According to Coulomb's law, which pair of charged particles has the lowest potential energy? a. a particle with a 1- charge separated by 150 pm from a particle with a 2+ charge b. a particle with a 1- charge separated by 150 pm from a particle with a 1+ charge c. a particle with a 1- charge separated by 100 pm from a particle with a 3+ charge

According to Coulomb's law, rank the interactions between charged particles from lowest potential energy to highest potential energy. a. a 1+ charge and a 1- charge separated by 100 pm b. a 2+ charge and a 1- charge separated by 100 pm c. a 1+ charge and a 1+ charge separated by 100 pm d. a 1+ charge and a 1- charge separated by 200 pm

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

Arrange the atoms according to decreasing effective nuclear charge experienced by their valence electrons: S, Mg, Al, Si.

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

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? b. Ca

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? c. O d. C

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. 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.