Choose the larger atom in each pair. a. Sn or Si b. Br or Ga c. Sn or Bi d. Se or Sn

Write the electron configuration for each ion. a. O^2-

Write the electron configuration for each ion. b. Br^-

Write the electron configuration for each ion. c. Sr²⁺ d. Co³⁺ e. Cu²⁺

Write the electron configuration for each ion. a. Cl^-

Write the electron configuration for each ion. b. P^3-

Write the electron configuration for each ion. c. K⁺

Write the electron configuration for each ion. d. Mo³⁺ e. V³⁺

Write orbital diagrams for each of these ions.Determine if the ion is diamagnetic or paramagnetic. a. V⁵⁺ b. Cr³⁺ c. Ni²⁺ d. Fe³⁺

Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. a. Cd²⁺ b. Au⁺ c. Mo³⁺ d. Zr²⁺

Which is the larger species in each pair? a. Li or Li⁺ b. Cs^- or Cs⁺ c. Cr^- or Cr³⁺ d. O or O^2-

Which is the larger species in each pair? a. Sr or Sr²⁺ b. N or N^3- c. Ni or Ni²⁺ d. S^2- or Ca²⁺

Arrange this isoelectronic series in order of increasing atomic radius: Se^2- , Sr²⁺ , Rb⁺ , Br^- .

Choose the element with the higher first ionization energy from each pair. a. Br or Bi

Choose the element with the higher first ionization energy from each pair. b. Na or Rb

Choose the element with the higher first ionization energy from each pair. c. As or At

Choose the element with the higher first ionization energy from each pair. d. P or Sn

Choose the element with the higher first ionization energy from each pair. a. P or I b. Si or Cl c. P or Sb d. Ga or Ge

Arrange these elements in order of increasing first ionization energy: Si, F, In, N.

For each element, predict where the 'jump' occurs for successive ionization energies. (For example, does the jump occur between the first and second ionization energies, the second and third, or the third and fourth?) a. Be b. N c. O d. Li

Consider this set of ionization energies. IE₁ = 578 kJ/mol IE₂ = 1820 kJ/mol IE₃ = 2750 kJ/mol IE₄ = 11,600 kJ/mol To which third-period element do these ionization values belong?

Choose the element with the more negative (more exothermic) electron affinity from each pair. a. Na or Rb

Choose the element with the more negative (more exothermic) electron affinity from each pair. b. B or S

Choose the element with the more negative (more exothermic) electron affinity from each pair. c. C or N d. Li or F

Choose the element with the more negative (more exothermic) electron affinity in each pair. a. Mg or S b. K or Cs c. Si or P d. Ga or Br

Choose the more metallic element from each pair. c. Cl or O