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2 Flashcards

1
Q

Study of matter

A

chemistry

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2
Q

any substance that has mass and occupies space

A

matter

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3
Q

cannot be broken down into simpler substances by any chemical reaction

A

elements

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4
Q

substances containing two or more elements that are combined chemically

A

compounds

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5
Q

law that states that pure compounds always contains the same element in exactly the same proportions

A

law of definite proportions or law of constant composition

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6
Q

material having variable composition which can be separated by physical means

A

mixture

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7
Q

compounds made of carbon and hydrogen

A

organic chemicals

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8
Q

The only hydroxide that alkaline earth metal that is not basic

A

beryllium

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9
Q

extremely small particle of matter that retains its identity during chemical reactions

A

atom

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10
Q

positively charged particle

A

proton

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11
Q

particle having a mass almost equal to that of a proton, but no charge

A

neutron

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12
Q

number of protons in the nucleus of an atom

A

atomic number

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13
Q

sum of the number of protons and neutrons in the nucleus of a particular element

A

mass number

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14
Q

chemically identical forms of an element having different numbers of neutron

A

isotopes

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15
Q

average atomic mass for the naturally occurring element

A

atomic weight

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16
Q

atomic weight is expressed as

A

amu or daltons

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17
Q

definite group of atoms that are chemically bonded and held together in a fixed geometric arrangement

A

molecule

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18
Q

chemical bond formed by electrostatic attraction between positive and negative ions

A

ionic bond

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19
Q

atom that loses electron

A

cation

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20
Q

positively charged ion

A

cation

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21
Q

atom that gains electron

A

anion

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22
Q

negatively charged ion

A

anion

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23
Q

compounds that tend to have a greater ability to draw an electron toward itself

A

high electronegativities

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24
Q

formed by sharing a pair of electrons between atoms

A

covalent bond

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25
Q

bond in which the bonding electrons are not equally shared

A

polar covalent bond

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26
Q

bond where the probability of finding electrons in the vicinity of one atom is greater than the other

A

polar covalent bond

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27
Q

Includes both dipole-dipole and dispersion force

A

Van der waals

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28
Q

weak short range attractive force that results from the instantaneous dipole/induced dipole interaction that can occur because of the varying positions of the electrons as they move around the nuclei

A

dispersion force

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29
Q

The higher the molecular weight, the ___ the dispersion force

A

stronger

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30
Q

weight of a mole of that particular substance

A

molecular weight

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31
Q

electrically charged atom or molecule

A

ion

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32
Q

number of moles per liter of solution

A

molarity (M)

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33
Q

symbolic representation of a chemical reaction in terms of chemical formula

A

chemical equation

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34
Q

Solid insoluble compound that is formed from the reaction of dissolved ions and other ions

A

precipitates

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35
Q

phase change reaction by which dissolved chemical form insoluble solid

A

precipitation reaction

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36
Q

A reaction where a single reactant breaks down into it’s ions, most often making an aqueous solution

A

dissolution reaction

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37
Q

any substance that can accept a proton

A

Bronsted-Lowry base

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38
Q

any substance that can donate proton

A

Bronsted-Lowry acid

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39
Q

Donate proton

A

acid

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40
Q

Accept proton

A

base

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41
Q

can act as either an acid or a base

A

amphoteric

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42
Q

the coordination of two or more atoms, molecules, or ions result in the formation of a more stable product

A

complexation reaction

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43
Q

compound consisting of either complex ions with other ions of opposite charge or neutral complex species

A

complex

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44
Q

metal ion with lewis bases

A

complex ions

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45
Q

lewis base attached to the metal atom in a complex

A

ligand

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46
Q

involves change in the oxidation state of an ion and the transfer of electrons

A

redox reaction

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47
Q

the solubility of oxygen ____ as the temperature decreases

A

increases

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48
Q

rate of the reaction proceeding to the right is equal to the the left

A

chemical equilibrium

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49
Q

rate of the forward reaction equals the rate of the reverse reaction

A

chemical equilibrium

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50
Q

product of the concentration divided by the product of the reaction, both raised to a power equivalent to the stoichiometric coefficient

A

equilibrium constant

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51
Q

the value of the equilibrium constant is constant for a particular reaction at a given time

A

law of mass action

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52
Q

solubility products were defined using

A

activities and not molar concentration

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53
Q

driving force for a reaction to reach equilibrium is driven by

A

Gibb’s free energy

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54
Q

degree of ionization of water can be measured by

A

dissociation constant or ionization constant

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55
Q

acids that do not completely dissociate in water

A

weak acid

56
Q

Weak acids

A

acetic, carbonic, hydrogen sulfide, hypochlorous acid, phosphoric

57
Q

at equilibrium, the partial pressure of a chemical in the gas phase is linearly proportional to the concentration in the aqueous phase

A

Henry’s law

58
Q

Henry’s constant greater than one then compound

A

prefers to be in air than in water

59
Q

Henry’s constant less than one

A

prefer water than air

60
Q

the study of the speed of the reactions such as radioactive decay and dissolution of rocks and minerals

A

reaction kinetic

61
Q

refers to the rate of formation or disappearance

A

rate of reaction

62
Q

reactions that take place in single phase

A

homogeneous reaction

63
Q

reaction that occur at surfaces between phases

A

heterogeneous reaction

64
Q

reaction rate constant is generally dependent on

A

temperature and pressure

65
Q

sum of the exponent in the reaction rate equation

A

order of reaction

66
Q

reaction where in the stoichiometric equation represents both mass balance and the reaction process on a molecular scale

