1. No category

Unit 4 Sample Questions
I.
II.
III.
IV.
V.
Light & Energy
a. Double Slit Experiment
Given:
b. Wave-Particle Duality
c =  & E = h
c. Properties of Waves (V = )
c = 2.998x108 m/s
d. Parts of a wave (see diagram below)
h = 6.626x10-34 Js
e. c = 
1 nm = 1x10-9 m
f. Electromagnetic (Light) Spectrum
1 cal = 4.184 J
g. E = h
1 Cal = 1,000 cal
h. Emission & Absorption Spectra
Foundations of Quantum Mechanics
a. Quantization of the Universe
1s
b. Ground State / Excited State
2s 2p
c. Quantum Numbers & Permitted values
3s 3p 3d
d. Light Emission mechanism
4s 4p 4d 4f
e. Orbital Shapes
5s 5p 5d 5f 5g
f. Orbitals/Nodes/Anti-Nodes
6s 6p 6d 6f 6g 6h
g. Pauli’s Exclusion Principle
7s 7p 7d 7f 7g 7h 7i
Quantum Mechanics
a. Aufbau Principle
b. Hund’s Rule
c. Orbital filling rules
d. Electron Configurations
e. Electron Box Diagrams – Paired/Unpaired electrons
f. Heisenberg’s Uncertainty Principle
g. Schrödinger’s Wave Equation (probabilistic nature of the universe)
h. Copenhagen Interpretation
Hydrogen Spectrum Lab
a. Interpreting Light Emission Diagrams
b. Calculating Energies of Transitions
Flame Test Lab
a. Identification techniques
b. Colors produced by copper (Cu+2), lithium (Li+1), potassium (K+1), and sodium (Na+1)
1. Label each part of the wave.
A
B
D
C
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2. What is the frequency of blue light with a wavelength of 450 nm?
3. What is the wavelength (in nm) of radiation with a frequency of 6.87x1014 Hz?
4. Which has more energy, infrared or ultraviolet light? Prove it using the following data:
IR = 1.96x1014 Hz & UV = 9.37x1014 Hz
5. Which photon of light has more energy, red (λ = 679 nm) or yellow (λ = 587 nm)? Prove it.
6. What is the wavelength (in nm) of a photon with 3.26x10-18 J of energy?
7. What is the energy of a photon of green light with a wavelength of 540 nm?
8. How much energy is required to emit 4.73x1012 photons of light with a wavelength of 467 nm?
9. How many photons with a wavelength of 1060 nm can be produced with 16.75 Cal of energy?
10. What wavelength of light would be emitted by an electron jumping from n=6 to n=4 given the following data:
λ62 = 293.9 nm
λ42 = 847.3 nm
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11. Which travels faster in a vacuum: x-rays or radio waves? Why?
12. Explain what happens to frequency as the wavelength gets longer and longer.
13. Explain what happens to the energy of a photon as the wavelength gets longer and longer.
14. Describe the process by which light is produced by electrons in atoms. Be specific!
15. Why do solutions containing copper (Cu+2) glow green when burned?
16. What is Pauli’s Exclusion Principle? Why is this an important principle?
17. What does the aufbau principle tell us?
18. What is Hund’s Rule? How does it affect the behavior of electrons?
19. What is the difference between the 2s & 4s orbitals? How many electrons can each hold?
20. Describe the importance of the double slit experiment in determining the properties of electrons.
21. Describe the properties & characteristics of orbitals within atoms.
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22. Write the complete electron configuration for calcium (Ca).
23. Draw an electron box diagram for silicon (Si).
24. Write the complete electron configuration for arsenic (As).
25. Draw the s, p, and d orbitals.
s orbital
px orbital
py orbital
pz orbital
d orbital
26. Based on the following sets of quantum numbers, identify a possible set of the four quantum numbers for an
outermost electron of silver, Ag. Then, explain why the other options would be impossible.
a
b
c
d
e
f
g
h
n
3
4
4
4
4.5
4
5
5
l
2
-2
2
3
2
2
2
3
ml
2
1
-1
0
-1
2
-2
2
ms
+1/2
+1/2
-1/2
+1/2
-1/2
+3/2
-1/2
+1/2
27. How many unpaired electrons do the following elements have?
A. Sodium
B. Cobalt
C. Tellurium
D. Dysprosium
E. Barium
F. Xenon
G. Tungsten
H. Silicon
I. Fermium
I. Tin
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