
Format for naming binary molecular compounds not containing hydrogen is :

prefix + first element followed by prefix + ________ ________ ________ ___ _____.
 Definition
Format for naming binary molecular compounds not containing hydrogen is :

prefix + first element followed by prefix + second element ending in "-ide".
Term
What is the name of this Binary Molecular Compound ?

CO (g)
 Definition
Carbon monoxide
Term
What is the name of this Binary Molecular Compound ?

SO₂ (g)
 Definition
Sulfer dioxide
Term
What is the name of this Binary Molecular Compound ?

CS₂ (g)
 Definition
Carbon disulfide
Term
What is the name of this Binary Molecular Compound ?

N₂O₃ (g)
 Definition
Dinitrogen trioxide
Term
What is the name of this Binary Molecular Compound ?

CCl₄
 Definition
Carbon tetrachloride
Term
What is the name of this Binary Molecular Compound ?

P₄0₁₀
 Definition
Tetraphosphorus decaoxide
Term
What is the IUPAC name for this formula ?

H₂O
 Definition
Water
Term
What is the IUPAC name for this formula ?

H₂O₂
 Definition
Hydrogen Peroxide
Term
What is the IUPAC name for this formula ?

NH₃
 Definition
Ammonia
Term
What is the IUPAC name for this formula ?

C₁₂H₂₂O₁₁
 Definition
Sucrose
Term
What is the IUPAC name for this formula ?

CH₄
 Definition
Methane
Term
What is the IUPAC name for this formula ?

C₃H₈
 Definition
Propane
Term
What is the IUPAC name for this formula ?

CH₃OH
 Definition
Methanol
Term
What is the IUPAC name for this formula ?

C₂H₅OH
 Definition
Ethanol
Term
What is the IUPAC name for this formula ?

H₂S
 Definition
Hydrogen Sulfide
Term
TRUE OR FALSE

Many important compounds are not ionic.
 Definition
TRUE

Many important compounds are not ionic.
Term
Water, methane, wax, caffeine & glucose are all __________ ________.
 Definition
Water, methane, wax, caffeine & glucose are all molecular compounds.
Term
Ionic compounds always contain _______ & _________.
 Definition
Ionic compounds always contain cations & anions.
Term
You can recognize an ionic compound by inspecting its formula, and noting the presence of a ________.
 Definition
You can recognize an ionic compound by inspecting its formula, and noting the presence of a cation.
Term
Ionic compounds have ____ melting points.
 Definition
Ionic compounds have high melting points.
Term
The attractions between the cation and the anions in a solid ionic compound are so strong that the ions are held in the tight, highly organized ______ _______. A ______ amount of energy must be added in the form of _____ before the ions can begin to move past each other in the liquid state.
 Definition
The attractions between the cation and the anions in a solid ionic compound are so strong that the ions are held in the tight, highly organized crystal lattice. A high amount of energy must be added in the form of heat before the ions can begin to move past each other in the liquid state.
Term
When a crystal is hit, positive ions lines up with each other, and negative ions line up with each other causing the crystal to break into a perfectly ____ ________. Ionic compounds retain their crystal shape.
 Definition
When a crystal is hit, positive ions lines up with each other, and negative ions line up with each other causing the crystal to break into a perfectly flat surface. Ionic compounds retain their crystal shape.
Term
All ionic compounds dissolve in water to some extent because both cations and anions are strongly attracted to water molecules. This occurs because each water molecule is _______.
 Definition
All ionic compounds dissolve in water to some extent because both cations and anions are strongly attracted to water molecules. This occurs because each water molecule is polar.
Term
TRUE OR FALSE

When an ionic crystal is placed in water, some ions on the surface of the undissolved crystal are attracted into the water.
 Definition
TRUE.

When an ionic crystal is placed in water, some ions on the surface of the undissolved crystal are attracted into the water.
Term
Are solutions containing ionic compounds good conductors of electricity ?
 Definition
Yes, solutions containing ionic compounds are good conductors of electricity, unlike pure water, which has almost no conductivity.
Term
TRUE OR FALSE.

The greater the concentration of ions in solution, the less conductive the solution is.
 Definition
FALSE.

The greater the concentration of ions in solution, the more conductive the solution is.
Term
Solutions of ionic compounds are considered to be excellent ____________.
 Definition
Solutions of ionic compounds are considered to be excellent electrolytes.
Term
An electrolyte is any solution that can conduct ___________.
 Definition
An electrolyte is any solution that can conduct electricity.
Term
TRUE OR FALSE.

If a solution does not contain ions, it will not conduct.
 Definition
TRUE.

If a solution does not contain ions, it will not conduct.
Term
A substance that dissolves well is considered to be very ________.
 Definition
A substance that dissolves well is considered to be very soluble.
Term
TRUE OR FALSE.

A chemical formula would be followed by the subscript (aq) when it's in solution.
 Definition
TRUE.

