Read each question carefully. Show all work. No partial credit can be given if work is not completely shown.

1. Answer the following questions by filling in each blank with the appropriate answer:

a) Which atom has the larger first ionization energy: Be or B? __________

b) Arrange the following atoms in order of increasing atomic radius:

Al, Cl, S, P ___________________________________.

c) Of all the known elements in the periodic table, the atom with the largest radius is: ________________

d) As we go down a particular group in the periodic table, the effective nuclear charge (increases/decreases/stays the same) ___________________

e) Identify the neutral element that is isoelectronic with the cation Po⁴⁺ ________

f) Provide the appropriate value for the missing quantum number:
n=1, l= 0, m_l= _______?, m_s=1/2

g) Which of the following isoelectronic species is largest: Rb⁺, Kr, Br^-, Se^2-? ______________

h) How many electrons can there be with m_l = 0 when n=5?

______________

2. Write down the complete electronic configuration for each of the following ions and classify each as a noble gas ion, a pseudo-noble gas ion or an inert pair ion.

i) As^3-

ii) Cd²⁺

iii) Sc³⁺

3. a) What trication has the configuration [Xe]6s²4f¹⁴5d¹⁰?

b) Is this ion paramagnetic or diamagnetic? Why or why not?

c) Classify this ion according to the type of electronic configuration.

4. Write down the complete electronic configurations for the following neutral atoms.

a) chromium

b) meitnerium (This is a newly discovered element of Z=109 which appears in the periodic table below iridium in group 9.)

5. Pick the best answers for the following multiple choice questions:

i) Hund’s rule states that the lowest energy configuration for an atom is the one with

a) maximum number of paired electrons

b) lowest value of n

c) minimum multiplicity

d) maximum number of unpaired electrons

ii) The electronegativity of an atom increases as the

a) Electron affinity decreases

b) Ionization potential increases

c) Effective nuclear charge decreases

d) Equilibrium constant increases

iii) The ability of a electron in an orbital to shield another electron from the nuclear charge is:

a) independent of the value of l

b) depends only on n

c) depends on m_s among other things

d) depends on l

6. The electron affinity for nitrogen is very small, whereas for oxygen and carbon it is larger. Explain this observation.

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