AP CHEMISTRY NAME
PRACTICE: QUANTUM THEORY & PERIODIC TABLE
1. Who was the first scientist to propose that the atom had a dense nucleus which occupied only a small fraction
of the volume of the atom?
2. Who proposed a model that successfully explained the photoelectric effect?
3. Who proposed the principle which states that one cannot simultaneously know the exact position and
velocity of a particle?
4. Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to
a. radio, visible, infrared, ultraviolet b. infrared, visible, ultraviolet, microwave
c. visible, ultraviolet, infrared, gamma rays d. X-radiation, visible, infrared, microwave
e. microwave, infrared, visible, ultraviolet
5. The AM station KBOR plays your favorite music from the 20’s and 30’s at 1290 kHz. Find the
wavelength of these waves.
6. A radio wave has a frequency of 8.6 108 Hz. What is the energy of one photon of this radiation?
7. For potassium metal, the work function (the minimum energy needed to eject an electron from the
metal surface) is 3.68 10-19 J. Which is the longest wavelength of the following which could excite
*8. Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom
undergoes a transition from n1 = 2 to n2 = 4. (R = 1.096776 107 m-1)
9. The Bohr theory of the hydrogen atom predicts the energy difference (in J) between the n = 3 and the
n = 5 state to be
*10. According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is
3.5 103 m/s, the uncertainty in its position (in m) is at least
11. The shape of an atomic orbital is associated with which quantum number?
12. Atomic orbitals developed using quantum mechanics
a. describe regions of space in which one is most likely to find an electron.
b. describe exact paths for electron motion.
c. give a description of the atomic structure, which is essentially the same as the Bohr model.
d. allow scientists to calculate an exact volume for the hydrogen atom.
e. are in conflict with the Heisenberg Uncertainty Principle.
13. Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?
a. n = 3, l = 0, ml = -1 b. n = 3, l = 1, ml = +3 c. n = 3, l = 2, ml = 3
d. n = 3, l = 3, ml = +2 e. n = 3, l = 2, ml = -2
14. In the quantum mechanical treatment of the hydrogen atom, which one of the following
combinations of quantum numbers is not allowed?
n l ml
a. 3 0 0
b. 3 1 -1
c. 3 2 2
d. 3 2 -1
e. 3 3 2
15. Explain the context and meanings of the terms “orbit” and “orbital”, making a clear distinction
16. The effective nuclear charge for an atom is less than the actual nuclear charge due to
17. In a single atom, what is the maximum number of electrons which can have quantum number n = 4?
18. Write the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of
19. Write the correct ground state electron configuration and orbital notation for Cu (Z = 29).
20. In the ground state of an atom of silver (Ag), how many electrons will there be with the quantum number
l = 1? (The n, ml and ms quantum numbers may have any appropriate values.)
21. An element with the electron configuration [noble gas]ns2(n - 1)d 8 has ___________ valence electrons.
22. Which of the following electron configurations represents the ground state for an element?
a. [Ne]3s13p1 b. [He]2s12p3 c. [Ne]3s23p23d1 d. [Ne]3s23p33d1
e. [Ne]3s 3p
23. Which of the following elements has the smallest atomic size?
a. Na b. Ar c. K d. Ca e. Kr
24. Which of the following elements has the largest first ionization energy?
a. Na b. Cl c. Ca d. Te
25. Which of the following elements has the largest second ionization energy (IE2)?
a. Li b. B c. O d. F e. Na
26. Elements with ________________ first ionization energies and ___________ electron affinities generally
27. Select the most basic compound from the following.
a. Bi2O3 b. SiO2 c. Cs2O d. Na2O e. H2O
28. Which of the following elements is paramagnetic?
a. Kr b. Zn c. Sr d. V e. Ar
29. Consider the set of isolectronic atoms and ions A2-, B-, C, D+, and E2+. Arrange them in increasing order of
30. What is the maximum number of electrons in an atom which can have
a. quantum number n = 4.
b. orbital designation 3d.
c. orbital designation 2pz.
31. State Hund’s rule, and show how it applies to the ground state of phosphorus atoms.