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Chapter 7: Problem 115

In each of the following sets, which atom or ion has the smallest radius? a. H, He b. Cl, In, Se c. element 120, element 119, element 116 d. Nb, Zn, Si e. \(\mathrm{Na}^{-}, \mathrm{Na}, \mathrm{Na}^{+}\)

Short Answer

Expert verified
In each of the following sets, the atom or ion with the smallest radius is: a. He b. Cl c. Element 120 d. Si e. \(\mathrm{Na}^{+}\)

Step by step solution

01

Set(a) - H, He

In this set, we have Hydrogen (H) and Helium (He). Both elements are in the first period of the periodic table. Atomic radii decrease from left to right across a period due to increasing nuclear charge. Therefore, Helium (He) has the smallest atomic radius in this set.
02

Set(b) - Cl, In, Se

In this set, we have Chlorine (Cl), Indium (In), and Selenium (Se). Chlorine is in period 3 and group 17, Indium is in period 5 and group 13, and Selenium is in period 4 and group 16. Atomic radii decrease from left to right across a period and increase down a group due to increasing electron shielding. Among these elements, Chlorine (Cl) has the smallest atomic radius.
03

Set(c) - element 120, element 119, element 116

In this set, we have element 120, 119, and 116. As atomic numbers increase, atomic radii generally increase due to added electron shielding. However, the periodic trends play a more significant role in determining atomic radii. Element 116 is in group 16, element 119 is in group 1, and element 120 is in group 2. Atomic radii decrease from left to right across a period, so element 120 (group 2) will have the smallest atomic radius.
04

Set(d) - Nb, Zn, Si

In this set, we have Niobium (Nb), Zinc (Zn), and Silicon (Si). Niobium is in period 5 and group 5, Zinc is in period 4 and group 12, and Silicon is in period 3 and group 14. Atomic radii decrease from left to right across a period and increase down a group. Silicon (Si) is located farthest to the right and highest among these elements, so it has the smallest atomic radius in this set.
05

Set(e) - \(\mathrm{Na}^{-}, \mathrm{Na}, \mathrm{Na}^{+}\)

In this set, we have a sodium anion (Na⁻), a neutral sodium atom (Na), and a sodium cation (Na⁺). Comparing these species, the sodium cation (Na⁺) has lost an electron, resulting in a higher effective nuclear charge and a smaller atomic radius. Conversely, the sodium anion (Na⁻) has gained an electron, leading to increased electron shielding and a larger atomic radius. Thus, the sodium cation (Na⁺) has the smallest atomic radius in this set.

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