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AP Chem > Unit 3 > Flashcards

Unit 3 Flashcards

1
Q

INTRAmolecular forces

A

are within a molecule
when broken or formed it is a chemical change

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2
Q

INTERmolecular forces

A

are between molecules
when weakened or strengthened there is a physical change

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3
Q

Are intramolecular forces or intermolecular forces stronger?

A

Intramolecular have a stronger attraction

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4
Q

LDF’s

A

come from the atom having a polarized electron cloud, which the electrons naturally shift to one side of the electron cloud

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5
Q

what has LDF?

A

all atoms/molecules have a LDF expect H+

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6
Q

Molar mass equals….

A

amount of electrons

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7
Q

More plorizable..

A

more electrons
stronger LDF
greater dipole-dipole

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8
Q

LDF’s create weak attractions between atoms called

A

temporary dipole
also an IMF

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9
Q

what happens to the molecule when surface area increases?

A

the polarity increases
greater temporary dipole

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10
Q

dipole-dipole attractions

A

already polar molecules are held by a temporary dipole

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11
Q

The higher the boiling point the ___ the IMF

A

stronger

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12
Q

Hydrogen bonding must have

A
  1. a hydrogen atom bonded DIRECTLY to N,O, or F
  2. a lone pair on another N,O, or F that is able to connect with hydrogen
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13
Q

When only CH compounds are present the compound is….

A

non-polar

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14
Q

How to find total pressure

A

add all total pressures

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15
Q

Ideal gas law

A

PV=nRT

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16
Q

If you have constant temperature and constant volume then pressure is..

A

constant

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17
Q

pressure and temperature are _____ related

A

directly

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18
Q

As volume increases, pressure ______
As volume decreases, pressure _______

A

decreases
increases

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19
Q

volume and temperature are _____ related

A

directly

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20
Q

Finding partial pressure given pressure total and % of elements

A

multiply the Ptot by %

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21
Q

When an elements pressure is reduced by a %

A

Multiply by that % then subtract

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22
Q

5 assumptions on kinetic molecular theory (ideal gases)

A
  1. Gas particle move in constant and random motion
  2. The volume of gas particles is negligible
  3. The average kinetic energy of the particles is proportional to the K temp
  4. All collisions between gas particles are perfectly elastic
  5. Gas particles have little to no attractive/repulsion between the particles
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23
Q

How is the speed of gas particles and temperature related?

A

They are directly related
Higher temp, faster particle

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24
Q

How is the speed of gas particles and mass related?

A

Inversely related
More mass, slower particle

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25
Q

Diffusion and Effusion

A

gas particles mixing together
faster particles faster diffusion or effusion

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26
Q

How to solve for MM?

A

MM=DRT/P

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27
Q

Units on density for gases?

A

g/L

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28
Q

Solve for density?

A

D=MM(P)/RT

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29
Q

How do moles define the state of a gas? Temp? Volume? Pressure?

A

Moles= the amount of gas
Temp= the average speed of a gas
Volume= the space a gas is able to move around
Pressure= how many collisions of particles

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30
Q

Boyles Law

A

P1V1=P2V2
pressure and volume are inversely proportional

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31
Q

Charles Law

A

V1/T1=V2/T2
Volume and temp are directly proportional

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32
Q

Gay- Lussacs Law

A

P1/T1=P2/T2
Pressure and temp are directly proportional

33
Q

Combined gas law

A

P1V1/T1=P2V2/T2
Predicts changes if the amount of gas is constant

34
Q

What happens when water vapor is present?

A

Water vapor must be subtracted from the total pressure

35
Q

Real Gas

A

will become less ideal when the gas particles become closer together

36
Q

When will a ideal gas deviate?

A

If there is a pressure increase (more collisions)
If there is a temp decrease (Particles move slower)
If stronger IMF’s (particles have stronger attraction)

37
Q

When stronger IMF’s gas…

A

deviates from its ideal behavior
IMF’s (up) pressure (down)

38
Q

When decreasing temp gas…

A

deviates from its ideal behavior
temp(down) pressure (down)

39
Q

What happens if the temp decreases too much?

