Deck 22: Chemistry of the Nonmetals

Question 1

Consider the following xenon compounds:
(i) XeF₂
(ii) XeF₄
(iii) XeO₄
(iv) XeOF₄
(v) XeO₃
Which of the compounds is(are) polar?

A) (i) only
B) (iii) and (iv)
C) (iv) and (v)
D) (ii) and (iii)
E) (iv) only

Answer 1

(iv) and (v)

Question 2

Of the following compounds, which is the most stable?

A) XeO₃
B) XeF₂
C) XeO₂F₂
D) XeF₆
E) XeOF₄

Answer 2

XeF₆

Question 3

Addition of B₂O₃ to soda- lime glass

A) results in a glass with a lower melting point.
B) results in opaque glass.
C) imparts a greater ability to withstand temperature change.
D) imparts a deep blue color.
E) results in a denser glass with a higher refractive index.

Answer 3

imparts a greater ability to withstand temperature change.

Question 4

Which one of the following is true concerning borax?

A) It is the hydrated sodium salt of tetraboric acid.
B) It is commonly used in cleaning products.
C) Its aqueous solutions are alkaline.
D) It is found in dry lake deposits in California.
E) All of the above are true.

Question 5

Which of the following statements is false?

A) Ozone decomposes to O₂ and O.
B) Ozone is an allotrope of oxygen.
C) Ozone is a better reducing agent than O₂ (g).
D) Ozone oxidizes all of the common metals except gold and platinum.
E) Ozone is produced by passing electricity through dry O₂ (g).

Question 6

How many oxygen atoms are bonded to each silicon atom in SiO₂?

A) 1
B) 2
C) 3
D) 4
E) none

Question 7

Nearly all commercial oxygen is obtained .

A) by thermal decomposition of potassium chlorate
B) by thermal cracking of petroleum
C) from air
D) by electrolysis of water
E) as a byproduct of the preparation of aluminum in the Hall process

Question 8

Which elemental halogen(s) can be used to prepare I₂ from NaI?

A) Br₂ only
B) F₂ only
C) Cl₂ only
D) both Cl₂ and Br₂, but not F₂
E) F₂, Cl₂, and Br₂

Question 9

Which of the following would produce the most strongly basic aqueous solution?

A) CO₂
B) CO
C) HCO₃^-
D) CO₃^2-
E) NaHCO₃

Question 10

The oxidation numbers of sulfur in the sulfate ion, sulfite ion, sulfur trioxide, and hydrogen sulfide are _, , _,and ,respectively.

A) +6, +4, +6, - 2
B) +4, +6, +4, - 2
C) - 2, +6, - 2, 0
D) +4, - 2, +4, +6
E) +6, +2, +4, +6

Question 11

What is the major commercial source of elemental sulfur?

A) sulfate minerals
B) sulfide minerals
C) coal and petroleum
D) underground deposits of elemental sulfur
E) seawater

Question 12

Which of the following equations correctly represents the combustion of hydrazine?

A) N₂H₄ (l) + 2O₂ (g) → 2NO₂ (g) + 2 H₂ (g)
B) N₂H₄ (l) + O₂ (g) → N₂ (g) + 2 H₂ (g) + O₂ (g)
C) N₂H₄ (l) + O₂ (g) → N₂ (g) + 2 H₂O (g)
D) N₂H₄ (l) + O₂ (g) → NH₃ (g) + HNO₂ (g)
E) N₂H₄ (l) + O₂ (g) → 2H₂NO (g)

Question 13

What is the function of the carbon fibers in a composite?

A) to provide ultraviolet protection
B) to provide resistance to oxidation
C) to provide a structure to help the epoxy resin solidify in the desired shape
D) to transmit loads evenly in all directions
E) to "spread out" the epoxy so that it remains more flexible

Question 14

Silicones are

A) flat sheets of silicon atoms.
B) three- dimensional covalent networks of silicon atoms.
C) three- dimensional covalent networks of SiO₄ tetrahedra.
D) flat sheets of silicon and hydrogen atoms.
E) chains of alternating silicon and oxygen atoms with attached organic groups.

Question 15

Which one of the following is false concerning pure hydrazine?

