Chapter 10 Flashcards

1
Q

solid

A

high density
very limited freed om of motion
strong IMFs

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2
Q

liquid

A

high density
some freed om of motion
moderate strength of IMFs

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3
Q

gas

A

low density
complete freedom of motion
weak IMFs

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4
Q

intermolecular forcesq

A

attractive forces that exists between molevules and atoms

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5
Q

four types of intermolecular forces

A
  1. dispersion forces
  2. dipol-dipole forces
  3. hydrongen bonding
  4. ion-dipole forces
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6
Q

dispersion forces(london forces)

A

exhibited by all atoms and molecules that results from rapid flutuating, temporay diples

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7
Q

induced dipole

A

temporary dipole formed when the electrons of an atom or molecule are distored by the instantaneous dipole of a neighboring atom or molecule

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8
Q

effects of molar mass on dispersion forces

A

larger the molar mass= stronger the attraction

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9
Q

effects of shape of molecule on dispersion forces

A

larger surface = stronger attraction

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10
Q

dipersion factors effect boiling point

A

strong dispersion forces = high boiling point

weak dispersion force= low boiling point

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11
Q

dipole-dipole forces

A

an IMF presented only in polar molecules

stronger than dispersion forces

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12
Q

polar bonds

A

electronegativity difference is (0.5-1.7)

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13
Q

for a molecule to be polar it must have

A
  1. polar bonds(large electronegativity differnece)

2. asymmetrical shape; polar bonds do not cancel out

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14
Q

nonpolar molecule with identical polar bonds

A

linear
trigonal planar
tetrahedral

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15
Q

polar molecule with polar bonds

A

bent

trigonal pyramidal

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16
Q

hydrogen bonding

A

present when polar molecules containg h atoms bodn directly to small and highly electronegative f, o, or n atoms
(stonger than dipole-dipole and dispersion forces)

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17
Q

ion-dipole forces

A

occurs when an ionic combound is mixed with a polar compound

stronger than any other Imfs

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18
Q

threee manifestation of imfs

A
  1. viscosity
  2. surface tension
  3. capillary
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19
Q

viscosity

A

measure of aliquid resisytance to flow

20
Q

how imf effects viscosity

A

stonger imf= higher viscosity

21
Q

how temperatuire effects viscosity

A

higher temperature= lower viscosity

22
Q

surface tension

A

the energy required to increase the surface area of a liquid by a unit amount

23
Q

how imfs effect surface tension

A

higher IMFs=higher surface tension

24
Q

how temperature effects surface tension

A

higher temperature = lower surface tension

25
vaporization
liquid to gas | endothermic process
26
heat of vaporization
the amount of heat required to vaporize one mole of a liquid to gas; always positive
27
condensation
gas to liquid exothermic process enrgy is released
28
heat of condensation
the amount of heat released when one mole of a gas condenses to liquid; always negative
29
the rate of vaporization increases with
increasing temperature increasing surface area decreasing strength of intermolecular forces
30
dynamic equilibriun
state of a system in which reciprocal process are occuring at equal rates the double arrou indicates a dynamic equilibrium
31
vapor pressure
pressure exterted bya a vapor in equilbrium witha solid or liquid at a given tenperatur in a clsoed system
32
how IMFs affect bapor pressure
weaker IMFs= higher vapor pressure
33
how temperature affects vapor pressure
higher temperature- higher vapor pressure
34
boiling point
is the temp. at which the vapor pressure of a liquid equals the pressure of a gas above it
35
how imf effect boiling point
stronger IMFs = higher boiling point
36
normal boiling point
the temp. at which it vapor pressure equals 1 atm
37
sublimation
the phase transition from solid to gas
38
deposition
the phase transition from gas to solids
39
melting/fusion
solid to liquid
40
melting point
temp at which the solid and liquid pahses of a substace are in equilibirum
41
freezing
liquid to solid
42
phase diuagram
presuure - temperature y-x sumeraizing condition under the pahses of a substance can exist
43
regions
the three main regions- solid, liquid, and gas- represent conditions where that particular state is stable
44
lines
the substances are in equalibrium between the two states on wither side of the line both states coestist, and equally stable
45
triple point
temperature and pressure at which the vapor, liquid, and solid, phases of a substance are in equilibrium