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Chapter 7: Problem 123

For each of the following pairs of elements $$(\mathrm{C} \text { and } \mathrm{N}) \quad(\text { Ar and Br })$$ pick the atom with a. more favorable (exothermic) electron affinity. b. higher ionization energy. c. larger size.

Short Answer

Expert verified
a. More favorable (exothermic) electron affinity: \(N\) and \(Br\) b. Higher ionization energy: \(N\) and \(Ar\) c. Larger size: \(C\) and \(Br\)

Step by step solution

01

Understand the trends in Electron Affinity, Ionization Energy, and Atomic size.

Examine the periodic table and know that: 1. Electron affinity generally increases moving from left to right across a period and decreases moving down a group. 2. Ionization energy generally increases moving from left to right across a period and decreases moving down a group. 3. Atomic size generally decreases moving from left to right across a period and increases moving down a group.
02

Identify the position of the given elements on the periodic table

Determine the position of each element in the periodic table: - C and N are in the same period (period 2) and different groups; C is Group 14 (IVA) and N is Group 15 (VA). - Ar and Br are in the same period (period 4) and different groups; Ar is Group 18 (VIII) and Br is Group 17 (VII).
03

Determine the electron affinity of the given pairs of elements

Compare the electron affinity of the elements using the periodic trend: a. For C and N: Since they are in the same period and N is to the right of C, N has a more favorable (exothermic) electron affinity. For Ar and Br: Since they are in the same period and Br is to the left of Ar, Br has a more favorable (exothermic) electron affinity.
04

Determine the ionization energy of the given pairs of elements

Compare the ionization energy of the elements using the periodic trend: b. For C and N: Since they are in the same period and N is to the right of C, N has a higher ionization energy. For Ar and Br: Since they are in the same period and Ar is to the right of Br, Ar has a higher ionization energy.
05

Determine the size of the given pairs of elements

Compare the size of the elements using the periodic trend: c. For C and N: Since they are in the same period and N is to the right of C, C has a larger size. For Ar and Br: Since they are in the same period and Ar is to the right of Br, Br has a larger size.
06

Summarize the results

For each of the pairs of elements, we can now provide the atom with more favorable electron affinity, higher ionization energy, and larger size: a. More favorable (exothermic) electron affinity: N and Br b. Higher ionization energy: N and Ar c. Larger size: C and Br

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