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Chemistry > Flashcards- Regents Chemistry Vocabulary > Flashcards

Flashcards- Regents Chemistry Vocabulary

1
Q

A chemical reaction in which a compound is broken down into simpler substances

A

decomposition

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1
Q

the process in which a gas changes directly into a solid; the reverse of sublimation

A

deposition

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1
Q

a molecule containing two identical atoms

A

diatomic molecule

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1
Q

the sharing of two pairs of electrons between two nuclei

A

double covalent bond

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1
Q

the process in which a solid changes directly into a gas; the reverse of deposition

A

sublimation

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2
Q

the site at which oxidation or reduction occurs; an anode or a cathode

A

electrode

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2
Q

substances that cannot be broken down or decomposed into simpler substances by chemical means

A

element

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2
Q

a chemical reaction that absorbs heat, producing products with more potential energy than the reactants

A

endothermic

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2
Q

a chemical reaction in which ions exchange places

A

double replacement

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2
Q

property of a metal that enables it to be drawn into a wire

A

ductility

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2
Q

a system in which there is an electric current flowing while a chemical reaction occurs

A

electrochemical cell

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3
Q

a process in which an electric current forces a nonspontaneous redox reaction to occur

A

electrolysis

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3
Q

A substance whose water solution conducts an electric current

A

electrolyte

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3
Q

a cell that requires electricity to cause a nonspontaneous chemical reaction to occur

A

electrolytic cell

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3
Q

a mathematical expression that shows the relationship of reactants and products of a system at equilibrium

A

equilibrium expression

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3
Q

a chemical reaction between an alcohol and an acid to produce an ester and water

A

esterification

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3
Q

an organic compound in which oxygen is bonded to two carbon atoms (R1-O-R2)

A

ether

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3
Q

a fundamental particle of matter having a negative charge

A

electron

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4
Q

the distribution of the electrons in an atom

A

electron configuration

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5
Q

a measure of the attraction of a nucleus for a bonded electron

A

electronegativity

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5
Q

substances that cannot be broken down or decomposed into simpler substances by chemical means

A

element

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6
Q

the distance from the nucleus to the outer energy level of the ion

A

ionic radius

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6
Q

the simplest integer ratio in which atoms combine to form a compound

A

empirical formula

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7
Q

a chemical reaction that absorbs heat, producing products with more potential energy than the reactants

A

endothermic

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8
Q

a measure of the disorder or randomness of a system

A

entropy

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8
Q

a condition in which the rates of opposing reactions are equal

A

equilibrium

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8
Q

the loss of electrons and an increase in oxidation state

A

oxidation

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9
Q

a mathematical expression that shows the relationship of reactants and products of a system at equilibrium

A

equilibrium expression

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9
Q

the organic product of an esterification reaction containing -COOC- as the functional group

A

ester

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10
Q

a chemical reaction between an alcohol and an acid to produce an ester and water

A

esterification

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11
Q

the amount of energy needed to remove the most loosely bound electron from a neutral gaseous atom

A

ionization energy

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11
Q

an organic compound in which oxygen is bonded to two carbon atoms (R1-O-R2)

A

ether

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11
Q

the process by which molecules in the liquid phase escape into the gaseous phase

A

evaporation

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11
Q

the distance from the nucleus to the outer energy level of the ion

A

ionic radius

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12
Q

the loss of electrons and an increase in oxidation state

A

oxidation

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13
Q

the condition that exists when the electrons of an atom occupy higher energy levels while lower energy levels are vacant

A

excited state

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14
Q

the amount of energy needed to remove the most loosely bound electron from a neutral gaseous atom

A

ionization energy

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14
Q

a chemical reaction that releases heat, producing products with less potential energy than the reactants

A

exothermic

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15
Q

the substance reduced in a redox reaction

A

oxidizing agent

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16
Q

the group comprised of an oxygen atom and a hydrogen atom (-OH) responsible for the properties of alcohols

A

hydroxyl group

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17
Q

a chemical reaction that releases heat, producing products with less potential energy than the reactants

A

exothermic

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18
Q

compounds with the same molecular formula but different structural arrangement

A

isomers

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19
Q

the ratio between the parts of solute per million parts of solution

A

parts per million

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21
Q

a phase of matter having a definite shape and volume; particles in this phase have a definite crystalline arrangement

A

solid phase

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22
Q

atom of an element that has a specific number of protons and neutrons

A

isotope

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23
Q

atom of an element that has a specific number of protons and neutrons

A

isotope

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24
Q

the concentration of a solution expressed as the ratio between the volume of the solute and total volume of the solution, expressed as a percent

A

percent by volume

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26
Q

a measure of how much solute will dissolve in a certain amount of solvent at a specific temperature

A

solubility

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27
Q

an organic reaction in which ethanol and carbon dioxide are produced from a carbohydrate

