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Chapter 2: Problem 70

Give the names and charges of the cation and anion in each of the following compounds: (a) CuS, (b) \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) (c) \(\mathrm{Al}\left(\mathrm{ClO}_{3}\right)_{3},(\mathbf{d}) \mathrm{Co}(\mathrm{OH})_{2},(\mathbf{e}) \mathrm{PbCO}_{3}\)

Short Answer

Expert verified
(a) CuS: Cu²⁺ (cation), S²⁻ (anion); (b) \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\): Ag⁺ (cation), SO₄²⁻ (anion); (c) \(\mathrm{Al}\left(\mathrm{ClO}_{3}\right)_{3}\): Al³⁺ (cation), ClO₃⁻ (anion); (d) \(\mathrm{Co}(\mathrm{OH})_{2}\): Co²⁺ (cation), OH⁻ (anion); (e) \(\mathrm{PbCO}_{3}\): Pb²⁺ (cation), CO₃²⁻ (anion).

Step by step solution

01

(a) CuS

CuS is a compound composed of copper (Cu) and sulfur (S). In this compound, copper acts as the cation and sulfur as the anion. Copper can have multiple oxidation states, but in this case, it's in the +2 oxidation state, giving it a charge of +2 (Cu²⁺). Sulfur, as the anion, has a -2 charge (S²⁻).
02

(b) \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\)

The compound \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) is composed of silver (Ag) cations and sulfate (SO₄) anions. Silver has only one oxidation state, +1, so the cation will have a +1 charge (Ag⁺). The sulfate anion has a -2 charge (SO₄²⁻).
03

(c) \(\mathrm{Al}\left(\mathrm{ClO}_{3}\right)_{3}\)

In the compound \(\mathrm{Al}\left(\mathrm{ClO}_{3}\right)_{3}\), the cation is aluminum (Al) with a +3 charge (Al³⁺) and the anion is chlorate (ClO₃) with a -1 charge (ClO₃⁻).
04

(d) \(\mathrm{Co}(\mathrm{OH})_{2}\)

For the compound \(\mathrm{Co}(\mathrm{OH})_{2}\), the cation is cobalt (Co) and the anion is the hydroxide ion (OH). Cobalt can have different oxidation states, but in this case, it has a +2 charge (Co²⁺). The hydroxide ion has a -1 charge (OH⁻).
05

(e) \(\mathrm{PbCO}_{3}\)

The compound \(\mathrm{PbCO}_{3}\) consists of lead (Pb) as the cation and the carbonate ion (CO₃) as the anion. Lead can have various oxidation states; in this instance, it has a +2 charge (Pb²⁺). The carbonate ion has a -2 charge (CO₃²⁻).

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Most popular questions from this chapter

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

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