Unit 11- Liquids and Solids Flashcards

1
Q

intermolec forces

A

attraction that hold molecs together in the liquid and solid states

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2
Q

gas

A
  • assumes vol/shape of cotainer
  • low density
  • easily compressed
  • kinetic energy &laquo_space;energy of attraction
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3
Q

liquid

A
  • def vol, assume shape of container
  • high density
  • nearly incompressible
  • kinetic energy = energy of attraction
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4
Q

solid

A
  • def vol and shape
  • high density
  • nearly incompressible
  • kinetic energy&raquo_space; energy of attraction
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5
Q

evaporation

A

process by which molecs escape from the liquid to the gas phase

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6
Q

condensation

A

process by which molecs go from the gas phase to the liquid phase

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7
Q

Maxwell-Boltzmann Distribution

A

as temp inc, # of molecs that can evap inc

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8
Q

gas pressure above liquids

A
  • pressure in gas phase inc as molec evap from liquid
  • pressure becomes const when evap = condensation
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9
Q

Dynamic equilibrium

A

state in which the 2 opposing changes occur at equal rates, so net change is apparent
- indicated by double arrow

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10
Q

vapor pressure

A

partial pressure of the gas when the rate of evapo = rate of condensation
- as temp inc, the vapor pressure of a liquid incs
- the stronger the intermolec forces, the lower the vapor pressure of the liquid at any temp

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11
Q

boiling point

A

temp the vapor pressure is = to external pressure

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12
Q

normal boiling point

A

temp at which vapor pressure = to 1 atm

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13
Q

enthalpy of vap

A

enthapy change that accompanies conversion of 1 mol of sub from a liquid to a gas at const temp (L —> g)

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14
Q

vap and intermolec forces

A

as strength of forces inc, VP dec, b.p inc, and deltaHvap inc

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15
Q

liquid-solid equilibrium

A

changes of a sub from liquid to solid (freezing) and from solid to liquid (melting or fusion)
- involve dynamic equilib

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16
Q

melting point

A

temp solid and liquid phases are in equilib when the pressure is 1 atm (pressure has little effect on melting point)

17
Q

enthalpy of fusion

A

enthalpy change that accompanies the change of 1 mol of solid into liquid at const temp

18
Q

heating curves

A

graph of temp of sample vs heat added
- first angle is solid
- second angle is liquid
- third angle is gas

19
Q

sublimation

A

solid to the gas phase

20
Q

deposition

A

gas to solid phase

21
Q

enthalpy of sublimation

A

enthalpy change fro the conversion of 1 mol of sub from solid to gas
deltaHsub = deltaHfus + deltaHvap

22
Q

phase diagrams

A

graph of pressure vs temp that shows the region of stability for each phase
- first inc= s-g equilib line
- second inc= l-g equilib line
- vertical line= s-l quilib line

23
Q

melting pt and pressure

A
  • if solid is more dense than liquid (common), melting pt INCS w/ INC pressure
  • If liquid more dense (H2O), melting point DECS w/ INC pressure
24
Q

electrostatic forces

A

accounts for all types of intermolec forces
- dipole-dipole attractions
- London dispersion
- Hydrogen bonding

*London < Dipole < hydro

25
Q

dipole-dipole attraction

A

results from electronic forces between molec dipoles. Must be POLAR
* polarity inc, dipole inc

26
Q

London dispersion forces

A