Chapter 22 1 How many oxygen atoms are bonded to each silicon atom

Chemistry: The Central Science, 13e (Brown et al.)

Chapter 22 Chemistry of the Nonmetals

22.1 Multiple-Choice

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

A) 1

B) 2

C) 3

D) 4

E) none

2) Of the atoms below, ________ is the most effective in forming π bonds.

A) C

B) P

C) N

D) Si

E) Ge

3) Which one of the following is false concerning tritium?

A) It is radioactive, emitting alpha particles with a half–life of 12.3 yr.

B) It can be produced by neutron bombardment of lithium–6.

C) It is formed continuously in the upper atmosphere.

D) It has the same chemical properties as protium but reacts more slowly.

E) The atomic number of tritium is 1.

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

A) electrolysis of water

B) reaction of zinc with acid

C) reaction of methane with steam

D) reaction of coke (carbon) with steam

E) reaction of metallic sodium with water

5) Water gas is ________.

A) H2O and H2

B) CO2 and O2

C) H2O and CO2

D) H2O and CO

E) H2 and CO

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

A) as a rocket fuel, especially on the space shuttle

B) hydrogenation of vegetable oils

C) manufacture of methanol

D) manufacture of ammonia by the Haber process

E) as an automobile fuel

7) Isotopes of hydrogen ________.

A) have the same atomic number and different mass numbers

B) have the same atomic number and the same mass number

C) have different atomic numbers and different mass numbers

D) have different atomic numbers and the same mass number

E) are exactly alike

8) Which of the following would produce a basic solution?

A) CO and CO2

B) Na2O and MgO

C) Na2O, MgO, and BeH2

D) BeH2 only

E) CO, CO2, and BeH2

9) Which of the following would produce an acidic solution?

A) Na2O and MgO

B) Na2O, MgO, and BeH2

C) CO2 only

D) BeH2 only

E) CO, CO2, and BeH2

10) How are the oxygen-containing compounds of xenon made?

A) by direct combination of the elements

B) by reaction of xenon with peroxide

C) by thermal decomposition of the xenon hydroxide

D) by reaction of the corresponding xenon fluoride with water

E) Xenon is inert and does not form compounds with oxygen.

11) Of the following compounds, which is the most stable?

A) XeF6

B) XeOF4

C) XeO3

D) XeO2F2

E) XeF2

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12) 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) (ii) and (iii)

C) (iv) only

D) (iii) and (iv)

E) (iv) and (v)

13) The heavier noble gases are more reactive than the lighter ones because ________.

A) the lighter noble gases exist as diatomic molecules.

B) the lighter noble gases have complete octets.

C) the heavier noble gases are more abundant.

D) the heavier noble gases have low ionization energies relative to the lighter ones.

E) the heavier noble gases have greater electron affinities.

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

A) Xe

B) He

C) Ne

D) Ar

E) Kr

15) Interhalogen compounds ________.

A) are exceedingly reactive

B) contain halogens in both positive and negative oxidation states

C) are powerful oxidizing agents

D) that contain fluorine are very active fluorinating agents

E) all of the above

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

A) F2 only

B) Cl2 only

C) Br2 only

D) both Cl2 and Br2, but not F2

E) F2, Cl2, and Br2

17) Which halogen is the most easily oxidized?

A) F

B) Cl

C) Br

D) I

18) Which equation correctly represents the reaction between silica and hydrofluoric acid?

A) SiCl4 + 4HF → SiF4 + 4HCl

B) SiO2 + 6HF → H2SiF6 + 2H2O

C) SiCl2 + 2HF → SiF2 + 2HCl

D) SiH4 + 4HF → SiF4 + 4H2

E) none of the above

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

A) iodine is large enough to accommodate three chlorine atoms around itself

B) bromine is not electronegative enough to react with chlorine

C) bromine is too electronegative to react with chlorine

D) iodine can have a positive oxidation state but bromine cannot

E) iodine can have a negative oxidation state but bromine cannot

20) Chlorine can have a positive oxidation state ________.

A) if it combines with bromine or iodine

B) if it combines with oxygen or fluorine

C) if it combines with hydrogen

D) if it combines with an alkali metal

E) in its elemental form

21) The oxidation state of fluorine in its compounds is ________.

