Deck 22: Nonmetallic Elements and Their Compounds

Question 1

When liquid phosphorus trichloride reacts with water, the products are

A) PCl₅ and H₃PO₄.
B) H₃PO₃ and Cl₂.
C) H₃PO₄ and HCl.
D) H₃PO₄ and Cl₂.
E) H₃PO₃ and HCl.

Answer 1

H₃PO₃ and HCl.

Question 2

The term catenation describes the

A) tendency of carbon atoms to form cations in the presence of alkali metals.
B) process of creating synthetic gas from coal.
C) extraction of precious metals with sodium or potassium cyanide.
D) ability of carbon atoms to form long chains and rings.
E) interaction of Group 4A elements with Group 8A elements at high pressures and temperatures to form coordination compounds.

Answer 2

ability of carbon atoms to form long chains and rings.

Question 3

Which one of these elements is not a gas at room temperature

A) chlorine
B) fluorine
C) nitrogen
D) oxygen
E) sulfur

Answer 3

sulfur

Question 4

Which of the following will oxidize gold

A) concentrated nitric acid
B) concentrated hydrochloric acid
C) aqua regia, a mixture of concentrated nitric acid and concentrated hydrochloric acid
D) all of the above can oxidize gold
E) none of the above can oxidize gold because it is a noble metal and too low on the activity series

Question 5

Determine all of the ionic hydrides from the compounds listed below.
I. CaH₂
II. H₂S
III. SiH₄

A) I only
B) II only
C) I and II
D) I and III
E) II and III

Question 6

Which of these substances is being considered as a replacement fuel for gasoline

A) D₂O
B) H₂
C) NO₂
D) F₂
E) He

Question 7

Based on the following options, select the compound with hydrogen in the - 1 oxidation state.

A) NaH
B) B₂H₆
C) H₂SO₄
D) H₂S
E) PH₃

Question 8

The presence of ozone in the upper atmosphere is important because

A) O₃ absorbs outgoing radiation from the earth's surface, thus helping to keep the earth warm.
B) O₃ absorbs harmful solar radiation.
C) O₃ dissolves in water droplets and is very reactive.
D) O₃ is a major reactant in photosynthesis.

Question 9

Ozone (O₃) and oxygen gas (O₂) are examples of

A) isotopes.
B) allotropes.
C) polymorphs.
D) alloys.
E) amphoterism.

Question 10

Phosphoric acid is the most important of the phosphorus oxoacids. Industrially, phosphoric acid is prepared by

A) the Ostwald process.
B) the Haber process.
C) the reaction of phosphate rock with sulfuric acid.
D) the reaction of P₄O₁₀ with water.
E) the Frasch process.

Question 11

The Ostwald process is the main method for the manufacture of nitric acid. In the first step of this process

A) nitrogen and hydrogen react to form NH₃.
B) ammonia is burned in O₂ to generate N₂ and H₂O.
C) nitrogen and oxygen react to form NO₂.
D) nitrogen and oxygen react to form NO.
E) ammonia is burned with O₂ to generate NO and H₂O.

Question 12

When phosphate rock, Ca₃(PO₄)₂(s), is converted to phosphorus,

A) one of the products of the reaction is water.
B) sulfuric acid is added to generate insoluble calcium sulfate.
C) hydrogen is used to reduce the phosphate to phosphorus.
D) silica is added to form a calcium silicate slag.
E) oxygen must be added to prevent reaction of P₄.

Question 13

Which of these reactions is an example of nitrogen fixation

A)2N₂O $\rarr$ 2N₂ + O₂
B)NH₃ + H₂O $\rarr$ NH₄⁺ + OH^-
C)N₂ + O₂ $\rarr$ 2NO
D)2NO₂ + H₂O $\rarr$ HNO₂ + HNO₃
E)2NO + O₂ $\rarr$ 2NO₂

Question 14

A chemical formula of the carbide ion is

A) Si^4-
B) C₂^-
C) C₂^2-
D) CN^-
E) C₃^-

Question 15

Based on the following options, select the substance with hydrogen in the +1 oxidation state.

A) KH
B) CH₄
C) H₂
D) AlH₃
E) SrH₂

Question 16

Which of the following substances is a superoxide

A) KO₂
B) Na₂O₂
C) CO₂
D) CaO
E) Al₂O₃

Question 17

Determine all of the covalent hydrides from the compounds listed below.
I. CaH₂
II. H₂S
III. SiH₄

A) I only
B) II only
C) I and II
D) I and III
E) II and III

Question 18

Select basic oxide from the choices given.

A) CaO
B) SiO₂
C) CO₂
D) P₄O₆
E) H₂O₂

Question 19

Which of the following substances is a peroxide

A) KO₂
B) Na₂O₂
C) CO₂
D) CaO
E) Al₂O₃

Question 20

Which one of these elements is a liquid at room temperature

A) bromine
B) chlorine
C) fluorine
D) iodine
E) selenium

Question 21

What element is the most abundant by mass in Earth's crust

A) Fe
B) H
C) K
D) P
E) O

Question 22

Which of these aqueous solutions has the highest pH

A) 0.100 M NaOH
B) 0.100 M Na₂O
C) 0.100 M Na₃N
D) All of these solutions have the same pH due to the leveling effect.
E) These all are solutions of weak bases, so K_b values are needed in order to decide.

Question 23

In which of the following compounds is sulfur in a positive oxidation state

A) H₂S
B) S₈
C) CaS
D) MnS
E) SO₃

Question 24

Choose the true statement concerning the relative acid strengths of H₂SO₄ and H₂SO_3.

A) H₂SO₄ is a stronger acid than H₂SO₃ because the S in H₂SO₄ has a more positive oxidation state than the S in H₂SO₃ which influences the polarity of the O-H bonds.
B) H₂SO₄ is a weaker acid than H₂SO₃ because the S in H₂SO₄ has a more positive oxidation state than the S in H₂SO₃ which influences the polarity of the O-H bonds.
C) H₂SO₄ is a stronger acid than H₂SO₃ because the S in H₂SO₄ has a less positive oxidation state than the S in H₂SO₃ which influences the polarity of the O-H bonds.
D) H₂SO₄ is a weaker acid than H₂SO₃ because the S in H₂SO₄ has a more negative oxidation state than the S in H₂SO₃ which influences the polarity of the O-H bonds.

Question 25

Which of these substances is the active ingredient in ordinary household bleach

A) HCl
B) Cl₂
C) NaCl
D) NaClO
E) NaClO₄

Question 26

In which of the following compounds is nitrogen in a positive oxidation state

A) NH₃
B) N₂H₄
C) NH₂OH
D) N₂
E) NO

Question 27

The bond energy of F₂ is unusually low, in comparison with the other halogens, due to the small size of the fluorine atom. Which of the following periodic properties is also unusually low in the case of fluorine

A) first ionization energy
B) electron affinity
C) electronegativity
D) diatomic bond length
E) ionic radius

Question 28

Which of these aqueous solutions has the lowest pH

A) 0.100 M NaOH
B) 0.100 M Na₂O
C) 0.100 M Na₃N
D) All of these solutions have the same pH due to the leveling effect.
E) These all are solutions of weak bases, so K_b values are needed in order to decide.

Question 29

Choose the formula that does not represent a stable allotrope.

A) N₂
B) S₈
C) O₂
D) P₂
E) I₂

Question 30

Which of the following choices is/are ionic oxides
I. SrO
II. SiO₂
III. SO₂

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 31

List the following acids in order of increasing acid strength: HOCl, HClO₃, HClO₄.

A) HOCl < HClO₃ < HClO₄
B) HClO₄ < HClO₃ < HOCl
C) HClO₃ < HClO₄ < HOCl
D) HOCl < HClO₄ < HClO₃
E) HClO₃ < HClO < HClO₄

Question 32

Select acidic oxide from the choices given.

A) CaO
B) Na₂O
C) Na₂O₂
D) P₄O₆
E) KOH

Question 33

Hydrogen plays an important role in many industrial processes. The following correctly represents a balanced chemical equation for its production by the reaction of propane (C₃H₈, obtained from natural gas) and steam.2 C₃H₈(g) + 3H₂O(g) $\rarr$ 6CO(g) + 7H₂(g)

Question 34

Which one of the following compounds can react with water to form hydrogen gas

A) PCl₅
B) NO₂
C) H₂O₂
D) KH
E) NH₃

Question 35

Which one of the following compounds can react with water to form oxygen gas

A) PCl₅
B) NO₂
C) H₂O₂
D) KH
E) NH₃

Question 36

Which of the following choices is/are covalent oxides
I. SrO
II. SiO₂
III. SO₂

A) I only
B) II only
C) III only
D) I and II
E) II and III

Question 37

Chlorine gas is prepared commercially by

A) electrolysis of carbon tetrachloride.
B) oxidation of chloride ion with F₂(g).
C) electrolysis of NaCl(aq).
D) oxidation of chloride ion with Br₂(aq).
E) electrolysis of AlCl₃(aq).

Question 38

Hydrogen plays an important role in many industrial processes. The following correctly represents a balanced chemical equation for its production by the water gas reaction.C(s) + H₂O(g) $\rarr$ CO(g) + H₂(g)

Question 39

The main commercial source of bromine is

A) silver bromide ore.
B) seawater.
C) the Frasch process.
D) phosphate rock.
E) the Ostwald process.

Question 40

Which of these industrial chemicals is produced in the greatest amount annually

A) HNO₃
B) H₃PO₄
C) H₂
D) H₂SO₄
E) HClO₃

Question 41

Write the chemical formula of the peroxide ion.

A) O^2-
B) O^-
C) O₂^-
D) O₂^2-
E) None of the above

Question 42

Write the chemical formula of the superoxide ion.

A) O^2-
B) O^-
C) O₂^-
D) O₂^2-
E) None of the above

Question 43

Carborundum, silicon carbide, SiC(s), can be prepared by reacting silicon dioxide with carbon as shown in the following balanced chemical equation:
SiO₂(s) + 3C(s) $\rarr$ SiC(s) + 2CO(g)

Question 44

The chemistry of fluorine differs in many ways from that of the rest of the halogens.

Question 45

Alkali metal hydrides are very reactive with water, forming H₂ gas.

Question 46

P₄O₆ and P₄O₁₀ are allotropes of phosphorus.

Question 47

The following is a balanced chemical equation that depicts the production of chlorine by the chlor-alkali process. $2 \mathrm{NaCl}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \xrightarrow{\text { electrolysis }~~} 2 \mathrm{NaOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{g})$

Question 48

Write the chemical formula of the oxide ion.

A) O^2-
B) O^-
C) O₂^-
D) O₂^2-
E) None of the above

Question 49

The following accurately depicts the balanced chemical equation for a laboratory preparation of nitrogen gas.NH₄NO₂(s) $\rarr$ 2H₂O(g) + N₂(g)

Question 50

Of the three oxides SiO₂, MgO, and P₄O₁₀, the most acidic oxide is P₄O₁₀.

Question 51

Write the formula for the binary hydride you would expect calcium to form.

A) CaH
B) Ca₂H
C) Ca₃H₂
D) CaH₂
E) None of the above

Question 52

It is especially dangerous to mix cyanide salts with acids because the cyanide ion reacts with acid to form hydrogen cyanide, a very weak acid that comes out of solution as a gas. Inhaled in even very small amounts it can rapidly cause death.