Workshop CHE 166
Problem Set #9
 

1. How many unpaired electrons does an atom of magnesium have? Is this atom diamagnetic or paramagnetic?

2. What is the maximum number of electrons that can occupy an energy level described by the principal quantum number, n?

3. Transition metal elements have atoms or ions with partially filled ____ orbitals.

4. Which element has the following electron configuration of [Ar]4s²3d¹⁰4p⁴? How many unpaired electrons are in this element?

5. How many unpaired electrons does an atom of chromium have? Is this atom diamagnetic or paramagnetic?

6. Write the ground state electron configuration for an atom of indium, ₄₉In.

7. Write the ground state electron configuration for the phosphorus atom in its ground state.

8. Give a possible set of quantum numbers [n, l, m_l, m_s] for the last electron added to complete an atom of germanium in its ground state.

9. Lanthanide or rare earth elements have atoms or ions with partially filled ____ orbitals.

10. Write the ground state electron configuration for a ground state nitrogen atom.

11. How many unpaired electrons does an atom of vanadium have? Is this atom diamagnetic or paramagnetic?

12. How many orbitals are allowed in a subshell if the angular momentum quantum number, l, for electrons in that subshell is 3?

13. In what group of the periodic table is the element with the following electron configuration?

[Kr]5s²4d¹⁰5p²

14. Which atom has the greatest electronegativity?

15. What is the charge on the monatomic ion that calcium forms in its compounds?

16. The radii of ions are always smaller than the radii of the corresponding atoms of the same element.

17. Which has the greater radius, an I ^- ion or an I atom? Explain.

18. The elements in Group 2A are known by what name?

19. Write the ground state electron configuration for

(a) Al³⁺
(b) Mg²⁺
(c) Br^-
(d) P^3-
(e) Zn²⁺

20. What type of chemical bond holds the atoms together within a water molecule?

21. Of the following substances or species; NO₂^- , NO₂, and N₂, which one is an exception to the octet rule.

22. Draw the Lewis dot symbol for nitrogen, ₇N and N^3- .

23. For each of the following, determine the total number of valence electrons, draw the Lewis structure, predict the shape of the molecule with the number of bonding and non-bonding electrons, and indicate the hydridization of the underlined atom:
 

a) C₂H₆
b) C₂H₄
c) CO₂
d) SF₆
e) SbCl₅
f) XeF₂

24. Given the following bond energies

BE(S ¾ O) = 347 kJ
BE(O=O) = 499 kJ

 

Estimate the enthalpy change for the reaction 2 SO_{2 (g)} + O_{2 (g)} ® 2 SO_{3 (g)}

25. Estimate the enthalpy of formation of HBr _(g) by means of bond energies.

H_{2 (g)} + Br_{2 (g)} ® 2 HBr _(g)

Given:

BE(H¾ H) = 436 kJ
BE(Br¾ Br) = 192 kJ
BE(H¾ Br) = 366 kJ

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