Chapter 8

If an element has a low electronegativity, is it likely to be classified as a metal or a nonmetal? Explain your answer.

In what groups in the periodic table are the most reactive metals found? Where do we find the least reactive metals?

When we say that aluminum is more reactive than iron, which kind of reaction of these elements are we describing?

Arrange the following metals in their approximate order of reactivity (most reactive first, least reactive last) based on their locations in the periodic table: (a) iridium (b) silver (c) calcium (d) iron

Complete and balance the following equations. If no reaction occurs, write "N.R." (a) \(\mathrm{KCl}+\mathrm{Br}_{2} \longrightarrow\) (b) \(\mathrm{NaI}+\mathrm{Cl}_{2} \longrightarrow\) (c) \(\mathrm{KCl}+\mathrm{F}_{2} \longrightarrow\) (d) \(\mathrm{CaBr}_{2}+\mathrm{Cl}_{2} \longrightarrow\) (e) \(\mathrm{AlBr}_{3}+\mathrm{F}_{2} \longrightarrow\) (f) \(\mathrm{ZnBr}_{2}+\mathrm{I}_{2} \longrightarrow\)

In each pair, choose the better oxidizing agent. (a) \(\mathrm{O}_{2}\) or \(\mathrm{F}_{2}\) (b) \(A s_{4}\) or \(P_{4}\) (c) \(\mathrm{Br}_{2}\) or \(\mathrm{I}_{2}\) (d) \(\mathrm{P}_{4}\) or \(\mathrm{S}_{8}\) (e) \(\mathrm{Se}_{8}\) or \(\mathrm{Cl}_{2}\) (f) \(\mathrm{As}_{4}\) or \(\mathrm{S}_{8}\)

Why do we usually place the least electronegative element in the center of a Lewis structure?

Why do Period 2 elements never form more than four covalent bonds? Why are Period 3 elements able to exceed an octet?

Define (a) single bond, (b) double bond, and (c) triple bond.

The Lewis structure for hydrogen cyanide is \(\mathrm{H}-\mathrm{C} \equiv \mathrm{N}:\) Draw circles enclosing electrons to show that carbon and nitrogen obey the octet rule.