FINAL - SECTION 1

Question 1

zA Z P

Answer 1

A = atomic mass
Z = atomic symbol
P = number of protons

Question 2

Frequency (v)

Answer 2

Number of cycles per second (s-1)

Question 3

Wavelength (λ)

Answer 3

Distance wave travels in 1 cycle (nm)

Question 4

Amplitude

Answer 4

Height of crest of wave

Question 5

Relationship between frequency and wavelength

Answer 5

Inversely proportional (small freq = big wavelength, big freq = small wavelength)

Question 6

Rank electromagnetic spectrum from lowest energy (big wavelength) to high energy (small wavelength)

Answer 6

1. Radio (10^5-10^-1)
2. Microwave (10^-1-10^-3)
3. Infrared (10^-3-10^-6)
4. Visible light (10^-6-10^-7)
5. UV (10^-7-10^-9)
6. X ray (10^-9-10^-11)
7. Gamma ray (10^-11-10^-15)

Question 7

Which ER has longest wavelength (small freq)

Answer 7

Radio

Question 8

Which ER has smallest wavelength (largest freq)

Answer 8

Gamma ray

Question 9

Rank visible light from low energy (big wavelength) to high energy (small frequency)

Answer 9

• Red
• Orange
• Yellow
• Green
  -Blue
• Violet

Question 10

Relationship between visible light and color

Answer 10

Amplitude determines brightness, frequency/wavelength determines color

Question 11

Important equations (5)

Answer 11

• c = λv
• λ = c/v
• v = c/λ
• E = hc/λ
• λ = hc/Ephoton

Question 12

Conversion of nm to m

Answer 12

nm x 1m/10^9nm

Question 13

Conversion of m to nm

Answer 13

m x 10^9nm/1m

Question 14

KE

Answer 14

Ephoton - Binding energy

Question 15

Energy of electron

Answer 15

En = -2.179x10^-18 J (z^2/n^2)
Z is atomic number
n is orbital

Question 16

Excitation

Answer 16

Energy is absorbed and electron gain enough energy to move to higher orbital

Question 17

Relaxation

Answer 17

Energy emitted (released) and electron moves to lower orbital

Question 18

Ground state

Answer 18

n=1 (lowest level)

Question 19

Excited state

Answer 19

n >= 2 (higher level)

Question 20

Difference in energy level

Answer 20

• Used then question is asking when n=5 goes to n=3
  (-2.179x10^-18 J)(z^2/n^2f-z^2/n^2i)

Question 21

DeBroglie equation

Answer 21

• λ = h/mv (velocity)
• Finds wavelength from mass of electron and velocity, so end unit should be m/nm

Question 22

Heisenberg uncertainty principle

Answer 22

States that we do not know the speed and position of particles with exact accuracy

Question 23

3 types of quantum numbers

Answer 23

• Describe orbitals in terms of their property
• Principal quantum number (n)
• Angular momentum quantum number (l)
• Magnetic quantum number (ml)

Question 24

Principle quantum number (n)

Answer 24

• Size and orbital energy
• n is integer
• Larger n = larger orbital (far from nucleus)

Question 25

Angular momentum number (l)

Answer 25

- Orbital shape - Dependant on n, is every shape from 0 to n-1

Question 26

Relationship of l with orbital subshell

Answer 26

- l = 0: s - l = 1: p - l = 2: d - l = 3: f - l = 4: d

Question 27

Magnetic quantum number (ml)

Answer 27

- Orientation of orbital - Integer from -l to 0 to +1 (DO EVERY l) - Number of ml = number of orbitals

Question 28

s orbital

Answer 28

Spherical in shape, as n increases the size of s orbital increase

Question 29

Spherical node

Answer 29

Round nodes found on 2s orbitals and up

Question 30

Angular (planar) node

Answer 30

Nodes at nucleus of p orbitals and up

Question 31

Node

Answer 31

Areas of 0 electron density (n-1)

Question 32

p orbital

Answer 32

First occur in n=2, there is 3 with different orientations

Question 33

d orbital

Answer 33

First occur in n=3, there is 5 with different orientations

Question 34

Draw the orbitals

Answer 34

Ok

Question 35

Spin orientation quantum number (ms)

Answer 35

If electron configuration has arrow UP = +1/2, if arrow down = -1/2

Question 36

3 rules for electron configuration

Answer 36

- Aufbau principle - Pauli exclusion principle - Hunds rule

Question 37

Aufbau principle

Answer 37

Electrons occupy lower energy orbitals first before going higher

Question 38

Pauli exclusion principle

Answer 38

2 electrons in orbitals must have different spins

Question 39

Hunds rule

Answer 39

Electrons will fill singly before pairing

Question 40

Periodic table blocks

Answer 40

- s block: alkali earth + alkali metal - p block: basic metal + metalloid + nonmetal + halogen + noble gas - d block: transition metal - f block: lanthanoid + actinide

Question 41

Diamagnetic atom

Answer 41

All paired electrons

Question 42

Paramagnetic atom

Answer 42

Unpaired electrons