A) positive unless it combines with another halogen

B) negative unless it combines with another halogen

C) negative unless it combines with oxygen

D) negative unless it combines with an active metal

E) always negative

22) The most stable allotrope of oxygen is ________.

A) H2O

B) O3

C) O2

D) HClO

E) O

23) Which of the following react with oxygen to form superoxides?

A) Ca

B) Na

C) K

D) Sr

E) Ba

24) Nearly all commercial oxygen is obtained ________.

A) from air

B) by electrolysis of water

C) by thermal decomposition of potassium chlorate

D) by thermal cracking of petroleum

E) as a byproduct of the preparation of aluminum in the Hall process

25) Which of the following statements is false?

A) Ozone is a better reducing agent than O2 (g).

B) Ozone is produced by passing electricity through dry O2 (g).

C) Ozone oxidizes all of the common metals except gold and platinum.

D) Ozone decomposes to O2 and O.

E) Ozone is an allotrope of oxygen.

26) A disproportionation reaction is one in which ________.

A) a single element is both oxidized and reduced

B) a compound is separated into its constituent elements

C) the ratio of combination of two elements in a compound changes

D) aqueous ions combine to form an insoluble salt

E) an insoluble salt separates into ions

27) The oxidation state of oxygen in OF2 is ________.

A) +1

B) +2

C) 0

D) -1

E) -2

28) Metal oxides are typically ________ while nonmetal oxides are typically ________.

A) basic, amphoteric

B) basic, acidic

C) amphoteric, basic

D) acidic, basic

E) amphoteric, acidic

29) Amphoteric oxides are also known as ________.

A) basic oxides

B) basic anhydrides

C) acidic oxides

D) acidic anhydrides

E) none of the above

30) Which element in group 6A is not found as the central atom in compounds with an expanded valence

shell?

A) oxygen

B) selenium

C) tellurium

D) polonium

E) sulfur

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

A) sulfur

B) selenium

C) oxygen

D) tellurium

E) polonium

32) What sulfur compound is used to sterilize wine?

A) H2SO4

B) H2S

C) Na2SO3

D) SO2

E) Na2S

33) What is the major commercial source of elemental sulfur?

A) sulfide minerals

B) sulfate minerals

C) underground deposits of elemental sulfur

D) seawater

E) coal and petroleum

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

A) rhombic sulfur

B) monoclinic

C) hexagonal

D) triclinic

E) tetraclinic

35) The prefix thio- denotes

A) replacement of an oxygen atom by a sulfur atom.

B) a sulfur—sulfur double bond.

C) sulfur in a negative oxidation state.

D) a sulfur—oxygen double bond.

E) an allotropic form of sulfur.

36) The oxidation numbers of sulfur in the sulfate ion, sulfite ion, sulfur trioxide, and hydrogen sulfide

are ________, ________, ________, and ________, respectively.

A) +4, -2, +4, +6

B) +6, +2, +4, +6

C) +6, +4, +6, -2

D) +4, +6, +4, -2

E) -2, +6, -2, 0

37) Which one of the following is sodium thiosulfate?

A) Na2SO4

B) Na2SO3

C) Na2S2O3

D) Na2S4O6

E) Na2S

38) Which one of the following is false concerning pure hydrazine?

A) It is an oily, colorless liquid.

B) It can be made by reaction of hypochlorite and ammonia.

C) It is used as a rocket fuel.

D) Hydrazine is quite poisonous.

E) It is a clear, red liquid that is highly viscous.

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

A) N2O

B) NO

C) NO2

D) N2O3

E) N2O5

40) The oxidation number of N in HNO3 is ________.

A) +1

B) +2

C) +3

D) +4

E) +5

41) The oxidation number of N in HNO2 is ________.

A) +1

B) +2

C) +3

D) +4

E) +5

42) The oxidation number of As in H2AsO3– is ________.

A) +1

B) +2

C) +3

D) +4

E) +5

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

A) N2H4 (l) + O2 (g) → NH3 (g) + HNO2 (g)

B) N2H4 (l) + 2O2 (g) → 2NO2 (g) + 2H2 (g)

C) N2H4 (l) + O2 (g) → 2H2NO (g)

D) N2H4 (l) + O2 (g) → N2 (g) + 2 H2O (g)

E) N2H4 (l) + O2 (g) → N2 (g) + 2H2 (g) + O2 (g)

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44) 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, -3, +5

C) +3, -2, +1, +3

D) -3, +2, +1, +5

E) -3, +2, -3, +3

45) Which equation correctly represents what happens when N dissolves in water?

