Chapter 5

Explain ionic bonding according to Lewis theory.

Explain covalent bonding according to Lewis theory.

Why is Lewis theory useful? Give some examples.

Draw electron dot structures for the following elements: \(\mathrm{Na}, \mathrm{Al}, \mathrm{P}, \mathrm{Cl}\), and Ar. Which are most chemically reactive? Which are least chemically reactive?

Explain VSEPR theory. According to this theory, what determines the shapes of molecules?

Describe a polar covalent bond.

What is the difference between a polar and a nonpolar bond? What is the difference between a polar and nonpolar molecule?

Why do polar molecules have a greater tendency to remain a liquid or a solid at room temperature?

Explain, in molecular terms, why oil and water do not mix.

Draw Lewis structures for each of the following elements. Which element is most chemically stable? a. C b. \(\mathrm{Ne}\) c. \(\mathrm{Ca}\) d. \(\mathrm{F}\)

Draw Lewis structures for each of the following elements. Which two elements are most chemically stable? a. \(\mathrm{Br}\) b. \(S\) c. \(\mathrm{Kr}\) d. He

Draw a Lewis structure for each of the following ionic compounds: a. \(\mathrm{KI}\) b. \(\mathrm{CaBr}_{2}\) c. \(\mathrm{K}_{2} \mathrm{~S}\) d. \(\mathrm{MgS}\)

Draw a Lewis structure for each of the following ionic compounds. What chemical formula does Lewis theory predict? a. sodium fluoride b. calcium chloride c. calcium oxide d. aluminum chloride

Draw a Lewis structure for each of the following ionic compounds. What chemical formula does Lewis theory predict? a. sodium oxide b. aluminum sulfide c. magnesium chloride d. beryllium oxide

Draw a Lewis structure for each of the following covalent compounds: a. \(\mathrm{I}_{2}\) b. \(\mathrm{NF}_{3}\) c. \(\mathrm{PCl}_{3}\) d. \(\mathrm{SCl}_{2}\)

Draw a Lewis structure for each of the following covalent compounds: a. \(\mathrm{OF}_{2}\) b. \(\mathrm{NI}_{3}\) c. \(\mathrm{CS}_{2}\) d. \(\mathrm{Cl}_{2} \mathrm{CO}\) (carbon is the central atom)

Determine whether each of the following compounds is ionic or covalent and draw an appropriate Lewis structure: a. \(\mathrm{MgS}\) b. \(\mathrm{PI}_{3}\) c. \(\mathrm{SrCl}_{2}\) d. \(\mathrm{CHClO}\) (carbon is the central atom)

Determine whether each of the following compounds is ionic or covalent and draw an appropriate Lewis structure: a. \(\mathrm{K}_{2} \mathrm{O}\) b. \(\mathrm{CHClO}\) (carbon is the central atom) c. \(\mathrm{SrS}\) d. \(\mathrm{CH}_{3} \mathrm{Cl}\) (Carbon is the central atom)

What is wrong with each of the following Lewis structures? Fix the problem and write a correct Lewis structure. a. \(: \ddot{N}=N=\ddot{0}\) : b. \(: \ddot{\mathrm{O}}-\ddot{\mathrm{S}}-\ddot{\mathrm{O}}=\) c. \(: \ddot{\mathrm{B}} \mathrm{r}-\ddot{\mathrm{B}} \mathrm{r}\) : d. \(: \ddot{\mathrm{O}}=\mathrm{Si}-\ddot{\mathrm{O}}\) :

Draw a Lewis structure and use VSEPR to determine the geometry of each of the following molecules. If the molecule has more than one central atom, indicate the geometry about each of these and draw the threedimensional structure. a. ClNO (nitrogen is the central atom) b. \(\mathrm{H}_{3} \mathrm{CCH}_{3}\) (two carbon atoms in the middle, each with three hydrogen atoms attached) c. \(\mathrm{N}_{2} \mathrm{~F}_{2}\) (nitrogen atoms in the center and fluorine atoms on the ends) d. \(\mathrm{N}_{2} \mathrm{H}_{4}\) (nitrogen atoms in the center and two hydrogen atoms attached to each nitrogen)

Draw a Lewis structure and use VSEPR to determine the geometry of each of the following molecules. If the molecule has more than one central atom, indicate the geometry about each of these and draw the threedimensional structure. a. HCCH (two carbon atoms in the middle, each with one hydrogen atom attached) b. \(\mathrm{CCl}_{4}\) c. \(\mathrm{PH}_{3}\) d. HOOH (two oxygen atoms in the middle, each with one hydrogen atom attached)

Determine whether each of the following molecules is polar: a. NO b. HF c. \(\mathrm{H}_{2}\) d. ICl

Determine whether each of the following molecules is polar: a. \(\mathrm{HCl}\) b. \(\mathrm{N}_{2}\) C. \(\mathrm{O}_{2}\) d. \(\mathrm{CO}\)