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Central Science: Chapter 22

front 1

How many oxygen atoms are bonded to each silicon atom in SiO2?
A) 1
B) 2
C) 3
D) 4
E) none

back 1

D

front 2

Of the atoms below, ________ is the most effective in forming π bonds.
A) C
B) P
C) N
D) Si
E) Ge

back 2

A

front 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 has the same chemical properties as protium but reacts more slowly.
D) The atomic number of tritium is 1.

back 3

A

front 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

back 4

C

front 5

Water gas is ________.
A) H2O and H2
B) CO2 and O2
C) H2O and CO2
D) H2O and CO
E) H2 and CO

back 5

E

front 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

back 6

D

front 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

back 7

A

front 8

Which of the following would produce a basic solution?
A) Na2O and CaO
B) CO and CO2
C) CaH2 only
D) Na2O, CaO, and CaH2
E) CO, CO2, and CaH2

back 8

D

front 9

Which of the following would produce an acidic solution?
A) Na2O and MgO
B) Na2O, MgO, and CaH2
C) only
D) CaH2 only
E) CO, CO2, and CaH2

back 9

C

front 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.

back 10

D

front 11

Which of the following compounds is the most stable?
A) XeOCl4
B) XeO2Cl2
C) XeO3
D) XeCl6
E) XeCl2

back 11

D

front 12

Consider the following xenon compounds:

(i) XeCl2 (ii) XeCl4 (iii) XeO4 (iv) XeOCl4 (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

back 12

C

front 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

back 13

D

front 14

Which noble gas is known to form a variety of binary compounds?
A) Xe
B) He
C) Ne
D) Ar
E) Kr

back 14

A

front 15

Interhalogen compounds ________.
A) are exceedingly reactive
B) contain halogens in both positive and negative oxidation states
C) are powerful oxidizing agents
D) all of the above

back 15

D

front 16

Which elemental halogen(s) can be used to prepare from NaI?
A) F2 only
B) Cl2 only
C) Br2 only
D) both Cl2 and Br2, but not F2
E) F2, Cl2, and Br2

back 16

E

front 17

Which halogen is the most easily oxidized?
A) F
B) Cl
C) Br
D) I

back 17

D

front 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

back 18

B

front 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 but bromine is not
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

back 19

A

front 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

back 20

B

front 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

back 21

E

front 22

The most stable allotrope of oxygen is ________.
A) H2O
B) O3
C) O2
D) HClO
E) O

back 22

C

front 23

Which of the following react with oxygen to form superoxides?
A) Ca
B) Na
C) K
D) Sr
E) Ba

back 23

C

front 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

back 24

A

front 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.

back 25

A

front 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

back 26

A

front 27

The oxidation state of oxygen in OF2 is ________.
A) +1
B) +2
C) 0
D) -1
E) -2

back 27

B

front 28

________ are typically basic while ________ are typically acidic.
A) Nonmetal oxides, metal oxides
B) Metals, nonmetals
C) Metal oxides, nonmetal oxides
D) Nonmetals, metals

back 28

C

front 29

Amphoteric oxides are also known as ________.
A) basic oxides
B) basic anhydrides
C) acidic oxides
D) acidic anhydrides
E) none of the above

back 29

E

front 30

Which element in group 7A is not capable of having an expanded valence shell?
A) astatine
B) fluorine
C) chlorine
D) bromine
E) iodine

back 30

B

front 31

Which element in group 6A is not capable of having an expanded valence shell?
A) sulfur
B) tellurium
C) selenium
D) oxygen
E) polonium

back 31

D

front 32

What sulfur compound is used to sterilize wine?
A) H2SO4
B) H2S
C) Na2SO3
D) SO2
E) Na2S

back 32

D

front 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

back 33

C

front 34

Which form of elemental sulfur is the most stable at room temperature?
A) rhombic sulfur
B) monoclinic
C) hexagonal
D) triclinic
E) tetraclinic

back 34

A

front 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

back 35

A

front 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

back 36

C

front 37

Which one of the following is sodium thiosulfate?
A) Na2SO4
B) Na2SO3
C) Na2S2O3
D) Na2S4O6
E) Na2S

back 37

C

front 38

Which one of the following is true concerning pure hydrazine?
A) It is a weak reducing agent.
B) It can be made by reaction of nitrogen and ammonia.
C) It is used as a rocket fuel.
D) It is a hydride of oxygen.
E) It is a hydride of ammonia.

