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| The study of composition, structure and properties of matter, the changes in which matter undergoes and the energy accompanying these changes. |
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scientific unit of measure
meter --> length
Kelvin --> temperature
moles --> number of particles
Liter --> volume
Amperes --> electric current
pascal --> pressure
joule --> heat
gram --> mass |
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| anything that has mass and occupies volume |
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| the amount of matter an object contains |
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| the force with which gravity attracts matter (not the same as mass) |
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| the amount of three dimensional space an object occupies |
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| Measures the average kinetic energy |
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| Number of digits that you report in the answer of a measurement you are taking or a problem you are solving |
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| zeroes that are located between nonzero digits are always significant e.g. 1,004 4 sigfigs |
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| zeroes located before other numbers are not significant e.g. 0.000005 1 sigfig |
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| zeroes located after the last non-zero digit sometimes significant e.g. 32,000. 5 sigfigs because it has a decimal point at the end of it, if it did not it would only have 2 sigfigs |
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| Multiplying and dividing with Significant Figures |
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Definition
1. Find the number with the least number of significant figures
2. Round your answer to the least number of significant figures
example: 2.35x3.845x8.9=80.418175 cm^3
only two significant figures 80. is what you should report |
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| Addiction and Subtractions for Significant Figures |
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Definition
1. Find the number with the least number of decimal places
2. Round your answer to the least number of decimal places
example: 2.35+3.845+8.9= 15.095
the smallest decimal place is the tenths so the answer would be 15.0 |
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Definition
A technique used to convert(or change) units
1. Determine the unit equality
2. Write down the given quantity
3. Determine the proper conversion factor
4. Set-up and solve
example: how many inches are in 37.84 feet?
37.84 feet x 12 inches equals 454.08 inches but
1 1 foot in sigfigs it is only 454.1 |
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| A measure of how close something is to that true value |
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| a measure of measurements to each other |
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| Precent error (Located on the back of the Reference Tables) |
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Definition
accepted-calculated x 100
accepted |
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| The smallest particle of an element that retains the properties of that element (ALWAYS NEUTRAL) |
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| The smallest particle of a compound that retains the properties of that compound |
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Particles are in an ordered geometric arrangement, they have definite shape and volume and the particles are very close together but are in constant motion
l l
l oo l
l oo l |
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Particles are in free motion, very close together and take the shape of the container
l l
loool
loool |
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Particles have free random motion and are usually far apart
l o o l
lo o ol
l o o l |
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| Movement of on substance through another high to low |
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| decreased distance between atoms |
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| Can be measured and/or observed without changing the identity or composition of a substance. e.g. color, odor, density, melting/boiling point |
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| Physical properties that depend on the amount of matter e.g. Mass and volume |
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| Physical properties that do not depend on the amount of matter e.g. Color, luster and density |
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| Properties that lead to changes in the identity or composition of a substance e.g. Flammability, and ability to rust or oxidize |
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| Changes in which the identity and composition of matter are not altered e.g. Physical Changes |
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| Changes in which the identity and composition of matter are altered; new substances are made as a result of a chemical change e.g. Iron turns to rust |
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| The Kelvin is the international unit for temperature. This scale is based on the concept of absolute zero of 0K |
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| The amount of heat required to convert a a solid at it's melting point to a liquid without an increase in temperature |
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| The amount of heat required to convert a liquid at its boiling point into vapor without an increase in temperature. |
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1. They are composed of individual particles that are in continuous, random, straight-lined motion
2. The distance between their particles are so great compared to the value of the individual particles that the value of the individual particles is considered to be negligible (i.e. ideal gas particles d not take up spaces)
3. The particles have no attraction forces between them
4. collisions between gas particles are completely elastic; in other words, an equal amount of energy is transferred between the particles- there is no net gain or loss of energy and the system remains constant |
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| Real Gases (like oxygen, nitrogen, etc.) |
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Definition
Do no behave exactly like an ideal gas because they are real
1. particles (atoms/molecules) have attraction for each other
2. particles occupy volume |
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real gases behave like ideal gases under certain conditions
P= pressure
L= low
I= ideal
G= gas
H= high
T= temperature |
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| the force applied to an object per unit area ex: pounds per square inch (lbs/inch^2) |
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| STP (Standard Temperature and Pressure) |
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Definition
conditions most often used to study or test a chemical
Standard Temperature- 273 K
Standard Pressure- 1atm= 760 mmHg= 101.3 kPa |
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| The pressure exerted as a liquid changes into a gas (as temperature increase vapor pressure increases) |
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| The temperature at which the vapor pressure of a liquid is equal to the pressure pushing down on the surface of the liquid. The normal boiling point of a liquid is the temperature at which the vapor pressure equals standard pressure. As vapor pressure goes up the boiling point will increase |
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| Boyle's Law (pressure acting on volume) |
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Definition
| At constant temperature, as pressure on a gas increases the volume decreases |
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| Charles' Law (temperature acting on volume) |
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Definition
| At constant pressure as the temperature of a gas is increased volume increases |
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| Gay-Lussac's Law (temperature acting on pressure) |
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Definition
| At constant volume, as the temperature of a gas increases the pressure increases |
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P1V1 = P2V2 (on the reference table)
T1 T2 |
