6. Quantum Chemistry problems

  1. How many electrons can be accommodated in each of the following subshells of an atom?
    1. 3p sub-shell                                                                                                      [6]
    2. 4s sub-shell                                                                                                       [2]
    3. 3d sub-shell                                                                                                     [10]
    4. 4f subshell                                                                                                        [14]
  2. How many electrons does it take to fill the n=3 shell of an atom?           [18]
  3. Which of the following has five electrons? Na, P, Mn, O, Br
  4. Hydrogen occurs in the forms H, H+, and H–, but not H2+.  Explain.
  5. Which of the following have the same electron configuration as a noble gas?
    Cl–, Mn2+, Fe3+, Na+, Al3+.
  6. Without consulting the periodic table, calculate the atomic number of the third noble gas, argon, using only the properties of the quantum numbers and the fact that noble gases have filled s and p shells.
  7. How many electrons are in the outermost p subshell of the group 16 (6A) elements, the Chalcogens?
  8. What is the total number of p electrons in a selenium atom?
  9. Using only a periodic table, calculate the number of electrons there are in a mercury atom.
  10. using only the periodic table, determine how many electrons there are in an atom of lead.
  11. If an element has the electronic configuration [Xe]4f145d76s2, to which of the following categories of the element belong?
    1. halogen
    2. alkaline earth
    3. transition elements
    4. rare earth
    5. noble gas
  12. Draw a box diagram for the ground state of each of the following atoms.
    N       Ti       Cu       Cr       Ne       S
  13. Which doubly charged negative ion has the same electronic configuration as Ar?
  14. Which doubly charged positive ion has the same electron configuration as Ne?
  15. Which positive ion X+ has the same electronic configuration as Cl–?
  16. What is the characteristic valence shell configuration for the chalcogens (Group 16, aka 6A)?
    ns2np2     ns1np3      ns2np4      ns2np5      ns2np6
  17. What is the characteristic valence shell configuration for the group 14 (4A) elements?
  18. Draw a box diagram for the ground state atom of each of the following ions.
    Na+    Cl–    O2-    V2+    Cu+    Cu2+    Fe3+    In+.    Note, in some cases, there is more than one way.
  19. State which of the following atomic orbital descriptions is impossible and explain why your choices are impossible.
    1. 4s
    2. 2d
    3. 3f
    4. 4d
    5. 99s
    6. 1p
    7. 2p
  20. State which of the following atomic configurations is impossible and explain why your choices are impossible.
    1. 1s22s3
    2. 1s22s22p2
    3. 1s22s22p63s23p6
    4. 1s22s22p63s23p63f3
    5. [Kr]4s2
    6. [Kr]5s1
    7. [Kr]4d12
    8. [Kr]5p1
  21. Which of the following combinations of quantum numbers is not possible for an electron in an atom.  For each impossible case, explain the rule that is broken.
n \ell m_{\ell} m_s
a 1 0 0 1/2
b 3 2 -1 -1/2
c 3 3 -2 1/2
d 3 1 2 -1/2
e 6 1 -1 1/2
  1. Calculate the energy of a mole of photons of
    1. infrared photons of wavelength 10 micrometers.                         [12 kJ]
    2. red light of wavelength 700 nanometers.                                      [171 kJ]
    3. violet light of wavelength 400 nanometers                                   [299 kJ]
    4. ultraviolet light of wavelength 180 nanometers                            [665 kJ]
    5. x-rays of wavelength 0.154 nanometers                                           [777 MJ]
  2. a laser produces a pulse of light of wavelength 337.1 nm. If the energy contained in each pulse of the laser if 10.0 mJ, how many photons are in each pulse?   [1.70×1016]
  3. the ionization energy of a neon atom is 2081 kJ/mol. What is the longest wavelength light that is capable of removing an electron from a neon atom?   [57.5 nm]
  4.  From the Rhydberg equation, calculate the wavelength of the line in teh balmer series in the spectrum of the hydrogen atom having the second shortest wavelength.                                                                                                             [486.27 nm]
  5. the first ionization energy of potassium is 419 kJ/mol. What is the longest wavelength of light that can ionize an atom of this element?                  [286 nm]
  6. Which of the following has the smallest ionization energy?
    Na    F    Mg    S    Li+    Al3+
  7. The ionization energy of a sodium atom is 486 kJ/mol and teh electron affinity of a chlorine atom is 394 kJ/mol.  Calculate the enthalpy change for the following electron transfer reaction
    Na(g) + Cl(g) → Na+(g) + Cl–(g).                                                                        [+147 kJ/mol]
  8. The ionization energy of a Cesium atom is 376 kJ/mol and the electron afinity of a fluorine atom si 328 kJ/mol.  What is the enthalpy change for the following reaction?
    Cs(g) + F(g) → Cs+(g) + F–(g).                                                                              [+48 kJ/mol]
  9. For each of the following ions, name the isoelectronic and neutral atom.
    1. Li+
    2. C+
    3. P+
    4. O–
    5. Br–
    6. Br+

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