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Gen Chem 2 > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

what type of crystal is hard, brittle, high melting point, and poor conductor of heat and electricity give example

A

ionic (NaCl) and covalent (C)

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2
Q

ionic cohesive forces

A

coulomb attraction and dispersion forces

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3
Q

covalent cohesive forces

A

covalent bonds

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4
Q

the quantitative measure off the force required to increase a liquids surface area

A

surface tension

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5
Q

curvature depends on the relative strength of _______ and ________ forces

A

cohesive
adhesive

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6
Q

a liquids resistance to flow is given by

A

viscosity

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7
Q

the pressure created in the container is called _______ _________ of the liquid

A

vapor pressure

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8
Q

liquids with high vapor pressure at room temp are called

A

volatile

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9
Q

Clausius Clapeyron equation

A

lnPvap= (-Hvap/R)1/T +C

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10
Q

2 point form of CC equation

A

lnp1/p2=Hvap/R(1/t2-1/t1)

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11
Q

atoms in crystalline solids have a ________ structure

A

lattice

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12
Q

the basic repeating unit that can be used to describe the __________ of the crystal

A

unit cell

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13
Q

simple cubic crystal system equation

A

a=b=c

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14
Q

to describe the packing of spheres the _________ number of each atom can be used

A

coordination

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15
Q

the arrangement of ordered stacks of atoms is called ________ _______ _______

A

simple cubic packing

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16
Q

primitive cubic coordination number

A

6

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17
Q

body centered coordination number

A

8

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18
Q

face centered coordination number

A

17

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19
Q

corner atoms

A

8 cells

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20
Q

edge atoms

A

4 cells

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21
Q

face atoms

A

2 cells

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22
Q

simple cubic equation

A

a=2r

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23
Q

body centered equation

A

a=4r/root 3

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24
Q

face centered equation

A

a=root 8 r

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25
Q

what type of crystal is soft, low melting point, poor conductor of heat and electricity

A

molecular (H2O)

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26
Q

molecular cohesive forces

A

dispersion, dipole-dipole, and hydrogen bonds

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27
Q

what type of crystal is variable hardness and melting point, good conductor of heat and electricity

A

metallic bonds (Na)

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28
Q

metallic cohesive forces

A

metallic

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29
Q

what is opposite of crystalline and only have short range order present

A

amorphous solids

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30
Q

braggs equation

A

2dsin theta = n^2

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31
Q

solid to liquid

A

fusion / melting

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32
Q

liquid to gas

A

vaporization

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33
Q

solid to gas

A

sublimation

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34
Q

liquid to solid

A

freezing

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35
Q

gas to liquid

A

condensation

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36
Q

gas to solid

A

deposition

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37
Q

phase change equation

A

delta G= delta H - T*delta S

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38
Q

above critical temp and pressure the state of matter is referred to as ______________

A

superficial fluid

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39
Q

the dissolved substance

A

solute

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40
Q

the major component

A

solvent

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41
Q

a solution that contains the max amount of solute that will dissolve in a given solvent

A

saturated solution

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42
Q

a solution that contains less solute than a solvent has the capacity to dissolve

A

unsaturated solution

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43
Q

a solution that contains more solute than would be present in a saturated solution

A

supersaturated solution

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44
Q

the process in which dissolved solute comes out of the solution and forms crystals

A

crystallization

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45
Q

the maximum amount of solute that can be dissolved in a solvent at a given temp

A

solubility

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46
Q

two or more liquids that are complexity soluble in each other in all proportions

A

miscible

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47
Q

what type of interaction are in polar solvents

A

ion or dipole interaction

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48
Q

what type of interactions are in non polar solvents

A

London dispersion forces

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49
Q

Like _______ like

A

dissolves

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50
Q

strong _______ solvent interaction are favorable

A

solute

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51
Q

the solute-solvent interactions are stronger than the solute solute and solvent solvent interaction (favorable)

A

exothermic

52
Q

the solute solvent interactions are weaker than the solute solute and solvent solvent interaction (unfavorable)

A

endothermic

53
Q

delta S is a measure of _____ and is always _______

A

randomenss
positive

54
Q

molarity (M) equation and units

A

moles solute/ L solution (mol/L)

55
Q

Mole fraction equation

A

X=moles A/ total moles

56
Q

mass % equation

A

mass A/ total mass

57
Q

parts per million

A

mass A/ total mass x 10^6

58
Q

parts per billion

A

mass A/ total mass x 10^9

59
Q

molality (m) equation and units

A

moles solute/ kg solvent (mol/kg)

60
Q

is dissolution temperature dependent

A

yes

61
Q

solids in liquids and liquids in liquids: usually ______ dependence on pressure

A

little

62
Q

gases in liquids _______ dependence on pressure

A

strong

63
Q

henrys solubility law

A

solubility = c= kxP

64
Q

what properties depend on the number of solute particles in the solution and they affect the properties of the solvent

