Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

AP Chemistry > Unit 3 > Flashcards

Unit 3 Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What are INTRAmolecular Forces?

A

Interaction(s) within a single molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are INTERmolecular Forces?

A

Interaction(s) between two different molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are the types of IMFs? (there’s 5)

A 
London Disperson Forces (LDFs)
Dipole-Dipole
Dipole-induced-Dipole
Hydrogen Bonding
Ion-Dipole
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

When are London Dispersion Forces experienced?

A

experienced between ANY/ALL molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

When is Dipole-Dipole experienced?

A

experienced between POLAR molecules ONLY

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

When is dipole-induced-dipole experienced?

A

experienced between POLAR AND NONPOLAR molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

When is Hydrogen Bonding experienced?

A

experienced when ONE OF TWO molecules have an (H)ydrogen atom bonded to a F,O,N atom.
(F)luorine
(O)xygen
(N)itrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

When is Ion-dipole IMFs experienced?

A

experienced between an ION AND POLAR molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How are ionic solids formed?

A

formed by CATION(+) - typically metal - and a nonmetal ANION(-)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

When are molecular solids formed?

A

formed by distinct individual NEUTRAL molecules (exclusively by NON-METAL ATOMS)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

When are covelent network solids formed?

A

formed by distinct atoms all bonded together (formed by Carbon AND Semimetals)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

When are metallic solids formed?

A

formed by metallic elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What do the variables in the equation PV = nRT stand for?

A 
(P)ressure
(V)olume
(n) moles
(R) constant
(T)emperature
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What does the IDEAL Gas Law entail?

A

1) No IMFs are present between particles

2) No volume (meaning infinitely compressable)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q 
What is (P)ressure?
[ideal gas law]
A

The force of gas particles on side of container and vice versa.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is (V)olume?

A

Amount of space the particles occupy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is (T)emperature?

A

Measure of average kinetic energy (of particles)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What do you do to convert Celcius to Kelvin? and vice versa?

A

C to K = add 273.15

K to C = subtract 273.15

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What units are used to measue (P)ressure?

most common

A

atm, KPa, mmHg, torr

1 mmHg = 1 torr

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

How do you convert mmHg to atm? and vice versa?

A

mmHg to atm = divide by 760

atm to mmHg = multiply by 760

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

(P)ressure on the walls of a container of mixed gases is the SUM of what?

A

partial pressures of the gases

had they been in seperate containers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What does the partial pressure of an individual gas depend on?

A

number of moles of that gas,

compared to total pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What does speed(v) depend on?

2 factors

A
  1. Average Kinetic Energy (T) or (KE)

2. Mass (Molar Mass)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q
  • Maxwell Boltzmann Distribution w/ T -

What happens to the graph of a particle when the particles get HEAVIER?

A

The curve gets squished/skinner and taller

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q
  • Maxwell Boltzmann Distribution w/ T -

What happens to the curve on the graph as (T) increases?

A

It flattens out.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q
  • Maxwell Boltzmann Distribution w/ T -

Why does a curve get shorter?

A

Curve shortens due to the distribution being SPREAD OUT over a wider range.
- at any speed(v), there are FEWER molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q
  • Deviations from the Ideal Gas Law -

Real gases _________ as Ideal gases

A

don’t always act

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q
  • Deviations from the Ideal Gas Law -

How do real gases DIFFER from ideal gases?

A

(P)ressures can be lower AND higher than what the ideal gas laws would predict.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q
  • Deviations from the Ideal Gas Law -

The ____ the IMFs, the LESS ideal a gas behaves

A

stronger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q
  • Deviations from the Ideal Gas Law -

How does the (P) in zone one on the graph (below 1.0) differ from the ideal gas law?

A

(P) is lower than the ideal gas law would predict in zone 1.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q
  • Deviations from the Ideal Gas Law -

How does the (P) in zone two on the graph (above 1.0) differ from the ideal gas law?

A

(P) is higher than the ideal gas law would predict

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q
  • Deviations from the Ideal Gas Law -

A gas is more ideal when IMFs are _____

A

weaker

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q
  • Deviations from the Ideal Gas Law -

How does increasing (T) and decreasing (P) make a gase more ideal?