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| Equal volumes of gases at the same temperature and pressure contain an equal number of gas particles: NUMBER TO REMEMBER 6.02 x 10^23 |
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| All matter is composed of tiny, indivisible particles he called atomes. His idea was dismissed by other Greek Philosophers including Aristotle |
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| Law of conservation of mass/matter: Matter is neither created nor destroyed |
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| Law of definite proportions: A given compound always contains the same elements in the same proportions by mass. The ratio is always fixed |
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| The properties of matter can be explained in terms of atoms |
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| Dalton's Atomic Theory of Matter |
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Definition
1. Each element is composed of extremely small, indivisible particles called atoms
2. All atoms of a given element are identical, but they are different from those of any other element
3. Atoms are neither created nor destroyed in any chemical reaction
4. A given compound always has the same relative numbers and kinds of atoms |
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| Cathode Ray Tube Experiment. passed an electrical curent through a glass tube containing different gases at low pressure with magnetic plates on either side of the tube. Concluded that the cathode ray was made up of negatively charged particles |
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Definition
Gold Foil Experiment. Aimed a beam of alpha particles at an extremely thin piece of gold foil and came to two important conclusions:
1. an atom is made up of mostly empty space
2. the majority of an atom's mass and all of it's positive charge are concentrated in a central core called the nucleus |
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Definition
Protons- positive charge, located in the nucleus and has a mass of 1
Neutrons- has no charge, located in the nucleus and has a mass fo 1
Electron- has a charge of negative one, located outside the nucleus and has a mass of 1/1840 |
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| The number of protons in the nucleus of an atom. The identity of an atom is determined by it's atomic number. Ex: every carbon atom has six protons |
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| The sum of the protons and neutrons in an atom. The number of neutrons can be determined by subtracting the atomic number from the mass number. If you see element-# that is showing the mass number |
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Atoms/elements with the same number of protons, but different number of neutrons
Ex. Carbon-12, Carbon-13, Carbon-14 |
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| When an atom gains or loses an electrons and has a net positive or negative charge. They have a charge either positive or negative |
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| This is weighted average of the naturally occurring isotopes for an element. This weighting is a result of their precent abundances on Earth. |
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Describe the approximate distance from the nucleus. The farther away fromt he nucleus, the more energy associated with that level.
- Energy levels are designated with the letter n; n can be the numbers 1-7
-1 is closest to the nucleus and has the least amount of energy associated with it |
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Describes the shape of the electron cloud or orbital
-sublevels designated s,p,d,f
-s has the lowest energy associated with it while f has the highest |
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| Each sublevel may contain one or more orbitals (or electron clouds) having different spatial orientations. These are the areas of highest probability of finding electrons |
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| When the atom (e^-) of an element occupies the lowest energy levels 1st (in order). Elements are in their most stable state when in the ground state |
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| When the atom absorbs energy and moves of jumps up energy level(s), they are considered to be int eh excited state (not in order). All atoms want to be in the most stable state possible. In order for an atom to be go back to ground state from the excited state the atom must release the energy they had originally absorbed. The energy is released in a form of light that is characteristic to each element. |
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| Dmitri Mendeleev arranged elements by increasing atomic mass and similar chemical properties. He found arranged this way had repetitive patterns. At this time, only 70 elements had been discovered. If no known elements seemed to "fit" in a place that went with the patterns. Mendeleev would leave the space blank and elements that had not yet been discovered that fit this pattern were put in these spaces. |
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| Henry Moseley determined the atomic number for all elements. He proposed the elements in the periodic table should be arranged by increasing atomic numbers which turnet out to be more accurate. This is how the Periodic Table is arranged today |
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| When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic trend. |
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| More than two thirds of all elements are metal. Metals are shiny, malleable, ductile, good conductors of heat and electricity, low ionization energy, lose electrons and form positive ions. Non-Metals are dull, brittle, poor conductors of heat and electricity, have high ionization levels, like to gain electrons and form negative ions. |
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| These are the elements surrounding the stair case, between the metals and non-metals. They have both metallic and non-metallic properties. They include: B, Si, Ge, As, Sb and Te. Metals are located to the left and non-metals are located to the right. |
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Group 1- Alkali Metals (no including H)
Group 2- Alkaline Earth Metals
(^These groups from strong basses)
Group 17- Halogens form Salts
Group 18- Noble Gases- Chemically un-reactive inert due to filled valence shells. They exist as monatomic molecules |
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| These are elements that naturally exist as diatomic molecules. Br2 I2 N2 Cl2 H2 O2 F2 |
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| One-half the distance between the nuclei of two identical atoms when they are joined together (i.e. the distance from the nucleus of atoms to the valence shell) |
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| The energy required to remove an electron from an atom in the gas phase. The energy need to remove the first electron is called the first ionization energy; to remove the second electron is called the second ionization energy, and so on. |
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| An atom's attraction for electrons when chemically bonded with another atom. |
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1. As you move down a group the atom's radius increases. This is because an increase in the number of occupied energy levels.
2. As you move down a group IE and EN decrease. This ia because the increased distance between the protons in the nucleus and the valence electrons.
3. As you move down a group metallic properties increase. |
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Definition
1. As you move from left to right within a period, the atomic radius decreases. This is because a greater molecular charge.
2. As you move from left to right within a period, the IE and EN both increase. This is because of the decreased distance between the protons and electrons |
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| When the innermost electrons block the attractive force of the protons on the valence electrons |
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| the innermost electrons and nucleus |
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| Atoms acquire eight valence electrons by taking or sharing electrons; they want to have an electron configuration like that of the closest noble gas. Most atoms are stabilized with 8 valence electrons. (Exceptions: H, He, Li, Be, B (these only need two) |
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