back 38

C

front 39

The Ostwald process is by which NH3 is converted commercially into ________.
A) HNO3
B) NO
C) NO2
D) N2O3
E) N2O5

back 39

A

front 40

The oxidation number of N in NO3- is ________.
A) +1
B) +2
C) +3
D) +4
E) +5

back 40

E

front 41

The oxidation number of N in NO2- is ________.
A) +1
B) +2
C) +3
D) +4
E) +5

back 41

C

front 42

The oxidation number of Pb in PbO2 is ________.
A) +1
B) +2
C) +3
D) +4
E) +5

back 42

D

front 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) → 2 NO (g)
D) N2H4 (l) + O2 (g) → N2 (g) + 2 H2O (g)
E) N2H4 (l) + O2 (g) → N2 (g) + 2H2 (g) + O2 (g)

back 43

D

front 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

back 44

A

front 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)

back 45

B

front 46

The reaction between nitrogen dioxide and water is a ________.
A) decomposition
B) combustion
C) disproportionation
D) neutralization
E) replacement

back 46

C

front 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

back 47

A

front 48

Which phosphorus chloride compound will form in the reaction of phosphorus with excess chlorine gas?
A) PCl3
B) PCl2
C) PCl5
D) PCl4
E) PCl

back 48

C

front 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

back 49

A

front 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

back 50

E

front 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.

back 51

D

front 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

back 52

B

front 53

Which of the following would produce the most strongly acidic aqueous solution?
A) HCO3-
B) CO
C) CO2
D) CO32-
E) CaCO3

back 53

D

front 54

How many lone pair of electrons are there in one molecule of carbon monoxide?
A) 0
B) 1
C) 2
D) 3
E) 4

back 54

C

front 55

Which of the following is not an allotropic form of carbon?
A) graphite
B) carbon dioxide
C) diamond
D) buckminsterfullerene
E) All of the above are allotropic forms of carbon.

back 55

B

front 56

Which of the following statements best describes graphite?
A) It is a soft, slippery, and black solid that has a metallic luster and conducts electricity.
B) It is a soft, slippery, and black gas that has a metallic luster and conducts electricity.
C) It is a soft, slippery, and black liquid that has a metallic luster and conducts electricity.
D) It is a soft, slippery, and black solid that has a metallic luster and does not conduct electricity.
E) It is a soft, slippery, and black solid that has a nonmetallic dull look and does not conduct electricity.

back 56

A

front 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

back 57

E

front 58

Which of the following would produce the strongest basic aqueous solution?
A) CO
B) CO2
C) H2CO3
D) Na2CO3
E) KHCO3

back 58

D

front 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)

back 59

A

front 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

back 60

B

front 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

back 61

D

front 62

Addition of 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

back 62

A

front 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

back 63

A

front 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

back 64

B

front 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

back 65

E

front 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

back 66

A

front 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

back 67

B

front 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

back 68

D

front 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

back 69

D

front 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.

back 70

E

front 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

back 71

C

front 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)

back 72

A

front 73

________ can violate the octet rule in its compounds.
A) carbon
B) nitrogen
C) boron
D) oxygen
E) none of these elements can violate the octet rule.

back 73

C

front 74

B2O3 is the anhydride of ________.
A) borous acid
B) diborane
C) tetraboric acid
D) boric acid
E) borax

back 74

D

front 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)

back 75

E

front 76

The most common isotope of hydrogen is sometimes referred to as ________.
A) deuterium
B) protium
C) tritium
D) heavy hydrogen
E) common hydrogen

back 76

B

front 77

In metallic hydrides, the oxidation number of hydrogen is considered to be ________.
A) -2
B) -1
C) 0
D) +1
E) +2

back 77

B

front 78

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

back 78

D

front 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

back 79

D

front 80

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

back 80

B

front 81

________ has the highest boiling point of following series.
A) Ne
B) He
C) Kr
D) Ar
E) Rn

back 81

E

front 82

The electron-pair geometry and molecular geometry of XeF4 are ________ and ________, respectively.
A) octahedral; square pyramidal
B) tetrahedral; tetrahedral
C) octahedral; linear
D) octahedral; square planar
E) octahedral; bent

back 82

D

front 83

Hybridization of Xe in XeF4 is ________ and in XeF2 is ________.
A) sp3d2, sp3d2
B) sp3d, sp3d2
C) sp3d2, sp3d
D) sp3, sp3d
E) sp3, sp3d2

