Unit 1 (chp 12 & 13) Flashcards
(176 cards)
1
Q
define INTRAMOLECULAR/BONDING FORCES
A
forces within a molecule allowing for chemical behavior to be the same despite different phases
2
Q
what allows for chemical behavior to be the same despite the substance being in different phases
A
intramolecular/bonding forces
3
Q
define INTERMOLECULAR/NONBONDING FORCES
A
forces between molecules that cause differences in physical behavior between phases
4
Q
differences in intermolecular force strength causes
A
differences in physical behavior between phases
5
Q
what produces intermolecular forces
A
the attraction of partial charges or ions + molecules
6
Q
t/f: intermolecular forces are stronger than intramolecular forces
A
false
7
Q
why are intermolecular forces weaker than intramolecular forces
A
they possess smaller charges farther apart
8
Q
define VAN DER WAALS DISTANCE
A
distance between 2 nonbonded atoms in adjacent molecules
9
Q
define VAN DER WAALS RADIUS
A
half closest distance between 2 nuclei of nonbonded atoms
10
Q
t/f: van der waals radius are always larger than the covalent radius
A
true
11
Q
why are van der waals radius always larger than the covalent radius
A
the covalent radius is smaller bc of overlapping orbitals
12
Q
what is the trend of covalent radii and van der waals radii
A
they increase down and to the left
13
Q
define ION DIPOLE FORCE
A
strong intermolecular force composing of an ion & nearby polar molecule
14
Q
an ionic compound dissolving in H2O is an example of which nonbonding force
A
ionic dipole
15
Q
what is the strongests nonbonding force
A
ion dipole
16
Q
define H BOND NONBONDING FORCE
A
2nd strongest nonbonding force composing of polar bond to hydrogen w/dipole charge
17
Q
define DIPOLE-DIPOLE
A
nonbonding force where positive pole of 1 polar molecule is attracted to negative pole of other polar molecules
18
Q
this nonbonding force only occurs in polar molecules
A
dipole-dipole
19
Q
compounds with similar molar masses have a ___ molecular dipole moment, which leads to a greater ____
A
greater; dipole-dipole force
20
Q
define DISPERSION/LONDON FORCES
A
nonbonding force where polarizable electron clouds cause a brief dipole producing polarity
21
Q
what is the weakest nonbonding force
A
dispersion
22
Q
an ___ in a dipole moment leads to increase ___
A
increase; strength
23
Q
why do molecules with higher dipole moments have a higher boiling point
A
has greater strength meaning it is harder to break apart the molecule
24
Q
molecules with a greater dipole moment have a greater ____
A
boiling point
25
substances with intermolecular hydrogen bonds have ____ boiling points
very high
26
define POLARIZABILITY
ease electron cloud is distorted by nearby electric field
27
polariziability causes nonpolar molecules to have a
temporary dipole moment
28
polarizablity causes polar molecules to
enhance the existing dipole moment
29
what factors causes a molecule/atom to be more polarizable
- large particle
- less Zeff
- anion
30
what is the trend for polarizability
it increases down and to the left
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why does polarizability follow a similar trend to atomic size
larger particles are held less tightly allowing it to be more easily disturbed by an electron cloud
32
polarizability correlates cloesly with ____ for similar particles
molar mass
33
t/f: anions are smaller than their parent atoms
false
34
t/f: cations are smaller than their parent atoms
true
35
what causes dispersion forces
instantaneous dipole induces a dipole in another particle leading to attraction
36
what nonbonding force is in all particles
london/dispersion
37
what do dispersion forces do in all particles
increase the energy of attraction in all matter
38
what is the only nonbonding force in nonpolar molecules
london/dispersion
39
t/f: london forces are stronger for more polarizable particles
true
40
larger particles have a ___ dispersion force than smaller particles
true
41
the molecular shape leads to greater ___ which produces stronger ___
surface area; attractions
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more intermolecular contact causes a ___ boiling point
higher
43
an ___ in molar mass leads to an increase in ____ which ___ boiling point
increase; dispersion force strength; increase
44
dispersion forces depend on
proximity
45
define PHASE
physically distinct, homogenous part of system
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how are phase properties determined
balance of potential & kinetic enregy
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potential energy __ particles
attracts
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kinetic energy __ particles
disperses
49
what is the kinetic and potential energy relationship in gases
kinetic > potential
50
what is the kinetic and potential energy relationship in liquids
potential > kinetic
51
what is the kinetic and potential energy relationship in solids
potential (drastic) > kinetic
52
gas has ___ compressibility and __ ability to flow
high; high
53
liquid has __ compressibility and __ ability to flow
low; moderate
54
soids have __ compressibility and __ ability to flow
almost no; almost no
55
define SUBLIMATION
solid to gas phase
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define DEPOSITION
gas to solid phase