A

elementary reaction

67
Q

States the effect of temperature on the elementary reaction

A

Arrhenius

68
Q
A
68
Q

Postulated the two-film theory

A

Lewis and Whitman

69
Q

the boundary between the gas phase and the liquid phase is composed of two distinct films that serve as barriers between the bulk phases

A

two-film theory

70
Q

driving force that causes gas to move from the gas phase to the gas film to liquid film and into the liquid phase

A

concentration gradient

71
Q

Saturation concentration is greater than the concentration

A

gas will go into the solution

72
Q

Concentration is greater than saturation concentration

A

gas will volatize from solution

73
Q

Difference between the saturation and actual concentration

A

deficit

74
Q

Father of environmental chemistry

A

Werner Stumm

75
Q

reaction at the solid-water interface

A

heterogenous reaction

76
Q

reactions in the solid-water interface is dependent on

A

the reactive surface area of the solid and the composition of mineral surfaces

77
Q

compounds that have single c-c bond

A

alkane

78
Q

compounds with double bond

A

alkene

79
Q

compounds with triple bond

A

alkynes

80
Q

Alkane Formula

A

Cn H(2n+2)

81
Q

Also called as paraffins or aliphatic hydrocarbon

A

alkanes

82
Q

organic compound that have the same molecular formula but different structure

A

structural isomers

83
Q

Alkene Formula

A

Cn H2n

84
Q

Alkynes Formula

A

CnHn

85
Q

Cyclic and have alternating double bond

A

aryl or aromatic compounds

86
Q

simplest aromatic compound

A

benzene

87
Q

three classes of aromatic compound

A

benzenelike hydrocarbons, aromatic hydrocarbons, and polychlorinated biphenyls

88
Q

Benzenelike hydrocarbons

A

BTX (Benzene, Toluene, Xylene)

89
Q

Polycyclic aromatic hydrocarbon is also known as

A

polynuclear aromatic hydrocarbons

90
Q

Biphenyls

A

two benzene ring

91
Q

Chlorinated biphenyls have ___ chlorine atoms bonded to each of the aromatic rings

A

one to five

92
Q

less easily biodegradable

A

recalcitrant

93
Q

mass per unit volume

A

mass density

94
Q

weight (force) per unit volume

A

specific weight

95
Q

resistance to movement

A

viscosity

96
Q

absolute viscosity

A

dynamic viscosity

97
Q

dynamic viscosity divided by the density

A

kinematic viscosity

98
Q

substances can exist in water in three classifications

A

suspended, colloidal, or dissolved

99
Q

liquid or substance itself is changed from liquid to gas in order to achieve separation

A

distillation

100
Q

substance combine with another chemical to form a solid phase

A

precipitation

101
Q

dissolved substances attaches to the surface of the solid particlees

A

adsorption

102
Q

separate water or solid by extracting it into another liquid

A

liquid extraction

103
Q

activated carbon works by

A

adsorption and absorption of dissolved substances onto the carbon

104
Q

mixture of liquid and suspended particles

A

suspension

105
Q

suspended solids are often defined operationally as those solids that can be filtered by a glass fiber filter

A

filterable solids

106
Q

colloidal particles

A

0.001 to 1 micrometer

107
Q

Why is milk colloid?

A

fat molecules are not dissolved but are held in suspension by attractive force of water

108
Q

Means to remove colloidal particles

A

ultracentrifugation or membrane filtration

109
Q

Molarity

A

mg/L

110
Q

molality

A

mg/kg sol

111
Q

Frequently used unit in softening and redox reaction

A

normality

112
Q

gram equivalent per liter

A

normality

113
Q

molecular weight divided by number of electrons transferred in redox reaction or by number of protons transferred in acid-base

A

equivalent weight

114
Q

solution that resists large changes in pH when acid or base is added

A

buffer

115
Q

most important buffer system in water

A

carbonate/bicarbonate

116
Q

Law of mass action

A

Le Chatelier’s principle

117
Q

Ability to resist change

A

buffering capacity

118
Q

water’s ability to resist changes in pH in the addition of acid

A

alkalinity/ acid neutralizing capacity

119
Q

Ability of water to resist change in pH due to addition of base

A

Acidity/ base-neutralizing capacity

120
Q

sum of all titratable bases to a pH of approximately 4.5

A

alkalinity

121
Q

Below pH 4.5

A

H2 CO3 - appreciable quanitity
OH - negligible

Alkalinity is negative

122
Q

pH from 7-8.3

A

HCO3 predominates
H+ concentration equals to OH conc.

Alkalinity equal to concentration of HCO3

123
Q

pH greater than 12.3

A

CO3 predominate, H+ negligible, OH cannot be ignored

124
Q

water with pH greater than 7

A

alkaline water

125
Q

water with high alkalinity

A

has high buffering capacity

126
Q

unit for alkalinity

A

mg as CaCO3 per L

127
Q

extent to which mass of soil can exchange a mass of a certain ion of interest

A

exchange capacity

128
Q

attachment of chemical to either the mineral or organic portion of soil particles and includes both adsorption and absorption

A

sorption

129
Q

forces that can result in the attachment of chemicals to the surface of soil

A

VDW, Hydrogen Bonding, Electrostatic interaction

130
Q

troposphere

A

13 km

131
Q

Mass of atmosphere in the troposphere

A

80-85%

132
Q

Stratosphere

A

50 km

133
Q

stratopause

A

Temperature is 0C

134
Q

Mesosphere

A

80 km

135
Q

Thermosphere

A

outermost layer

136
Q

Found that the total pressure exerted by mixture of gases is equal to sum of the pressure of each type of gas

A

John Dalton

D (9 decks)

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