Term
| Name all the prefixes in the metric system in increasing order. |
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Definition
| Mili, Centi, Deci, Deca, Hecto, Kilo |
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Term
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Definition
| A method of writing or displaying numbers in terms of a decimal number between 1 and 10 multiplied by a power of 10. |
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Term
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Definition
| Density= Mass divided by volume |
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Term
| List the physical properties of a substance. |
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Definition
-Color
-Smell
-Brittle
-Density
-Melting Point
-Boiling Point |
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Term
| List chemical properties of a substance: |
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Definition
-Flammability
-Rusting
-PH
-Reactivity with acid |
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Term
| What is a homogeneous mixture? |
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Definition
| Appears the same throughout |
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Term
| Give examples of homogeneous mixtures: |
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Definition
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Term
| What is a heterogeneous mixture? |
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Definition
| Does not look the same throughout. |
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Term
| Name some examples of a heterogeneous mixture |
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Definition
| Cereal, oil and water, Sand |
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Term
| How would you separate homogeneous mixture like alcohol and water? |
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Definition
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Term
| How can you separate a compound and a mixture? |
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Definition
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Term
| What is the difference between a compound and a mixture? |
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Definition
| Compound Cannot be easily separated |
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Term
| How do you write a chemical symbol? |
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Definition
| The first letter is capitalized. |
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Term
| List the steps to separate a mixture of water, salt, and iron filings. |
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Definition
1)Use magnet to remove iron
2)Boil water, collect salt crystals |
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Term
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Definition
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Term
| Which phase takes the shape of its container and has a definate volume? Which has its own shape? |
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Definition
| Liquid takes the shape of its caontainer, solid has its own shape. |
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Term
| Give 2 examples of a chemical change. |
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Definition
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Term
| Give 2 examples of a physical change. |
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Definition
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Term
| Law of Conservation of Matter |
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Definition
| Matter can't be created or destroyed. It can only be transformed |
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Term
| Law of Conservation of Energy state |
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Definition
| Energy is never created or destroyed only converted. |
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Term
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Definition
| The basic unit of a chemical element |
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Term
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Definition
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Term
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Definition
| A substance that cannot be broken down by chemical means, defined by the number of protons they possess. |
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Term
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Definition
| The positively charged central core of an atom, containing most of its mass. |
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Term
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Definition
| A stable subatomic particle occurring in all atomic nuclei, with a positive electric charge equal to an electron. |
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Term
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Definition
| A subatomic particle of about the same mass as a proton but without an electric charge. |
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Term
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Definition
| A stable subatomic particle with a charge of negative electricity, found in all atoms and acting as the primary carrier of electricity |
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Term
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Definition
| An atom or molecule with a net electric charge due to the loss or gain of one or more electrons. |
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Term
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Definition
| Element that contains equal numbers of protons but different numbers of neutrons. |
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Term
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Definition
| An electron in the outer shell of an atom which can combine with other atoms to form molecules. |
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Term
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Definition
Diagrams used to show how the orbitals of a subshell are
occupied by electrons |
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Term
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Definition
| The lowest energy state of an atom or other particle. |
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Term
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Definition
| A state of a physical system that is higher in energy than the ground state. |
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Term
| What is the atomic number equal to? |
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Definition
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Term
| What is the atomic mass or mass number equal to? |
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Definition
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Term
| What particle changes in an atom with an increase in atomic number? |
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Definition
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Term
| How do you find the number of neutrons in an atom? |
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Definition
| Subtract the atomic number from the atomic mass. |
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Term
| What must happen to change an atom from an atom into an ion? |
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Definition
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Term
| What particle changes in an atom to make it an isotope? |
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Definition
| The number of neutrons changes. |
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Term
| Why are atomic masses written in decimal form on the periodic table? |
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Definition
| They are the average of all masses. |
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Term
| Explain the steps to the flame test and how light was created in the flame test. |
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Definition
| Different chemicals created different colors of light. |
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Term
| How do electrons move up and down energy levels? |
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Definition
| They get into an excited state and jump levels. |
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Term
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Definition
| The principle that chemical properties of the elements are periodic functions of their atomic numbers. |
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Term
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Definition
| A table of the chemical elements arranged in order of atomic number. |
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Term
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Definition
| A solid material that is typically hard, and shiny with good electrical and thermal conductivity. |
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Term
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Definition
| Chemical elements that form negative ions, have acidic oxides, and are generally poor conductors of heat and electricity |
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Term
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Definition
| An element whose properties are intermediate between those of metals and solid nonmetals |
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Term
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Definition
| The energy required to remove an electron from an ion. |
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Term
| What is a period on the Periodic Table and how many are there? |
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Definition
| Horizontal rows in the Periodic Table. There are seven. |
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Term
| How does the size of an atom vary as you go across a period? |
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Definition
| The atomic radius decreases |
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Term
| How does the Ionization energy vary as you go across a period? |
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Definition
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Term
| What is a family or group on the Periodic Table? |
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Definition
| The vertical columns on the Periodic Table. |
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Term
| What happens to the size of atoms as you go down a family? |
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Definition
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Term
| What happens to the ionization energy as you go down a family? |
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Definition
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Term
| Why are valence electrons so important? |
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Definition
| Tells how an element will react. |
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Term
| What are the characteristics of metals? |
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Definition
| Good conductors of electricity and heat, shiny, lose electrons, high melting point. |
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Term
| What are the characteristics of a nonmetal? |
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Definition
| Not good conductors, not shiny |
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Term
| Where are nonmetals located on the periodic table? |
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Definition
| The top right of the table. |
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Term
| What are the 7 metalloids, and where are they located? |
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Definition
Boron-Family 13
Carbon-Family 14
Nitrogen-Family 15
Oxygen-Family 16
Fluorine-Family 17 |
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Term
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Definition
| A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion |
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Term
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Definition
| A chemical bond that involves sharing a pair of electrons between atoms in a molecule. |
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Term
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Definition
| States that elements in the second row of the periodic table cannot have more than eight valence electrons around them them, whether as non-bonding electrons or in chemical bonds. |
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Term
| What kinds of elements make up an ionic bond? |
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Definition
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Term
| What is happening in a covalent bond? |
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Definition
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Term
| What types of elements are bonded together in a covalent bond? |
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Definition
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Term
| How do you determine what a charge on an atom will be? |
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Definition
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Term
| When does an atom gain electrons and when does it lose electrons? |
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Definition
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Term
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Definition
| Chemical compounds that consist only of hydrogen and carbon atoms and are bonded exclusively by single bonds |
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Term
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Definition
| Unsaturated hydrocarbons that contain at least one double bond. |
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Term
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Definition
| Chemical compounds that consist only of hydrogen and carbon atoms and are bonded exclusively by single bonds |
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Term
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Definition
| The study of the thousands of carbon, containing the compounds. |
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Term
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Definition
| Hydrocarbons with a triple bond. |
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Term
| Name the first 10 prefixes used for carbon compounds. |
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Definition
| Mono, Di Tri, Tetra, Penta, Hexa, Hepta, Octa, Nona, Deca. |
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Term
| When do you use the endings -ene and -yne? |
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Definition
-ene One double, 2 singles
-yne One double, 2 triples |
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Term
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Definition
| shows the bonding between atoms of a molecule. |
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Term
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Definition
| The tendency of an atom or to attract electrons to itself. |
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Term
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Definition
| Distance from the nucleus of the atom to the outermost level. |
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