Exam 1 Flashcards
(126 cards)
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)
2
Q
ionic cohesive forces
A
coulomb attraction and dispersion forces
3
Q
covalent cohesive forces
A
covalent bonds
4
Q
the quantitative measure off the force required to increase a liquids surface area
A
surface tension
5
Q
curvature depends on the relative strength of _______ and ________ forces
A
cohesive
adhesive
6
Q
a liquids resistance to flow is given by
A
viscosity
7
Q
the pressure created in the container is called _______ _________ of the liquid
A
vapor pressure
8
Q
liquids with high vapor pressure at room temp are called
A
volatile
9
Q
Clausius Clapeyron equation
A
lnPvap= (-Hvap/R)1/T +C
10
Q
2 point form of CC equation
A
lnp1/p2=Hvap/R(1/t2-1/t1)
11
Q
atoms in crystalline solids have a ________ structure
A
lattice
12
Q
the basic repeating unit that can be used to describe the __________ of the crystal
A
unit cell
13
Q
simple cubic crystal system equation
A
a=b=c
14
Q
to describe the packing of spheres the _________ number of each atom can be used
A
coordination
15
Q
the arrangement of ordered stacks of atoms is called ________ _______ _______
A
simple cubic packing
16
Q
primitive cubic coordination number
A
6
17
Q
body centered coordination number
A
8
18
Q
face centered coordination number
A
17
19
Q
corner atoms
A
8 cells
20
Q
edge atoms
A
4 cells
21
Q
face atoms
A
2 cells
22
Q
simple cubic equation
A
a=2r
23
Q
body centered equation
A
a=4r/root 3
24
Q
face centered equation
A
a=root 8 r
25
what type of crystal is soft, low melting point, poor conductor of heat and electricity
molecular (H2O)
26
molecular cohesive forces
dispersion, dipole-dipole, and hydrogen bonds
27
what type of crystal is variable hardness and melting point, good conductor of heat and electricity
metallic bonds (Na)
28
metallic cohesive forces
metallic
29
what is opposite of crystalline and only have short range order present
amorphous solids
30
braggs equation
2dsin theta = n^2
31
solid to liquid
fusion / melting
32
liquid to gas
vaporization
33
solid to gas
sublimation
34
liquid to solid
freezing
35
gas to liquid
condensation
36
gas to solid
deposition
37
phase change equation
delta G= delta H - T*delta S
38
above critical temp and pressure the state of matter is referred to as ______________
superficial fluid
39
the dissolved substance
solute
40
the major component
solvent
41
a solution that contains the max amount of solute that will dissolve in a given solvent
saturated solution
42
a solution that contains less solute than a solvent has the capacity to dissolve
unsaturated solution
43
a solution that contains more solute than would be present in a saturated solution
supersaturated solution
44
the process in which dissolved solute comes out of the solution and forms crystals
crystallization
45
the maximum amount of solute that can be dissolved in a solvent at a given temp
solubility
46
two or more liquids that are complexity soluble in each other in all proportions
miscible
47
what type of interaction are in polar solvents
ion or dipole interaction
48
what type of interactions are in non polar solvents
London dispersion forces
49
Like _______ like
dissolves
50
strong _______ solvent interaction are favorable
solute
51
the solute-solvent interactions are stronger than the solute solute and solvent solvent interaction (favorable)
exothermic
52
the solute solvent interactions are weaker than the solute solute and solvent solvent interaction (unfavorable)
endothermic
53
delta S is a measure of _____ and is always _______
randomenss
positive
54
molarity (M) equation and units
moles solute/ L solution (mol/L)
55
Mole fraction equation
X=moles A/ total moles
56
mass % equation
mass A/ total mass
57
parts per million
mass A/ total mass x 10^6
58
parts per billion
mass A/ total mass x 10^9
59
molality (m) equation and units
moles solute/ kg solvent (mol/kg)
60
is dissolution temperature dependent
yes
61
solids in liquids and liquids in liquids: usually ______ dependence on pressure
little
62
gases in liquids _______ dependence on pressure
strong
63
henrys solubility law
solubility = c= kxP
64
what properties depend on the number of solute particles in the solution and they affect the properties of the solvent
