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Chapter 3: Problem 110

Write the formula for each of the following compounds: a. chromium(III) hydroxide b. magnesium cyanide c. lead(IV) carbonate d. ammonium acetate

Short Answer

Expert verified
The chemical formulas for the given compounds are: a. chromium(III) hydroxide: \[Cr(OH)_3\] b. magnesium cyanide: \[Mg(CN)_2\] c. lead(IV) carbonate: \[Pb(CO_3)_2\] d. ammonium acetate: \[(NH_4)(CH_3COO)\]

Step by step solution

01

a. chromium(III) hydroxide

1. Identify the cation and the anion Chromium(III) is the cation and has a charge of +3. Hydroxide (OH) is the anion and has a charge of -1. 2. Balance the charges To balance the charges in the compound, we need to find the lowest common multiple of the charges. In this case, it's 3. So, we need one chromium(III) ion and three hydroxide ions. 3. Write the formula The formula for chromium(III) hydroxide is: \[Cr(OH)_3\]
02

b. magnesium cyanide

1. Identify the cation and the anion Magnesium (Mg) is the cation and has a charge of +2. Cyanide (CN) is the anion and has a charge of -1. 2. Balance the charges To balance the charges in the compound, we need the lowest common multiple of the charges, which in this case is 2. We need one magnesium ion and two cyanide ions. 3. Write the formula The formula for magnesium cyanide is: \[Mg(CN)_2\]
03

c. lead(IV) carbonate

1. Identify the cation and the anion Lead(IV) is the cation and has a charge of +4. Carbonate (CO_3) is the anion and has a charge of -2. 2. Balance the charges To balance the charges in the compound, we need the lowest common multiple of the charges, which in this case is 4. We need one lead(IV) ion and two carbonate ions. 3. Write the formula The formula for lead(IV) carbonate is: \[Pb(CO_3)_2\]
04

d. ammonium acetate

1. Identify the cation and the anion Ammonium (NH_4) is the cation and has a charge of +1. Acetate (CH_3COO) is the anion and has a charge of -1. 2. Balance the charges In this case, the charges are already balanced with one ammonium ion and one acetate ion. 3. Write the formula The formula for ammonium acetate is: \[(NH_4)(CH_3COO)\]

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Most popular questions from this chapter

Without using Fig. \(3-4,\) predict the order of increasing electronegativity in each of the following groups of elements. a. \(\mathrm{Na}, \mathrm{K}, \mathrm{Rb}\) \(\mathbf{b} . \mathbf{B}, \mathbf{O}, \mathbf{G a}\) c. \(F, C\), \(B r\) d. \(s, O, F\)

Which member of the following pairs would you expect to be more energetically stable? Justify each choice. a. NaBr or \(\mathrm{NaBr}_{2}\) b. \(\mathrm{ClO}_{4}\) or \(\mathrm{ClO}_{4}^{-}\) c. \(\mathrm{SO}_{4}\) or \(\mathrm{XeO}_{4}\) d. \(\mathrm{OF}_{4}\) or \(\mathrm{SeF}_{4}\)

Name each of the following compounds. Assume the acids are dissolved in water. a. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) b. \(\mathrm{NH}_{4} \mathrm{NO}_{2}\) c. \(\mathrm{Co}_{2} \mathrm{S}_{3}\) d. ICl e. \(\mathrm{Pb}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) f. \(\mathrm{KClO}_{3}\) g. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) \(\mathbf{h} . \mathrm{Sr}_{3} \mathrm{N}_{2}\) i. \(\quad \mathrm{Al}_{2}\left(\mathrm{SO}_{3}\right)_{3}\) J. \(\mathrm{SnO}_{2}\) \(\mathbf{k} . \mathrm{Na}_{2} \mathrm{CrO}_{4}\) I. \(\mathrm{HClO}\)

Given the following information: Energy of sublimation of \(\mathrm{Li}(s)=166 \mathrm{kJ} / \mathrm{mol}\) Bond energy of \(\mathrm{HCl}=427 \mathrm{kJ} / \mathrm{mol}\) Ionization energy of \(\mathrm{Li}(g)=520 . \mathrm{kJ} / \mathrm{mol}\) Electron affinity of \(\mathrm{Cl}(g)=-349 \mathrm{kJ} / \mathrm{mol}\) Lattice energy of \(\mathrm{LiCl}(s)=-829 \mathrm{kJ} / \mathrm{mol}\) Bond energy of \(\mathrm{H}_{2}=432 \mathrm{kJ} / \mathrm{mol}\) Calculate the net change in energy for the following reaction: $$ 2 \mathrm{Li}(s)+2 \mathrm{HCl}(g) \longrightarrow 2 \mathrm{LiCl}(s)+\mathrm{H}_{2}(g) $$

Write electron configurations for a. the cations \(\mathrm{Sr}^{2+}, \mathrm{Cs}^{+}, \mathrm{In}^{+},\) and \(\mathrm{Pb}^{2+}\) b. the anions \(P^{3-}, S^{2-},\) and \(B r^{-}\)
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