back 83

C

front 84

The number of electrons in the valence shell of Xe in XeF6 is ________
A) 10
B) 12
C) 14
D) 6
E) 8

back 84

C

front 85

What is the oxidation state of xenon in XeO2F2?
A) 0
B) +4
C) +8
D) +2
E) +6

back 85

E

front 86

What is the oxidation state of xenon in XeO4?
A) +8
B) +6
C) +4
D) +2
E) 0

back 86

A

front 87

Br2 can be prepared by combining NaBr with ________.
A) Cl2
B) HBr
C) HCl
D) NaCl
E) I2

back 87

A

front 88

The active ingredient in many liquid bleaches is ________.
A) NaCl
B) NaClO
C) NaClO2
D) NaClO3
E) NaClO4

back 88

B

front 89

Which halogen can react with fluorine to form the compound XF7?
A) bromine
B) fluorine
C) chlorine
D) iodine
E) astatine

back 89

D

front 90

Which halogen forms an oxyacid with the formula HXO2?
A) bromine
B) fluorine
C) chlorine
D) iodine
E) astatine

back 90

C

front 91

The primary commercial use of oxygen is ________.
A) for the treatment of respiratory distress
B) in oxyacetylene welding
C) as a household bleach
D) as an oxidizing agent
E) to charge oxygen-containing cylinders used by deep-sea divers

back 91

D

front 92

Only the most active metals react with oxygen to form ________.
A) oxides
B) superoxides
C) peroxides
D) ozonides
E) water

back 92

B

front 93

Dissolving 2.0 mol of ________ in 1.0 L of water at 25 °C would yield the most acidic solution.
A) CO2
B) Na2O
C) SO3
D) CO
E) CaO

back 93

C

front 94

The nitride ion is a strong Br∅nsted-Lowry base. Mg3N2 reacts with water to produce ________.
A) N2
B) N2O
C) NO
D) NO2
E) NH3

back 94

E

front 95

The primary commercial use of elemental nitrogen is in the manufacture of ________.
A) plastics
B) explosives
C) nitrogen-containing fertilizers
D) rubber
E) chlorine bleach

back 95

C

front 96

What is the coefficient of NO2 when the following disproportionation reaction is balanced?

NO2 (g) + H2O (l) →H+ (aq) + NO3- (aq) + NO (g)

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

back 96

C

front 97

The Haber process is used to make ________ from ________.
A) HNO3, N2
B) O2, KClO3
C) NH3, N2
D) NO2, O2
E) NO, N2

back 97

C

front 98

Most mined phosphate rock is ________.
A) used as a strong acid
B) used as a reducing agent
C) used as a detergent
D) converted to fertilizer
E) discarded as a by-product

back 98

D

front 99

The white allotropic form of ________ bursts into flame when exposed to air.
A) phosphorus
B) carbon
C) sulfur
D) selenium
E) oxygen

back 99

A

front 100

The two allotropic forms of phosphorus are ________ and ________.
A) black, red
B) white, black
C) white, yellow
D) white, red
E) black, yellow

back 100

D

front 101

The principal combustion products of compounds containing carbon and hydrogen in the presence of excess O2 are ________.
A) CO2 and H2O
B) CO2 and H2O2
C) CO2 and H
D) C(graphite) and H2
E) CO2 and H2

back 101

A

front 102

________ is formed when wood is heated strongly in the absence of air.
A) Buckminsterfullerene
B) Carbon black
C) Sulfur dioxide
D) Coke
E) Charcoal

back 102

E

front 103

To produce carbon black, ________.
A) diamond is exposed to extremely high pressures and temperatures
B) wood is strongly heated in the absence of oxygen
C) coal is strongly heated in the absence of oxygen
D) hydrocarbons such as methane are heated in a very limited supply of oxygen
E) graphite is cooled to -273 °C

back 103

D

front 104

Although CaCO3 is essentially insoluble in pure water, it dissolves slowly in acidic ground water due to formation of ________.
A) insoluble Ca(OH)2
B) soluble Ca(OH)2
C) insoluble Ca(HCO3)2
D) soluble Ca(HCO3)2
E) soluble CaO

back 104

D

front 105

The compound whose formula is CaC2 is ________.
A) calcium carbide
B) carborundum
C) carbon calcide
D) calcium dicarbon
E) limestone

back 105

A

front 106

An example of a form of pure carbon that contains only sp3 hybridized carbon atoms is ________.
A) diamond
B) charcoal
C) graphite
D) carbon black
E) carborundum