A

fermentation

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27
Q

a bond formed by the transfer of electrons from one atom to another

A

ionic bond

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28
Q

a bond formed by the transfer of electrons from one atom to another

A

ionic bond

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31
Q

splitting of large nuclei into middle-weight nuclei and neutrons

A

fission

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31
Q

material with a high solubility

A

soluble

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32
Q

splitting of large nuclei into middle-weight nuclei and neutrons

A

fission

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33
Q

material with a low solubility

A

insoluble

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35
Q

the composition of a compound as a percentage of each element compared with the total mass of the compound

A

percentage composition

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36
Q

the sum of the atomic masses of all atoms present

A

formula mass

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37
Q

the sum of the atomic masses of all atoms present

A

formula mass

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39
Q

a horizontal row of the periodic table

A

period

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40
Q

symbols and subscripts used to represent the composition of a substance

A

formula

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40
Q

a homogenous mixture of substances in the same physical state

A

solution

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41
Q

symbols and subscripts used to represent the composition of a substance

A

formula

43
Q

the properties of elements are periodic functions of their atomic numbers

A

periodic law

45
Q

the temperature at which both the solid and liquid phases of a substance exist in equilibrium; the same temperature as the substance’s melting point

A

freezing point

45
Q

the temperature at which both the solid and liquid phases of a substance exist in equilibrium; the same temperature as the substance’s melting point

A

freezing point

46
Q

matter is neither created nor destroyed in chemical reactions

A

law of conservation of mass

49
Q

any change in concentration, pressure, or temperature on an equilibrium system

A

stress

50
Q

the constant temperature process in which particles in the liquid phase lose energy and change into the solid phase; also known as solidification; the reverse of the melting process

A

freezing

50
Q

the constant temperature process in which particles in the liquid phase lose energy and change into the solid phase; also known as solidification; the reverse of the melting process

A

freezing

52
Q

the negative logarithm of the hydrogen ion concentration of a solution

A

pH

54
Q

the atom or atoms that replace a hydrogen atom in a hydrocarbon and give a class of organic compounds characteristics properties

A

functional group

55
Q

a system at equilibrium will react to reduce a stress

A

Le Chatelier’s principle

56
Q

a system at equilibrium will react to reduce a stress

A

Le Chatelier’s principle

58
Q

the number written after a chemical symbol in a formula indicating the number of atoms present

A

subscript

59
Q

the constant temperature process in which particles in the solid phase gain enough energy to break away into the liquid phase; also known as melting; the reverse of the freezing process; OR the combining of light nuclei into a heavier nucleus

A

fusion

60
Q

a diagram that depicts valence electrons as dots around the atomic symbol of the element

A

Lewis dot diagram

61
Q

a diagram that depicts valence electrons as dots around the atomic symbol of the element

A

Lewis dot diagram

63
Q

one or more hydrogen atoms is removed from a saturated hydrocarbon and replaced by another atom

A

substitution reaction

65
Q

a phase of matter having definite volume but no definite shape

A

liquid phase

66
Q

a covalently bonded group of atoms that have a net electric charge

A

polyatomic ion

67
Q

a covalently bonded group of atoms that have a net electric charge

A

polyatomic ion

68
Q

a phase of matter without definite shape or volume

A

gaseous phase

70
Q

the property of metals that allows them to be hammered into shapes

A

malleability

72
Q

a reaction in which two or more substances combine to form one product

A

synthesis

73
Q

the total number of protons and neutrons in the nucleus of an atom

A

mass number

74
Q

the total number of protons and neutrons in the nucleus of an atom

A

mass number

76
Q

an organic reaction in which many small units are joined together to form a long chain

A

polymerization

77
Q

the condition of an atom or ion in which the electrons occupy the lowest available energy levels

A

ground state

79
Q

anything that has mass and volume

A

matter

80
Q

an alcohol with a hydroxyl group attached to a carbon atom that is attached to three other carbon atoms

A

tertiary alcohol

81
Q

an alcohol with a hydroxyl group attached to a carbon atom that is attached to three other carbon atoms

A

tertiary alcohol

82
Q

a vertical column on the periodic table

A

group

84
Q

a diagram showing the changes in potential energy as a reaction proceeds

A

potential energy diagram

85
Q

the process of determining the concentration of an unknown solution by a reaction with a solution of known concentration

A

titration

87
Q

element whose atoms lose electrons in chemical reactions to become positive ions

A

metal

88
Q

element whose atoms lose electrons in chemical reactions to become positive ions

A

metal

89
Q

an alcohol with a hydroxyl group attached to a carbon atom at the end of a chain

A

primary alcohol

90
Q

a radioisotope used to track a chemical reaction

A

tracer

91
Q

the attraction of valence electrons for the positive kernels of metallic atoms

A

metallic bond

92
Q

the attraction of valence electrons for the positive kernels of metallic atoms

A

metallic bond

94
Q

a substance formed in a chemical reaction, shown to the right of the arrow in an equation

