Unit 4 – Electrons. Exam Review. 1. What is the next atomic orbital in the series: 1s, 2s, 2p, 3s, 3p, ? A. 3d B. 4s C. 4p D. 3f. 2. In Bohr’s model of the atom, where are the electrons? A. Evenly throughout the entire atom. B. In orbitals . C. In orbits.
A. Evenly throughout the entire atom.
B. In orbitals.
C. In orbits.
D. His model did not include electrons.
3. How does the energy of an electron change when the electron moves closer to the nucleus?
C. remains the same
4. If the spin of one electron in an orbital is “clockwise”, what is the spin of the other electron in that orbital?
C. it doesn’t spin because the cancel each other
D. towards the nucleus
5. What is the approximate energy of a photon having a frequency of 4.0 x 1015 Hz? (h = 6.63 x 10-34 J . s)
A. 1.7 x 10-41 J
B. 1.678 x 10-41 J
C. 2.652 x 10-18 J
D. 2.7 x 10-18 J
8. According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other quantity CANNOT be known?
D. none of the above
B. gamma rays
C. radio waves
D. UV rays
11. What is the number of electrons in the outermost energy level of an oxygen atom?
12. How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a vacuum?
C. the same
D. you can’t compare them
A. the energy level of the electron
B. the spin of the electron
C. the sublevel of the electron
D. the shape of the orbital
C. de Broglie
15. What is the maximum number of electrons in the second principal energy level?
16. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed?
A. All in one orbital
B. 2 of them will be in one orbital; 1 in another
C. 1 electron in each orbital
D. they can’t all fit in the 2p orbitals
A. 5.0 x 106 m
B. 5.0 m
C. 5.0 x 103 m
D. 5.0 x 10-1 m
18. When an electron moves from a lower to a higher energy level, the electron _____.
A. must give off a photon of energy
B. must absorb a photon of energy
C. must slow down
D. must stay in the same position
19. According to the aufbau principle, electrons enter orbitals of ___ first.
A. lowest energy
B. highest energy
C. lowest monemtum
D. highest momentum
20. What is the maximum number of “f” orbitals in any single energy level of an atom?
21. What types of atomic orbitals (s, p, d, or f) are in the third principal energy level?
A. s and p
B. s, p, and f
C. s, p, and d
D. s, p, d, and f
22. How would the atomic emission spectra of a sodium atom on Earth compare with sodium in the sun?
A. it would be the same
B. it would be different
C. you can’t compare the two
D. sodium doesn’t have an emission spectra
A. moves from a lower to higher energy level
B. moves from a higher to lower energy level
C. releases a photon
D. both b and c
25. Who predicted that all matter can behave as waves as well as particles?
C. de Broglie
A. completely filled energy sublevels
B. 3 electrons in the energy level
C. equal number of electrons and neutrons
D. all of the above
28. What is the maximum number of “d” orbitals in a principal energy level?
A. directly proportional
B. inversely proportional
C. the have no relation
A. energy B. wavelength
C. the speed of light
33. How many electrons are in the highest occupied energy level of a neutral atom of arsenic?
1. B 11. B 21. C 31. A
2. C 12. C 22. A 32. D
3. B 13. A 23. B 33. B
4. B 14. D 24. D
5. D 15. B 25. C
6. C 16. C 26. B
7. C 17. B 27. A
8. B 18. B 28. C
9. B 19. A 29. B
10. A 20. D 30. D