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define FUSION
solid to liquid phase
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define VAPORIZATION
liquid to gas phase
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define CONDENSATION
gas to liquid phase
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define FREEZING
liquid to solid phase
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what value is freezing
negative delta H fusion
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what value is fusion
positive delta H fusion
63
what value is vaporization
positive delta H vaporization
64
what value is condensation
negative delta H vaporization
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which is always larger: delta H vap or delta H fus
delta H vap
66
why is delta H vap always larger than delta H fus
it takes more energy to completely separate molecules
67
delta H sublimation =
delta H vap + delta H fus
68
delta H deposition =
negative delta H subl = negative delta H vap + negative delta H fus
69
what changes within a phase
temperature and kinetic energy
70
what changes during a phase change
average particle distance
71
t/f: the temperature changes during a phase change
false; the temperature is constant
72
what is the formula for heat/energy within phase
q = mc(delta T)
73
what is the formula for heat/energy during phase change
q = mol(delta H of phase change)
74
define DYNAMIC EQUILIBRIUM
molecules leaving and entering at same rate
75
define VAPOR PRESSURE
pressure exerted by vapor on liquid
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vapor pressure is constant at __
equilibrium
77
what are the 2 factors of vapor pressure
temperature and type of gas
78
higher temperature causes __ vapor pressure
higher
79
weaker intermolecular forces of a gas causes ___ vapor pressure
higher
80
what is the purpose of the clausius-clapeyron equation
relate vapor pressure to temperature
81
define BOILING POINT
temperature where vapor pressure = external pressure
82
define NORMAL BOILING POINT
boiling temperature at STP of 760 torr/1atm
83
as external pressure __ , boiling point __
increases; increases
84
define CRITICAL POINT
point where densities of gas and liquid phases are =
85
define TRIPLE POINT
point where all 3 phases are in equilibrium
86
define SURFACE TENSION
energy required to increase surface area of liquid
87
stronger forces lead to ___ surface tension
stronger
88
surface tension __ with an increase in temperature
decrease
89
surface molecules experience a net attraction downward. this causes the ___ surface area possible for liquids
smallest
90
define CAPILLARITY
rising of liquid thru narrow spaces against gravity
91
define VISCOSITY
resistance of fluid to flow because of intermolecular attractions impeding movement of molecules around & past each other
92
stronger intermolecular forces have a __ viscosity
higher
93
__ molecules have a higher viscosity
longer
94
an increase in temperature causes a ___ in viscosity
decrease
95
the intermolecular hydrogen bonding of water causes
- solvent power
- high heat capacity & Hvap
- surface tension & capillarity
- open hexagonal structure of ice
96
if a molecule only has ions, it has what nonbonding force
ionic
97
if a molecule has ions and polar molecules, it has what nonbonding force
ion-dipole
98
if a molecule has only nonpolar atoms, it has what nonbonding force
dispersion
99
if a molecule has only polar atoms, it has what force
dipole dipole
100
if a molecule has both polar and nonpolar molecules, it has what nonbonding force
dipole induced dipole
101
if a molecule has ions and nonpolar molecules, it has what nonbonding force
ion induced dipole
102
t/f: dipole induced dipole and ion induced dipoles are both strong nonbonding forces
false, they're both weak
103
t/f: metals have high boiling points
true
104
an increase in enthalpy of vaporization causes an increase in ___
boiling point
105
a decrease in enthalpy of vaporization causes a ___ in vapor pressure
increase
106
define a SOLUTION
homeogenous mixture of atoms/ions/molecules in 1 phase
107
define a COLLOID
heterogenous mixture existing as 2 or more phases
108
colloids are made of
macromolecules/clumps of molecules
109
t/f: colloids can be visibly distinct
true
110
define SOLVENT
most abundant component that dissolves the solute
111
define SOLUTE
thing that is dissolving in solvent
112
define SOLUBILITY
max amount of solute that dissolves in certain amount of solvent at a given temperature
113
t/f: substances with dissimilar intermolecular forces dissolve in each other
false, like dissolves in like
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define MISCIBLE
solute & solvent soluble in each other at any proportion
115
define IMMISCIBLE
liquids that don't dissolve in each other
116
define ALCOHOLS
organic compounds with dual polarity
117
as solubility in water increases, the boiling point ___
increases
118
is delta Hsoln endo or exothermic and why
either depending on whether it is less or negative the sum of Hsolv and Hsol
119
what are the steps to solution formation
1. clump solute + heat --> separate solute
2. clump solvent + heat --> separate solvent
3. separate solute + separate solvent --> solution & heat
120
the separatino of solute and solvent into aqueous states are endo or exothermic reactions?