colligative properties
65
raoults law
delta P= Xsolute*P0solv
66
raoults law manipulated
Ptotal=XaP0a+XbP0b
67
boling point elevation equation
delta Tb= Tb-T0B=Kb*m
68
solutions have ________ entropy than pure solvents
higher
69
freezing point depression equation
delta Tf= T0f-Tf= Kf*m
70
freezing point is usually _______ sensitive than boiling point
more
71
what refers to the selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated one
osmosis
72
the pressure required to stop osmosis
osmotic pressure
73
osmosis equation
Pie = MxRxT
74
solutions that have equal concentration of solute
isotonic
75
solutions with higher concentration of solute
hypertonic
76
solutions with lower concentration of solute
hypotonic
77
vant hoff factor I:
actual number of particles in solution after dissolution
-------------------------------------------------------
number of formula units initially dissolved in solution
78
colligative property equation for boiling point
delta Tb = iKbm
79
colligative property equation for freezing point
delta Tf= iKfm
80
colligative osmosis property equation
pie = iMRT
81
gas and liquid and gas and solid
aerosol
82
liquid and gas and solid and gas
foam
83
liquid and liquid
emulsion
84
liquid and solid
sol
85
solid and liquid
gel
86
solid and solid
solid sol
87
colloids in water are characterized as ________ and _________
hydrophilic and hydrophobic
88
colloids are important for _______ folding
protein
89
a hydrophobic colloid would usually form ______ in water
clumps
90
the change in concentration of a reactant or product with time M/s
reaction rate
91
reaction rate equations
-delt [A]/ delta t and delta [B]/ delta t
or k[A]^x[B]^y
92
the rate of decomposition gets a ______ sign
minus
93
what is the average rate
average reaction rate over a period of time
94
what is the instantaneous rate
the rate at a single point in time
95
what is the initial rate
the instantaneous reaction rate at the start of the reaction
96
k =
rate constant
97
what does the rate constant depend on
temperature and is constant for all
98
general rate of reaction
-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
zero order rate law, integrated rate law, and half life
rate law: rate = k
integrated rate: [A]t= -kt + [A]0
half life : [A]0/2k
100
first order rate law, integrated rate law, and half life
rate law: rate = k[A]
integrated: ln[A]t/[A]0 = -kt
half life: 0.693/k
101
second order rate law, integrated rate law, and half life
rate law: rate= k[A]^2
integrated: 1/[A]t=kt+1/[A]0
half life: 1/k[A]0
102
the _____ _________ is the proportionally constant between the rate and the concentration reactants
rate constant
103
zero order reaction units
ms^-1
104
first order reaction units
s^-1
105
second order reaction units
m^-1s^-1
106
third order reaction units
m^-2s^-1
107
reaction rate ________ rate constant
does NOT equal
108
if its a zero reaction the rate
stays the same
109
if it is a first order reaction the rate goes up by a factor of
2
110
if it is a second order reaction the rate goes up by a factor of
4
111
the concentrations of reactants and products as a function of time depend on the ______ ______
reaction order
112
linear line for zero order reaction
[A]0
113
linear line for first order reaction
ln[A]0
114
linear line for a second order reaction
1/[A]0
115
successive half lives for a zero order reaction
get shorter
116
succesive half lives for a first order reaction are
identical
117
successive half lives for a second order reaction
double
118
T or F: a rate law can be determined from an overall chemical reaction
F
119
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
T
120
T or F reaction rates depend on concentration
F
121
T or F the units of the rate constant k, depend on the order of the reaction
T
122
T or F molecular solids generally have low melting points because of weak intermolecular forces
T
123
T or F for a spontaneous dissolution the enthalpy of solution must be negative
F
124
T or F molality is temp dependent
T
125
T or F solubility increases with increasing temp for both solids in liquids and gases in liquids
F
126
T or F colligative properties depend one the amount of solute added, not the chemical properties of the solute
both