A) It is used as a rocket fuel.
B) It can be made by reaction of hypochlorite and ammonia.
C) It is an oily, colorless liquid.
D) It is a clear, red liquid that is highly viscous.
E) Hydrazine is quite poisonous.

Question 16

Which one of the following compounds is peroxide?

A) H₂O
B) both Na₂O₂ and CsO₂
C) Na₂O₂
D) CsO₂
E) Li₂O

Question 17

The least electronegative of the elements below is .

A) I
B) H
C) Br
D) F
E) Cl

Question 18

Carbon dioxide is produced

A) by fermentation of sugar during the production of ethanol.
B) by combustion of carbon- containing substances in an excess of oxygen.
C) when carbonates are heated.
D) by all of these processes.
E) in blast furnaces when metal oxides are reduced with CO.

Question 19

Which group 6A element is not commonly found in a positive oxidation state?

A) tellurium
B) oxygen
C) selenium
D) polonium
E) sulfur

Question 20

Interhalogen compounds _.

A) are very active fluorinating agents
B) that contain fluorine are powerful oxidizing agents
C) contain halogens in both positive and negative oxidation states
D) are exceedingly reactive
E) all of the above

Question 21

Which one of the following is false concerning tritium?

A) The atomic number of tritium is 1.
B) It has the same chemical properties as protium but reacts more slowly.
C) It is radioactive, emitting alpha particles with a half- life of 12.3 yr.
D) It can be produced by neutron bombardment of lithium- 6.
E) It is formed continuously in the upper atmosphere.

Question 22

Which of the following is the nitride ion?

A) N^-
B) N^3-
C) N₃^-
D) NO₂^-
E) NO₃^-

Question 23

Which form of elemental sulfur is the most stable at room temperature?

A) triclinic
B) hexagonal
C) rhombic sulfur
D) tetraclinic
E) monoclinic

Question 24

The prefix "thio" denotes

A) a sulfur-sulfur double bond.
B) replacement of an oxygen atom by a sulfur atom.
C) an allotropic form of sulfur.
D) sulfur in a negative oxidation state.
E) a sulfur-oxygen double bond.

Question 25

Which of the following would produce the most strongly acidic aqueous solution?

A) CaCO₃
B) CO₃^2-
C) CO₂
D) CO
E) HCO₃^-

Question 26

In the reaction of phosphorus with chlorine to form a phosphorus chloride, whether PCl₃ or PCl₅ forms depends on

A) whether the chlorine used is molecular or atomic.
B) the amount of moisture present.
C) whether the reaction is carried out in the gas phase or in solution.
D) which allotropic form of phosphorus is used.
E) the amount of chlorine present.

Question 27

The reaction between nitrogen dioxide and water is a

A) neutralization
B) decomposition
C) combustion
D) disproportionation
E) replacement

Question 28

Isotopes of hydrogen

A) have different atomic numbers and different mass numbers.
B) have different atomic numbers and the same mass number.
C) are exactly alike.
D) have the same atomic number and the same mass number.
E) have the same atomic number and different mass numbers.

Question 29

Which compound would produce a basic aqueous solution?

A) HCl
B) CH₃OH
C) H₂S
D) MgH₂
E) HI

Question 30

What method is used to produce the most hydrogen gas in the United States?

A) reaction of metallic sodium with water
B) reaction of coke (carbon) with steam
C) reaction of zinc with acid
D) reaction of methane with steam
E) electrolysis of water

Question 31

Which of the following is not an allotropic form of carbon?

A) carbide
B) buckminsterfullerene
C) graphite
D) diamond
E) All of the above are allotropic forms of carbon.

Question 32

What is the F-Xe-F bond angle in XeF₂?

A) 109°
B) 60°
C) 90°
D) 120°
E) 180°

Question 33

Which equation correctly represents what happens when NO₂ dissolves in water?

A) NO₂ (g) + H₂O (l) → H₂O₂ (aq) + NO (g)
B) 2NO₂ (g) + H₂O (l) → 2H⁺ (aq) + NO₄^2- (aq) + NO (g)
C) NO₂ (g) + H₂O (l) → 2H⁺ (aq) + NO₃^- (aq)
D) 2NO₂ (g) + 2H₂O (l) → 2 HNO₂ (aq) + O₂ (g) + H₂ (g)
E) 3NO₂ (g) + H₂O (l) → 2H⁺ (aq) + 2NO₃^- (aq) + NO (g)

Question 34

The arrangement of oxygen atoms around a silicon atom in SiO₄^4- is

A) octahedral
B) trigonal pyramidal
C) linear
D) tetrahedral
E) square planar

Question 35

Which one of the following is sodium thiosulfate?