A chemical formula would be followed by the subscript (aq) when it's in solution.
Term
Are Alkali metals are very soluble ?
 Definition
Yes.
Term
TRUE OR FALSE.

Most compounds that contain chloride ions are soluble, with a few exceptions.
 Definition
TRUE.

Most compounds that contain chloride ions are soluble, with few exceptions.
Term
TRUE OR FALSE.

Most phosphates and carbonates are very soluble.
 Definition
FALSE.

Most phosphates and carbonates are only slightly soluble.
Term
Sometimes, when ionic solutions are mixed they form a _________.
 Definition
Sometimes, when ionic solutions are mixed they form a precipitate.
Term
A precipitate is a solid with low solubility that forms a __________.
 Definition
A precipitate is a solid with low solubility that forms a solution.
Term
Precipitates may form when solutions of two different ______ compounds are mixed.
 Definition
Precipitates may form when solutions of two different ionic compounds are mixed.
Term
___________ is the process involved in forming a precipitate.
 Definition
Precipitation is the process involved in forming a precipitate.
Term
Molecular compounds are made up of _________.
 Definition
Molecular compounds are made up of molecules.
Term
TRUE OR FALSE.

Each molecule of a compound always has the same number and proportion of atoms in it.
 Definition
TRUE.

Each molecule of a compound always has the same number and proportion of atoms in it.
Term
The attraction between individual atoms in a molecule is very ______. The attraction between neighboring molecules is ______.
 Definition
The attraction between individual atoms in a molecule is very strong. The attraction between neighboring molecules is weak.
Term
Do molecular compounds have a higher melting point or a lower melting point than ionic compounds ?
 Definition
The melting points of molecular compounds tend to be much lower than the melting points of ionic compounds.
Term
TRUE OR FALSE.

In molecular compounds, only a small amount of energy is required for the molecules to begin sliding past one another.
 Definition
TRUE.

In molecular compounds, only a small amount of energy is required for the molecules to begin sliding past one another.
Term
Can crystals of molecular compounds crumble easily ?
 Definition
Yes, Unlike crystals of ionic compounds, crystals of molecular compounds crumble easily. The relatively weak attractions between molecules mean that the crystals do not hole their shape.
Term
All molecules are electrically ________, both as solids and in solutions, so they _____ conduct electricity in either state.
 Definition
All molecules are electrically neutral, both as solids and in solutions, so they don't conduct electricity in either state.
Term
Precipitates may form when solutions of two different ______ compounds are mixed.
 Definition
Precipitates may form when solutions of two different ionic compounds are mixed.
Term
___________ is the process involved in forming a precipitate.
 Definition
Precipitation is the process involved in forming a precipitate.
Term
Molecular compounds are made up of _________.
 Definition
Molecular compounds are made up of molecules.
Term
TRUE OR FALSE.

Each molecule of a compound always has the same number and proportion of atoms in it.
 Definition
TRUE.

Each molecule of a compound always has the same number and proportion of atoms in it.
Term
The attraction between individual atoms in a molecule is very ______. The attraction between neighboring molecules is ______.
 Definition
The attraction between individual atoms in a molecule is very strong. The attraction between neighboring molecules is weak.
Term
Do molecular compounds have a higher melting point or a lower melting point than ionic compounds ?
 Definition
The melting points of molecular compounds tend to be much lower than the melting points of ionic compounds.
Term
TRUE OR FALSE.

In molecular compounds, only a small amount of energy is required for the molecules to begin sliding past one another.
 Definition
TRUE.

In molecular compounds, only a small amount of energy is required for the molecules to begin sliding past one another.
Term
Can crystals of molecular compounds crumble easily ?
 Definition
Yes, Unlike crystals of ionic compounds, crystals of molecular compounds crumble easily. The relatively weak attractions between molecules mean that the crystals do not hole their shape.
Term
All molecules are electrically ________, both as solids and in solutions, so they _____ conduct electricity in either state.
 Definition
All molecules are electrically neutral, both as solids and in solutions, so they don't conduct electricity in either state.
Term
Is water polar ?
 Definition
Yes, one of water's most important properties is that it is polar; each water molecule has a negative end and a positive end. Water has this interesting property because of its bent shape and because of the unequal sharing of electrons in the bonds holding the hydrogen and oxygen together. This makes the oxygen end of water slightly negative and the hydrogen side slightly positive.
Term
TRUE OR FALSE

Water would boil at a much higher temperature if it was not polar.
 Definition
FALSE.

Water would boil at a much lower temperature if it was not polar, at about -80˚C.
Term
If water was not ______, oceans would be boiling year round.
 Definition
If water was not polar, oceans would be boiling year round.
Term
TRUE OR FALSE

As liquid turns to ice, the molecules spread out.
 Definition
TRUE.