back 106

A

front 107

What is the oxidation state of carbon in the carbonate ion?
A) +4
B) +2
C) 0
D) -2
E) -4

back 107

A

front 108

The correct name of H2CO3 is ________.
A) hydrogen carbide
B) hydrogen carbonate ion
C) carbonate ion
D) carbonic acid
E) carboxylic acid

back 108

D

front 109

The most common oxidation state of silicon is ________.
A) -4
B) +2
C) +6
D) -2
E) +4

back 109

E

front 110

Pyrex® glass is formed by adding an oxide of ________ to soda-lime glass.
A) lead
B) cobalt
C) boron
D) silver
E) phosphorous

back 110

C

front 111

SiO44- is the ________ ion.
A) orthosilicate ion
B) silicide ion
C) thiosilicate ion
D) silicon tetroxide ion
E) siliconate ion

back 111

A

front 112

The oxidation state of silicon in SiO44- is ________.
A) 0
B) +6
C) +2
D) +4
E) -4

back 112

D

front 113

The disilicate ion is ________.
A) Si2O88-
B) Si2O76-
C) Si2O84-
D) Si2O86-
E) Si2O72-

back 113

B

front 114

Glass is ________ whereas quartz is ________.
A) hard, soft
B) crystalline, amorphous
C) amorphous, crystalline
D) pure Si , a mixture of Si and carbonates
E) breakable, not breakable

back 114

C

front 115

What is the formula of borax?
A) H3BO3
B) H2B4O7
C) P5O8
D) B2O3
E) Na2B4O7 ∙ 10H2O

back 115

E

front 116

Which group 3A element is a metalloid?
A) B
B) Al
C) Ga
D) In
E) Tl

back 116

A

front 117

Tetraboric acid, H2B4O7, is prepared by heating boric acid, H3BO3 (a condensation reaction involving water loss). If 400.0 mmol H3BO3 are used, what mass (g) of H2O is formed, assuming quantitative stoichiometric conversion?
A) 5.77
B) 0.500
C) 0.320
D) 7.21
E) 9.01

back 117

E

front 118

Diborane is ________.
A) B10H14
B) B2O3
C) BH3
D) B2H6
E) H3BO3

back 118

D

front 119

Boric oxide is ________.
A) B2O
B) BO2
C) BO
D) B2O3
E) B2O4

back 119

D

front 120

The correct name for NaBH4 is ________.
A) sodium borohydride
B) sodium borate
C) sodium boride
D) sodium borite
E) sodium hydroboride

back 120

A

front 121

The most nonmetallic element is ________.
A) S
B) P
C) Cl
D) Br
E) Se

back 121

C

front 122

The least electronegative of the elements below is ________.
A) Se
B) S
C) F
D) Cl
E) Br

back 122

A

front 123

In the following chemical equation

PCl3 + 3H2O →

the products (when the equation is balanced) are ________.
A) H3PO3 + 3HCl
B) P(OH)3 + 3HCl
C) H(ClO)3 + PH3
D) HPCl2 + Cl(OH)3
E) PO3 + 3HCl

back 123

A

front 124

Which of the following is a molecular hydride?
A) H2O
B) CsH
C) MgH2
D) TiH2
E) LiOH

back 124

A

front 125

Which of the following is an ionic hydride?
A) CaH2
B) C2H4
C) HCl
D) NH3
E) CsOH

back 125

A

front 126

Which of the following compounds would produce the most acidic aqueous solution?
A) MgH2
B) C2H2
C) HF
D) KH
E) H2

back 126

C

front 127

The oxidation state of sulfur in the SO3 molecule is ________.
A) +6
B) +2
C) -2
D) +4
E) 0

back 127

A

front 128

The oxidation state of phosphorous in the PF5 molecule is ________.
A) +5
B) +4
C) -5
D) +6
E) 0

back 128

A

front 129

The oxidation state of chlorine in the ClO- molecule is ________.
A) +1
B) +3
C) +4
D) +5
E) -1

back 129

A

front 130

Which one of the following compounds is superoxide?
A) NaO2
B) Na2O
C) Na2O2
D) NaOH
E) H2O

back 130

A

front 131

Which compound would produce a basic aqueous solution?
A) KH
B) H2S
C) C2H6
D) CH3OH
E) H2O