endothermic
121
define SOLVATION
process which solute particle is surrounded by solvent particles
122
aka solvation but with water
hydration
123
delta Hsol is = to
delta Hlattice
124
what is required to break an ionic solute into gaseous ions
delta H lattice energy (aka delta H solute)
125
t/f: the delta Hsol is always greater than 0
true
126
the hydration of ion is always ___
exothermic
127
why is the hydration of the ion always exothermic
the ion-dipole is very strong
128
delta Hhydr for ions depends on
charge density
129
what is the trend for delta Hhydr and charge density
increase up and to the right
130
charge density =
charge/volume
131
a __ charge and __ radius causes the ion to be closer to the oppositely charged pole of H2O, which causes a __ attraction
higher; lower; stronger
132
define ENTROPY
the # of ways a system can disperse its energy & freedom of motion of particles
133
what phase has the highest entropy
gases
134
which has a higher entropy: the solution or the solute + solvent
solution
135
an __ in entropy is favored for physical and chemical processes
increase
136
physical & chemical change happens at a decrease in __ and increase in __
enthalpy; entropy
137
define SATURATED SOLUTION
max amount of dissolved solute at givent temp in presence of undissolved solute
138
in a saturated solution, what is the relationship between undissolved and dissolved solute
undissolved solute = dissolved solute
139
define UNSATURATED SOLUTION
decrease in equilibrium concenntration of dissolved solute
140
define SUPERSATURATED SOLUTION
increase in equilibrium concentration (generally because an increase of temperature)
141
t/f: supersaturated solutions are unstable
true
142
the instability of supersaturated solutions cause ___ when it is disturbed
crystallization of solute
143
most solids are __ soluble at higher temperature
more
144
gases are less __ as temperature increases
soluble
145
an uncrease in pressure on gas particles cause them to be __ soluble
more
146
define HENRY'S LAW
solubility of a gas is directly proprtional to partial pressure of gas above the solution
147
define MOLARITY
mol of solute/L solution
148
define MOLALITY
mol solute/kg solvent
149
define MOLE FRACTION
mole solute/(mol solute + mol solvent)
150
define PARTS BY MASS
mass solute/mass solution
151
define PARTS BY VOLUME
volume solute/volume solution
152
ppm =
X(10^6)
153
how is mass converted to volume
density
154
define COLLIGATIVE PROPERTIES
properties dependent on number of solute particles and not chemical identity
155
define NONELECTROLYTE
doesn't dissolve into ions
156
vapore pressure of nonvolatile nonelectrolyte is __ than vapor pressure of pure solvent
lower
157
define RAOULT'S LAW
vapor pressur eof solvent above solution isproprotional to mole fraction of the solvent present
158
in volatile nonelectrolyte solutions, the solute and solvent __ the vapor pressure of the other
decrease
159
an increase in mole fraction of th emore volatile component causes
vapor
160
t/f: the vapor of a volatile nonelectrolyte solution is the same as the solution itself
false
161
why do solutions boil at higher temperatures than the pure solvent
decrease in vapor pressure
162
why do solutions freeze at lower temperature than pure solvent
decrease in vapor pressure
163
define OSMOSIS
solvent moves from lower to higher solute concentration regions to reach equilibrium
164
define OSMOTIC PRESSURE
pressure to prevent net flow of solvent that increases the volume
165
define isotonic
osmotic pressure is equal and maintained
166
define HYPOTONIC
too dilute
167
define HYPERTONIC
too concentrated
168
define VANT HOFF FACTOR
takes into account dissociation of strong electrolyte to predict the effect on solution
169
what is the i
the meausred value for electrolyte solution/expected value for nonelectrolyte solution
170
vapor pressure, boiling point elevation, freezing point depression, and osmotic pressure are all
colligative properties
171
ionic atmospher
ions in solution clustered near ions of opposite charges
172
the effective concentration of dissolved particles in ionic atmospheres are __ than expected
lower
173
t/f: ions act independently in an ionic atmospher
false
174
concentration is =
mass solute/volume solution
175
a higher molality leads to a __ boiling point
higher
176
