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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.

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) calcium sulfide and calcium hydrogen sulfide, (b) hydrobromic acid and bromic acid, (c) aluminum nitride and aluminum nitrite, (d) iron(II) oxide and iron(III) oxide, (e) ammonia and ammonium ion, (f) potassium sulfite and potassium bisulfite, (g) mercurous chloride and mercuric chloride, (h) chloric acid and perchloric acid.

Write the correct symbol, with both superscript and subscript, for each of the following. Use the list of elements inside the front cover as needed: (a) the isotope of platinum that contains 118 neutrons, (b) the isotope of krypton with mass number \(84,(\mathbf{c})\) the isotope of arsenic with mass number \(75,(\mathbf{d})\) the isotope of magnesium that has an equal number of protons and neutrons.

Complete the table by filling in the formula for the ionic compound formed by each pair of cations and anions, as shown for the first pair. $$ \begin{array}{|l|c|c|c|c|} \hline \text { Ion } & \mathrm{Na}^{+} & \mathrm{Ca}^{2+} & \mathrm{Fe}^{2+} & \mathrm{Al}^{3+} \\ \hline \mathrm{O}^{2-} & \mathrm{Na}_{2} \mathrm{O} & & & \\ \hline \mathrm{NO}_{3}^{-} & & & & \\ \hline \mathrm{SO}_{4}{ }^{2-} & & & & \\ \hline \mathrm{AsO}_{4}{ }^{3-} & & & & \\ \hline \end{array} $$

(a) What do ethane and ethanol have in common? (b) How does 1 -propanol differ from propane?
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