A) Na₂S₂O₃
B) Na₂S
C) Na₂SO₃
D) Na₂S₄O₆
E) Na₂SO₄

Question 36

Of the following, which is most likely to form interstitial carbides?

A) boron and silicon
B) transition metals
C) active metals
D) alkali metals
E) alkaline earth metals

Question 37

Sodium borohydride, NaBH₄, is a strong reducing agent because .

A) Na⁺ is easily reduced to Na (s).
B) hydrogen can be easily oxidized from - 1 oxidation state to +1
C) boron easily changes its oxidation number from +3 to - 3
D) boron is readily oxidized from - 3 oxidation state to +3
E) hydrogen is easily reduced from +1 oxidation state to 0

Question 38

Which noble gas is known to form a variety of binary compounds?

A) He
B) Ne
C) Xe
D) Ar
E) Kr

Question 39

The primary commercial use of nitric acid is .

A) in the manufacture of anti- depressant drugs
B) in the manufacture of explosives
C) in the manufacture of fertilizers
D) in the manufacture of plastics
E) in pool water maintenance

Question 40

A disproportionation reaction is one in which

A) an insoluble salt separates into ions.
B) aqueous ions combine to form an insoluble salt.
C) the ratio of combination of two elements in a compound changes.
D) a compound is separated into its constituent elements.
E) a single element is both oxidized and reduced.

Question 41

A borane is a

A) compound containing only boron and hydrogen.
B) compound containing only boron and oxygen.
C) compound containing only boron and carbon.
D) three- dimensional covalent network of boron atoms.
E) compound containing only boron and aluminum.

Question 42

Which compound would produce an acidic aqueous solution?

A) H₂S
B) H₂O
C) CaH₂
D) KH
E) NH₃

Question 43

Soda- lime glass contains

A) SiO₂, CO₂, and citric acid
B) SiO₂, CO₂, Na₂O
C) pure SiO₂
D) SiO₂ and aluminum
E) SiO₂, CaO, and Na₂O

Question 44

What is the primary commercial use of hydrogen in the United States?

A) manufacture of methanol
B) as a rocket fuel, especially on the space shuttle
C) as an automobile fuel
D) hydrogenation of vegetable oils
E) manufacture of ammonia by the Haber process

Question 45

Which equation correctly represents the reaction between carbon dioxide and water?

A) CO₂ (aq) + H₂O (l)→ H₂ (g) + CO (g) + O₂ (g)
B) CO₂ (aq) + 2H₂O (l) → CH₄ (g) + 2O₂ (aq)
C) CO₂ (aq) + H₂O (l) → H₂O₂ (aq) + CO (g)
D) CO₂ (aq) + H₂O (l) → H₂CO (aq) + O₂ (g)
E) CO₂ (aq) + H₂O (l) → H₂CO₃ (aq)

Question 46

The oxidation numbers of nitrogen in the nitride ion, hydrazine, ammonium cation, and nitrate ion are _, , _,and ,respectively.

A) +3, - 2, - 3, +5
B) - 3, +2, +1, +5
C) +3, - 2, +1, +3
D) - 3, - 2, - 3, +5
E) - 3, +2, - 3, +3

Question 47

What are the products of the reaction of PF₃ (g) and water?

A) phosphoric acid and phosphorous acid
B) elemental phosphorus and fluorine gas
C) phosphoric acid and fluorine gas
D) phosphorous acid and hydrofluoric acid
E) elemental phosphorus and hydrofluoric acid

Question 48

Boron can violate the octet rule in its compounds in that

A) it can have an expanded octet.
B) boron cannot violate the octet rule.
C) it can exist in a molecule with an odd number of electrons.
D) it can have fewer than eight valence electrons.
E) its compounds are all ionic.

Question 49

Which of the following would produce a basic solution?

