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My Science Bowl > Chemistry Glossary CliffsNotes > Flashcards

Chemistry Glossary CliffsNotes Flashcards

Finished. Very basic. I want everyone to go over it to gain basic chemistry knowledge.

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1
Q

Acid

A

A compound that yields H+ ions in solution or a solution in which the concentration of H+ exceeds OH-.

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2
Q

Acid ionization constant

A

The equilibrium constant describing the degree of ionization of an acid.

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3
Q

Actinides

A

The row of elements below the main section of the periodic table, from thorium to lawrencium.

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4
Q

Alkali

A

Synonym for base.

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5
Q

Alkali metals

A

The column of elements from lithium to francium.

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6
Q

Alkaline earth metals

A

The column of elements from beryllium to radium.

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7
Q

Alkene

A

A hydrocarbon with one or more double bonds and no triple bond.

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8
Q

Alkane

A

A hydrocarbon without a double bond, triple bond, or ring structure.

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9
Q

Alkyne

A

A hydrocarbon with one or more triple bonds.

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10
Q

Alpha particle

A

A cluster of two protons and two neutrons emitted from a nucleus in one type of radioactivity.
(Helium-4 Nucleus)

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11
Q

Anoin

A

A chemical species with a negative charge.

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12
Q

Anode

A

The electrode at which oxidation occurs.

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13
Q

Aqueous

A

Refers to a solution with water as the solvent.

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14
Q

Aromatic

A

Refers to an organic compound with a benzene-like ring.

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15
Q

Atom

A

The smallest amount of an element; a nucleus surrounded by electrons.

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16
Q

Atomic number

A

The number of protons in the nucleus of the chemical element.

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17
Q

Atomic mass

A

The mass in grams of one mole of the chemical element; approximately the number of protons and neutrons in the nucleus.

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18
Q

Avogadro’s Law

A

Equal volumes of gases at the same temperature and pressure contain the same number of molecules.

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19
Q

Avogadro’s Number (or Avogadro’s constant)

A

6.02 x 10^23, the number of molecules in one mole of a substance.

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20
Q

Base

A

A compound that yields OH- ions in solution or a solution in which the concentration of OH- exceeds H+.

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21
Q

Beta particle

A

An extremely fast moving electron emitted from a nucleus in one type of radioactivity.

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22
Q

Boiling point

A

the temperature at which a liquid changes to a gas. (Technically, boiling point is the temperature at which the vapor pressure of the liquid is equal to atmospheric pressure).

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23
Q

Boiling point elevation

A

An increase in the boiling point of a solution, proportional to the concentration of solute particles.

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24
Q

Boyle’s Law

A

The volume of a gas varies inversely with pressure.

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25
Q

Calorie

A

A unit of energy, equal to 4.184 joules.

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26
Q

Catalyst

A

A substance that accelerates a chemical reaction without itself being consumed.

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27
Q

Cathode

A

The electrode at which reduction occurs.

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28
Q

Cation

A

An atom or molecules with a positive charge.

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29
Q

Charles’ Law

A

The volume of a gas varies directly with absolute temperature.

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30
Q

Chemical Equation

A

A shorthand way of describing a chemical change using symbols of elements and formulas of compounds.

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31
Q

Compound

A

A substance formed by the chemical combination of two or more elements.

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32
Q

Concentration

A

The relative amount of a solute in a solution.

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33
Q

Congeners

A

Related chemical substances “related to each other by origin, structure, or function”

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34
Q

Conjugate

A

An acid and a base that are related by removing or adding a single hydrogen ion.

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35
Q

Covalent bond

A

Atoms linked together by sharing valence electrons.

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36
Q

Critical point

A

A point in a phase diagram where the liquid and gas states cease to be distinct.

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37
Q

Crystalline

A

The regular, geometric arrangement of atoms in a solid.

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38
Q

Decomposition

A

A chemical reaction in which a compound is broken down into simpler compounds or elements.

