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From Flashcardlet > AP Chem Ch 6-7 > Flashcards

AP Chem Ch 6-7 Flashcards

0
Q

Ozone

A

O3 is very harmful. 10-50 km above the earth. O2 reacts with a photon to produce O3. Then O3 reacts with O3 to produce O2 and energy, increasing the temperature in the stratosphere

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1
Q

Collecting gas over water

A

Pressure of gas = pressure of room - pressure of water vapor at given temperature
Then use PV=nRT to get moles given volume

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2
Q

Energy

A

The capacity to do work or produce heat

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3
Q

Law of Conservation of energy

A

Energy cannot be created or destroyed. It is transferred. E total is constant in the universe.

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4
Q

Potential energy

A

Due to the position or composition

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5
Q

Kinetic energy

A

Due to motion.

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6
Q

Heat

A

Involves the transfer of energy between two objects due to temperature difference.

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7
Q

Temperature

A

Average KE. property that reflects random motion of particles

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8
Q

Work

A

Force acting over a distance

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9
Q

Change in energy = ?

A

Delta E = W + q

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10
Q

State function

A

Property that is independent of path. Doesn’t matter the order to get there.

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11
Q

Energy/heat/work state function?

A

Energy is a state function. Path independent.
Heat and work are path dependent. The path does matter.
This shows there are different pathways to get to the same value–> Hess law.

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12
Q

Exothermic

A

Generating/ producing heat energy. Delta E is negative. Heat is released.

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13
Q

Endothermic

A

Heat is absorbed. Heat absorbation. Delta E is positive.

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14
Q

Poentitial energy diagram

A

Shows the progression of the rxn vs the PE. if the products below the reactants then delta E is neg and exothermic.
If products above reactants then delta E is positive and enedotheermic.

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15
Q

If a system does work, then work is …

A

NEGATIVE

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16
Q

If work is done on a system, then work is…

A

Positive

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17
Q

Expansion/compression

A

Expansion has volume going up. Gas does work. So work is negative.
Compression has surroundings doing work on the gas so volume goes down. So work is positive

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18
Q

Volume and work relationship

A

W = - pressure * delta V
Volume up, work down.
Volume down, work up

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19
Q

Ex. Calculate delta E of a system undergoing an endothermic process in which 15.6 kJ of heat flows and where 1.4 kJ of work is done on the system

A

Work done on the system is positive.

Delta E = q + W. Add the values

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20
Q

Enthalpy

A

H
= E + PV

Delta H = qp = mc delta T at constant pressure.
Change in enthalpy is equal to the energy flow of heat at constant pressure.

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21
Q

When delta H is positive

A

Endothermic

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22
Q

When delta H is negative

A

Exothermic

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23
Q

Delta H rxn = ?

A

H products - H reactants

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24
Q

Calorimetry

A

Science of measuring heat

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25
Q

Heat capacity

A

Describes heat energy required to increase the temperature by one degree.

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26
Q

Specific heat capacity

A

Heat energy required to increase the temperature of one gram of substance by one degree Celsius.
J/degree c * gram

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27
Q

If the temperature of water goes up, why is delta H negative in a calorimeter problem

A

Temperature goes up in the surroundings so thus heat is released as water absorbs the heat yet it leaves the solution. Delta H is negative

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28
Q

Extensive property

A

Depends on amount of material present. Something involving mass or volume

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29
Q

Intensive property

A

Amount of substance doesn’t affect it. Such as density

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30
Q

What happens in a constant volume situation?

A

No work is done. So the delta energy = qv

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31
Q

Rank these from most positive delta E to most negative delta E
A. Spring is compressed and heated
B. Compress spring expands and is cooled.
C. Spring is compressed and cooled
D. Compressed spring expands and is heated

A

A. Is the most. Volume goes down so work is positive. Heated so q is up. Delta E = q + W so since both positive it is the most positive.
B. Is the least. Volume up so work down. Heat down.
C and D you don’t know bc depends on how much it’s increased by.

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32
Q

Hess’s law

A

Standard heats of formation = sum of the products - sum of the reactants’ heat of formation.

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33
Q

Standard heat of formation at what temperature?