A) BeH₂ only
B) CO, CO₂, and BeH₂
C) CO and CO₂
D) Na₂O, MgO, and BeH₂
E) Na₂O and MgO

Question 50

The oxidation state of oxygen in OF₂ is

A) +2
B) - 1
C) - 2
D) +1
E) 0

Question 51

Which element in group 6A is not found in compounds with an expanded valence shell?

A) selenium
B) oxygen
C) sulfur
D) polonium
E) tellurium

Question 52

Of the following, which is an ionic hydride?

A) BaH₂
B) CaH₂
C) LiH
D) SrH₂
E) all of the above

Question 53

The pentahydrated salt of sodium thiosulfate, Na₂S₂O₃ · 5H₂O, is used in photographic developing to convert _.

A) insoluble AgBr to insoluble Ag₂S₂O₃
B) insoluble AgBr to soluble Na₃[Ag(S₂O₃)₂]
C) insoluble AgBr to soluble Ag₂S₂O₃
D) soluble AgBr to insoluble Ag₂S₂O₃
E) insoluble AgBr to insoluble Na₃[Ag(S₂O₃)₂]

Question 54

In a group of nonmetals, which element(s) is (are) most likely to be form stable n bonds?

A) the top element
B) the second element
C) the bottom element
D) the middle element
E) None of them, nonmetals do not do this.

Question 55

The most stable allotrope of oxygen is .

A) H₂O
B) HClO
C) O₂
D) O₃
E) O

Question 56

Chlorine can have a positive oxidation state

A) if it combines with hydrogen.
B) if it combines with bromine or iodine.
C) if it combines with oxygen or fluorine.
D) if it combines with an alkali metal.
E) in its elemental form.

Question 57

Replacement of CaO by PbO in soda- lime glass results in

A) denser glass with a high refractive index.
B) a softer glass with a lower melting point.
C) glass with a deep blue color.
D) opaque glass.
E) a harder glass with a higher melting point.

Question 58

Boric acid condenses to form tetraboric acid according to the equation

A) 2H₃BO₃ (s) → HB₂O₂ (s) + 4H₂O (g).
B) 4H₃BO₃ (s) → HB₄O₈ (s) + 4H₂O (g).
C) 4H₃BO₃ (s) → H₂B₄O₇ (s) + 5H₂O (g).
D) 4H₃BO₃ (s) → 2H₂B₂O₇ (s) + 3H₂O (g).
E) 2H₃BO₃ (s) → H₂B₄O₇ (s) + 3H₂O (g).

Question 59

Replacement of Na₂O by K₂O in soda- lime glass results in

A) a harder glass with a higher melting point.
B) glass with a deep blue color.
C) opaque glass.
D) denser glass with a high refractive index.
E) a softer glass with a lower melting point.

Question 60

Metal oxides are typically while nonmetal oxides are typically _.

A) amphoteric, acidic
B) basic, acidic
C) amphoteric, basic
D) basic, amphoteric
E) acidic, basic

Question 61

What are the products of the reaction of PCl₃ (g) and water?

A) elemental phosphorus and hydrochloric acid
B) elemental phosphorus and chlorine gas
C) phosphoric acid and chlorine gas
D) phosphoric acid and hydrochloric acid
E) phosphoric acid and phosphorous acid

Question 62

How are the oxygen- containing compounds of xenon made?

A) by direct combination of the elements
B) by thermal decomposition of the xenon hydroxide
C) by reaction of the corresponding xenon fluoride with water
D) by reaction of xenon with peroxide
E) Xenon is inert and does not form compounds with oxygen.

Question 63

The careful, thermal decomposition of solid ammonium nitrate will yield .

A) N₂O
B) N₂O₃
C) N₂O₅
D) NO₂
E) NO

Question 64

Which pair of formula/name is incorrect?

A) N₂O₄ / dinitrogen trioxide
B) NO / nitric oxide
C) N₂O / nitrous oxide
D) N₂O₅ / dinitrogen pentoxide
E) NO₂ / nitrogen dioxide

Question 65

The interhalogen compound ICl₃ can form but BrCl₃ cannot form. This is because

A) bromine is not electronegative enough to react with chlorine.
B) iodine can have a negative oxidation state but bromine cannot.
C) bromine is too electronegative to react with chlorine.
D) iodine is large enough to accommodate three chlorine atoms around itself
E) iodine can have a positive oxidation state but bromine cannot.