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39
Q

Dissociation

A

The separation of a solute into constituent ions.

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40
Q

Electrochemical cell

A

A device that uses a chemical reaction to produce or use an electric current.

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41
Q

Electrode

A

The point in an electrochemical cell at which reduction or oxidation occurs.

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42
Q

Electrolysis

A

The decomposition of a substance by an electric current.

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43
Q

Electrolyte

A

A substance that forms ions when dissolved in water.

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44
Q

Electromotive force

A

The electrical potential produced by a chemical reaction, voltage.

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45
Q

Electron

A

A light subatomic particle with negative charge; found in orbitals surrounding an atomic nucleus.

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46
Q

Electronegativity

A

A number describing the attraction of an element for electrons in a chemical bond.

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47
Q

Element

A

A substance that cannot be decomposed; each chemical element is characterized by the number of protons in the nucleus.

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48
Q

EMF

A

Electromotive force (See that card)

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49
Q

Endothermic

A

Refers to a reaction that absorbs heat.

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50
Q

Energy

A

The concept of motion or heat required to do work.

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51
Q

Enthalpy

A

The thermodynamic quantity measuring the heat content of a substance.

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52
Q

Entropy

A

The thermodynamic quantity measuring the disorder of a substance.

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53
Q

Equilibrium

A

A balance condition resulting from two opposing reactions or processes.

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54
Q

Equilibrium constant

A

The ratio of concentrations of products to reactants for a reaction at chemical equilibrium.

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55
Q

Exothermic

A

Refers to a reaction that releases heat.

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56
Q

Faraday

A

A unit of electric charge equal to that of one mole of electrons.

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57
Q

Faraday’s Laws

A

Two laws of electrolysis relating the amount of substance to the quantity of electric charge.

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58
Q

Fluid

A

Any substance that flows or deforms under an applied shear stress; any liquid or gas.

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59
Q

Free energy

A

The thermodynamic quantity measuring the tendency of a reaction to proceed; also called Gibbs free energy.

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60
Q

Freezing point

A

The temperature at which a liquid changes into a solid.

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61
Q

Freezing point depression

A

The decrease in freezing point of a solution, proportional to the concentration of solute particles.

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62
Q

Fusion

A

Melting. (?)

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63
Q

Gamma radiation

A

Energy released from a nucleus during radioactive decay.

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64
Q

gas

A

A state of matter in which molecules are widely separated, fluid, expandable, and compressible.

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65
Q

Gas constant

A

R equals 0.082 liter-atmospheres per mole-unit Kelvin.

66
Q

Gram formula mass

A

An amount of a substance equal in grams to the sum of the atomic mass.

67
Q

Ground state

A

The electronic configuration of lowest energy for an atom.

68
Q

Group

A

A column of elements in the periodic table.

69
Q

Half-reaction

A

An oxidation or reduction reaction with free electrons as a product or reactant.

70
Q

Halogens

A

The column of elements from fluorine to astatine.

71
Q

Heat

A

A form of energy that spontaneously flows from a warm body to a cold body. (Snuggles! :)

72
Q

Heat capacity

A

The amount of energy needed to raise the temperature of a substance by one degree Celsius.

73
Q

Hydrocarbon

A

An organic compound containing only carbon and hydrogen.

74
Q

Hydrogen bond

A

A weak, secondary bond between a partially positive hydrogen atom and a partially negative N, O, or F atom; an intermolecular force of attraction.

75
Q

Hydroxide

A

Refers to the OH- ion.

76
Q

Ideal gas equation

A

The equation relating the volume of a gas to its pressure, temperature, and moles of gas.

77
Q

Inert gases

A

The column of elements from helium to radon; also called noble gases.

78
Q

Ion

A

An atom with an electric charge due to gain or loss of electrons.

79
Q

Ionic bond

A

Atoms linked together by the attraction of opposite charges.

