Review Unit 3
1. Label each part of the wave as crest, trough, wavelength, and amplitude.
2. Give the three main relationships between frequency, wavelength, and energy
As λ ____, F ____
As E ____, F ____
As λ ___, E ___
3. What has a higher energy of emitted energy, n=2 to n=1 or n=3 to n=1
4. What has a higher energy of emitted energy, n=1 to n=4 or n=4 to n=2
c= λf
E = hf
c = 3x108m/s
h = 6.63x10-34 Js
E=(hc)/λ
5. What is the wavelength of a photon which has a frequency of 8.6x1012hz?
6. Determine the energy in red light with a wavelength of 660nm.
Vocabulary
Photon
Quantum
Wave-particle duality
Pauli exclusion Principle
Principal quantum number
Quantum number
Orbital
Sub-level
Angular QN/Subshell QN
Aufbau principle
Ground state electron
configuration
Hund’s Rule
Magnetic QN/Orbital QN
Spin QN
Bohr Model
Quantum Model
Describe the shape of an “S” Describe the shape of an “P” Describe the shape of an
orbital
orbital
“D” orbital
Describe the shape of an “F”
orbital
Use a Periodic Table to answer the following questions.
1. State the four quantum numbers and the possible values they may have.
2. Name the sublevels described by the following quantum numbers
a. n = 2, L = 0
b. n = 3, L = 1
c. n = 6, L = 2
d. n = 5, L = 0
3.
Give the n and L values for the following orbitals
a. 1s
b. 3f
c. 2p
d. 4d
e. 5f
4. Place the following sublevels in order of increasing energy:
1s, 3s, 4s, 6s, 3d, 4f, 3p, 7s, 5d, 5p
5. What and the possible mL values for the following types of orbitals?
a. s
b. p
c. d
d. f
5.
How many possible orbitals are there for n =
a. 6
b. 2
6. How many electrons are in n=
a. 3
b. 17
7. Give the longhand electron configuration for the following elements:
a. Rh
b. Gd
c. P
d. Cs
e. Yb
8. Give the shorthand electron configuration for the following elements:
a. Kr
b. Ca
c. Zn
d. As
e. Ce
Identify the element whose highest energy electron would have the following four quantum numbers:
9. 3, 1, -1, +1/2___________________________________________________
10. 4, 2, +1, +1/2___________________________________________________
11. 6, 1, 0, -1/2____________________________________________________
12. 4, 3, +3, -1/2___________________________________________________
13. 2, 1, +1, -1/2___________________________________________________
Which of the following represents a permissible set of quantum numbers? (answer “yes” if permissible and “no” if
no permissible)
14.
15.
16.
17.
18.
2, 2, +1, -1/2___________________________________________________
5, 1, 0, +1/2____________________________________________________
6, 3,-2, +1/2____________________________________________________
7, 0, 0, -1/2____________________________________________________
4, 1, 8, +1/2____________________________________________________
19. Fill the boxes below with the arrow notation for electrons showing the correct ground state electron configuration for
the element manganese.
Give the four quantum numbers for the following elements
20. Ru
21. H
22. Pd
23. Ho
24. The 15th electron in Pb
25. The 5th electron in oxygen
26. The 45th electron in uranium
How many orbitals are in these sublevels?
L=0
L= 1
L=2
L=3
How many electrons are in the following subshells/orbitals?
4th principle energy level
The px orbital
2nd energy level
The d-1 orbital
What type of orbital do the following indicate?
N= 3 L=0 mL =0
N= 2 L=1 mL =1
N= 1 L=0 mL =0
N= 5 L=3 mL =-2
Review from the Past
1. Convert 103 nm to km
2. Convert 13.43 mL to L
3. Convert 195 cg to µg
4. Draw and label the following atomic models:
Dalton’s Model
Rutherford’s Model
J.J. Thomson’s Model
Bohr’s Model
Quantum Model
5. How many protons, neutrons, and electrons in the following elements?
a. He
b. S
c. Pt
d. Ho
6. Using proper significant figures solve the following problems:
a. A piece of metal has a mass of 25.2g and a density of 13.14 g/mL. What is its volume? (D = m/v)
b. Determine the energy in orange light with a wavelength of 560nm. (E = (hc)/λ)
c. A liquid has a volume of 0.152 L and a density of 2.01 g/mL. What is its mass?