A) NO2 (g) + H2O (l) → 2H+ (aq) + NO3– (aq)

B) 3NO2 (g) + H2O (l) → 2H+ (aq) + 2NO3– (aq) + NO (g)

C) NO2 (g) + H2O (l) → H2O2 (aq) + NO (g)

D) 2NO2 (g) + H2O (l) → 2H+ (aq) + NO42– (aq) + NO (g)

E) 2NO2 (g) + 2H2O (l) → 2HNO2 (aq) + O2 (g) + H2 (g)

46) The reaction between nitrogen dioxide and water is a ________.

A) decomposition

B) combustion

C) disproportionation

D) neutralization

E) replacement

47) Of the following substances, ________ is both a very strong acid and a powerful oxidizing agent.

A) HNO3

B) H2SO4

C) HCl

D) H3PO4

E) HF

48) In the reaction of phosphorus with chlorine to form a phosphorus chloride, whether PCl3 or PCl5

forms depends on ________.

A) which allotropic form of phosphorus is used

B) the amount of chlorine present

C) whether the reaction is carried out in the gas phase or in solution

D) whether the chlorine used is molecular or atomic

E) the amount of moisture present

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

A) phosphorous acid and hydrofluoric acid

B) elemental phosphorus and hydrofluoric acid

C) phosphoric acid and fluorine gas

D) elemental phosphorus and fluorine gas

E) phosphoric acid and phosphorous acid

50) What are the products of the reaction of PCl5 (g) and water?

A) phosphoric acid and phosphorous acid

B) elemental phosphorus and hydrochloric acid

C) phosphoric acid and chlorine gas

D) elemental phosphorus and chlorine gas

E) phosphoric acid and hydrochloric acid

51) Which one of the following is false concerning buckminsterfullerene?

A) It is the most recently discovered crystalline allotrope of carbon.

B) It consists of individual molecules like C60 and C70.

C) It is a molecular form of carbon.

D) It is made up of Cl2 molecules.

E) It is made up of molecules that resemble soccer balls.

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

A) active metals

B) transition metals

C) boron and silicon

D) alkaline earth metals

E) alkali metals

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

A) HCO3–

B) CO

C) CO2

D) CO32-

E) CaCO3

54) How many pairs of unpaired electrons are there in one molecule of carbon monoxide?

A) 0

B) 1

C) 2

D) 3

E) 4

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

A) graphite

B) diamond

C) carbide

D) buckminsterfullerene

E) All of the above are allotropic forms of carbon.

56) A carbonyl compound contains ________.

A) a carbon-oxygen double bond

B) a carbon-oxygen triple bond

C) a carbon atom with a lone pair of electrons

D) a carbon-carbon triple bond

E) a carbon-carbon double bond

57) Carbon dioxide is produced ________.

A) in blast furnaces when metal oxides are reduced with CO

B) by combustion of carbon-containing substances in an excess of oxygen

C) when carbonates are heated

D) by fermentation of sugar during the production of ethanol

E) by all of the above processes

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

A) CO

B) CO32-

C) CO2

D) HCO3–

E) NaHCO3

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

A) CO2 (aq) + H2O (l) → H2CO3 (aq)

B) CO2 (aq) + H2O (l) → H2 (g) + CO (g) + O2 (g)

C) CO2 (aq) + H2O (l) → H2O2 (aq) + CO (g)

D) CO2 (aq) + 2H2O (l) → CH4 (g) + 2O2 (aq)

E) CO2 (aq) + H2O (l) → H2CO (aq) + O2 (g)

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

A) to provide a structure to help the epoxy resin solidify in the desired shape

B) to transmit loads evenly in all directions

C) to provide resistance to oxidation

D) to provide ultraviolet protection

E) to “spread out” the epoxy so that it remains more flexible

61) The arrangement of oxygen atoms around a silicon atom in SiO44- is ________.

A) square planar

B) octahedral

C) linear

D) tetrahedral

E) trigonal pyramidal

62) Addition of B2O3 to soda-lime glass ________.

A) imparts a greater ability to withstand temperature change

B) imparts a deep blue color

C) results in a denser glass with a higher refractive index

D) results in a glass with a lower melting point

E) results in opaque glass

63) Replacement of CaO by PbO in soda-lime glass results in ________.