80
Q

Ionic disassociation

A

Separation of cations and anions from an ionic compound by polar water molecules.

81
Q

Ionization

A

Removing electrons from an atom; alternatively, the dissociation of a solute into ions.

82
Q

Isoelectronic

A

Refers to several dissimilar atoms or ions with identical electronic configurations.

83
Q

Isomers

A

Several molecules with the same composition but different structures.

84
Q

Isotope

A

A variety of an element characterized by a specific number of neutrons in the nucleus.

85
Q

Joule

A

A unit of energy equal to 0.239 calorie.

86
Q

Lanthanides

A

The row of elements beneath the main section of the periodic table, from cerium to lutetium; also called rare earths.

87
Q

Le Chatelier’s Principle

A

A system that is in equilibrium is disturbed adjusts so as to minimize the disturbance.

88
Q

Liquid

A

A state of matter in which the molecules are touching, fluid, and incompressible.

89
Q

Litmus

A

An indicator that turns red in acid and blue in alkaline solution.

90
Q

Mass number

A

The sum of the number of neutrons and protons in the nucleus of an atom.

91
Q

Mass percent

A

The percentage found by taking the mass of an element and dividing it by the mass of a sample and then multiplying by 100.

92
Q

Melting point

A

The temperature at which a solid changes to a liquid.

93
Q

Metallic bond

A

Atoms linked together by the migration of electrons from atom to atom.

94
Q

Metals

A

The elements in the middle and left parts of the periodic table, except for hydrogen.

95
Q

Molality

A

The number of moles of solute in one kilogram of solvent.

96
Q

Molar heat capacity

A

the amount of heat required to raise the temperature of one mole of substance one degree Celsius.

97
Q

Molarity

A

The number of moles of solute in one liter of solution.

98
Q

Mole

A

An amount of a substance equal in grams to the sum of the atomic weights.

99
Q

Mole fraction

A

The fraction of moles (or molecules) of one substance in the total moles (or molecules) of all substances in the mixture. If the mole fraction of substance A is 0.1, one tenth of all the molecules in a mixture are A molecules.

100
Q

Molecular formula

A

Describes the ration of moles of the elements in a molecule.

101
Q

Molecule

A

A group of atoms linked together by covalent bonds.

102
Q

Neutralization

A

The chemical reaction of an acid and base to yield a salt and water.

103
Q

Neutron

A

A heavy subatomic particle with zero charge; found in an atomic nucleus.

104
Q

Noble gases

A

The column of elements from helium to radon; also called inert gases.

105
Q

Nonmetals

A

The elements in the upper right part of the periodic table, and also hydrogen.

106
Q

Nucleon

A

A proton or neutron found in an atomic nucleus.

107
Q

Nucleus

A

The core of an atom, containing protons and neutrons.

108
Q

Orbital

A

A region in space surrounding the nucleus, which is occupied by up to two electrons. (bullcrap- can have 8)

109
Q

Organic

A

Refers to compounds based on carbon.

110
Q

Organic chemistry

A

An area of chemistry dealing principally with the chemistry of carbon.

111
Q

Oxidation

A

The loss of electrons by a species.

112
Q

Oxidation number

A

A signed integer representing the real or hypothetical charge of an atom due to the gain or loss of electrons.

113
Q

Oxidation-reduction reaction

A

Reaction in which electrons are transferred between atoms.

114
Q

Oxide

A

A compound of oxygen and another element.

115
Q

Oxidizing agent

A

The species that is reduced during a redox reaction.

116
Q

Period

A

A horizontal row of elements in the periodic table.

117
Q

pH

A

A number describing the concentration of hydrogen ions in a solution; equals -log[H+]

118
Q

Phase

A

A substance with uniform composition and definite physical state.

119
Q

Polar bond

A

A bond with both ionic and covalent characteristics.

120
Q

Polyprotic

A

Refers to an acid with several hydrogens that can ionize.

