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Chapter 2: Problem 58

Using the periodic table, predict the charge of the most stable ion of the following elements: \((\mathbf{a}) \mathrm{Li} (\mathbf{b})\) Ba, (c) Po, \((\mathbf{d}) \mathrm{I},\) (e) Sb.

Short Answer

Expert verified
The most stable ions for the elements Li, Ba, Po, I, and Sb will have the following charges: \( (\textrm{a}) \: \mathrm{Li}: +1, (\textrm{b}) \: \mathrm{Ba}: +2, (\textrm{c}) \: \mathrm{Po}: -2, (\textrm{d}) \: \mathrm{I}: -1, (\textrm{e}) \: \mathrm{Sb}: -3\).

Step by step solution

01

1. Locate the Elements in the Periodic Table

First, look at the periodic table to find the group and period for each of the elements Li, Ba, Po, I, and Sb.
02

2. Determine Electron Configurations

Based on their position in the periodic table, find the electron configuration for each element: (a) Li: 1s² 2s¹ (b) Ba: [Xe] 6s² (c) Po: [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p⁴ (d) I: [Kr] 5s² 4d¹⁰ 5p⁵ (e) Sb: [Kr] 5s² 4d¹⁰ 5p³
03

3. Predict the Charges of the Most Stable Ions

Based on the electron configurations, determine how many electrons the element will lose or gain to achieve a stable octet: (a) Li: 2s¹ -> To achieve a stable octet, Li will lose 1 electron from the 2s orbital, resulting in a charge of +1. (b) Ba: 6s² -> To achieve a stable octet, Ba will lose 2 electrons from the 6s orbital, resulting in a charge of +2. (c) Po: 6p⁴ -> To achieve a stable octet, Po will gain 2 electrons in the 6p orbital, resulting in a charge of -2. (d) I: 5p⁵ -> To achieve a stable octet, I will gain 1 electron in the 5p orbital, resulting in a charge of -1. (e) Sb: 5p³ -> To achieve a stable octet, Sb will gain 3 electrons in the 5p orbital, resulting in a charge of -3.
04

4. Summary of Predicted Charges

Based on the electron configurations and periodic trends, the most stable ions for each element will have the following charges: (a) Li: +1 (b) Ba: +2 (c) Po: -2 (d) I: -1 (e) Sb: -3

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Most popular questions from this chapter

Selenium, an element required nutritionally in trace quantities, forms compounds analogous to sulfur. Name the following ions: (a) \(\mathrm{SeO}_{4}^{2-}\), (b) \(\mathrm{Se}^{2-}\), (c) \(\mathrm{HSe}^{-}\), (d) \(\mathrm{HSeO}_{3}^{-}\).

Because many ions and compounds have very similar names, there is great potential for confusing them. Write the correct chemical formulas to distinguish between (a) sodium carbonate and sodium bicarbonate, (b) potassium peroxide and potassium oxide, \((\mathbf{c})\) calcium sulfide and calcium sulfate, \((\mathbf{d})\) manganese (II) oxide and manganese (III) oxide, (e) hydride ion and hydroxide ion, \((\mathbf{f})\) magnesium nitride and magnesium nitrite, \((\mathbf{g})\) silver nitrate and silver nitrite, \((\mathbf{h})\) cuprous oxide and cupric oxide.

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Write the correct symbol, with both superscript and subscript, for each of the following. Use the list of elements in the front inside cover as needed: (a) the isotope of hafnium that contains 106 neutrons, \((\mathbf{b})\) the isotope of mercury with mass number \(201,(\mathbf{c})\) the isotope of rhenium with mass number \(187,(\mathbf{d})\) the isotope of calcium that has an equal number of protons and neutrons.

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