A
  1. Increase in (T) makes the gases move faster past each other
  2. Decrease in (P) allows the gases to move and stay far apart
    THUS…. making IMFs weaker, resulting in a more ideal gas.
34
Q
  • Deviations from the Ideal Gas Law -

When are gases most ideal?

A

At a high (T), but low (P)

35
Q
  • Deviations from the Ideal Gas Law -

When are gases least ideal?

A

at a low (T) but with high (P)

36
Q
  • Deviations from the Ideal Gas Law -
    How do IMFs affect (P)?
    (relates to zone one)
A 
IMFs cause (P) to be LOWER than expected b/c molecules are attracted towards each other.....
resulting in less force of the collisions on the container
37
Q
  • Solutions and Mixtures -

what is a HOMOgenous mixture?

A

mixture of TWO OR MORE substances whos properties (microscopic) DO NOT vary (change) throughout the mixtures

38
Q
  • Solutions and Mixtures -

What is a HETEROgenous mixture?

A

properties CAN be changed depending on location within the mixture.

39
Q
  • Solutions and Mixtures -

What do the variables in the equation n = C x V stand for?

A 
n = moles
C = concetration
V = volume
40
Q
  • Solutions and Mixtures -

what are the common units for n, C, and V?

A 
n = n, Quantity
C = M, molarity
V = L, liters
41
Q
  • Solutions and Mixtures -

In a solution, the C is the _____ throughout

A

same

42
Q
  • Solutions and Mixtures -

What is a solute?

A

MINOR component of the mixture

43
Q
  • Solutions and Mixtures -

What is a solvent?

A

MAJOR component of the mixture

44
Q
  • Solutions and Mixtures -

What’s the equation for M, Molarity?

A 
Molarity, M = moles of solute per liter of solution
AKA: C = n/V
- Variations -
n = C x V
V = n/C
45
Q
  • Solutions and Mixtures -

(V) ______ needs to be expressed in liters

A

ALWAYS

46
Q
  • Solutions and Mixtures -

What do you need to do to dissolve an ionic substance into multiple seperate ions?

A
  1. use the same equation C = n/v

2. multiply the subscript of each ion to the (C)

47
Q
  • Solutions and Mixtures -

what is the equation.. C = n1+n2 / V1+V2 used for?

A

Adding two mixtures containing the SAME SOLUTE

48
Q
  • Solutions and Mixtures -

What steps do you need to take when mixing solutions? (3)

A
  1. Find moles present in each solution, then add them together
  2. Add volumes of both solutions
  3. Divide sum of 2 mol by the new volume
  • when adding or subtracting solvent from an equation, moles of solute stay the same.
49
Q
  • Solutions and Mixtures -

When you add or subract solvent from an equation, _____ of _____ stay the _____

A
  1. moles
  2. solute
  3. SAME
50
Q
  • Representations of Solutions -
    How do you properly drawing a particle view diagram for a solution containing ions?
    (dipole)
A
  1. (+) end of H2O’s dipole should face (-) ion

2. (-) end of H2O’s dipole should face (+) ion

51
Q
  • Representations of Solutions -

When three different containers have the same V but different number of particles, what is different?

A

The C

52
Q
  • Representations of Solutions -
    If container A and B contain the same number of particles, but A has 2x the Volume, how does the concetration of the two compare?
A

Concetration of container A is double of that of B’s

53
Q
  • Separation of Solutions and Mixtures Chromatography -

What are the most common separation techniques? (3)

A
  1. Filtration
  2. Distillation
  3. Chromatography
54
Q
  • Separation of Solutions and Mixtures Chromatography -

When using the filtration technique, the separation is based on _____

A

solubility (IMF type)

55
Q
  • Separation of Solutions and Mixtures Chromatography -

When using the distillation technique, separation is based on _____ _____

A

Boiling point (IMF strength)

56
Q
  • Separation of Solutions and Mixtures Chromatography -

When using chromatography, separation is based on _____

A

Polarity (IMF type)

57
Q
  • Separation of Solutions and Mixtures Chromatography -

What does filtration separate?

