1. No category

Name: ______________________________
Date: ___________________ Pd: ________
CP Chem
CP Unit 4 Sample Questions
____ 1. Frequency and Wavelength are related ______________.
a. directly
b. inversely
c. proportionally
d. distantly
____ 2. Who is usually considered the father of Quantum Mechanics?
a. Bohr
b. Dalton
c. Mendel
d. Werner
____ 3. The symbol for wavelength is:
a. alpha ()
b. lambda ()
c. nu ()
d. psi ()
____ 4. The symbol for frequency is:
a. alpha ()
b. lambda ()
c. nu ()
d. psi ()
____ 5.How many unpaired electrons does neon have?
a. 0
b. 1
c. 6
d. 10
____ 6. How many unpaired electrons does phosphorus have?
a. 0
b. 2
c. 3
d. 15
____ 7. Which element has this electron configuration? 1s22s22p63s23p64s1
a. Calcium
b. Neon
c. Phosphorus
d. Potassium
____ 8. A flame test produces a light purple. Which of these cations could be responsible for the color? (What are the others?)
a. Cu+2
b. Li+1
c. K+1
d. Na+1
____ 9. The wavelength of ultraviolet radiation is longer than:
a. radio waves
b. gamma rays
c. microwaves
d. visible waves
____ 10. The Pauli Exclusion Principle states that electrons in the same atom cannot:
a. share an orbital
b. resonate
c. touch
d. have the same quantum #’s
____ 11. The speed of light in a vacuum is:
a. 2.998x10-8 m/s
b. 2.998 m/s
d. 2.998 million mph
c. 2.998x108 m/s
____ 12. Long wavelength light has _________ energy compared to shorter wavelength light.
a. the same
b. no
c. less
d. more
____ 13. Frequency of radiation is measured in:
a. m/s
b. s
c. J
d. Hz
____ 14. In order to fill the 5p orbitals, _____ electrons are required.
a. 5
b. 6
c. 7
d. 8
____ 15. The next orbital to gain electrons after the 4s is:
a. 3p
b. 4p
d. 5s
c. 3d
____ 16. What is the probability of finding an electron within its orbital?
a. 100%
b. 90%
c. 50%
d. 10%
____ 17. What is the term for a region within an orbital where you never find the electron?
a. azimuth
b. node
c. singlet
d. Tibet
____ 18. The “s” in 3s2 tells us the______________ the orbital.
a. energy of
b. size of
c. number of electrons in d. shape of
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CP Chem
____ 19. The “3” in 3s2 tells us the______________ the orbital.
a. energy of
b. size of
c. number of electrons in d. shape of
____ 20. The “2” in 3s2 tells us the______________ the orbital.
a. energy of
b. size of
c. number of electrons in d. shape of
21. What is the frequency of blue light with a wavelength of 450 nm?
22. What is the wavelength (in nm) of radiation with a frequency of 6.87x1014 Hz?
23. Which has more energy, infrared or ultraviolet light? Prove it using the following data:
IR = 1.96x1014 Hz & UV = 9.37x1014 Hz
24. Which photon of light has more energy, red (λ = 679 nm) or yellow (λ = 587 nm)? Prove it.
25. What is the wavelength (in nm) of a photon with 3.26x10-18 J of energy?
26. What is the energy of a photon of green light with a wavelength of 540 nm?
27. How much energy is required to emit 4.73x1012 photons of light with a wavelength of 467 nm?
28. How many photons with a wavelength of 1060 nm can be produced with 70.08 kJ of energy?
29. Which travels faster in a vacuum: x-rays or radio waves? Why?
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CP Chem
30. Explain what happens to frequency as the wavelength gets longer and longer.
31. Explain what happens to the energy of a photon as the wavelength gets longer and longer.
32. Describe the process by which light is produced by electrons in atoms. Be specific!
33. Why do solutions containing copper (Cu+2) glow green when burned?
34. Pauli’s Exclusion Principle forbids electrons from stacking up on each other. Why is this an important principle?
35. What does the aufbau principle tell us?
36. What is Hund’s Rule? How does it affect the behavior of electrons?
37. What is the difference between the 2s & 4s orbitals? How many electrons can each hold?
38. Describe the importance of the double slit experiment in determining the properties of electrons.
39. Describe the properties & characteristics of orbitals within atoms.
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CP Chem
40. Write the complete electron configuration for calcium (Ca).
41. Write the complete electron configuration for arsenic (As).
42. Draw an electron box diagram for silicon (Si).
43. Draw an electron box diagram for lead (Pb).
44. Draw the s, p, and d orbitals.
s orbital
px orbital
45. How many unpaired electrons do the following
elements have?
A) Sodium
py orbital
pz orbital
d orbital
46. Identify the parts of the following wave diagram:
A
B
B) Manganese
C) Tellurium
D) Americium
D
E) Barium
C
F) Xenon
G) Tungsten
H) Silicon
I) Tin
Given:
c = 
E = h
h = 6.626x10-34 Js
1 nm = 1x10-9 m
1 kJ = 1,000 J
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f 5g
6f 6g 6h
7f 7g 7h 7i
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