Discussion 2 - Worksheet PDF

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WORKSHEET 2 1.

Predict the most stable ion generally formed by (a) Sr, (b) Se, (c) Al, (d) As, (d) Te.

2.

Predict the charges on the ions formed when magnesium reacts with nitrogen. What is the formula unit of the ionic compound that is formed?

3.

Predict the formula unit (or empirical formula) for the ionic compounds formed from the following pairs of elements: (a) Rb, Cl (b) Ba, S (c) Al, Cl (d) Ga, O (e) Li, N

4.

Write the formula of the compound that forms between calcium and each polyatomic anion. (a) Carbonate (b) Phosphate (c) Hydrogen phosphate (d) Perchlorate (e) Nitrate (f) Sulfate (g) Nitrite

5.

Write the formula unit for each compound: gallium fluoride, iron(II) sulfide, iron(III) oxide, and zinc sulfate.

6.

Rubidium iodide has a lattice energy of –617 kJ·mol–1, while potassium bromide has a lattice energy of –671 kJ·mol–1. Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?

7.

Arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO.

8.

Which substance would you expect to have the greatest lattice energy, AgCl, CuO, or MnP?

9.

In which pair do both compounds exhibit predominantly ionic bonding? (a) PCl5 and HF (b) NaF and H2O (c) Na2SO3 and BH3 (d) RbCl and CaO (e) KI and O3

10. Which of the following bonds is/are non-polar? (a) C—O (b) O—F (c) H—C (d) S—Cl (e) They are all non-polar 11. Classify each compound as ionic, covalent, or metallic. (a) CO2(g) (b) NiCl2(s) (c) PCl5(s) (d) NaI(s) (e) Cr(s) (f) NH4NO3(s) (g) CaSO4(s) 12. Consider the bonds formed between the atoms in each formula. CsCl

O2

Hg2Cl2

NO

IBr

In each case, identify the atom that carries either a positive charge or a partial positive charge. 13. Order the bonds in each of the following groups in order of increasing bond polarity. (a) N—O, N—F, C—F (b) C—F, C—Cl, C—Br (c) Cl—Cl, F—Cl, F—Br, Br—Cl 14. In which case is the bond polarity incorrect?

15.

Draw Lewis dot structures (including resonance structures where necessary) for the following molecules. (a) O2 (b) PF5 (c) SeF2 (d) OCS (e) I3– (f) O3 (g) BrF3 (h) SF4

16.

For each of the following compounds: 1. Draw Lewis structure(s). 2. Give the shape of the molecule. 3. Give approximate bond angle(s) 4. Indicate whether the molecule has a net dipole moment or zero dipole moment. (a) SeH2 (b) BrF3 (c) SF4 (d) AsF5 (e) IF4+ (f) I3–...