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Chapter 2: Problem 61

Give the chemical formula for (a) chlorite ion, (b) chloride ion, (c) chlorate ion, (d) perchlorate ion, (e) hypochlorite ion.

Short Answer

Expert verified
The chemical formulas for the different chlorine-based ions are as follows: (a) Chlorite ion: \(ClO_2^-\) (b) Chloride ion: \(Cl^-\) (c) Chlorate ion: \(ClO_3^-\) (d) Perchlorate ion: \(ClO_4^-\) (e) Hypochlorite ion: \(ClO^-\)

Step by step solution

01

(a) Chlorite ion

The chlorite ion has the chlorine in an oxidation state of +3. To find the formula for the chlorite ion, we need to balance the charges between the chlorine atom and the oxygen atoms that it is bonded to. Because the oxygen atom has a charge of -2 and we need to reach a total charge of -1 for the ion, the formula for the chlorite ion becomes ClO2^-.
02

(b) Chloride ion

The chloride ion has the chlorine in an oxidation state of -1. In this case, there are no oxygen atoms bonded to the chlorine atom. Thus, the formula for the chloride ion is simply Cl^-.
03

(c) Chlorate ion

The chlorate ion has the chlorine in an oxidation state of +5. To find the formula for the chlorate ion, we need to balance the charges between the chlorine atom and the oxygen atoms that it is bonded to. Due to the oxygen atom having a charge of -2 and we need to obtain a total charge of -1 for the ion, the formula for the chlorate ion becomes ClO3^-.
04

(d) Perchlorate ion

The perchlorate ion has the chlorine in an oxidation state of +7. To find the formula for the perchlorate ion, we need to balance the charges between the chlorine atom and the oxygen atoms that it is bonded to. With the oxygen atom having a charge of -2 and the aim of reaching a total charge of -1 for the ion, the formula for the perchlorate ion becomes ClO4^-.
05

(e) Hypochlorite ion

The hypochlorite ion has the chlorine in an oxidation state of +1. To find the formula for the hypochlorite ion, we need to balance the charges between the chlorine atom and the oxygen atoms that it is bonded to. Due to the oxygen atom having a charge of -2 and meeting a total charge of -1 for the ion, the formula for the hypochlorite ion becomes ClO^-.

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Most popular questions from this chapter

Assume that you encounter the following sentences in your reading. What is the chemical formula for each substance mentioned? (a) Sodium hydrogen carbonate is used as a deodorant. (b) Calcium hypochlorite is used in some bleaching solutions. (c) Hydrogen cyanide is a very poisonous gas. (d) Magnesium hydroxide is used as a cathartic. (e) \(\operatorname{Tin}(\mathrm{II})\) fluoride has been used as a fluoride additive in toothpastes. (f) When cadmium sulfide is treated with sulfuric acid, fumes of hydrogen sulfide are given off.

(a) Define atomic number and mass number. (b) Which of these can vary without changing the identity of the element?

Name each of the following oxides. Assuming that the compounds are ionic, what charge is associated with the metallic element in each case? (a) \(\mathrm{NiO},(\mathbf{b}) \mathrm{MnO}_{2},\) (c) \(\mathrm{Cr}_{2} \mathrm{O}_{3},(\mathrm{~d}) \mathrm{MoO}_{3}\).

Name the following ionic compounds: (a) \(\mathrm{Li}_{2} \mathrm{O},\) (b) \(\mathrm{FeCl}_{3}\), (c) \(\mathrm{NaClO}\) (d) \(\mathrm{CaSO}_{3}\), (e) \(\mathrm{Cu}(\mathrm{OH})_{2},\) (f) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\), (g) \(\mathrm{Ca}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\), (h) \(\mathrm{Cr}_{2}\left(\mathrm{CO}_{3}\right)_{3}\) (i) \(\mathrm{K}_{2} \mathrm{CrO}_{4},(\mathrm{j})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\)

The natural abundance of \({ }^{3} \mathrm{He}\) is \(0.000137 \% .\) (a) How many protons, neutrons, and electrons are in an atom of \({ }^{3}\) He? (b) Based on the sum of the masses of their subatomic particles, which is expected to be more massive, an atom of \({ }^{3}\) He or an atom of \({ }^{3} \mathrm{H}\) (which is also called tritium)? (c) Based on your answer to part (b), what would need to be the precision of a mass spectrometer that is able to differentiate between peaks that are due to \({ }^{3} \mathrm{He}^{+}\) and \({ }^{3} \mathrm{H}^{+}\) ?
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