A) denser glass with a higher refractive index

B) glass with a deep blue color

C) opaque glass

D) a softer glass with a lower melting point

E) a harder glass with a higher melting point

64) Soda-lime glass contains ________.

A) SiO2 and aluminum

B) SiO2, CaO, and Na2O

C) SiO2, CO2, and citric acid

D) SiO2, CO2, Na2O

E) pure SiO2

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

A) ability to withstand temperature change

B) color

C) hardness

D) melting point

E) any of the above

66) Silicones are ________.

A) chains of alternating silicon and oxygen atoms with attached organic groups

B) three-dimensional covalent networks of SiO4 tetrahedra

C) three-dimensional covalent networks of silicon atoms

D) flat sheets of silicon atoms

E) flat sheets of silicon and hydrogen atoms

67) Silicones can be oils or rubber-like materials depending on ________.

A) the silicon-to–oxygen ratio

B) the length of the chain and degree of cross-linking

C) the percentage of carbon in the chain

D) the percentage of sulfur in the chain

E) the oxidation state of silicon in the chain

68) Sodium borohydride, NaBH4, is a strong reducing agent because ________.

A) Na+ is easily reduced to Na (s)

B) boron easily changes its oxidation number from +3 to –3

C) boron is readily oxidized from -3 oxidation state to +3

D) hydrogen can be easily oxidized from -1 oxidation state to +1

E) hydrogen is easily reduced from +1 oxidation state to 0

69) The primary commercial use of nitric acid is ________.

A) in the manufacture of plastics

B) in the manufacture of explosives

C) in pool water maintenance

D) in the manufacture of fertilizers

E) in the manufacture of anti-depressant drugs

70) Which one of the following is true concerning borax?

A) It is the hydrated sodium salt of tetraboric acid.

B) It is found in dry lake deposits in California.

C) Its aqueous solutions are alkaline.

D) It is commonly used in cleaning products.

E) All of the above are true.

71) A borane is a ________.

A) compound containing only boron and oxygen

B) compound containing only boron and aluminum

C) compound containing only boron and hydrogen

D) compound containing only boron and carbon

E) three-dimensional covalent network of boron atoms

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

A) B2H6 (g) + 3O2 (g) → B2O3 (s) + 3H2O (g)

B) B2H6 (g) + O2 (g) → B2O2 (s) + 3H2 (g)

C) B2H6 (g) + 2O2 (g) → B2H2 (s) + 2H2O2 (aq)

D) B2H6 (g) + 2O2 (g) → B2O2 (s) + 3H2 + O2 (g)

E) B2H6 (g) + O2 (g) → H2B2O2 (s) + 2H2 (g)

73) Boron can violate the octet rule in its compounds in that ________.

A) it can have an expanded octet

B) it can exist in a molecule with an odd number of electrons

C) its compounds are all ionic

D) it can have fewer than eight valence electrons

E) Boron cannot violate the octet rule.

74) B2O3 is the anhydride of ________.

A) borous acid

B) diborane

C) tetraboric acid

D) boric acid

E) borax

75) Boric acid condenses to form tetraboric acid according to the equation ________.

A) 4H3BO3 (s) → 2H2B2O7 (s) + 3H2O (g)

B) 2H3BO3 (s) → HB2O2 (s) + 4H2O (g)

C) 4H3BO3 (s) → HB4O8 (s) + 4H2O (g)

D) 2H3BO3 (s) → H2B4O7 (s) + 3H2O (g)

E) 4H3BO3 (s) → H2B4O7 (s) + 5H2O (g)

22.2 Bimodal Questions

1) The most common isotope of hydrogen is sometimes referred to as ________.

A) deuterium

B) protium

C) tritium

D) heavy hydrogen

E) common hydrogen

2) In metallic hydrides, the oxidation number of hydrogen is considered to be ________.

A) -2

B) -1

C) 0

D) +1

E) +2

3) Hydrogen can form hydride ions. Elements in group ________ typically form ions with the same

charge as the hydride ion.

A) 1A

B) 2A

C) 6A

D) 7A

E) 3A

4) Hydrogen can combine with ________ to form a metallic hydride.

A) an element from group 5A

B) an element from group 7A

C) an element from group 8A

D) an element from group 1A

E) an element from group 6A