A

The gas will begin to turn into a liquid

40
Q

As pressure goes up volume…

A

goes up

41
Q

Changing from a solid to a liquid

A

Fusion, weakens IMF’s, endothermic

42
Q

Changing from a liquid to a gas

A

vaporizatrion, weakens IMF’s, endothermic

43
Q

Changing from liquid to solid

A

solidfication/freezing, strengthens IMF’s, exothermic

44
Q

Changing from gas to liquid

A

condensation, strengthens IMF’s, exothermic

45
Q

Whenever to oppositely charged particles move closer together they must be _____ energy

A

losing
favorable

46
Q

Boiling point is when

A

The weaker the IMF’s the the lower temp needed
vapor pressure = atmospheric pressure

47
Q

Surface tension

A

the attractions on the surface of a liquid
Stronger IMF’s = stronger tension

48
Q

Viscosity

A

the stickiness of a liquid due to liquid particles moving past eachother
Weaker IMF’s = more flowy

49
Q

Vapor pressure

A

the amount of liquid turning into a gas

50
Q

Adhesion

A

molecules attracted to the surface

51
Q

Cohesion

A

molecules attracted to each other

52
Q

endothermic phase changes…

A

melting, evaporation, sublimation

53
Q

exothermic phase changes…

A

freezing, condensation, deposition

54
Q

Fusion/melting

A

changing from solid to liquid
weakens IMF’s
endothermic

55
Q

vaporization/evaporation

A

changing from liquid to gas
weakens IMF’s
endothermic

56
Q

solidification/ freezing

A

changing from liquid to solid
Strengthens IMF’s
exothermic

57
Q

Condensation

A

Changing from gas to liquid
Strengthens IMF’s
exothermic

58
Q

why does liquid to solid require more energy?

A

Because it is a larger change in IMF’s becuase solids have a stronger force of attration

59
Q

when vapor pressure = atmospheric pressure

A

its a boiling point

60
Q

Solids

A

low kinetic energy
definite shape
Stronger IMF’s

61
Q

Liquids

A

mid kinetic energy
flowy
Strongish IMF’s

62
Q

Gases

A

High kinetic energy
fly around
Little to no IMF’s

63
Q

Rf

A

distance traveled / distance traveled of solvent

64
Q

seperating solutions

A

gravimeter analysis- filter
reactions form perciptates
solubility
distillation

65
Q

Distillation

A

purifying liquid then cooling
weakest IMF distillates first

66
Q

chromatography

A

identifies the substance present

67
Q

chromatography layer

A

polar will move with polar, non-polar will move with non-polar

68
Q

polar substances often mix with

A

polar solutes due to similar dipole-dipole attractions

69
Q

ion-dipole

A

the stronger the ion charge, the stronger the ion-dipole interaction

70
Q

if ionic compound is soluble (Ksp>1) the ion-dipole forces are greater than

A

the ion-ion attraction and dipole-dipole attractition = solubility

71
Q

An ionic compound is a precipitate

A

the ion-ion attraction is much stronger than the ion-dipole attraction

72
Q

if a nonpolar solvent mixes with ionic compounds

A

the ion-ion attraction is stronger than the ion
therefore, will not mix

73
Q

if nonpolar tries to mix with polar

A

the dipole-dipole attraction in the polar substance is stronger than the dipole induced dipole attraction, will not mix

74
Q

ionic compounds not dissolve in water

A

the ion-ion attraction is stronger than the ion-dipole attraction between the solute and solvent

75
Q

Ionic bonds

A

high meltiong point, particles called ions, greater charge stronger bond

76
Q

covalent network

A

Diamond, graphite, SiO2, SiC, high melting point, particles called atoms

77
Q

molecular

A

bonded by IMF;s, low melting point, called molecules

78
Q

metallic

A

range of metling point, called atoms

AP Chem (9 decks)

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