Which experience a greater effective nuclear charge: the valence electrons in beryllium or the valence electrons in nitrogen? Why?

If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? a. K

In Section 3.6, we estimated the effective nuclear charge on beryllium's valence electrons to be slightly greater than 2+. What would a similar treatment predict for the effective nuclear charge on boron's valence electrons? Would you expect the effective nuclear charge to be different for boron's 2s electrons compared to its 2p electron? In what way? (Hint: Consider the shape of the 2p orbital compared to that of the 2s orbital.)

Choose the larger atom in each pair. a. P or O b. Si or Sn c. S or Sb d. B or N

Choose the larger atom in each pair. a. I or In b. Sb or P c. Te or Br d. S or Ge

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. a. Cl^-

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. Cl or Sb

Choose the element with the higher first ionization energy from each pair. b. Li or K

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

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

Choose the element with the higher first ionization energy from each pair. a. Ge or Br b. P or In c. S or Te d. As or Br

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, the third and fourth, and so on?) a. B b. Na C. P d. S

Consider this set of ionization energies.

IE1 = l000 kJ/mol

IE2 = 2250 kJ/mol

IE3 = 3360 kJ/mol

IE4 = 4560 kJ/mol

IE5 = 7010 kJ/mol

IE6 = 8500 kJ/mol

IE = 27,I00 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. c. P or S

Choose the element with the more negative (more exothermic) electron affinity in each pair. a. Ca or Se b. Ge or S c. Al or O d. Se or I

Choose the more metallic element from each pair. a. Rb or Sn b. P or Sb c. Te or Cl d. O or P

Choose the more metallic element from each pair. a. As or Sn b. Ca or Ga c. I or Bi d. Br or At

Arrange these elements in order of increasing metallic character: Fr, Sb, In, S, Ba, Se.