Deck 21: Chemistry of the Nonmetals

Question 1

Which of the following elements is the strongest oxidizing agent?

A) N₂
B) O₂
C) F₂
D) Cl₂
E) P₄

Answer 1

F₂

Question 2

What is the overall reaction for the disproportionation of hydrogen peroxide in water?

A) H₂O₂(aq)→ 2OH−(aq)
B) H₂O₂(aq)→ O₂(g)+ H₂(g)
C) 2H₂O₂(aq)→ O₂(g)+ 2H₂O(l)
D) H₂O₂(aq)→ O₂(g)+ 2H⁺(aq)
E) H₂O₂(aq)+ H₂O(l)→ 4H⁺(aq)+ O₃(g)

Answer 2

2H₂O₂(aq)→ O₂(g)+ 2H₂O(l)

Question 3

Fluorine and chlorine gases are primarily produced by

A) distillation.
B) oxidation by electrolysis.
C) oxidation by hydronium ion.
D) reduction by carbon monoxide.
E) roasting with copper(II)sulfide.

Answer 3

oxidation by electrolysis.

Question 4

Hydrazine is made commercially by reacting aqueous ammonia with hypochlorite ion.Write a balanced equation for this reaction.

A) 2NH₃(aq)+ ClO₄−(aq)→ N₂H₄(aq)+ ClO₃−(aq)+ H₂O(l)
B) 2NH₃(aq)+ ClO₃−(aq)→ N₂H₄(aq)+ ClO₂−(aq)+ H₂O(l)
C) 2NH₃(aq)+ ClO₂−(aq)→ N₂H₄(aq)+ Cl−(aq)+ H₂O₂(aq)
D) 2NH₃(aq)+ ClO−(aq)→ N₂H₄(aq)+ Cl−(aq)+ H₂O(l)
E) 2NH₃(aq)+ ClO−(aq)→ N₂H₄(aq)+ H₂(aq)+ ClO−(aq)

Question 5

Write a balanced chemical equation for the reaction of hydrogen peroxide and iodide ion in an acidic solution.

A) H₂O₂(aq)+ 2I−(aq)+ 2H⁺(aq)→ I₂(s)+ 2H₂O(l)
B) H₂O₂(aq)+ 2I−(aq)→ I₂(s)+ 2OH−(aq)
C) H₂O₂(aq)+ I₂(s)→ 2I−(aq)+ H₂(g)+ O₂(g)
D) H₂O₂(aq)+ I₂(s)+ 2H⁺(aq)→ 2HI(s)+ 2OH−(aq)
E) H₂O₂(aq)+ 2I−(aq)→ I₂(s)+ H₂(g)+ O₂(g)

Question 6

Write a balanced net ionic equation for the reaction of chlorine gas with aqueous potassium iodide.

A) Cl₂(g)+ 2KI(aq)→ 2KCl(s)+ I₂(aq)
B) Cl₂(g)+ 2I−(aq)→ 2ICl(aq)
C) Cl₂(g)+ 2I−(aq)→ 2Cl−(aq)+ I₂(aq)
D) Cl₂(g)+ 2I−(aq)→ Cl₂I(aq)+ I−(aq)
E) Cl₂(g)+ K⁺(aq)+ I−(aq)→ KCl(s)+ ICl(g)

Question 7

Which of the following reactions represents the disproportionation of chlorine in water?

A) Cl₂(g)+ H₂O(l) ? Cl?(aq)+ H₂(g)+ ClO⁺(aq)
B) Cl₂(g)+ H₂O(l) ? Cl?(aq)+ H⁺(aq)+ HClO(aq)
C) Cl₂(g)+ H₂O(l) ? Cl?(aq)+ HCl(aq)+ OH?(aq)
D) Cl₂(g)+ 2H₂O(l) ? Cl?(aq)+ 3H⁺(aq)+ HClO₂(aq)
E) Cl₂(g)+ 4H₂O(l) ? Cl?(aq)+ 8H⁺(aq)+ ClO₄?(aq)

Question 8

Write a balanced chemical equation for the reaction of aqueous solutions of hydrofluoric acid and potassium carbonate.

A) 2HF(aq)+ CO₃²⁻(aq)→ CO₂(g)+ H₂O(l)+ 2F−(aq)
B) 2HF(aq)+ K₂CO₃(aq)→ F₂CO₃(s)+ H₂(g)
C) 2HF(aq)+ K₂CO₃(s)→ 2KF(s)+ H₂CO₃(s)
D) 2H⁺(aq)+ CO₃²⁻(aq)→ H₂CO₃(s)
E) 2H⁺(aq)+ CO₃²⁻(aq)→ CO₂(g)+ H₂O(l)

Question 9

Which of the following elements is the least chemically reactive?

A) N₂
B) O₂
C) F₂
D) Cl₂
E) P₄

Question 10

Write a half-reaction for the oxidation of hydrogen peroxide.

A) H₂O₂(aq)→ 2OH−(aq)+ 2e−
B) H₂O₂(aq)→ H₂(g)+ O₂(g)
C) H₂O₂(aq)→ H₂(g)+ O₂(g)+ 2e−
D) 2H₂O₂(aq)→ O₂(g)+ 2H₂O(l)+ 2e−
E) H₂O₂(aq)→ O₂(g)+ 2H⁺(aq)+ 2e−

Question 11

Which of the halogens are solids at 298 K and 1 atmosphere?

A) Cl₂
B) Br₂
C) I₂
D) Cl₂ and Br₂
E) Br₂ and I₂

Question 12

Which of the following nitrogen containing compounds or ions is not capable of acting as an oxidizing agent?

A) NO₃−
B) NO₂−
C) NH₃
D) N₂
E) NO₂

Question 13

What intermolecular bonds or forces are present in P₄(s)?

A) Hydrogen bonds
B) Covalent bonds
C) Ionic bonds
D) Dipole forces
E) Dispersion forces

Question 14

Which of the following molecules is a product of most chemical explosives?

A) H₂
B) N₂
C) O₂
D) SO₂
E) HCl

Question 15

All of the following oxidation states are observed for sulfur EXCEPT _____.

A) −2
B) +2
C) +4
D) +6
E) +7

Question 16

Which of the following lists of nonmetals contains only elements that can be found in nature in their elemental forms?

A) Chlorine,nitrogen,oxygen
B) Silicon,arsenic,sulfur
C) Nitrogen,phosphorus,arsenic
D) Bromine,carbon,oxygen
E) Nitrogen,oxygen,sulfur

Question 17

Write a balanced equation for the reaction of gaseous ammonia with hydrogen chloride.

A) NH₃(g)+ HCl(g)→ NH₂Cl(g)+ H₂(g)
B) NH₃(g)+ HCl(g)→ NH₄Cl(s)
C) NH₃(g)+ 3HCl(g)→ NCl₃(g)+ 3H₂(g)
D) NH₃(g)+ 2HCl(g)→ NH₅(g)+ Cl₂(g)
E) 2NH₃(g)+ 2HCl(g)→ N₂(g)+ 4H₂(g)+ Cl₂(g)

Question 18

Write a half-reaction for the reduction of aqueous hydrogen peroxide in an acidic solution.

A) H₂O₂(aq)+ 2e− → H₂(g)+ O₂²⁻(aq)
B) 2H₂O₂(aq)+ 2e− → O₂(g)+ 2H₂O(l)
C) H₂O₂(aq)+ 2e− → 2OH−(aq)
D) H₂O₂(aq)+ 2H⁺(aq)+ 2e− → 2H₂O(l)
E) Hydrogen peroxide cannot be reduced under acidic conditions.

Question 19

What is the molecular formula for chlorous acid?

A) HCl
B) HClO
C) H₂ClO
D) HClO₂
E) HClO₃

Question 20

Which of the following acids is never stored in glass containers because it reacts with silicon dioxide and ionic silicates?

A) HNO₃
B) HClO₄
C) H₂SO₄
D) HF
E) HI

Question 21

Which reddish-brown gas is a major factor in the formation of photochemical smog?

A) NO
B) NO₂
C) SO₂
D) CO₂
E) CO

Question 22

Which of the following nitrogen containing compounds is not able to act as an oxidizing agent?

A) HNO₃
B) NH₃
C) HNO₂
D) N₂H₄
E) All of the above can act as oxidizing agents.

Question 23

Place the following acids in order from smallest to largest K_a value: HClO,HBrO,and HIO.

A) HClO < HBrO < HIO
B) HClO < HIO < HBrO
C) HBrO < HClO < HIO
D) HBrO < HIO < HClO
E) HIO < HBrO < HClO

Question 24

Which of the following oxoanions of chlorine cannot act as an oxidizing agent?

A) HClO
B) HClO₂
C) HClO₃
D) HClO₄
E) All of the above can act as oxidizing agents.

Question 25

The standard reduction potential of H₂O₂ = +1.763 V.Which of the following species will be oxidized by hydrogen peroxide? $\begin{array}{l}\begin{array}{l}\\\mathrm{Co}^{2+}(a q) \rightarrow \mathrm{Co}^{3+}(a q)+2 e \\\Lambda \mathrm{g}(s) \rightarrow \mathrm{Ag}^{\prime}(a q)+e^{-} \\\mathrm{Co}(s) \rightarrow \mathrm{Co}^{2+}(a q)+2 e \\\mathrm{Zn}(s) \rightarrow \mathrm{Zn}^{2+}(a q)+2 e^{-} \\\mathrm{Na}(s) \rightarrow \mathrm{Na}^{+}(a q)+e-\end{array}\begin{array}{l} E_{\mathrm{red}}^{\circ} \\+1.953 \mathrm{~V} \\+0.799 \mathrm{~V} \\-0.282 \mathrm{~V} \\-0.762 \mathrm{~V} \\-2.714 \mathrm{~V}\end{array}\end{array}$

A) Co²⁺
B) Co²⁺ and Ag(s)
C) Co(s)and Co²⁺
D) Zn(s)and Na(s)
E) Ag(s),Co(s),Zn(s),and Na(s)

Question 26

Write a balanced chemical equation for the oxidation of chromium metal with nitric acid.Assume the reaction products are Cr³⁺ and NH₄⁺.

A) H⁺(aq)+ NO₃−(aq)+ Cr(s)→ NH₄⁺(aq)+ Cr³⁺(aq)
B) 4H⁺(aq)+ NO₃−(aq)+ Cr(s)→ NH₄⁺(aq)+ Cr³⁺(aq)
C) 10H⁺(aq)+ NO₃−(aq)+ 3Cr(s)→ NH₄⁺(aq)+ 3Cr³⁺(aq)+ 3H₂O(l)
D) 10H⁺(aq)+ NO₃−(aq)+ Cr(s)→ NH₄⁺(aq)+ Cr³⁺(aq)+ 3H₂O(l)
E) 30H⁺(aq)+ 3NO₃−(aq)+ 8Cr(s)→ 3NH₄⁺(aq)+ 8Cr³⁺(aq)+ 9H₂O(l)

Question 27

Which of the following molecules has the ability to dilate blood vessels,thereby lowering blood pressure?

A) NO
B) N₂O
C) CO
D) HCl
E) SO₃

Question 28

Write a balanced chemical equation for the oxidation of iron metal with nitric acid.Assume the reaction products are Fe³⁺ and NO gas.

A) Fe(s)+ NO₃−(aq)→ Fe³⁺(aq)+ NO(g)+ O₂(g)
B) Fe(s)+ HNO₃(aq)→ Fe³⁺(aq)+ NO(g)+ OH−(aq)
C) Fe(s)+ 4H⁺(aq)+ NO₃−(aq)→ Fe³⁺(aq)+ NO(g)+ 2H₂O(l)
D) Fe(s)+ H⁺(aq)+ NO₃−(aq)→ Fe³⁺(aq)+ NO(g)+ O₂H−(aq)
E) 2Fe(s)+ 12H⁺(aq)+ 3NO₃−(aq)→ 2Fe³⁺(aq)+ 3NO(g)+ 6H₂O(l)

Question 29

The first step in the synthesis of nitric acid involves the reaction of ammonia with oxygen to produce nitrogen monoxide. 4NH₃(g)+ 5O₂(g)→ 4NO(g)+ 6H₂O(g)
What volume of NO is produced if 14.0 L NH₃ is reacted with 15.0 L O₂? Assume the reaction is 100% efficient.

A) 12.0 L
B) 14.0 L
C) 15.0 L
D) 23.2 L
E) 29.0 L

Question 30

Which of the following molecules are paramagnetic: N₂O,NO,and NO₂?

A) N₂O only
B) NO only
C) NO₂ only
D) N₂O and NO
E) NO and NO₂

Question 31

Which of the following oxoacids has the largest K_a value?

A) HClO₄
B) HClO₃
C) HClO₂
D) HClO
E) All of the above oxoacids have similar K_a values.

Question 32

Write a balanced chemical equation for the reaction of sulfur trioxide with water.

A) SO₃(g)+ H₂O(l)→ S(s)+ H₂(g)+ 2O₂(g)
B) SO₃(g)+ H₂O(l)→ H₂SO₃(aq)
C) SO₃(g)+ H₂O(l)→ SO₂(g)+ H₂O₂(g)
D) SO₃(g)+ H₂O(l)→ H₂S(aq)+ 2O₂(g)
E) SO₃(g)+ H₂O(l)→ H₂SO₄(aq)

Question 33

Calculate the pH of a 0.35 M solution of sodium hypobromite,NaClO.The acid dissociation constant for HBrO is 2.6 × 10−⁹.

A) 2.94
B) 4.96
C) 8.13
D) 9.04
E) 11.06

Question 34

Write a balanced chemical equation for the reaction of dinitrogen trioxide with water.

A) N₂O₃(g)+ H₂O(l)→ N₂O₄(g)+ H₂(g)
B) N₂O₃(g)+ H₂O(l)→ 2HNO₂(aq)
C) N₂O₃(g)+ 3H₂O(l)→ 2HNO₃(aq)+ 2H₂(g)
D) N₂O₃(g)+ H₂O(l)→ N₂H₂(g)+ 2O₂(g)
E) N₂O₃(g)+ 3H₂O(l)→ 2NH₃(g)+ 3O₂(g)

Question 35

In which of the following compounds does phosphorus have an oxidation number of +3?

A) P₄S₃
B) H₃PO₃
C) H₃PO₄
D) P₄O₁₀
E) PH₃

Question 36

Nonmetal oxides react with water to form

A) solids.
B) fullerenes.
C) Lewis bases.
D) Brønsted-Lowry acids.
E) precipitates.

Question 37

Write a balanced chemical equation for the combustion of white phosphorus.

A) P₄(s)+ 8O₂(g)→ 4PO₄(g)
B) P₄(s)+ 3O₂(g)→ 2P₂O₃(s)
C) P₄(s)+ 5O₂(g)→ P₄O₁₀(s)
D) P₄(s)+ 8O₂(g)→ 4PO₄³⁻(g)
E) P₄(s)+ O₂(g)→ 2P₂O(g)

Question 38

H₃PO₄ is a weak,triprotic acid.The acid dissociation constants are K_a1 = 7.1 × 10?³,K_a2 = 6.2 × 10?⁸,and K_a3 = 4.5 × 10?¹³.Calculate the equilibrium constant for the reaction below. H₃PO₄(aq) ? PO₄^3?(aq)+ 3H⁺(aq)

A) 2.0 × 10?²²
B) 4.4 × 10?¹⁰
C) 2.0 × 10?⁸
D) 8.7 × 10?⁶
E) 7.1 × 10?³

Question 39

Write a balanced chemical equation for the reaction of N₂O₅ and water.

A) N₂O₅(s)+ H₂O(l)→ N₂O₄(s)+ H₂O₂(l)
B) N₂O₅(s)+ H₂O(l)→ N₂O(g)+ H₂O(l)+ 2O₂(g)
C) N₂O₅(s)+ 3H₂O(l)→ NH₃(g)+ 4O₂(g)
D) N₂O₅(s)+ H₂O(l)→ 2HNO₃(l)
E) N₂O₅(s)+ H₂O(l)→ 2HNO₂(l)+ O₂(g)

Question 40

Write a balanced chemical equation for the disproportionation of chlorate ion in water.The products are chloride and perchlorate ions.

A) 2ClO₃−(aq)+ H₂O(l)→ Cl−(aq)+ ClO₄−(aq)+ 2H⁺(aq)
B) 3ClO₃−(aq)+ 2H₂O(l)→ Cl−(aq)+ 2ClO₄−(aq)+ 4H⁺(aq)
C) 4ClO₃−(aq)→ Cl−(aq)+ 3ClO₄−(aq)
D) 4ClO₃−(aq)→ 2ClO₂−(aq)+ 2ClO₄−(aq)
E) 5ClO₃−(aq)+ 6H⁺(aq)→ 2Cl−(aq)+ 3ClO₄−(aq)+ 3H₂O(l)

Question 41

Write a balanced equation for the reaction of Al³⁺ with aqueous ammonia.

A) Al³⁺(aq)+ 2NH₃(aq)→ Al(s)+ 3H₂(g)+ N₂(g)
B) Al³⁺(aq)+ 3NH₃(aq)+ 3H₂O(l)→ Al(OH)₃(s)+ 3NH₄⁺(aq)
C) Al³⁺(aq)+ 2NH₃(aq)→ Al(NH₃)₂³⁺(aq)
D) Al³⁺(aq)+ 3NH₃(aq)+ 3H⁺(aq)→ Al(NH₄)₃⁶⁺(aq)
E) Al³⁺(aq)+ 6NH₃(aq)→ Al(NH₃)₆³⁺(aq)

Question 42

Write a balanced equation for the reaction of Ni²⁺ with H₂S.

A) Ni²⁺(aq)+ 2H₂S(aq)→ Ni(HS)₂(s)+ 2H⁺(aq)
B) Ni²⁺(aq)+ H₂S(aq)→ NiH₂(s)+ S²⁻(aq)
C) Ni²⁺(aq)+ H₂S(aq)→ NiS(s)+ 2H⁺(aq)
D) Ni²⁺(aq)+ H₂S(aq)→ Ni(s)+ S(s)+ 2H⁺(aq)
E) No reaction will occur.

Question 43

All of the following statements concerning oxoanions and oxoacids are true EXCEPT

A) MnO₄− can never act as an oxidizing agent.
B) Cr₂O₇²⁻ can never act as a reducing agent.
C) ClO₄− is a stronger oxidizing agent than ClO−.
D) ClO₂− can behave as either an oxidizing or a reducing agent.
E) HClO₃ is a stronger acid than HClO₂.

Question 44

Hydrogen sulfide is used to remove sulfur dioxide in power plant smokestacks.The reaction produces elemental sulfur and water.Write a balanced chemical equation for this reaction.

A) H₂S(l)+ SO₂(g)→ 2HSO(s)
B) H₂S(l)+ SO₂(g)→ 2S(s)+ 2OH−(aq)
C) 2H₂S(l)+ SO₂(g)→ 3S(s)+ 2H₂O(l)
D) H₂S(l)+ SO₂(g)→ 2S(s)+ H₂O₂(aq)
E) H₂S(l)+ SO₂(g)+ 2H⁺(aq)→ 2S(s)+ 2H₂O(l)

Question 45

The average concentration of bromine (as bromide)in seawater is 65 ppm.Calculate the volume of seawater (d = 64.0 lb/ft³)in cubic feet required to produce one kilogram of liquid bromine.

