Question

1. 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

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

3. Which outer electron configuration would you expect to belong to a reactive metal? To a reactive nonmetal?

a) ns2 b) ns2 p6 c) ns2 np5 d) ns2 np2

4. Bromine is a highly reactive liquid while krypton is an inert gas. Explain this difference based on their electron configurations.

5. Write the electron configuration and draw the orbital diagram for each ion. Indicate whether the ion is diamagnetic or paramagnetic: a) Co2+ b) N2- c) Na+

1. Arrange these elements in order of increasing atomic radius: Ca, Rb, S, Si, Ge.

2. Which is a larger species: N or N3-

3. Arrange the following in order of increasing first ionization energy: Si, F, In, N Name: .

4. Chemistry, A Molecular Approach, 4e- Tro. 4. Choose the element with more negative electron affinity: Mr or S, K or Cs

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

6. Consider this set of ionization energies below, to which third element do these ionization values belong: IE1 = 578 kJ/mol IE2 = 1820 kJ/mol IE3 = 2750 kJ/mol IE4 = 11,600 kJ/mol

7. The first ionization energies of P and S are 1060 and 1005 kJ/mol. This does not follow the general trend across the periodic table, why?

Answer 1