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Chapter 8: Problem 60
Which of these elements would you expect to have the greatest electron affinity? He, \(\mathrm{K}, \mathrm{Co}, \mathrm{S}, \mathrm{Cl}\).
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You are given four substances: a fuming red liquid, a dark metallic-looking solid, a pale-yellow gas, and a yellow-green gas that attacks glass. You are told that these substances are the first four members of Group \(7 \mathrm{~A},\) the halogens. Name each one.
Why are the Group \(1 \mathrm{~B}\) elements more stable than the Group IA elements even though they seem to have the same outer electron configuration \(n s^{1}\) in which \(n\) is the principal quantum number of the outermost shell?
In each of the following pairs, indicate which one of the two species is smaller: (a) \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-},\) (b) Na or \(\mathrm{Na}^{+}\), (c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-},\) (d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+},\) (e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\).
Use the third period of the periodic table as an example to illustrate the change in first ionization energies of the elements as we move from left to right. Explain the trend.
Without referring to a periodic table, write the electron configurations of elements with these atomic numbers: (a) \(9,\) (b) \(20,\) (c) \(26,\) (d) 33. Classify the elements.
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