A

HETEROgeneous mixtures or suspensions

solid substances and the solutes dissolved

58
Q
  • Separation of Solutions and Mixtures Chromatography -

What does distillation separate?

A

HOMOgeneous mixtures

59
Q
  • Separation of Solutions and Mixtures Chromatography -

What does chromatography separate?

A

HOMOgeneous mixtures

based on differences in polarity of the solutes in a solvent

60
Q
  • Separation of Solutions and Mixtures Chromatography -

What are two phases in chromatography?

A

Stationary and mobile phase

61
Q
  • Solubility -
    The strength of the _____ between 2 molecules must be ____ ____ the strength of the IMFs/____ lost in each separate substance
A

IMFs
greater than
bonds

62
Q
  • Solubility -

The more _____ the IMF types, the ____ they dissolve.

A

similar

better

63
Q
  • Solubility -

Nonpolar molecules tend to dissolve best in _______ molecules because the two ONLY have London Dispersion forces IMFs

A

nonpolar

64
Q
  • Solubility -

Polar molecules tend to dissolve best in _____ molecules because they both have LDFs, di-di, and hydrogen bonding IMFs

A

Polar

65
Q
  • Spectroscopy and Electromagnetic Spectrum -

What type of radiation transitions in electronic energy levels?

A

Ultraviolet/visible radiation

66
Q
  • Spectroscopy and Electromagnetic Spectrum -

What type of radiation transitions in the molecular vibrational levels?

A

Infared

67
Q
  • Spectroscopy and Electromagnetic Spectrum -

What type of radiation transitions in the molecular ROTATIONAL levels?

A

Microwave

68
Q
  • Spectroscopy and Electromagnetic Spectrum -
    With ultraviolet radiation, e- can get ____ as they absorb ____ and they’ll emit _____ in that region when they go back to _____ state.
A

excited
photons
photons
ground

69
Q
  • Spectroscopy and Electromagnetic Spectrum -

Infared radiation makes _____ wiggle

A

bonds

70
Q
  • Spectroscopy and Electromagnetic Spectrum -

Infared radiation makes _____ wiggle

A

bonds

71
Q
  • Spectroscopy and Electromagnetic Spectrum -

Microwave radiation makes molecules _____

A

spin

72
Q
  • Spectroscopy and Electromagnetic Spectrum -
    EM spec., contains all _____ of EM radiation.
    All radiation on the spec., travel at the ____ __ _____.
A

ranges

speed of light

73
Q
  • Spectroscopy and Electromagnetic Spectrum -

What are photons?

A

individual wave/particle of light

74
Q
  • Spectroscopy and Electromagnetic Spectrum -

The energy of a photon depends on what?

A

Their frequency and wavelength

75
Q
  • Photoelectric Effect -

What two equations are associated with light?

A
  1. E = hv

2. c = λv

76
Q
  • Photoelectric Effect -

What variables in the two equations for light are constants?

A

h (Planck’s constant) and c (speed of light)

77
Q
  • Photoelectric Effect -

What do the variables in E = hv stand for?

A

E - energy
h - Planck’s constant ( 6.626 x 10^-34 J s )
v - frequency

78
Q
  • Photoelectric Effect -

What do the variables in c = λv stand for?

A

c - speed of light ( 2.998 x 10^8 m s^-1 )
λ - wavelength
v - frequency

79
Q
  • Photoelectric Effect -
    In the two equations for light, what variable can be used in one equation to find the information from the other equation?
    (if given c and λ, what can you use to find E?)
A

v - frequency

80
Q
  • Photoelectric Effect -

what is Wavelength (λ)?

A

distance between two same points on a wave

distance a wave travels in an individual oscillation

81
Q
  • Photoelectric Effect -

what is frequency?

A

how many oscillations per second OR how often a wave moves up and down.

82
Q
  • Photoelectric Effect -

what is energy?

A

Amount of energy (J) carried by a single photon

AP Chemistry (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions