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Chapter 4: Problem 86

Assign oxidation states for all atoms in each of the following compounds. a. $\mathrm{UO}_{2}^{2+} \quad \quad f. \mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}$ b. $\mathrm{As}_{2} \mathrm{O}_{3} \quad \quad g. \mathrm{Na}_{2} \mathrm{P}_{2} \mathrm{O}_{3}$ c. \(\mathrm{NaBiO}_{3} \quad h. \mathrm{Hg}_{2} \mathrm{Cl}_{2}\) d. $\mathrm{As}_{4} \quad\quad \quad i. \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}$ e. \(\mathrm{HAsO}_{2}\)

Short Answer

Expert verified
Short Answer: a. U(+6), O(-2) b. As(+3), O(-2) c. Na(+1), Bi(+5), O(-2) d. As(0) e. H(+1), As(+3), O(-2) f. Mg(+2), P(+5), O(-2) g. Na(+1), P(+2), O(-2) h. Hg(+1), Cl(-1) i. Ca(+2), N(+5), O(-2)

Step by step solution

01

Rule reminder

When assigning oxidation states, follow these rules: 1. The oxidation state of an atom in its elemental state is always 0. 2. The oxidation state of a monatomic ion is equal to its charge. 3. Hydrogen has an oxidation state of +1 (except when bonded to metals where it has an oxidation state of -1). 4. Oxygen has an oxidation state of -2 (except in peroxides, where it is -1). 5. The sum of the oxidation states must equal the overall charge of a compound.
02

a. \(\mathrm{UO}_{2}^{2+}\)

Oxygen has an oxidation state of -2. Two oxygens: 2*(-2) = -4 The overall charge of the compound is +2, so the oxidation state of U must be +6 (thus the sum of all oxidation states is equal to the overall charge: +6-4=+2). Oxidation states: U(+6), O(-2).
03

b. \(\mathrm{As}_{2}\mathrm{O}_{3}\)

Oxygen has an oxidation state of -2. Three oxygens: 3*(-2) = -6 The overall charge of the compound is 0, so the sum of the oxidation states of the two As atoms must be +6 (thus the sum of all oxidation states is equal to the overall charge: 2*(+3) -6=0). Oxidation states: As(+3), O(-2).
04

c. \(\mathrm{NaBiO}_{3}\)

Na has an oxidation state of +1. Oxygen has an oxidation state of -2. Since the overall charge of the compound is 0, Bi's oxidation state is +5 (thus the sum of all oxidation states is equal to the overall charge: +1 +5 -2*3=0). Oxidation states: Na(+1), Bi(+5), O(-2).
05

d. \(\mathrm{As}_{4}\)

Since As is in its elemental state, its oxidation state is 0. Oxidation state: As(0).
06

e. \(\mathrm{HAsO}_{2}\)

Hydrogen has an oxidation state of +1. Oxygen has an oxidation state of -2. Since the overall charge of the compound is 0, As's oxidation state is +3 (thus the sum of all oxidation states is equal to the overall charge: +1 +3 -2*2=0). Oxidation states: H(+1), As(+3), O(-2).
07

f. \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\)

Mg has an oxidation state of +2. Oxygen has an oxidation state of -2. Two Mg atoms: 2*(+2)=+4 Seven oxygens: 7*(-2)=-14 Since the overall charge of the compound is 0, P's oxidation state is +5 (thus the sum of all oxidation states is equal to the overall charge: +4 + 2*(+5) -14=0). Oxidation states: Mg(+2), P(+5), O(-2)
08

g. \(\mathrm{Na}_{2} \mathrm{P}_{2}\mathrm{O}_{3}\)

Na has an oxidation state of +1. Oxygen has an oxidation state of -2. Two Na atoms: 2*(+1)=+2 Three oxygens: 3*(-2)=-6 Since the overall charge of the compound is 0, P's oxidation state is +2 (thus the sum of all oxidation states is equal to the overall charge: +2 + 2*(+2) -6=0). Oxidation states: Na(+1), P(+2), O(-2).
09

h. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\)

Hg and Cl are both in their +1 and -1 oxidation states in this compound (thus the sum of all oxidation states is equal to the overall charge for the compound: 2*(+1) + 2*(-1)=0). Oxidation states: Hg(+1), Cl(-1).
10

i. \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\)

Ca has an oxidation state of +2. In each NO3 group: Oxygen has an oxidation state of -2. Three oxygens: 3*(-2)=-6 Since the overall charge of the NO3 group is -1, N's oxidation state is +5 (thus the sum of all oxidation states is equal to the overall charge: +5 -6=-1). Oxidation states: Ca(+2), N(+5), O(-2).

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Most popular questions from this chapter

Assign the oxidation state for the element listed in each of the following compounds: \(\mathrm{S}\) in \(\mathrm{MgSO}_{4}\)_______ \(\mathrm{Pb}\) in \(\mathrm{PbSO}_{4}\)______ \(\mathrm{O}\) in \(\mathrm{O}_{2}\)___________ \(\mathrm{Ag}\) in Ag _________________________ \(\mathrm{Cu}\) in \(\mathrm{CuCl}_{2}\)_______

A student mixes four reagents together, thinking that the solutions will neutralize each other. The solutions mixed together are 50.0 mL of 0.100 M hydrochloric acid, 100.0 mL of 0.200 M of nitric acid, 500.0 mL of 0.0100 M calcium hydroxide, and 200.0 mL of 0.100 M rubidium hydroxide. Did the acids and bases exactly neutralize each other? If not, calculate the concentration of excess \(\mathrm{H}^{+}\) or \(\mathrm{OH}^{-}\) ions left in solution.

Complete and balance each acid-base reaction. a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow\) Contains three acidic hydrogens b. $\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow$ Contains two acidic hydrogens c. $\mathrm{H}_{2} \operatorname{Se}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow$ Contains two acidic hydrogens d. $\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow$ Contains two acidic hydrogens

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ $$\mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g)$$ A 10.00-g mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture is then reacted with 156 mL of 3.00 M silver nitrate to produce the maximum possible amount of silver chloride. a. Determine the percent magnesium by mass in the original mixture. b. If 78.0 mL of HCl was added, what was the concentration of the HCl?

A \(10.00-\mathrm{mL}\) . sample of vinegar, an aqueous solution of acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right),\) is titrated with \(0.5062 \mathrm{M} \mathrm{NaOH},\) and 16.58 mL is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is \(1.006 \mathrm{g} / \mathrm{cm}^{3},\) what is the mass percent of acetic acid in the vinegar?
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