As liquid turns to ice, the molecules spread out.
Term
Are there few molecules in a litre of ice or a litre of water ?
 Definition
The ordering of water molecules in ice also means that there are fewer molecules in a litre of ice than in a litre of water, so that liquid water is denser than ice. This is why ice floats.
Term
An _____ is a compound that dissolves in water to form a solution with a pH lower than 7.
 Definition
An acid is a compound that dissolves in water to form a solution with a pH lower than 7.
Term
A _____ is a compound that dissolves in water to form a solution with a pH greater than 7.
 Definition
A base is a compound that dissolves in water to form a solution with a pH greater than 7.
Term
The ___ measurement indicates how acidic or basic a substance is.
 Definition
The pH measurement indicates how acidic or basic a substance is.
Term
An organ called the _______ produces sodium hydrogencarbonate and other bases that neutralize stomach acid.
 Definition
An organ called the pancreas produces sodium hydrogencarbonate and other bases that neutralize stomach acid.
Term
TRUE OR FALSE.

When acids and bases are neutralized, they lose their characteristic properties.
 Definition
TRUE.

When acids and bases are neutralized, they lose their characteristic properties.
Term
Sodium hydrogencarbonate is an example of a _______. It is a substance that can keep the pH of a solution nearly constant despite the addition of a small amount of acid or base.
 Definition
Sodium hydrogencarbonate is an example of a buffer. It is a substance that can keep the pH of a solution nearly constant despite the addition of a small amount of acid or base.
Term
TRUE OR FALSE.

Adding a metal to a solution could help determine if the solution is acidic or basic.
 Definition
TRUE.

Adding a metal to a solution could help determine if the solution is acidic or basic. Acids react with metals, although some acids, such as nitric acid, react more vigorously with metals than other acids. Most bases do not attack metals.
Term
ACID
RED
BASE
BLUE.
 Definition
DD
BB
Term
Is this property acidic or basic ?

taste : sour
 Definition
acidic
Term
Is this property acidic or basic ?

touch : not slippery
 Definition
acidic
Term
Is this property acidic or basic ?

reaction with metals : metal corrodes H₂ bubbles form
 Definition
acidic
Term
Is this property acidic or basic ?

litmus indicator : red
 Definition
acidic
Term
Is this property acidic or basic ?

electrical conductivity : conductive
 Definition
acidic
Term
Is this property acidic or basic ?

taste : bitter
 Definition
basic
Term
Is this property acidic or basic ?

touch : slippery
 Definition
basic
Term
Is this property acidic or basic ?

reaction with metals : no reaction
 Definition
basic
Term
Is this property acidic or basic ?

litmus indicator : blue
 Definition
basic
Term
Is this property acidic or basic ?

electrical conductivity : conductive
 Definition
basic
Term
Is this property acidic or basic ?

pH of solution : >7
 Definition
basic
Term
Is this property acidic or basic ?

pH of solution : <7
 Definition
acidic
Term
Mixtures in which separate components are not visible are called ___________ mixtures.
 Definition
Mixtures in which separate components are not visible are called homogeneous mixtures.
Term
In fermentation by bacteria, starch and sugars present in food are converted into _____ _____.
 Definition
In fermentation by bacteria, starch and sugars present in food are converted into lactic acid.
Term
The names of acids that contain hydrogen and one other non-metallic element can be written with the prefix _______ and the suffix ___.
 Definition
The names of acids that⁻ contain hydrogen and one other non-metallic element can be written with the prefix "hydro-" and the suffix "-ic". EX. HYDROCHLORIC ACID,
Term
Bases are (more/less) difficult to recognize by their formulas than acids are.
 Definition
Bases are more difficult to recognize by their formulas than acids are.
Term
The presence of the hydroxide ion (OH⁻) with a metal ion or the ammonium ion usually indicates that a substance is _____.
 Definition
The presence of the hydroxide ion (OH⁻) with a metal ion or the ammonium ion usually indicates that a substance is basic.
Term
When ammonia is dissolved in water, the resulting solution is ______.
 Definition
When ammonia is dissolved in water, the resulting solution is basic.
Term
Any compound with ____ solubility and an ___ on the right side of the formula is a base.
 Definition
Any compound with high solubility and an OH on the right side of the formula is a base.
Term
When acids and bases react together, both acidic and basic properties disappear. This is the process of _____________.
 Definition
When acids and bases react together, both acidic and basic properties disappear. This is the process of neutralization.
Term
Neutralization is the reaction between an acid and a base that produces _____ & _____.
 Definition
Neutralization is the reaction between an acid and a base that produces water & salt.
Term
All substances, natural and manufactured, are _______.
 Definition
All substances, neutral and manufactured, are chemicals.
Term
___________ (____) are non-toxic, non-flammable chemicals used mostly in cooling systems.
 Definition
Chloroflourocarbons (CFCs) are non-toxic, non-flammable chemicals used mostly in cooling systems.
Term
Many people use chemical substances for recreational purposes, and some of these substances can be toxic. The two most commonly used hazardous recreation chemicals are _______ & ________.
 Definition
Many people use chemical substances for recreational purposes, and some of these substances can be toxic. The two most commonly used hazardous recreation chemicals are alcohol & nicotine.
Term
The alcohol used in beverages is ________.
 Definition
The alcohol used in beverages is ethanol.
Term
TRUE OR FALSE.

