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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
Diffusion and Effusion
gas particles mixing together faster particles faster diffusion or effusion
26
How to solve for MM?
MM=DRT/P
27
Units on density for gases?
g/L
28
Solve for density?
D=MM(P)/RT
29
How do moles define the state of a gas? Temp? Volume? Pressure?
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
30
Boyles Law
P1V1=P2V2 pressure and volume are inversely proportional
31
Charles Law
V1/T1=V2/T2 Volume and temp are directly proportional
32
Gay- Lussacs Law
P1/T1=P2/T2 Pressure and temp are directly proportional
33
Combined gas law
P1V1/T1=P2V2/T2 Predicts changes if the amount of gas is constant
34
What happens when water vapor is present?
Water vapor must be subtracted from the total pressure
35
Real Gas
will become less ideal when the gas particles become closer together
36
When will a ideal gas deviate?
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
When stronger IMF's gas...
deviates from its ideal behavior IMF's (up) pressure (down)
38
When decreasing temp gas...
deviates from its ideal behavior temp(down) pressure (down)
39
What happens if the temp decreases too much?
The gas will begin to turn into a liquid
40
As pressure goes up volume...
goes up
41
Changing from a solid to a liquid
Fusion, weakens IMF's, endothermic
42
Changing from a liquid to a gas
vaporizatrion, weakens IMF's, endothermic
43
Changing from liquid to solid
solidfication/freezing, strengthens IMF's, exothermic
44
Changing from gas to liquid
condensation, strengthens IMF's, exothermic
45
Whenever to oppositely charged particles move closer together they must be _____ energy
losing favorable
46
Boiling point is when
The weaker the IMF's the the lower temp needed vapor pressure = atmospheric pressure
47
Surface tension
the attractions on the surface of a liquid Stronger IMF's = stronger tension
48
Viscosity
the stickiness of a liquid due to liquid particles moving past eachother Weaker IMF's = more flowy
49
Vapor pressure
the amount of liquid turning into a gas
50
Adhesion
molecules attracted to the surface
51
Cohesion
molecules attracted to each other
52
endothermic phase changes...
melting, evaporation, sublimation
53
exothermic phase changes...
freezing, condensation, deposition
54
Fusion/melting
changing from solid to liquid weakens IMF's endothermic
55
vaporization/evaporation
changing from liquid to gas weakens IMF's endothermic
56
solidification/ freezing
changing from liquid to solid Strengthens IMF's exothermic
57
Condensation
Changing from gas to liquid Strengthens IMF's exothermic
58
why does liquid to solid require more energy?
Because it is a larger change in IMF's becuase solids have a stronger force of attration
59
when vapor pressure = atmospheric pressure
its a boiling point
60
Solids
low kinetic energy definite shape Stronger IMF's
61
Liquids
mid kinetic energy flowy Strongish IMF's
62
Gases
High kinetic energy fly around Little to no IMF's
63
Rf
distance traveled / distance traveled of solvent
64
seperating solutions
gravimeter analysis- filter reactions form perciptates solubility distillation
65
Distillation
purifying liquid then cooling weakest IMF distillates first
66
chromatography
identifies the substance present
67
chromatography layer
polar will move with polar, non-polar will move with non-polar
68
polar substances often mix with
polar solutes due to similar dipole-dipole attractions
69
ion-dipole
the stronger the ion charge, the stronger the ion-dipole interaction
70
if ionic compound is soluble (Ksp>1) the ion-dipole forces are greater than
the ion-ion attraction and dipole-dipole attractition = solubility
71
An ionic compound is a precipitate
the ion-ion attraction is much stronger than the ion-dipole attraction
72
if a nonpolar solvent mixes with ionic compounds
the ion-ion attraction is stronger than the ion therefore, will not mix
73
if nonpolar tries to mix with polar
the dipole-dipole attraction in the polar substance is stronger than the dipole induced dipole attraction, will not mix
74
ionic compounds not dissolve in water
the ion-ion attraction is stronger than the ion-dipole attraction between the solute and solvent
75
Ionic bonds
high meltiong point, particles called ions, greater charge stronger bond
76
covalent network
Diamond, graphite, SiO2, SiC, high melting point, particles called atoms
77
molecular
bonded by IMF;s, low melting point, called molecules
78
metallic
range of metling point, called atoms

AP Chem (9 decks)

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