A

25 degrees Celsius

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34
Q

Isoberic

A

Pressure is constant

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35
Q

Isochloric

A

Delta V = 0

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36
Q

Ex. Decomposition of CaCO3 (s) in limestone is used industrially to generate CO2.
CaCO3 (s) –> CaO (s) + CO2 (g)
Heat of formation = 571 kJ
Assume constant external pressure

A 
Delta H = delta E + P delta V
PV= nRT 
P delta V = delta n RT = (1 mol of gas - 0)(8.314)(298) = 2.5 kJ
571 = delta E + 2.5
Delta E = 568. KJ
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37
Q

Electromagnetic Radiation

A

A way for energy to travel through space. The transfer of light energy

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38
Q

Rankings of different rays from highest energy to lowest energy

A 
Gamma rays
X rays
UV rays
Visible light (VIBGYOR)
Infared
Microwaves
Radio waves
39
Q

Relationship between energy, frequency, and wavelength

A

Energy and frequency are proportional
Wavelength and frequency are inversely properitional
Wavelength and energy are inversely proportional

40
Q

What has the lowest wavelength

A

Highest energy

So that would be gamma rays

41
Q

What has the highest wavelength?

A

Lowest energy

Radio waves

42
Q

Relationship between wavelength and frequency

A

c= wavelength * frequency

Where c is the speed of light in a vacuum, 3.0*10^8 m/s

43
Q

Wavelength (lambda)

A

The distance between two identical points on a wave. Easiest to measure from a trough to a trough or a crest to a crest
Measured in meters- visible light in nano meters - 10^-9 m

44
Q

Frequency (f or the Greek v)

A

The number of oxidation per second.

In 1/second, of Hertz

45
Q

Speed of light

A

C, 3.0*10^8 M/s

All light travels at same speed in a vacuum

46
Q

Planck’s constant

A

6.62610^-34 Jsec

47
Q

Energy and frequency relationship

A

E=nhf

Where n is an integer, h is planks constant, and f is frequency

48
Q

What does the energy frequency relationship show us?

A

Energy is not continuous, but it is quantized. Jumps as n increases by an integer amount rather than being able to be any value, it has specific values that it can be

49
Q

Photon

A

A packet of energy

50
Q

Photoelectric effect

A

Phenomenon in which electrons are emitted from a metal surface when light strikes it.

51
Q

What does the photoelectric effect depend on?

A

Frequency and wavelength, NOT intensity. Must be over the threshold energy to eject the electrons.

52
Q

Photoelectric effect key requirements:

A
  1. If frequency is varied, studies show that no electrons are emitted below a specific threshold frequency, f not
  2. Light with frequency lower than the threshold frequency – electrons are not emitted regardless of the intensity
  3. Light with frequency greater than or equal to the threshold frequency emits electrons – as the intensity of light increases, the number of electrons emitted increases as well.
  4. Light with frequency greater than or equal to the threshold frequency– the kinetic energy of the emitted electron increases linearly with the frequency of light.
53
Q

Mass and energy relationship

A

Energy in light = the threshold frequency (ejection) + excess energy
This excess energy is kinetic energy which = hf-hf not

E= m c squared
So we solve for mass, m= E/c^2
Energy = hf and f=c/lambda, so E = hc/lambda
So, mass = h/lamba c

M = h/ (lambda c)
Energy has mass in the relativistic sense (not classically). Thus, energy is a wave and particle

54
Q

What does energy having mass show us

A

Wave and particle

55
Q

De Broglie equation

A

Wavelength = h/mass* velocity
Replace c with velocity in general– allows us to compare wavelengths of electrons with balls. The wavelength of a ball is incredible small

56
Q

What’s de broglie explain

A

All matter can be thought of as both particles and as waves

57
Q

Diffraction

A

Light scattering from a regular array of points or lines. Allows for the separation of electromagnetic radiation

58
Q

Constructive interference

A

When the peaks match the peaks of the waves, reinforces the wave

59
Q

Destructive interference

A

The peak of the wave matches the trough, canceling it out

60
Q

Crystal Latrice

A

Solid state of matter with regular array pattern– hit x rays to generate a diffraction pattern.
This pattern supports electrons moving as waves

61
Q

Atomic emmision spectra

A

Energy added to a system, so electron gets excited, and then it emits a photon– this results in the emission spectrum of the hydrogen atom with lines for specific wavelengths but not all values, thus it is quantized.

62
Q

What happens when Hydrogen goes to the excited state?

A

Energy is added to the system, making the Hydrogen excited. Then goes back to the ground state, emitting or releasing the same amount of energy that was originally abosrobed. This happens when the energy of the final state - energy of initial state is negative.
Goes from excited to the ground state
When from ground to excited, it absorbs the photon of

63
Q

Transitions in energy levels that are visible

A

All ending at n=2–> n=6–>n=2…

64
Q

Bohr model

A

Change in energy = -2.178 *10^-18 J ((1/n2 ^2) - (1/n1 ^2))
Only works for hydrogen because one electron
N is the energy level
Predicted circular model

65
Q

Standing wave

A

Has fixed ends –> n has to be an integer to have standing waves, which is important so that the wave can come around and get back to where it was without distructive interference causing the wave to get cancelled out.