Alcohol abuse can lead to psychological dependance.
 Definition
TRUE.

Alcohol abuse can lead to psychological dependance.
Term
A heavy smoke has a __x greater chance of developing lung cancer than a non-smoker does.
 Definition
A heavy smoker has a 20x greater chance of developing lung cancer than a non-smoker does.
Term
We can manage hazardous substances through a combination of :
1) Understanding the properties of __________;
2) Using careful and clever design and process engineering;
3) Placing ________ ________ and environmental protection as the top priority; and
4) Enforcing effective regulations.
 Definition
We can manage hazardous substances through a combination of :
1) Understanding the properties of materials;
2) Using careful and clever design and process engineering;
3) Placing personal safety and environmental protection as the top priority; and
4) Enforcing effective regulations.
Term
Chemical change occurs when a substance or substances react in a ______ ______ to create a different substance or substances. The substances that react are called _________, and their reaction produces new substances called ________. The products have completely different properties from the reactants.
 Definition
Chemical change occurs when a substance or substances react in a chemical reaction to create a different substance or substances. The substances that react are called reactants, and their reaction produces new substances called products. The products have completely different properties from the reactants.
Term
Chemical changes are always accompanied by ______ _____. These _____ of _______ into or out of systems drive chemical reactions.
 Definition
Chemical changes are always accompanied by energy flows. These flows of energy into or out of our systems drive chemical reactions.
Term
TRUE OR FALSE

All chemical reactions are fast.
 Definition
FALSE.

Not all chemical reactions are fast.
Term
Metals are _____, except mercury which is liquid.
 Definition
Metals are solid, except mercury which is liquid.
Term
Metals are solid, except _______ which is liquid.
 Definition
Metals are solid, except mercury which is liquid.
Term
Most of the diatomic elements are gases: ___, ___, ___, ___, and ___. Bromine is a liquid and iodine is a solid: ___, ___.
 Definition
Most of the diatomic elements are gases: H₂, N₂, O₂, F₂, and Cl₂. Bromine is a liquid and iodine is a solid: Br₂ and I₂.
Term
What state are Sulfur, phosphorus, and carbon at room temperature ?
 Definition

Sulfur, phosphorus, and carbon are solids at room temperature.

 
Term
All ionic compounds are ____ at room temperature.
 Definition
All ionic compounds are solid at room temperature.
Term
All ionic compound that is very ______ is shown as aqueous when it is dissolved in water. An ionic compound that is slightly soluble is usually shown as a solid, even when its water.
 Definition
All ionic compound that is very soluble is shown as aqueous when it is dissolved in water. An ionic compound that is slightly soluble is usually shown as a solid, even when its water.
Term
Molecular compounds are very difficult to predict the state of. The ______ the molecules are, the more they tend to be gases. The _______ they are, the more they tend to be liquids and then solids.
 Definition
Molecular compounds are very difficult to predict the state of. The smaller the molecules are, the more they tend to be gases. The larger they are, the more they tend to be liquids and then solids..
Term
Energy flow is an essential part of any _______ ________.
 Definition
Energy flow is an essential part of any chemical reaction.
Term
____________ reactions release energy, usually in the form of heat, light, or electricity.
 Definition
Exothermic reactions release energy, usually in the form of heat, light or electricity.
Term
An important exothermic reaction is the combustion of fossil fuels: ____, ___, and ______ ___.
 Definition
An important exothermic reaction is the combustion of fossil fuels: coal, oil and natural gas.
Term
An important __________ reaction is the combustion of fossil fuels: coal, oil and natural gas.
 Definition
An important exothermic reaction is the combustion of fossil fuels: coal, oil and natural gas.
Term
_______ is a chemical reaction that occurs when oxygen reacts rapidly with a substance to form a new substance and gives off energy.
 Definition
Combustion is a chemical reaction that occurs when oxygen reacts rapidly with a substance to form a new substance and gives off energy. *burning*
Term
___________ reactions absorb energy.
 Definition
Endothermic reactions absorb energy.
Term
__________ reactions may be endothermic or exothermic.
 Definition
Biochemical reactions may be endothermic or exothermic.
Term
Biochemical reactions may be ___________ or _____________.
 Definition
Biochemical reactions may be endothermic or exothermic.
Term
Biochemical reactions may be ____________ or exothermic.
 Definition
Biochemical reactions may be endothermic or exothermic.
Term
Biochemical reactions may be endothermic or ____________.
 Definition
Biochemical reactions may be endothermic or exothermic.
Term
TRUE OR FALSE.

Biochemical reactions happen at an organism's internal temperature.
 Definition
TRUE.

