91Ó°ÊÓ

Name an element in the fourth period (row) of the periodic table with: $$\begin{array}{l}{\text { a. five valence electrons }} \\ {\text { b. four } 4 p \text { electrons }} \\ {\text { c. three } 3 d \text { electrons }} \\\ {\text { d. a complete outer shell }}\end{array}$$

Name an element in the third period (row) of the periodic table with: $$\begin{array}{l}{\text { a. three valence electrons }} \\ {\text { b. four } 3 p \text { electrons }} \\ {\text { c. six } 3 p \text { electrons }} \\\ {\text { d. two } 3 \text {s electrons and no } 3 p \text { electrons }}\end{array}$$

Determine the number of valence electrons in each element. $$\text { a. } \mathrm{Ba} \quad \text { b. } \mathrm{Cs} \quad \text { c. Ni } \quad \text { d. } \mathrm{S}$$

Determine the number of valence electrons in each element. Which elements do you expect to lose electrons in chemical reactions? Which do you expect to gain electrons? $$\text { a. } \mathrm{Al}\quad \text { b. } \mathrm{Sn} \quad \text { c. Br } \quad \text { d. } \mathrm{Se}$$

Which outer electron configuration would you expect to correspond to a reactive metal? To a reactive nonmetal? $$\text { a. }n s^{2} \quad \text { b. } n s^{2} n p^{6} \quad \text { c. } n s^{2} n p^{5} \quad \text { d. } n s^{2} n p^{2}$$

Which outer electron configurations would you expect to correspond to a noble gas? To a metalloid? $$\text { a. } n s^{2} \quad \text { b. } n s^{2} n p^{6} \quad \text { c. } n s^{2} n p^{5} \quad \text { d. } n s^{2} n p^{2}$$

List the number of valence electrons for each element and classify each element as an alkali metal, alkaline earth metal, halogen, or noble gas. $$\begin{array}{lll}{\text { a. sodium }} & {\text { b. iodine }} & {\text { c. calcium }} \\ {\text { d. barium }} & {\text { e. krypton }}\end{array}$$

List the number of valence electrons in each element and classify each element as an alkali metal, alkaline earth metal, halogen, or noble gas. $$\begin{array}{llllll}{\text { a. } F} & {\text { b. Sr }} & {\text { c. } K} & {\text { d. Ne }} & {\text { e. At }}\end{array}$$

Which pair of elements do you expect to be most similar? Why? $$ \begin{array}{l}{\text { a. nitrogen and oxygen }} \\ {\text { b. titanium and gallium }} \\ {\text { c. lithium and sodium }} \\ {\text { d. germanium and arsenic }} \\ {\text { e. } \text { argon and bromine }}\end{array} $$

Predict the charge of the ion formed by each element and write the electron configuration of the ion. $$ \text { a. O } \quad \text { b. } \mathrm{K} \quad \text { c. Al } \quad \text { d. Rb } $$