66
Q

Wave function equation

A 
H hat (triton) = E (triton)
H hat is an operator-- set of allowed mathematical instructions
E is total energy of the system, PE+ KE
triton is the wave function-- basically the orbital, where the electron is
Triton squared is the probability of finding an electron near a particular point in space.
67
Q

Wave function squared probability example

A

Say we have two positions in space–> (x1,y1,z1) and (x2,y2,z2)
Relative probability of finding the electron at positions 1 and 2 is given by substituting the values of x, y, and z for the two positions into the wave function, squaring the function value, and computing the following ratio:
(Triton (X1,y1,z1))^2 / (triton (x2,y2,z2))^2 = N1/N2
N1/N2 is the ratio of probabilities of finding the electron at positions 1 and 2. If the ratio were 100, then the electron is 100 times more likely to be found at position 1 than position 2

68
Q

Electron density and electron probability relationship

A

They’re the same!

This explains what the orbitals look like

69
Q

What happens to the electron probability as the distance from nucleus increases?

A

1/x format. Probability goes down as distance increasss

70
Q

Node

A

When wave crosses the origin. Electrons can’t be there

N=3, 2 nodes. Has n-1 nodes.

71
Q

Cut off atomic radius significance

A

Cut off atomic radius at 90%–> size of an orbital is arbitrarily defined as the surface that contains 90% of the total electron probability

72
Q

Quantum numbers

A

4 QN’s that explain where we can find the electron

73
Q

4 QN’s

A
  1. Principle QN (n)
  2. Angular momentum QN (l)
  3. Magnetic QN (ml)
  4. Spin QN (Ms)
74
Q

Principle QN (n)

A

The energy level. Integer (1,2,3…)

Increases further from nucleus

75
Q

Angular momentum QN (l)

A 
From 0--> n-1
If n = 1, then L=0
If n= 3, then L = 0,1,2
0 = s
1=p
2=d
3=f
4=g
76
Q

Magnetic QN (ml)

A

Ranges from -L to positive L

If l is 1, then -1,0,1

77
Q

Spin QN (Ms)

A

Positive or negative 1/2

78
Q

Pauli exclusion principle

A

No 2 electrons can be in the same spot in the same system

79
Q

S orbital shape and reason

A

In the S orbital, there is only one posibility for ml, 0, and Ms can be +/- 1/2. So in a sphere shape. Two electrons in the sphere.

80
Q

P orbital shape and reason

A

P orbital is a dumbbell. 3 different possibilities with 2 electrons in each since ml can be -1,0,1

81
Q

Phosphorus electron config

A 
1 s2 
2 s2
2 p6
3 s2
3 p3 
Or [Ne] 3s 2 3p 3
82
Q

Valence electrons

A

All the electrons not in the noble gas config.

83
Q

Photoelectron spectoscopy

A

Ability to measure the KE of an electron in the photoelectric effect and thus measure the ionization energy.

84
Q

Photoelectron spec big equation

A

KEphoton = KE electron + IE

85
Q

Ionization energy

A

Energy required to remove an electron
Energy associated with the reaction:
Metal–> M+ + e-

86
Q

Ionization energy

A

Energy required to remove an electron
Energy associated with the reaction:
Metal–> M+ + e-

87
Q

Ionization energy graph

A

More ionization energy to remove energy levels closer to the nucleus. Relative number of electrons vs ionization energy

88
Q

Ionization energy graph

A

More ionization energy to remove energy levels closer to the nucleus. Relative number of electrons vs ionization energy

89
Q

What can ionization energy diagrams tell us

A

Explains what atom it is based on electron relative height in the last column to the right.
Also tells us how to understand the electron structure of elements and the energy levels. 1s on bottom because most energy is required to remove a 1s electron

90
Q

What can ionization energy diagrams tell us

A

Explains what atom it is based on electron relative height in the last column to the right.
Also tells us how to understand the electron structure of elements and the energy levels. 1s on bottom because most energy is required to remove a 1s electron

91
Q

Aufbau principle

A

Fill lowest energy orbital first

92
Q

Aufbau principle

A

Fill lowest energy orbital first

93
Q

Hund’s rule

A

First fill the electrons unpaired and then pair them

94
Q

Hund’s rule

A

First fill the electrons unpaired and then pair them

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