Biochemical reactions happen at an organism's internal temperature.
Term
Biochemical reactions happen at an organism's internal temperature, and they are almost always helped by ________ (biological catalysts).
 Definition
Biochemical reactions happen at an organism's internal temperature, and they are almost always helped by enzymes (biological catalysts).
Term
Biochemical reactions happen at an organism's internal temperature, and they are almost always helped by enzymes (_________ _________).
 Definition
Biochemical reactions happen at an organism's internal temperature, and they are almost always helped by enzymes (biological catalysts).
Term
________ are chemicals that speed up a reaction but are not used up by it.
 Definition
Catalysts are chemicals that speed up a reaction but are not used up by it.
Term
TRUE OR FALSE.

All of the oxygen in our atmosphere comes from photosynthesis.
 Definition
FALSE.

Most of the oxygen in our atmosphere comes from photosynthesis.
Term
What is the reverse version of photosynthesis ?
 Definition
Cellular respiration is the reverse of photosynthesis. Both plants and animals use cellular respiration to release energy that is then used to drive all the chemical reactions in their tissues and organs.
Term
In an exothermic reaction the energy appears on the ____ side of the equation.
 Definition
In an exothermic reaction the energy appears on the right side of the equation.
Term
In an _____________ reaction the energy appears on the right side of the equation.
 Definition
In an exothermic reaction the energy appears on the right side of the equation.
Term
In an endothermic reaction the energy appears on the ____ side of the equation.
 Definition
In an endothermic reaction the energy appears on the left side of the equation.
Term
In an _____________ reaction the energy appears on the left side of the equation.
 Definition
In an endothermic reaction the energy appears on the left side of the equation.
Term
All reactions involve the production of new substances with their own characteristic properties. These properties include: _____ at room temperature, _______ ____, _____ and _______.
 Definition
All reactions involve the production of new substances with their own characteristic properties. These properties include: state at room temperature, melting point, colour and density.
Term
All reactions involve the ____ of ______. This may be detected by a change in temperature during the reaction. Endothermic reactions absorb energy from the environment. Exothermic reactions release energy from the environment.
 Definition
All reactions involve the flow of energy. This may be detected by a change in temperature during the reaction. Endothermic reactions absorb energy from the environment. Exothermic reactions release energy from the environment.
Term
When new substances form in a chemical reactions, sometimes change of state can be observed, for example, formation of a ___ (bubbles) or a _____ (precipitate).
 Definition
When new substances form in a chemical reactions, sometimes change of state can be observed, for example, formation of a gas (bubbles) or a solid (precipitate).
Term
All chemical reactions are consistent with the law of _____________ ___ _____.
 Definition
All chemical reactions are consistent with the law of conservation of mass.
Term
TRUE OR FALSE

Regardless of the type of chemical reaction, the total mass of the reaction system never changes.
 Definition
TRUE

Regardless of the type of chemical reaction, the total mass of the reaction system never changes.
Term
What theory is this ?

Regardless of the type of chemical reaction, the total mass of the reaction system never changes.
 Definition
The Law of Conservation of Mass.
Term
What theory is this ?

When a system of chemicals reacts completely, the total mass of all the reactants equal the total mass of the products.
 Definition
The Law of Conservation of Mass.
Term
TRUE OR FALSE.

No exceptions to Lavoisier's proposal about the conservation of mass during a chemical reaction are known.
 Definition
TRUE.

No exceptions to Lavoisier's proposal about the conservation of mass during a chemical reaction are known.
Term
Who discovered the Law of Conservation of Mass ?
 Definition
Antoine Lavoisier
Term
TRUE OR FALSE.

The total number of atoms present before a reaction is equal to the total number of atoms present after a reaction.
 Definition
TRUE.

The total number of atoms present before a reaction is equal to the total number of atoms present after a reaction.
Term
A _________ ________ is a process involving chemical change. Chemist record such a process in a _______ _______ that uses chemical symbols and formulas. This equation is a shorthand way of showing what happens during a reaction.
 Definition
A chemical reaction is a process involving chemical change. Chemists record such a process in a chemical equation that uses chemical symbols and formulas. This equation is a shorthand way of showing what happens during a reaction.
Term
TRUE OR FALSE.

The first step in writing a chemical equation is to recognize that a chemical change has actually occurred.
 Definition
TRUE.

The first step in writing a chemical equation is to recognize that a chemical change has actually occurred.
Term
The presence of bubbles indicates that a ___ is being produced.
 Definition
The presence of bubbles indicates that a gas is being produced.
Term
Solid magnesium metal reacts with aqueous __________ _____ to produce aqueous magnesium chloride and hydrogen gas.
 Definition
Solid magnesium metal reacts with aqueous hydrochloric acid to produce aqueous magnesium chloride and hydrogen gas.
Term
Solid __________metal reacts with aqueous hydrochloric acid to produce aqueous magnesium chloride and hydrogen gas.
 Definition
Solid magnesium metal reacts with aqueous hydrochloric acid to produce aqueous magnesium chloride and hydrogen gas.
Term
Solid magnesium metal reacts with aqueous hydrochloric acid to produce aqueous _________ ________ and hydrogen gas.
 Definition
Solid magnesium metal reacts with aqueous hydrochloric acid to produce aqueous magnesium chloride and hydrogen gas.
Term
Solid magnesium metal reacts with aqueous hydrochloric acid to produce aqueous magnesium chloride and _________ ____.
 Definition
Solid magnesium metal reacts with aqueous hydrochloric acid to produce aqueous magnesium chloride and hydrogen gas.
Term
Solid magnesium metal reacts with aqueous hydrochloric acid to produce aqueous __________ _______ and __________ ___.
 Definition
Solid magnesium metal reacts with aqueous hydrochloric acid to produce aqueous magnesium chloride and hydrogen gas.
Term
________ means that the substance is dissolved in water.
 Definition
Aqueous means that the substance is dissolved in water.
Term
What does Aqueous mean ?
 Definition
Aqueous means that the substance is dissolved in water.
Term
TRUE OR FALSE.

