1) Give the full ground state electron configuration for As. 2) Give the full ground state electron configuration for Pb.
3) Give the ground state electron configuration for the ion that Cs forms. Is it more or less stable than the neutral atom?
4) Identify the isoelectronic (same number of electrons) elements. Show your work.
A) CI-, F., Br, 1-, At
B) N3-S2-, Br, Cst, Sr2+
C) N3, 02-, F., Na+, Mg2+
D) Lit, Nat, K+, Rb. st E) Ne, Ar, Kr, Xe, He
5) Identify the elements correctly shown by decreasing radii size. Provide a brief reason.
A) N3->N
B) K+ >K
C)N > N3
D) Cu2+ > Cut
E) S-> S2
6) What period 3 element has the following ionization energies (all in kJ/moly? And, why? IE1 - 1000; IE2 = 2250; IE3 - 3360: IE4 = 4560; IE5 - 7010; IE6 = 8500; IE7 = 27,100
7) Place the following in order of decreasing IE]. Provide a reason. Cs Ar Mg
8) Write the reaction that represents electron affinity of potassium (K) atom? Is the product more or less stable than the reactant? Why?
9) Give the set of four quantum numbers that could represent the extra electron added (using the Aufbau principle) to the neutral Ne atom.
10) Which 2nd period element has the most negative electron affinity? Why? - Bonus questions
11) Which ionization process requires the most energy? Why?
A) Se(g) Set(g) +e-
B) Set(g) Se2+(g) +
C) Br(g) Br) +-
D) Brt (8) Br2+(g) +e
12) Place the following in order of decreasing metallic character. Explain your reason. P As K -