Unit 3 Flashcards
(82 cards)
1
Q
What are INTRAmolecular Forces?
A
Interaction(s) within a single molecule
2
Q
What are INTERmolecular Forces?
A
Interaction(s) between two different molecules
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
4
Q
When are London Dispersion Forces experienced?
A
experienced between ANY/ALL molecules
5
Q
When is Dipole-Dipole experienced?
A
experienced between POLAR molecules ONLY
6
Q
When is dipole-induced-dipole experienced?
A
experienced between POLAR AND NONPOLAR molecules
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
8
Q
When is Ion-dipole IMFs experienced?
A
experienced between an ION AND POLAR molecule
9
Q
How are ionic solids formed?
A
formed by CATION(+) - typically metal - and a nonmetal ANION(-)
10
Q
When are molecular solids formed?
A
formed by distinct individual NEUTRAL molecules (exclusively by NON-METAL ATOMS)
11
Q
When are covelent network solids formed?
A
formed by distinct atoms all bonded together (formed by Carbon AND Semimetals)
12
Q
When are metallic solids formed?
A
formed by metallic elements
13
Q
What do the variables in the equation PV = nRT stand for?
A
(P)ressure (V)olume (n) moles (R) constant (T)emperature
14
Q
What does the IDEAL Gas Law entail?
A
1) No IMFs are present between particles
2) No volume (meaning infinitely compressable)
15
Q
What is (P)ressure? [ideal gas law]
A
The force of gas particles on side of container and vice versa.
16
Q
What is (V)olume?
A
Amount of space the particles occupy
17
Q
What is (T)emperature?
A
Measure of average kinetic energy (of particles)
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
19
Q
What units are used to measue (P)ressure?
most common
A
atm, KPa, mmHg, torr
1 mmHg = 1 torr
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
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
22
Q
What does the partial pressure of an individual gas depend on?
A
number of moles of that gas,
compared to total pressure
23
Q
What does speed(v) depend on?
2 factors
A
- Average Kinetic Energy (T) or (KE)
2. Mass (Molar Mass)
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
25
- Maxwell Boltzmann Distribution w/ T -
| What happens to the curve on the graph as (T) increases?
It flattens out.
26
- Maxwell Boltzmann Distribution w/ T -
| Why does a curve get shorter?
Curve shortens due to the distribution being SPREAD OUT over a wider range.
- at any speed(v), there are FEWER molecules
27
- Deviations from the Ideal Gas Law -
| Real gases _________ as Ideal gases
don't always act
28
- Deviations from the Ideal Gas Law -
| How do real gases DIFFER from ideal gases?
(P)ressures can be lower AND higher than what the ideal gas laws would predict.
29
- Deviations from the Ideal Gas Law -
| The ____ the IMFs, the LESS ideal a gas behaves
stronger
30
- 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?
(P) is lower than the ideal gas law would predict in zone 1.
31
- 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?
(P) is higher than the ideal gas law would predict
32
- Deviations from the Ideal Gas Law -
| A gas is more ideal when IMFs are _____
weaker
33
- Deviations from the Ideal Gas Law -
| How does increasing (T) and decreasing (P) make a gase more ideal?
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
- Deviations from the Ideal Gas Law -
| When are gases most ideal?
At a high (T), but low (P)
35
- Deviations from the Ideal Gas Law -
| When are gases least ideal?
at a low (T) but with high (P)
36
- Deviations from the Ideal Gas Law -
How do IMFs affect (P)?
(relates to zone one)
```
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
- Solutions and Mixtures -
| what is a HOMOgenous mixture?
mixture of TWO OR MORE substances whos properties (microscopic) DO NOT vary (change) throughout the mixtures
38
- Solutions and Mixtures -
| What is a HETEROgenous mixture?
properties CAN be changed depending on location within the mixture.
39
- Solutions and Mixtures -
| What do the variables in the equation n = C x V stand for?
```
n = moles
C = concetration
V = volume
```
40
- Solutions and Mixtures -
| what are the common units for n, C, and V?
```
n = n, Quantity
C = M, molarity
V = L, liters
```
41
- Solutions and Mixtures -
| In a solution, the C is the _____ throughout
same
42
- Solutions and Mixtures -
| What is a solute?
MINOR component of the mixture
43
- Solutions and Mixtures -
| What is a solvent?
MAJOR component of the mixture
44
- Solutions and Mixtures -
| What's the equation for M, Molarity?
```
Molarity, M = moles of solute per liter of solution
AKA: C = n/V
- Variations -
n = C x V
V = n/C
```
45
- Solutions and Mixtures -
| (V) ______ needs to be expressed in liters
ALWAYS
46
- Solutions and Mixtures -
| What do you need to do to dissolve an ionic substance into multiple seperate ions?
