chem ch5 review
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Chemistry Chapter 5 Review:
1. How does the energy of an electron change when it moves closer to the nucleus?
2. The principle quantum number indicates what property of an electron?
3. What shape are s orbitals and p orbitals?
4. What is the maximum number of f orbitals in one energy level of an atom?
5. What is the maximum number of d orbitals in one principal energy level of an atom?
6. What is the maximum number of orbitals in a p sublevel?
7. What is the maximum number of electrons in the second principal energy level (n=2)?
8. What happens when an electron moves from a lower to a higher energy level?
9. What does the level “p” in the symbol 4p3 indicate?
10. If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?
11. What types of atomic orbitals are in the third principal energy level (n=3)?
12. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
13. What does the Aufbau principle state?
14. What is the number of electrons in the outermost energy level of an potassium atom?
15. What is the electron configuration of oxygen?
16. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?
17. How many half-filled orbitals are in a chlorine atom?
18. How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a vacuum?
19. Which color of visible light has the shortest wavelength?
20. How are the frequency and wavelength of light related? (what equation(s))?
21. What is the wavelength of an electromagnetic wave that travels at 3× 108 m/s and has a frequency of 80 MHz? (1 MHz= 1,000,000 Hz)?
22. Emission of light from an atom occurs when an electron does what?
23. As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit increase or
Chemistry Chapter 5 Review:
1. How does the energy of an electron change when it moves closer to the nucleus?
2. The principle quantum number indicates what property of an electron?
3. What shape are s orbitals and p orbitals?
4. What is the maximum number of f orbitals in one energy level of an atom?
5. What is the maximum number of d orbitals in one principal energy level of an atom?
6. What is the maximum number of orbitals in a p sublevel?
7. What is the maximum number of electrons in the second principal energy level (n=2)?
8. What happens when an electron moves from a lower to a higher energy level?
9. What does the level “p” in the symbol 4p3 indicate?
10. If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?
11. What types of atomic orbitals are in the third principal energy level (n=3)?
12. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
13. What does the Aufbau principle state?
14. What is the number of electrons in the outermost energy level of an potassium atom?
15. What is the electron configuration of oxygen?
16. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals?
17. How many half-filled orbitals are in a chlorine atom?
18. How does the speed of visible light compare with the speed of gamma rays, when both speeds are measured in a vacuum?
19. Which color of visible light has the shortest wavelength?
20. How are the frequency and wavelength of light related? (what equation(s))?
21. What is the wavelength of an electromagnetic wave that travels at 3× 108 m/s and has a frequency of 80 MHz? (1 MHz= 1,000,000 Hz)?
22. Emission of light from an atom occurs when an electron does what?
23. As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit increase or