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
- 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
- Use the Crossover Method to determine the following ionic chemical formula.
- a. iron(III) sulfide
- b. calcium hydride
- c. magnesium nitride
- d. aluminum fluoride
- 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.
- Draw the Lewis dot structures for: (Note: make sure it satisfies the octet rule)
- a. NI3
- b. CS2
- c. N2F2
- d. CH2Cl2
- a. Which bond is more polar, H-Cl or H-O?
- Which of the following bonds is the most polar, that is, has the greatest ionic character: H-Br, N-H, N-O, P-Cl?
- Write the formulas and names for the compounds of the following ions:
F- O2- P3-
K+Ga3+
- Which families or groups are likely to form the following ions?
- a. +1
- b. -1
- c. +2
- d. -2
- e. +3
- f. -3
- Draw the following compounds by representing them as covalent bonds using VSEPR Theory:
- a. CO2
- b. H2SO4
- c. CH3OH
- d. N2O3
- 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