A) 109 ft³
B) 448 × 10³ ft³
C) 240 ft³
D) 154 × 10² ft³
E) 529 ft³

Question 46

Write a balanced equation for the reaction of table sugar,C₁₂H₂₂O₁₁,with concentrated sulfuric acid.

A) C₁₂H₂₂O₁₁(s)→ 12C(s)+ 11H₂O(l)
B) C₁₂H₂₂O₁₁(s)+ H₂SO₄(aq)→ C₁₂H₂₃O₁₁⁺(s)+ HSO₄−(aq)
C) C₁₂H₂₂O₁₁(s)+ H₂SO₄(aq)+ 6O₂(g)→ 12CO₂(g)+ SO₂(g)+ H₂O(l)
D) C₁₂H₂₂O₁₁(s)+ 2H⁺(aq)+ SO₄²⁻(aq)→ C₁₂H₂₄O₁₁²⁺(s)+ SO₄²⁻(aq)
E) C₁₂H₂₂O₁₁(s)+ 2H⁺(aq)+ SO₄²⁻(aq)→ 12CO(g)+ SO₂(g)+ 2OH⁺(aq)+ H₂O(l)

Question 47

Nitric acid solutions slowly turn brown when exposed to sunlight.Which of the following reactions is responsible?

A) NO₃−(aq)→ NO(g)+ O₂(g)
B) 2NO₃−(aq)→ 2NO₂(g)+ O₂(g)
C) 2H⁺(aq)+ NO₃−(aq)→ NO₂(g)+ H₂O(l)
D) 4H⁺(aq)+ 4NO₃−(aq)→ 4NO₂(g)+ 2H₂O(l)+ O₂(g)
E) 4H⁺(aq)+ NO₃−(aq)→ NO(g)+ 2H₂(g)+ O₂(g)

Question 48

Which of the following compounds will react with water to produce a basic solution: NH₃,H₂O₂,and H₂S?

A) NH₃ only
B) H₂O₂ only
C) H₂S only
D) NH₃ and H₂S
E) H₂O₂ and H₂S

Question 49

Write a balanced equation for the reaction of concentrated sulfuric acid with copper metal.Assume two products are sulfur dioxide and Cu²⁺.

A) Cu(s)+ SO₄²⁻(aq)→ Cu²⁺(aq)+ O₂(g)+ SO₂(g)
B) Cu(s)+ 4H⁺(aq)+ SO₄²⁻(aq)→ CuS(s)+ 2O₂(g)
C) Cu(s)+ 2H⁺(aq)+ SO₄²⁻(aq)→ Cu²⁺(aq)+ H₂O(l)+ SO₂(g)
D) Cu(s)+ 4H⁺(aq)+ SO₄²⁻(aq)→ Cu²⁺(aq)+ 2H₂O(l)+ SO₂(g)
E) Cu(s)+ 8H⁺(aq)+ SO₄²⁻(aq)→ Cu²⁺(aq)+ 4H₂O(l)+ S(g)

Question 50

Which of the following statements is INCORRECT?

A) Sodium dihydrogen phosphate,NaH₂PO₄,is used in acidic cleaners.
B) Sodium phosphate,Na₃PO₄,is used in strongly basic cleaners.
C) Calcium dihydrogen phosphate,Ca(H₂PO₄)₂ is used in fertilizers.
D) The principal use of Na₂HPO₄ is as an emulsifier in the manufacture of cheese.
E) Phosphoric acid is a strong acid,a powerful oxidizing agent,and a drying agent.

Question 51

In modern forensic laboratories,arsenic poisoning is detected by testing

A) a strand of hair.
B) samples of brain tissue.
C) samples of liver tissue.
D) heart tissue.
E) bone fragments.

Question 52

As one might predict,one allotrope of arsenic has the formula

A) As₄
B) As₈
C) As₂
D) As₃
E) As₁₀