Chapter 6: Q49E (page 336)
Question:49. Using complete subshell notation (1s22s22p6, and so forth), predict the electron configuration of each of the
following atoms:
(a) N
(b) Si
(c) Fe
(d) Te
(e) Tb
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Based on their positions in the periodic table, rank the following atoms or compounds in order of increasing first ionization energy:\({\bf{Mg}},{\rm{ }}{\bf{O}},{\rm{ }}{\bf{S}},{\rm{ }}{\bf{Si}}\).
Question:Based on their positions in the periodic table, predict which has the smallest first ionization energy: Li, Cs, N, F, I.
Question:Which atom would be expected to have a half-filled 4ssubshell?
What is the energy in joules and the wavelength in meters of the photon produced when an electron falls from then= 5 to then= 3 level in a\({\bf{H}}{{\bf{e}}^ + }\)ion (\(Z = {\rm{ }}{\bf{2}}\)for\({\bf{H}}{{\bf{e}}^{\bf{ + }}}\))?
List the following ions in order of increasing radius: \({\bf{L}}{{\bf{i}}^ + },{\rm{ }}{\bf{M}}{{\bf{g}}^{{\bf{2}} + }},{\rm{ }}{\bf{B}}{{\bf{r}}^--},{\rm{ }}{\bf{T}}{{\bf{e}}^{{\bf{2}}--}}.\)
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