Deck 22: Chemistry of the Nonmetals

Question 1

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

Answer 1

if it combines with oxygen or fluorine

Question 2

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.

Answer 2

by reaction of the corresponding xenon fluoride with water

Question 3

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

A)C
B)P
C)N
D)Si
E)Ge

Answer 3

C

Question 4

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

Question 5

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

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

Question 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

Question 7

Of the following compounds, which is the most stable?

A)XeF₆
B)XeOF₄
C)XeO₃
D)XeO₂F₂
E)XeF₂

Question 8

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

Question 9

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.

Question 10

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.

Question 11

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

Question 12

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

Question 13

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

Question 14

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

Question 15

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)

Question 16

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

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

Question 17

Water gas is ________.

A)H₂O and H₂
B)CO₂ and O₂
C)H₂O and CO₂
D)H₂O and CO
E)H₂ and CO

Question 18

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

Question 19

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

Question 20

Which halogen is the most easily oxidized?

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

Question 21

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.

Question 22

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

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

Question 23

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.

Question 24

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

A)N₂O
B)NO
C)NO₂
D)N₂O₃
E)N₂O₅

Question 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.

Question 26

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

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

Question 27

The oxidation state of oxygen in OF₂ is ________.

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

Question 28

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

Question 29

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

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

Question 30

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

Question 31

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

Question 32

Which one of the following is sodium thiosulfate?

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

Question 33

Which of the following react with oxygen to form superoxides?

A)Ca
B)Na
C)K
D)Sr
E)Ba

Question 34

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

Question 35

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

Question 36

The most stable allotrope of oxygen is ________.

A)H₂O
B)O₃
C)O₂
D)HClO
E)O

Question 37

What sulfur compound is used to sterilize wine?

A)H₂SO₄
B)H₂S
C)Na₂SO₃
D)SO₂
E)Na₂S

Question 38

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

Question 39

The oxidation number of N in HNO₃ is ________.

A)+1
B)+2
C)+3
D)+4
E)+5

Question 40

Amphoteric oxides are also known as ________.

A)basic oxides
B)basic anhydrides
C)acidic oxides
D)acidic anhydrides
E)none of the above

Question 41

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)

Question 42

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

A)0
B)1
C)2
D)3
E)4

Question 43

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.

Question 44

The reaction between nitrogen dioxide and water is a ________.

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

Question 45

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.

Question 46

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

Question 47

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

Question 48

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

Question 49

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

Question 50

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)

Question 51

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

Question 52

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

Question 53

The oxidation number of N in HNO₂ is ________.

A)+1
B)+2
C)+3
D)+4
E)+5

Question 54

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

Question 55

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

A)CO
B)CO₃^2-
C)CO₂
D)HCO₃^-
E)NaHCO₃

Question 56

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

A)HCO₃^-
B)CO
C)CO₂
D)CO₃^2-
E)CaCO₃

Question 57

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

Question 58

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

Question 59

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) + NO₄^2- (aq) + NO (g)
E)2NO₂ (g) + 2H₂O (l) → 2HNO₂ (aq) + O₂ (g) + H₂ (g)

Question 60

The oxidation number of As in H₂AsO₃^- is ________.

A)+1
B)+2
C)+3
D)+4
E)+5

Question 61

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

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

Question 62

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

Question 63

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

Question 64

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

Question 65

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

A)deuterium
B)protium
C)tritium
D)heavy hydrogen
E)common hydrogen

Question 66

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

Question 67

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

Question 68

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)

Question 69

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.

Question 70

B₂O₃ is the anhydride of ________.

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

Question 71

Hydrogen can have oxidation states of ________.

A)+1 only
B)-1, 0, and +1
C)0 and +1 only
D)-1 and +1 only
E)0 only

Question 72

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.

Question 73

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

Question 74

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)

Question 75

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

Question 76

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

Question 77

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

Question 78

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

Question 79

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

Question 80

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

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