Chapter 4 Compounds and Their Formulas

Homework #4
You must show your entire work on a separate sheet(s) of paper to get full credit.

Chapter 4

1. Draw the Lewis dot structures for the following imaginary elements

  • a. X, an element from the Group IA family
  • b. Z, an element from the Group IIA family
  • c. J, an element from the Group IVA family
  • d. K, an element from the Group VIA family

2. Use the Crossover Method to determine the following ionic chemical formula.

  • a. iron(III) sulfide
  • b. calcium hydride
  • c. magnesium nitride
  • d. aluminum fluoride

3. Using the chemical formulas from question 2 to write the structures step–by–step to obtain the Lewis dot structures and show how you balance the charges.

4. Draw the Lewis dot structures for: (Note: make sure it satisfies the octet rule)

  • a. NI3
  • b. CS2
  • c. N2F2
  • d. CH2Cl2

5. a. Which bond is more polar, H–Cl or H–O?
b. Which of the following bonds is the most polar, that is, has the greatest ionic character: H–Br, N–H, N–O, P–Cl?

6. Write the formulas and names for the compounds of the following ions:
F– O2– P3–
K+Ga3+

7. Which families or groups are likely to form the following ions?

  • a. +1
  • b. –1
  • c. +2
  • d. –2
  • e. +3
  • f. –3

8. Draw the following compounds by representing them as covalent bonds using VSEPR Theory:

  • a. CO2
  • b. H2SO4
  • c. CH3OH
  • d. N2O3

9. Show the dipole moment of each bond and then predict the overall molecule as either being polar or nonpolar?

  • a. CH4
  • b. H2S
  • c. PH3
  • d. SO3