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Chapter 4: Problem 198

Of the following atoms, which has the largest first ionization energy? (a) \(\mathrm{Br}\) (b) \(\overline{\mathrm{O}}\) (c) \(\mathrm{C}\) (d) \(\mathrm{P}\) (e) I

Short Answer

Expert verified
The atom with the largest first ionization energy is (b) \(\overline{\mathrm{O}}\) (Oxygen).

Step by step solution

01

Identify the positions of the given elements on the periodic table.

Locate the positions of Br (Bromine), O (Oxygen), C (Carbon), P (Phosphorus), and I (Iodine) on the periodic table. Br is in group 17 and period 4. O is in group 16 and period 2. C is in group 14 and period 2. P is in group 15 and period 3. I is in group 17 and period 5.
02

Compare the ionization energies based on periodic trends.

Recall that ionization energy generally increases as we move from left to right within a period and decreases as we move from top to bottom within a group. Based on the left-to-right trend, C (group 14) will have a higher ionization energy than P (group 15), and O (group 16) will have a higher ionization energy than C (group 14). Based on the top-to-bottom trend, O (period 2) will have a higher ionization energy than P (period 3). Now, compare Br and I which are both in group 17. According to the top-to-bottom trend, Br (period 4) will have a higher ionization energy than I (period 5).
03

Determine the atom with the largest ionization energy.

Since O has a higher ionization energy than C and P, and Br has a higher ionization energy than I, we only need to compare O and Br. O (in period 2) is above Br (in period 4), so according to the top-to-bottom trend, O will have a higher ionization energy than Br. So, out of the given atoms, O (Oxygen) has the largest first ionization energy. The answer is (b) \(\overline{\mathrm{O}}\).

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