In a chemical equation it matters what order the reactants are written.
 Definition
FALSE.

In a chemical equation it does not matter what order the reactants are written.
Term
A ________ _______ shows the identities of the substances involved in the reaction, and which elements are present. Does not show the correct proportions of the reactants and the products.
 Definition
A skeleton equation shows the identities of the substances involved in the reaction, and which elements are present. Does not show the correct proportions of the reactants and the products.
Term
A ________ _________ uses the chemical formulas of reactants and products in a chemical equation to represent a chemical equation.
 Definition
A formula equation uses the chemical formulas of reactants and products in a chemical equation to represent a chemical equation.
Term
TRUE OR FALSE.

An equation is properly balanced if the number of each type of atom on the reactants side of an equation is equal to the number of each type of atom on the products side.
 Definition
TRUE.

An equation is properly balanced if the number of each type of atom on the reactants side of an equation is equal to the number of each type of atom on the products side.
Term
How do you balance an equation ?
 Definition
You balance an equation by making sure that the number of atoms of each element left of the arrow is equal to the number of atoms of each element right of the arrow.
Term
Never change a subscript to balance an equation. Instead, add coefficients.
 Definition
Never change a subscript to balance an equation. Instead, add coefficients.
Term
What are the five common types of reactions ?
 Definition
Formation, Decomposition, Hydrocarbon Combustion, Single Replacement & Double Replacement
Term
In the simplest form of __________ ______, two elements combine to form a compound. This type of reaction is also known as a _________ ________.
 Definition
In the simplest type of formation reaction, two elements combine to form a compound. This type of reaction is also known as a synthesis reaction.
Term
What type of reaction is this ?

element + element ->compound.
 Definition
Formation Reaction
Term
What type of reaction is this ?

A + B -> AB
 Definition
Formation Reaction
Term
What type of reaction is this ?

Word Equation : Sulfur + Oxygen -> Sulfur Dioxide
Skeleton Equation : S₈ + O₂ -> SO₂
 Definition
Formation Reaction
Term
Sulfure dioxide can combine with ______ in the air to form acid rain.
 Definition
Sulfur dioxide can combine with water in the air to form acid rain.
Term
Sulfur dioxide can combine with water in the air to form ____ ____.
 Definition
Sulfur dioxide can combine with water in the air to form acid rain.
Term
What type of reaction is this ?

Word Equation : hydrogen + nitrogen -> ammonia
Skeleton Equation : H₂ + N₂ -> NH₃
 Definition
Formation Reaction.
Term
TRUE OR FALSE.

You cannot always predict the formula of molecular compounds that form because more than one combination of elements is possible.
 Definition
TRUE.

You cannot always predict the formula of molecular compounds that form because more than one combination of elements is possible.
Term
TRUE OR FALSE.

No formation reactions occur between metals and non-metals.
 Definition
FALSE.

Many formation reactions occur between metals and non-metals.
Term
What type of reaction is this ?

Word Equation : sodium + chlorine -> sodium chloride.
Skeleton Equation : Na + Cl₂ -> NaCl
 Definition
Formation Reaction.
Term
When one reactant is a metal and the other is a non-metal, how do you predict the product ?
 Definition
When one reactant is a metal and the other is a non-metal, predict the product by writing the ionic compound they form.
Term
Decomposition Reactions are the opposite of ________ _______.
 Definition
Decompositions Reaction are the opposite of Formation Reactions.
Term
Products can be broken down to yield the reactants again in a ____________ ______.
 Definition
Products can be broken down to yield the reactants again in a decomposition reaction.
Term
In the simplest form of __________ ______, two elements combine to form a compound. This type of reaction is also known as a _________ ________.
 Definition
In the simplest type of formation reaction, two elements combine to form a compound. This type of reaction is also known as a synthesis reaction.
Term
What type of reaction is this ?

element + element ->compound.
 Definition
Formation Reaction
Term
What type of reaction is this ?

A + B -> AB
 Definition
Formation Reaction
Term
What type of reaction is this ?

