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Chapter 7: Problem 87

Elements in group 17 in the periodic table are called the halogens; elements in group 16 are called the chalcogens. (a) What is the most common oxidation state of the chalcogens compared to the halogens? (b) For each of the following periodic properties, state whether the halogens or the chalcogens have larger values: atomic radii, ionic radii of the most common oxidation state, first ionization energy, second ionization energy.

Short Answer

Expert verified
(a) The most common oxidation state for chalcogens is -2, while for halogens, it is -1. (b) 1. Halogens have smaller atomic radii compared to chalcogens. 2. Chalcogens have larger ionic radii in their most common oxidation state (-2) than halogens in their most common oxidation state (-1). 3. Halogens have higher first ionization energies compared to chalcogens. 4. Halogens have larger second ionization energies compared to chalcogens.

Step by step solution

01

Part (a): Most Common Oxidation State

To determine the most common oxidation state of elements in group 16 and 17, remember that elements usually achieve the most stable configuration by having a full valence electron shell. Group 16 elements have 6 valence electrons and need to gain 2 more electrons to achieve a stable, full valence electron shell. Thus, the most common oxidation state for chalcogens is -2. On the other hand, Group 17 elements have 7 valence electrons and need to gain only 1 more electron to reach a stable configuration. Therefore, the most common oxidation state for halogens is -1.
02

Part (b): Atomic Radii

As we move across a period (or row) in the periodic table, atomic radii generally decrease because of the increased effective nuclear charge. Since halogens are further to the right in the periodic table compared to chalcogens, halogens have smaller atomic radii.
03

Part (b): Ionic Radii of Most Common Oxidation State

After gaining the electrons, resulting in negatively-charged anions, chalcogens in their -2 oxidation state have a higher electron-repulsion within their outer electron shell compared to halogens with their -1 oxidation state. This causes chalcogens to expand their electron cloud. As a result, chalcogens have larger ionic radii in their most common oxidation state than halogens.
04

Part (b): First Ionization Energy

Ionization energy increases across a period due to an increase in effective nuclear charge. Halogens, being further to the right, have higher effective nuclear charges, thus needing more energy to remove the first electron. Therefore, halogens have higher first ionization energies compared to chalcogens.
05

Part (b): Second Ionization Energy

The second ionization energy refers to the energy required to remove a second electron from the atom. Halogens have a higher effective nuclear charge than chalcogens, meaning that halogens hold onto their electrons more tightly. This makes it harder to remove a second electron from halogens than from chalcogens. So, halogens have larger second ionization energies.

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Most popular questions from this chapter

Write a balanced equation for the reaction that occurs in each of the following cases: (a) White phorphrous, \(\mathrm{P}_{4}(\mathrm{~s})\), reacts with chlorine gas. (b) Sodium metal reacts with water. (c) Hydrogen bromide gas reacts with chlorine gas. (d) Aluminum trichloride reacts with aqueous sodium hydroxide.

Detailed calculations show that the value of \(Z_{\text {eff }}\) for the outermost electrons in \(\mathrm{Na}\) and \(\mathrm{K}\) atoms is \(2.51+\) and \(3.49+\), respectively. (a) What value do you estimate for \(Z_{\text {eff }}\) experienced by the outermost electron in both \(\mathrm{Na}\) and \(\mathrm{K}\) by assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant? (b) What values do you estimate for \(Z_{\text {eff }}\) using Slater's rules? (c) Which approach gives a more accurate estimate of \(Z_{\text {eff }}\) ? (d) Does either method of approximation account for the gradual increase in \(Z_{\text {eff }}\) that occurs upon moving down a group? (e) Predict \(Z_{\text {eff }}\) for the outermost electrons in the \(\mathrm{Rb}\) atom based on the calculations for \(\mathrm{Na}\) and \(\mathrm{K}\).

Tungsten has the highest melting point of any metal in the periodic table: \(3422^{\circ} \mathrm{C}\). The distance between \(\mathrm{W}\) atoms in tungsten metal is 274 pm. (a) What is the atomic radius of a tungsten atom in this environment? (This radius is called the metallic radius.) (b) If you put tungsten metal under high pressure, predict what would happen to the distance between W atoms.

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