Question 66

Which of the following would produce an acidic solution?

A) CO₂ only
B) BeH₂ only
C) CO, CO₂, and BeH₂
D) Na₂O, MgO, and BeH₂
E) Na₂O and MgO

Question 67

In the following chemical equation the products (when the equation is balanced) are

A) 3NaO + PH₆
B) 3NaOH + PH₃
C) 3NaH + POH₃
D) NaOH + 3PH
E) H₂PO₃ + 3NaH

Question 68

B₂O₃is the anhydride of

A) diborane
B) borax
C) boric acid
D) borous acid
E) tetraboric acid

Question 69

Which equation correctly represents the reaction between elemental fluorine and sodium iodide?

A) F + NaI → I + NaF
B) F^- + NaI → I^- + NaF
C) F₂ + NaI → NaF₂ + I^-
D) F + NaI → 1/2I₂ + NaF
E) F₂ + 2NaI → I₂ + 2NaF

Question 70

Write the correctly balanced equation for the reaction between elemental fluorine and sodium iodide.

Question 71

Which of the following approaches will produce PF₃ reliably?

A) 2PCl₃ (l) + (excess) F₂ (g)→ 2PF₃ (g) + 3Cl₂ (g) + (excess) F₂ (g)
B) PCl₃ (l) + AsF₃ (l) → PF₃ (g) + AsCl₃ (l)
C) P (s) + (excess) F₂ (g) → PF₃ (g) + (excess) F₂ (g)
D) PF₅ (g) → PF₃ (g) + F₂ (g)
E) none of these approaches will produce PF₃

Question 72

The oxidation state of fluorine in its compounds is

A) negative unless it combines with oxygen.
B) negative unless it combines with another halogen.
C) positive unless it combines with another halogen.
D) always negative.
E) negative unless it combines with an active metal.

Question 73

A carbonyl compound contains

A) a carbon- oxygen double bond
B) a carbon- carbon triple bond
C) a carbon- oxygen triple bond
D) a carbon- carbon double bond
E) a carbon atom with a lone pair of electrons

Question 74

The heavier noble gases are more reactive than the lighter ones because

A) the lighter noble gases have complete octets.
B) the heavier noble gases are more abundant.
C) the lighter noble gases exist as diatomic molecules.
D) the heavier noble gases have low ionization energies relative to the lighter ones.
E) the heavier noble gases have greater electron affinities.

Question 75

Which one of the following is false concerning buckminsterfullerene?

A) It consists of individual molecules like C₆₀ and C₇₀.
B) It is made up of molecules that resemble soccer balls.
C) It is made up of Cl₂molecules.
D) It is the most recently discovered crystalline allotrope of carbon.
E) It is a molecular form of carbon.

Question 76

The oxidation state of oxygen in O₂F₂ is

A) +2
B) 0
C) - 1
D) +1
E) - 2

Question 77

The molecular shape of the SF₆ molecule is .

A) trigonal pyramidal
B) octahedral
C) tetrahedral
D) trigonal bipyramidal
E) T- shaped

Question 78

Additives can be used in soda- lime glass to alter its .

A) hardness
B) ability to withstand temperature change
C) color
D) melting point
E) any of the above

Question 79

Which of the following equations correctly represents the reaction of B₂H₆ with oxygen?

A) B₂H₆ (g) + 2O₂ (g) → B₂O₂ (s) + 3H₂ + O₂ (g)
B) B₂H₆ (g) + O₂ (g) → H₂B₂O₂ (s) + 2H₂ (g)
C) B₂H₆ (g) + O₂ (g) → B₂O₂ (s) + 3H₂ (g)
D) B₂H₆ (g) + 2O₂ (g) → B₂H₂ (s) + 2H₂O₂ (aq)
E) B₂H₆ (g) + 3O₂ (g) → B₂O₃ (s) + 3H₂O (g)

Question 80

Silicones can be oils or rubber- like materials depending on

A) the oxidation state of silicon in the chain.
B) the silicon- to- oxygen ratio.
C) the percentage of sulfur in the chain.
D) the length of the chain and degree of cross- linking.
E) the percentage of carbon in the chain.