1. use the same equation C = n/v
| 2. multiply the subscript of each ion to the (C)
47
- Solutions and Mixtures -
| what is the equation.. C = n1+n2 / V1+V2 used for?
Adding two mixtures containing the SAME SOLUTE
48
- Solutions and Mixtures -
| What steps do you need to take when mixing solutions? (3)
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
- Solutions and Mixtures -
| When you add or subract solvent from an equation, _____ of _____ stay the _____
1. moles
2. solute
3. SAME
50
- Representations of Solutions -
How do you properly drawing a particle view diagram for a solution containing ions?
(dipole)
1. (+) end of H2O's dipole should face (-) ion
| 2. (-) end of H2O's dipole should face (+) ion
51
- Representations of Solutions -
| When three different containers have the same V but different number of particles, what is different?
The C
52
- 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?
Concetration of container A is double of that of B's
53
- Separation of Solutions and Mixtures Chromatography -
| What are the most common separation techniques? (3)
1. Filtration
2. Distillation
3. Chromatography
54
- Separation of Solutions and Mixtures Chromatography -
| When using the filtration technique, the separation is based on _____
solubility (IMF type)
55
- Separation of Solutions and Mixtures Chromatography -
| When using the distillation technique, separation is based on _____ _____
Boiling point (IMF strength)
56
- Separation of Solutions and Mixtures Chromatography -
| When using chromatography, separation is based on _____
Polarity (IMF type)
57
- Separation of Solutions and Mixtures Chromatography -
| What does filtration separate?
HETEROgeneous mixtures or suspensions
| solid substances and the solutes dissolved
58
- Separation of Solutions and Mixtures Chromatography -
| What does distillation separate?
HOMOgeneous mixtures
59
- Separation of Solutions and Mixtures Chromatography -
| What does chromatography separate?
HOMOgeneous mixtures
| based on differences in polarity of the solutes in a solvent
60
- Separation of Solutions and Mixtures Chromatography -
| What are two phases in chromatography?
Stationary and mobile phase
61
- Solubility -
The strength of the _____ between 2 molecules must be ____ ____ the strength of the IMFs/____ lost in each separate substance
IMFs
greater than
bonds
62
- Solubility -
| The more _____ the IMF types, the ____ they dissolve.
similar
| better
63
- Solubility -
| Nonpolar molecules tend to dissolve best in _______ molecules because the two ONLY have London Dispersion forces IMFs
nonpolar
64
- Solubility -
| Polar molecules tend to dissolve best in _____ molecules because they both have LDFs, di-di, and hydrogen bonding IMFs
Polar
65
- Spectroscopy and Electromagnetic Spectrum -
| What type of radiation transitions in electronic energy levels?
Ultraviolet/visible radiation
66
- Spectroscopy and Electromagnetic Spectrum -
| What type of radiation transitions in the molecular vibrational levels?
Infared
67
- Spectroscopy and Electromagnetic Spectrum -
| What type of radiation transitions in the molecular ROTATIONAL levels?
Microwave
68
- 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.
excited
photons
photons
ground
69
- Spectroscopy and Electromagnetic Spectrum -
| Infared radiation makes _____ wiggle
bonds
70
- Spectroscopy and Electromagnetic Spectrum -
| Infared radiation makes _____ wiggle
bonds
71
- Spectroscopy and Electromagnetic Spectrum -
| Microwave radiation makes molecules _____
spin
72
- Spectroscopy and Electromagnetic Spectrum -
EM spec., contains all _____ of EM radiation.
All radiation on the spec., travel at the ____ __ _____.
ranges
| speed of light
73
- Spectroscopy and Electromagnetic Spectrum -
| What are photons?
individual wave/particle of light
74
- Spectroscopy and Electromagnetic Spectrum -
| The energy of a photon depends on what?
Their frequency and wavelength
75
- Photoelectric Effect -
| What two equations are associated with light?
1. E = hv
| 2. c = λv
76
- Photoelectric Effect -
| What variables in the two equations for light are constants?
h (Planck's constant) and c (speed of light)
77
- Photoelectric Effect -
| What do the variables in E = hv stand for?
E - energy
h - Planck's constant ( 6.626 x 10^-34 J s )
v - frequency
78
- Photoelectric Effect -
| What do the variables in c = λv stand for?
c - speed of light ( 2.998 x 10^8 m s^-1 )
λ - wavelength
v - frequency
79
- 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?)
v - frequency
80
- Photoelectric Effect -
| what is Wavelength (λ)?
distance between two same points on a wave
| distance a wave travels in an individual oscillation
81
- Photoelectric Effect -
| what is frequency?
how many oscillations per second OR how often a wave moves up and down.
82
- Photoelectric Effect -
| what is energy?
Amount of energy (J) carried by a single photon