Word Equation : Sulfur + Oxygen -> Sulfur Dioxide
Skeleton Equation : S₈ + O₂ -> SO₂
 Definition
Formation Reaction
Term
Sulfure dioxide can combine with ______ in the air to form acid rain.
 Definition
Sulfur dioxide can combine with water in the air to form acid rain.
Term
Sulfur dioxide can combine with water in the air to form ____ ____.
 Definition
Sulfur dioxide can combine with water in the air to form acid rain.
Term
What type of reaction is this ?

Word Equation : hydrogen + nitrogen -> ammonia
Skeleton Equation : H₂ + N₂ -> NH₃
 Definition
Formation Reaction.
Term
TRUE OR FALSE.

You cannot always predict the formula of molecular compounds that form because more than one combination of elements is possible.
 Definition
TRUE.

You cannot always predict the formula of molecular compounds that form because more than one combination of elements is possible.
Term
TRUE OR FALSE.

No formation reactions occur between metals and non-metals.
 Definition
FALSE.

Many formation reactions occur between metals and non-metals.
Term
What type of reaction is this ?

Word Equation : sodium + chlorine -> sodium chloride.
Skeleton Equation : Na + Cl₂ -> NaCl
 Definition
Formation Reaction.
Term
When one reactant is a metal and the other is a non-metal, how do you predict the product ?
 Definition
When one reactant is a metal and the other is a non-metal, predict the product by writing the ionic compound they form.
Term
Decomposition Reactions are the opposite of ________ _______.
 Definition
Decompositions Reaction are the opposite of Formation Reactions.
Term
Products can be broken down to yield the reactants again in a ____________ ______.
 Definition
Products can be broken down to yield the reactants again in a decomposition reaction.
Term
In the simplest form of __________ ______, two elements combine to form a compound. This type of reaction is also known as a _________ ________.
 Definition
In the simplest type of formation reaction, two elements combine to form a compound. This type of reaction is also known as a synthesis reaction.
Term
What type of reaction is this ?

element + element ->compound.
 Definition
Formation Reaction
Term
What type of reaction is this ?

A + B -> AB
 Definition
Formation Reaction
Term
What type of reaction is this ?

Word Equation : Sulfur + Oxygen -> Sulfur Dioxide
Skeleton Equation : S₈ + O₂ -> SO₂
 Definition
Formation Reaction
Term
Sulfure dioxide can combine with ______ in the air to form acid rain.
 Definition
Sulfur dioxide can combine with water in the air to form acid rain.
Term
Sulfur dioxide can combine with water in the air to form ____ ____.
 Definition
Sulfur dioxide can combine with water in the air to form acid rain.
Term
What type of reaction is this ?

Word Equation : hydrogen + nitrogen -> ammonia
Skeleton Equation : H₂ + N₂ -> NH₃
 Definition
Formation Reaction.
Term
TRUE OR FALSE.

You cannot always predict the formula of molecular compounds that form because more than one combination of elements is possible.
 Definition
TRUE.

You cannot always predict the formula of molecular compounds that form because more than one combination of elements is possible.
Term
TRUE OR FALSE.

No formation reactions occur between metals and non-metals.
 Definition
FALSE.

Many formation reactions occur between metals and non-metals.
Term
What type of reaction is this ?

Word Equation : sodium + chlorine -> sodium chloride.
Skeleton Equation : Na + Cl₂ -> NaCl
 Definition
Formation Reaction.
Term
When one reactant is a metal and the other is a non-metal, how do you predict the product ?
 Definition
When one reactant is a metal and the other is a non-metal, predict the product by writing the ionic compound they form.
Term
Decomposition Reactions are the opposite of ________ _______.
 Definition
Decompositions Reaction are the opposite of Formation Reactions.
Term
Products can be broken down to yield the reactants again in a ____________ ______.
 Definition
Products can be broken down to yield the reactants again in a decomposition reaction.
Term
What type of reaction is this ?

compound -> element + element
 Definition
Decomposition reaction.
Term
What type of reaction is this ?

AB -> A + B
 Definition
decomposition reaction.
Term
What type of reaction is this ?

2 H₂O -> 2H₂ + o₂
 Definition
Decomposition reaction.
Term
__________ are substances that contain hydrogen and carbon.
 Definition
Hydrocarbons are substance that contain hydrogen and carbon.
Term
TRUE OR FALSE.

Methane is the simplest hydrocarbon.
 Definition
TRUE.

Methane is the simplest hydrocarbon.
Term
What type of reaction is this ?

CₓHₔ + O₂ -> CO₂ + H₂O
 Definition
Hydrocarbon Combustion.
Term
What type of reaction is this ?

CH₄ + 2O₂ -> CO₂ + 2H₂O
 Definition
Hydrocarbon Combustion.
Term
What type of reaction is this ?

