Question

8.52 Arrange the following in order of increasing first ionization energy: F, K, P, Ca, and Ne. Explain why. 8.54 In general, ionization energy increases from left to right across a given period. Aluminum, how- ever, has a lower ionization energy than magne- sium. Explain. 8.56 Two atoms have the electron configurations $1s^22s^22p^6$ and $1s^22s^22p^63s^1$. The first ionization energy of one is 2080 kJ/mol, and that of the other is 496 kJ/mol. Match each ionization energy with one of the given electron configurations. Justify your choice. 8.62 Specify which of the following elements you would expect to have the greatest electron affin- ity and which would have the least: He, K, Co, S, Cl. 8.64 Explain why alkali metals have a greater affinity for electrons than alkaline earth metals. 7.39 Write equations that show the processes that describe the first, second, and third ionization energies of an aluminum atom. Which process would require the least amount of energy?

          8.52 Arrange the following in order of increasing first
ionization energy: F, K, P, Ca, and Ne. Explain why.
8.54 In general, ionization energy increases from left
to right across a given period. Aluminum, how-
ever, has a lower ionization energy than magne-
sium. Explain.
8.56 Two atoms have the electron configurations $1s^22s^22p^6$
and $1s^22s^22p^63s^1$. The first ionization energy of one
is 2080 kJ/mol, and that of the other is 496 kJ/mol.
Match each ionization energy with one of the given
electron configurations. Justify your choice.
8.62 Specify which of the following elements you
would expect to have the greatest electron affin-
ity and which would have the least: He, K, Co,
S, Cl.
8.64 Explain why alkali metals have a greater affinity for
electrons than alkaline earth metals.
7.39 Write equations that show the processes that describe the
first, second, and third ionization energies of an aluminum
atom. Which process would require the least amount of
energy?

8.52 Arrange the following in order of increasing first
ionization energy: F, K, P, Ca, and Ne. Explain why.
8.54 In general, ionization energy increases from left
to right across a given period. Aluminum, how-
ever, has a lower ionization energy than magne-
sium. Explain.
8.56 Two atoms have the electron configurations 1s^22s^22p^6
and 1s^22s^22p^63s^1. The first ionization energy of one
is 2080 kJ/mol, and that of the other is 496 kJ/mol.
Match each ionization energy with one of the given
electron configurations. Justify your choice.
8.62 Specify which of the following elements you
would expect to have the greatest electron affin-
ity and which would have the least: He, K, Co,
S, Cl.
8.64 Explain why alkali metals have a greater affinity for
electrons than alkaline earth metals.
7.39 Write equations that show the processes that describe the
first, second, and third ionization energies of an aluminum
atom. Which process would require the least amount of
energy?

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