A

product

95
Q

the changing of a nucleus of one element into that of a different element

A

transmutation

97
Q

an element that has both metallic and nonmetallic properties

A

metalloid

98
Q

the positively charged particle in the nucleus of an atom

A

proton

98
Q

the positively charged particle in the nucleus of an atom

A

proton

99
Q

the sharing of three pairs of electrons between two nuclei

A

triple bond

101
Q

the concentration of a substance in moles per liter of solution

A

molarity

103
Q

a compound or an element; a material in which the composition is the same throughout

A

pure substance

104
Q

energy transferred from one substance to another; measured in units of calories or joules

A

heat

105
Q

energy transferred from one substance to another; measured in units of calories or joules

A

heat

106
Q

the number of carbon atoms present in 12.000g of carbon-12

A

mole

107
Q

one of a set of four numbers that describes a property of an electron in an atom

A

quantum number

109
Q

the amount of heat needed to convert a unit mass of a substance from a solid to a liquid at its melting point

A

heat of fusion

110
Q

the actual ratio of the atoms in a molecule

A

molecular formula

110
Q

the actual ratio of the atoms in a molecule

A

molecular formula

112
Q

a concept that relates the chemical behavior of atoms to energy being transferred in discrete units called quanta

A

quantum theory

114
Q

the amount of heat needed to convert a unit mass of a substance from a liquid to a vapor at its boiling point

A

heat of vaporization

115
Q

the smallest unit of a covalently bonded substance that has the properties of that substance

A

molecule

116
Q

an unstable nucleus that is radioactive

A

radioisotope

118
Q

a mixture in which the substances are not uniformly mixed

A

heterogeneous

119
Q

each individual unit of a polymer

A

monomer

120
Q

a starting substance in a reaction, show the the left of the arrow in an equation

A

reactant

121
Q

the constant temperature process in which particles in the liquid phase gain enough energy to break away into the gaseous phase; also known as boiling; the reverse of condensation

A

vaporization

121
Q

the constant temperature process in which particles in the liquid phase gain enough energy to break away into the gaseous phase; also known as boiling; the reverse of condensation

A

vaporization

122
Q

a substance in which the particles are uniformly mixed

A

homogeneous

124
Q

the reaction between an acid and a base to produce water and a salt

A

neutralization

125
Q

the substance oxidized in a redox reaction

A

reducing agent

126
Q

a group of related compounds in which each member differs from the one before it by the same additional unit

A

homologous series

128
Q

the uncharged particle in the nucleus of an atom

A

neutron

129
Q

the gain of electrons and the loss of oxidation number

A

reduction

130
Q

the current model of the atom that deals with the wave-particle duality of nature

A

wave-mechanical model

130
Q

the crystalline form of an ionic substance that contains definite number of water molecules

A

hydrate

131
Q

the crystalline form of an ionic substance that contains definite number of water molecules

A

hydrate

132
Q

a nonreactive element that is in group 18 on the periodic table

A

noble gas

133
Q

the product (other than water) of a neutralization reaction; an ionic substance consisting of a metallic cation and anion other than the hydroxide ion

A

salt

135
Q

element whose atoms will gain or share electrons in chemical reactions

A

nonmetal

136
Q

a part of a voltaic cell that connects two containers and allows the flow of ions

A

salt bridge

137
Q

the attraction of a hydrogen atom in one molecule for an oxygen, nitrogen, or fluorine atom in another molecule

A

hydrogen bond

138
Q

a bond formed by the equal sharing of a pair of electrons between two nuclei

A

nonpolar covalent bond

138
Q

a bond formed by the equal sharing of a pair of electrons between two nuclei

A

nonpolar covalent bond

140
Q

the reaction of an alkali and a fat to produce glycerol and a soap

A

saponification

142
Q

the dense, positively charged central core of an atom

A

nucleus

143
Q

A solution containing the maximum amount of solute that will dissolve at a given temperature; OR organic compounds containing only single covalent bonds

A

saturated

144
Q

H3O+, formed by the combination of water with a hydrogen ion

A

hydronium ion

145
Q

the stable valence electron configuration

A

octet (8 electrons)

146
Q

an alcohol with a hydroxyl group attached to a carbon atom that is attached to two other carbon atoms

A

secondary alcohol

147
Q

a region in an atom in which an electron of a particular amount of energy is most likely to be located

A

orbital

147
Q

the polyatomic anion produced by the ionization of a water molecule

A

hydroxide ion

148
Q

a region in an atom in which an electron of a particular amount of energy is most likely to be located

A

orbital

150
Q

an organic compound containing one or more carboxyl groups (-COOH)

A

organic acid

151
Q

a substance that undergoes a color change that can be used to determine when a reaction is complete

A

indicator

152
Q

an organic compound in which one or more hydrogen atoms have been replaced by an atom of a halogen; also known as halocarbon

A

organic halide

153
Q

number assigned to keep track of electron gain or loss in redox reactions

A

oxidation number (state)

Chemistry (1 decks)

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