121
Q

Precipitate

A

A solid that separates from solution.

122
Q

Product

A

A substance on the right side of a chemical equation, which is produced or formed during a chemical reaction.

123
Q

Proton

A

A heavy subatomic particle with a positive charge; found in an atomic nucleus.

124
Q

Radioactive decay

A

The spontaneous disintegration of an unstable nucleus producing a different nucleus and various types of radiation particles.

125
Q

Radioactivity

A

The emission of subatomic particles from a nucleus.

126
Q

Rare earths

A

The elements from cerium to lutetium; lanthanides.

127
Q

Reactant

A

A substance on the left side of a chemical equation which is one of the beginning substances in a chemical reaction.

128
Q

Redox

A

Refers to a reaction in which simultaneous reduction and oxidation occur.

129
Q

Reducing agent

A

The species that is oxidized during a redox reaction.

130
Q

Reduction

A

The gain of electrons by a species.

131
Q

Salt

A

A solid compound composed of both metallic and nonmetallic elements, often as ions.

132
Q

Saturated

A

Describes a solution that holds as much solute as possible.

133
Q

Saturated hydrocarbon

A

A hydrocarbon containing only single bonds between the carbon atoms.

134
Q

Shell

A

A set of electron orbitals with the same principal quantum number.

135
Q

Solid

A

A state of matter in which the molecules are touching and possessing rigid shape and which is not compressible.

136
Q

Solubility

A

The upper limit of concentration of a solute.

137
Q

Solubility product

A

The constant obtained by multiplying the ion concentrations in a saturated solution raised to their balancing coefficients.

138
Q

Solute

A

The substance that is dissolved in a solution.

139
Q

Solution

A

A homogenous mixture consisting of a solvent and one or more solutes.

140
Q

Solvent

A

The host substance of dominant abundance in a solution.

141
Q

Specific heat capacity

A

The amount of heat required to raise 1 gram of a substance 1 degree Celsius.

142
Q

Standard Temperature and Pressure (STP)

A

0 degrees Celsius and 1 atmosphere pressure. (Note: 1 mole of any gas at STP has a volume of 22.4 liters.)

143
Q

States of matter

A

Solid, liquid, gas.

144
Q

Stoichiometric

A

Refers to compounds or reactions in which the components are in fixed, who-number rations.

145
Q

Strong electrolyte

A

An acid, base, or salt that dissociates almost completely to ions in aqueous solution.

146
Q

Structural formula

A

Depicts the bonding of atoms in a molecule.

147
Q

Sublimation

A

The transformation of a solid directly to a gas without an intervening liquid state.

148
Q

Subshell

A

A set of electron orbitals with the same principal and second quantum number. 2p, 3s, etc are examples.

149
Q

Supersaturated

A

Describes a solution that holds more solute than is theoretically possible at that given temperature.

150
Q

Symbol

A

An abbreviation for the name of an element.

151
Q

Thermodynamics

A

The study of energy, principally heat energy, that accompanies chemical or physical changes.

152
Q

Transition metals

A

The three rows of elements in the middle of the periodic table, from scandium to zinc, the yttrium to cadmium, and lanthanum to mercury.

153
Q

Transmutation

A

The process of changing one chemical element to another element during radioactive decay.

154
Q

Triple point

A

A point in a phase diagram where the three states of matter are in equilibrium.

155
Q

Unsaturated

A

Describes a solution that does not hold as much solute as possible.

156
Q

Unsaturated hydrocarbon

A

A hydrocarbon that contains double or triple bonds between at least two of its carbon atoms.

157
Q

Valence

A

A signed integer describing the combining power of an atom.

158
Q

Valence electrons

A

The outermost shell of electrons in an atom or ion.

159
Q

Voltaic cell

A

A device that uses chemical reaction to produce electricity.

160
Q

Weak electrolyte

A

An acid, base, or salt that dissociates only slightly to form ions in solution.

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