A

colligative properties

65
Q

raoults law

A

delta P= Xsolute*P0solv

66
Q

raoults law manipulated

A

Ptotal=XaP0a+XbP0b

67
Q

boling point elevation equation

A

delta Tb= Tb-T0B=Kb*m

68
Q

solutions have ________ entropy than pure solvents

A

higher

69
Q

freezing point depression equation

A

delta Tf= T0f-Tf= Kf*m

70
Q

freezing point is usually _______ sensitive than boiling point

A

more

71
Q

what refers to the selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated one

A

osmosis

72
Q

the pressure required to stop osmosis

A

osmotic pressure

73
Q

osmosis equation

A

Pie = MxRxT

74
Q

solutions that have equal concentration of solute

A

isotonic

75
Q

solutions with higher concentration of solute

A

hypertonic

76
Q

solutions with lower concentration of solute

A

hypotonic

77
Q

vant hoff factor I:

A

number of formula units initially dissolved in solution

78
Q

colligative property equation for boiling point

A

delta Tb = iKbm

79
Q

colligative property equation for freezing point

A

delta Tf= iKfm

80
Q

colligative osmosis property equation

A

pie = iMRT

81
Q

gas and liquid and gas and solid

A

aerosol

82
Q

liquid and gas and solid and gas

A

foam

83
Q

liquid and liquid

A

emulsion

84
Q

liquid and solid

A

sol

85
Q

solid and liquid

A

gel

86
Q

solid and solid

A

solid sol

87
Q

colloids in water are characterized as ________ and _________

A

hydrophilic and hydrophobic

88
Q

colloids are important for _______ folding

A

protein

89
Q

a hydrophobic colloid would usually form ______ in water

A

clumps

90
Q

the change in concentration of a reactant or product with time M/s

A

reaction rate

91
Q

reaction rate equations

A

-delt [A]/ delta t and delta [B]/ delta t
or k[A]^x[B]^y

92
Q

the rate of decomposition gets a ______ sign

A

minus

93
Q

what is the average rate

A

average reaction rate over a period of time

94
Q

what is the instantaneous rate

A

the rate at a single point in time

95
Q

what is the initial rate

A

the instantaneous reaction rate at the start of the reaction

96
Q

k =

A

rate constant

97
Q

what does the rate constant depend on

A

temperature and is constant for all

98
Q

general rate of reaction

A

-1/a delta [A]/delta t = -1/b delta [B]/ delta t= 1/c delta [C]/ delta t = 1/d delta[D]/ delta t

99
Q

zero order rate law, integrated rate law, and half life

A

rate law: rate = k
integrated rate: [A]t= -kt + [A]0
half life : [A]0/2k

100
Q

first order rate law, integrated rate law, and half life

A

rate law: rate = k[A]
integrated: ln[A]t/[A]0 = -kt
half life: 0.693/k

101
Q

second order rate law, integrated rate law, and half life

A

rate law: rate= k[A]^2
integrated: 1/[A]t=kt+1/[A]0
half life: 1/k[A]0

102
Q

the _____ _________ is the proportionally constant between the rate and the concentration reactants

A

rate constant

103
Q

zero order reaction units

A

ms^-1

104
Q

first order reaction units

A

s^-1

105
Q

second order reaction units

A

m^-1s^-1

106
Q

third order reaction units

A

m^-2s^-1

107
Q

reaction rate ________ rate constant

A

does NOT equal

108
Q

if its a zero reaction the rate

A

stays the same

109
Q

if it is a first order reaction the rate goes up by a factor of

A

2

110
Q

if it is a second order reaction the rate goes up by a factor of

A

4

111
Q

the concentrations of reactants and products as a function of time depend on the ______ ______

A

reaction order

112
Q

linear line for zero order reaction

A

[A]0

113
Q

linear line for first order reaction

A

ln[A]0

114
Q

linear line for a second order reaction

A

1/[A]0

115
Q

successive half lives for a zero order reaction

A

get shorter

116
Q

succesive half lives for a first order reaction are

A

identical

117
Q

successive half lives for a second order reaction

A

double

118
Q

T or F: a rate law can be determined from an overall chemical reaction

A

F

119
Q

T or F: Rate vs [A]0 data, [A] vs time data, and half life data are three ways to determine the order with respect to A

A

T

120
Q

T or F reaction rates depend on concentration

A

F

121
Q

T or F the units of the rate constant k, depend on the order of the reaction

A

T

122
Q

T or F molecular solids generally have low melting points because of weak intermolecular forces

A

T

123
Q

T or F for a spontaneous dissolution the enthalpy of solution must be negative

A

F

124
Q

T or F molality is temp dependent

A

T

125
Q

T or F solubility increases with increasing temp for both solids in liquids and gases in liquids

A

F

126
Q

T or F colligative properties depend one the amount of solute added, not the chemical properties of the solute

A

both

Gen Chem 2 (3 decks)

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