A + BC -> B + AC
 Definition
Single Replacement Reactions.
Term
In a ______ ___________ _______, a reactive element reacts with an ionic compound. After the reaction, the element ends up in a compound, and one of the elements in the reactant compound ends up by itself as an element.
 Definition
In a single replacement reaction, a reactive element reacts with an ionic compound. After the reaction, the element ends up in a compound, and one of the element in the reactant compound ends up by itself as an element.
Term
What kind of reactions often take place in a solution?
 Definition
Single replacement reactions often take place in solution.
Term
In one type of _________ __________ reaction, a metal atom trades places with a metal ion in a compound.
 Definition
In one type of single replacement reaction, a metal atom trades places with a metal ion in a compound.

ex. magnesium + silver nitrate -> silver + magnesium nitrate.
Term
What type of reaction is this ?

magnesium + silver nitrate -> silver + magnesium nitrate.
 Definition
Single Replacement Reaction.
Term
Any metal on its own is present as ____.
 Definition
Any metal on its own is present as atoms.
Term
Any metal element in a compound is present as an ____.
 Definition
Any metal element in a compound is present as an ion.
Term
The ______ ______ determines how the compound is written.
 Definition
The ionic charge determines how the compound is written.
Term
What type of reaction is this ?

Skeleton Equation : Mg + NO₃ -> Ag + Mg(NO₃)₂
Balanced Equation : Mg + 2 AgNO₃ -> 2 Ag + Mg(NO₃)₂
 Definition
Single Replacement Equation.
Term
What type of reaction is this ?

D + BC -> C + BD
 Definition
Single Replacement Equation.
Term
What type of reaction is this ?

Balanced Equation : Cl₂ + 2AgBr -> Br₂ + 2AgCl
 Definition
Single Replacement Equation.
Term
_______ __________ reactions commonly occur between two ionic compounds.
 Definition
Double Replacement reactions commonly occur between two ionic compounds.
Term
Ionic compounds are always _____ at room temperature.
 Definition
Ionic compounds are always solid at room temperature.
Term
______ ________ reactions commonly occur between two ionic compounds. Ionic compounds are always solid at room temperature, so these reaction happen in a ______ (dissolved in liquid), where the ions have an opprotunity to mix. This type of reaction often results in the formation of at least one __________.
 Definition
Double Replacement reactions commonly occur between two ionic compounds. Ionic compounds are always solids at room temperature, so these reactions happen in solution (dissolved in liquid), where the ions have the opportunity to mix. This type of reaction often results in the formation of at least one precipitate.
Term
What type of reaction is this ?

AB + CD -> AD + CB
 Definition
Double replacement reaction.
Term
The ____ in the first compound join with
the ____ from the second compound. This is called a double replacement reaction because two new ______ compounds are formed.
 Definition
The ions in the first compound join with the ions from the second compound. This is called a double replacement reaction because two new ionic compounds are formed.
Term
In AB + CD -> AD + CB

A & C are both positive ions. They will never pair up together because they repel each other.
A & C will always appear first in formulas because positive ions are always written first.
B & D are negative ions, so they will combine with any positive ions. They are always written second in formulas.
 Definition
In AB + CD -> AD + CB

A & C are both positive ions. They will never pair up together because they repel each other.
A & C will always appear first in formulas because positive ions are always written first.
B & D are negative ions, so they will combine with any positive ions. They are always written second in formulas.
Term
Is it possible for a reaction to not fit into the five categories of chemical reactions ?
 Definition
Yes, there are many kinds of reactions that do not fit into the five categories that you have just learned. There are even variations of these five types for which the products are difficult to predict.
Term
The quantity that chemists use to measure the elements and compounds is called the ____.
 Definition
The quantity that chemists use to measure the elements and compounds is called the mole.
Term
The number of particles in 1 mol is called ________ _______.
 Definition
The number of particles in 1 mol is called Avogadro's number (Nₐ).
Term
What is Avogadro's number ?
 Definition
Approx 6.02 X 10²³.

OR

602 000 000 000 000 000 000 000.
Term
What kind of particles can the mole be used to measure ?
 Definition
The mole can be used to measure any kind of particles, atoms, ions, molecules, and formula units.
Term
Avogadro's number was named in honor of _______ ______, an _____ ______ (___-___).
 Definition
Avogadro's number was named in honor of Amedeo Avogadro, an Italian scientist (1776-1856).
Term
The mass of one mole of a substance is called its _____ ____.
 Definition
The mass of one mole of a substance is called its molar mass.
Term
The ______ _____ ____ of an element is the average mass in grams of one mole of atoms of that element.
 Definition
The atomic molar mass of an element is the average mass in grams of one mole of atoms of that element.
Term

m = n x M what do n & M equal ?

 

m is the quantity of matter (mass) in grams

 

 Definition

m = n x M

m is the quantity of matter (mass) in grams,

n is the quantity of matter in moles

M is the molar mass.
Term
The ____________ method is a simple technique for converting between the number of moles of a substance and its mass. This method is based on the idea that different units can represent the same quantity of matter.
 Definition
The factor-label method is a simple technique form converting between the number of moles of a substance and its mass. This method is based on the idea that different units can represent the same quantity of matter.
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