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Chem 102 > Chapter 11 > Flashcards

Chapter 11 Flashcards

1
Q

intermolecular forces

A

hold any 2 molecules together; weaker than intramolecular forces

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2
Q

intramolecular forces

A

hold 2 same atoms together
- covalent, ionic, metallic

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3
Q

↑ boiling/melting point = ___IMF

A

↑ IMF

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4
Q

↑ surface tension = ___IMF

A

↑ IMF

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5
Q

↑ viscosity = ___ IMF

A

↑ IMF

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6
Q

↑ capillary action = ___ IMF

A

↑ IMF

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7
Q

↑ volatility = ___ IMF

A

↓ IMF

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8
Q

↑ vapor pressure (ideal gas law) = ___ IMF

A

↓ IMF

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9
Q

Viscosity

A

resistance of a liquid to flow

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10
Q

Surface tension

A

surface of water behaves like elastic

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11
Q

Cohesive forces

A

forces bind similar molecules
- ex: hydrogen bonding in water

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12
Q

Adhesive forces

A

forces bind substance to surface

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13
Q

Capillary action

A

rise of liquids up very narrow tubes

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14
Q

Thermodynamically favored phase

A

least costly phase for 1 material

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15
Q

metastable phase

A

less costly phase, but less stable

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16
Q

Phase change

A

change of state of pure substance by heating or cooling

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17
Q

solid –> liquid

A

melting (fusion)

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18
Q

liquid –> gas

A

vaporization

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19
Q

gas –> solid

A

deposition

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20
Q

solid –> gas

A

sublimination

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21
Q

Heat (Enthalpy) of fusion

A

↑ freedom of motion of particles requires energy
- ex: boiling water

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22
Q

Maxwell Distribution

A

velocities of molecules in vapor phase @ given temp are diff
- relates temp to particles and velocity
- bell curve

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23
Q

Phase Diagram

A

summarizes conditions under equilibria b/w diff states of matter

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24
Q

Critical point

A

at/above only 1 gas-like phase exists
- no surface tension

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25
Q

Triple point

A

all 3 phases coexist in equilibrium:
- all 3 curves intersect
- doesn’t matter what phase

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26
Q

Permanent gases

A

substance w/ critical point ↓ than room temp
- Helium, hydrogen, nitrogen, argon, oxygen

27
Q

Clausius Clapeyron Equation (constraint of coexistence): R =

A

8.314 J/molK = 8.34 x 10^-3 KJ/molK

28
Q

Clausius Clapeyron Equation (constraint of coexistence): pressure =

A

1 atom = 101 kPa

29
Q

Clausius Clapeyron Equation (constraint of coexistence): T =

A

temp in Kelvin

30
Q

4 main classes of materials (compounds):

A

ionic compounds, metals, network covalent, molecular

31
Q

ionic compounds

A

Electrostatic attraction b/w cation and anion:
- ability to form crystals
- ↑ enthalpies of fusion/vaporization
- ↑ melting/boiling points
- hard
- conduct electricity
- stronger than covalent bonds

32
Q

metals

A

Collectively share valence e-:
- ↑ melting/boiling points
- shiny
- hard
- good heat conductors

33
Q

network covalent

A
  • Compound w/ atoms bonded by covalent bonds in a continuous network
  • weak interactions
  • covalent bonds extend throughout large region; many repeating units
  • crystals; often oxides or sulfides
  • = rate A common: Si, SiC, SiO2 (quartz), C (diamond), C (graphite), BN, Ge
34
Q

molecular

A
  • Doesn’t conduct electricity
  • insoluble in water (soluble in nonpolar solvents)
  • smelly (volatile)
  • ↓ melting/boiling points
35
Q

Dispersion force

A

instantaneous dipole on one atom causes atoms to be attracted
- all interactions b/w dipole forces
- ALL molecules have dispersion forces

36
Q

↑ molar mass =

A

↑ dispersion force = ↑ boiling point

37
Q

dispersion force: D(t) =

A

q(t) *R
- R = distance/length of molecule
-larger molecule = stronger force

38
Q

Dipole force

A

polar molecules with +/- ends

39
Q

Dipole-dipole interactions

A

presence of permanent dipole moment in a polar molecule

40
Q

Ion-dipole force

A

b/w ion and polar molecule
- cation (+) attracted to (-) end of dipole
- anion (-) attracted to (+) end of dipole

41
Q

critical temp

A

highest temp a liquid phase can form

42
Q

critical pressure

A

pressure required to liquify at critical temp
- ↑ intermolecular forces = ↑ critical temp of substance

43
Q

Vapor pressure

A

pressure of vapor attains constant value

44
Q

most ionic (most polar)

A

atoms in molecule further apart on PT = more ionic

45
Q

Hydrogen bonds…

A

increase boiling point

46
Q

Hydrogen bonds…

A

increase boiling point

47
Q

↑ heat of fusion (enthalpy to melt) = ___ IMF

48
Q

boiling point: polar molecule ___ nonpolar molecule

49
Q

hydrogen bonding:

A

bond b/w X-H:
- X = N, O, F
- R-X-H:———:X-H

50
Q

hydrogen bonding attractive forces

A

all 3: dispersion, dipolar (dipole-dipole), hydrogen bonding

51
Q

H bond affects boiling point how?

A

↑ attraction (bc of all 3 forces) = ↑ boiling point

52
Q

if an atom has at least 1 hydrogen bond it must…

A

have all 3 attractive forces (dispersion, dipolar, hydrogen bonding)

53
Q

forces by molecule: nonpolar molecules

A

dispersion forces

54
Q

forces by molecule: polar molecules

A

dispersion forces + dipole/dipole = ↑ boiling p.

55
Q

forces by molecule: hydrogen bonding in molecule

A

dispersion forces + dipole/dipole + hydrogen bonding

56
Q

What elements form a hydrogen bond w/ H?

57
Q

how does a hydrogen bond impact boiling point?

58
Q

nonpolar solvents…

A

will NOT dissolve in water

59
Q

solvents with 5+ C’s…

A

will NOT dissolve in water

60
Q

polar solvents…

A

WILL dissolve in water

61
Q

hydrophilic molecules

A
  • cation + anion
  • charged ions
    polar molecules
62
Q

hydrophobic molecules

A

hydrocarbons and nonpolar molecules

63
Q

Molecules w/ hydrophobic and hydrophilic parts:

A
  • Still soluble; increased C = less soluble
  • 5+ C = not soluble
64
Q

↑ in carbon chains = ↓ in

A

in solubility in water

Chem 102 (6 decks)

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