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. Al or In b. Si or N c. P or Pb d. Si or Cl

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. 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. 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.

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

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

Arrange these elements in order of decreasing metallic character: Sr, N, Si, P, Ga, Al.

Both vanadium and its 3+ ion are paramagnetic. Refer to their electron configurations to explain this statement.

Life on Earth evolved based on the element carbon. Based on periodic properties, what two or three elements would you expect to be most like carbon?