back 131

A

front 132

What is the F—Xe—F bond angle in XeF2?
A) 180°
B) 90°
C) 109.5°
D) 120°
E) 60°

back 132

A

front 133

The oxidation number of xenon in XeF4 is ________.
A) +4
B) +3
C) +5
D) +1
E) -6

back 133

A

front 134

Which equation correctly represents the reaction between elemental chlorine and sodium iodide?
A) Cl + NaI → I + NaCl
B) Cl- + NaI → I- + NaCl
C) Cl2 + 2NaI → I2 + 2NaCl
D) Cl + NaI → 1/2 I2 + NaCl
E) Cl2 + NaI → NaCl2 + I-

back 134

C

front 135

Which one of the following compounds is peroxide?
A) Li2O2
B) Li2O
C) LiO2
D) both Li2O2 and LiO2
E) H2O

back 135

A

front 136

The oxidation state of oxygen in O2F2 is ________.
A) +1
B) -1
C) +2
D) 0
E) -2

back 136

A

front 137

What is the molecular shape of the SF2 molecule?
A) tetrahedral
B) linear
C) bent
D) trigonal planar
E) trigonal pyramidal

back 137

C

front 138

The oxidation state of nitrogen in the NO2 molecule is ________.
A) +4
B) +3
C) +5
D) +2
E) -3

back 138

A

front 139

The oxidation state of As in the As2O3 molecule is ________.
A) 3
B) 2
C) 4
D) -3
E) 0

back 139

A

front 140

The oxidation number of B in B2O3 is ________.
A) +3
B) +2
C) +1
D) +4
E) +5

back 140

A

front 141

Which of the following is the nitride ion?
A) N3-
B) N3-
C) NO3-
D) N-
E) NO2-

back 141

A

front 142

Which pair of formula/name is incorrect?
A) NO2 / dinitrogen oxide
B) N2O / nitrous oxide
C) NO / nitric oxide
D) N2O4 / dinitrogen tetroxide
E) N2O5 / dinitrogen pentoxide

back 142

A

front 143

The molecular shape of the PF3 molecule is ________.
A) trigonal pyramidal
B) trigonal bipyramidal
C) see-saw
D) T-shaped
E) octahedral

back 143

A

front 144

How many lone pair of electrons are there in one molecule of dinitrogen monoxide?
A) 4
B) 3
C) 5
D) 2
E) 1

back 144

A

front 145

What are the five crystalline allotropes of carbon?

back 145

graphene, carbon nanotubes, diamond, graphite, and buckminsterfullerene

front 146

Of Li, K, P and Ne which is the most electronegative?

back 146

P is the most electronegative

front 147

In a proton transfer reaction the weaker a Br∅nsted-Lowry acid the ________ is its conjugate.

back 147

stronger

front 148

D2O, deuterium oxide, is also known as ________.

back 148

heavy water

front 149

H2 is reacted with ________ to produce methanol.

back 149

CO; carbon monoxide

front 150

What noble gas is radioactive?

back 150

radon

front 151

Of the nonradioactive halogens, which is the largest?

back 151

iodine

front 152

Which group 7A halogen is radioactive?

back 152

astatine

front 153

In a hypohalous acid, the oxidation state of the halogen is ________.

back 153

+1

front 154

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

back 154

F2 + 2 NaI → I2 + 2 NaF

front 155

Write the correctly balanced equation for the reaction between elemental iodine and sodium bromide.

back 155

I2 + NaBr → no reaction

front 156

The acid and salts of which halogen-oxyanion are the most stable?

back 156

perchlorate

front 157

What anion containing Cl is used as a rocket fuel?

back 157

perchlorate

front 158

Group 8A elements are all gases at room temperature except for ________.

back 158

radon

front 159

What is the oxidation state of oxygen in the superoxide ion?

back 159

- 1/2

front 160

In oxygen compounds, a disproportionation reaction is a reaction in which oxygen is simultaneously ________.

back 160

oxidized and reduced

front 161

What process replenishes O2?

back 161

photosynthesis

front 162

Hydrogen peroxide is a highly polar and strongly hydrogen-bonded liquid. It decomposes to form water and ________.

back 162

oxygen gas

front 163

If a metal forms more than one oxide, the acidic character of the oxide increases as the oxidation state of the metal ________.

back 163

increases

front 164

What sulfur gas is used to sterilize wine?

back 164

SO2

front 165

The electrical conductivity of ________ is low in the dark, but increases on exposure to light.

back 165

selenium

front 166

The danger from mixing ammonia with bleach is the production of ________.

back 166

chloramine; NH2Cl

front 167

KNO3 and NaNO3 are also known as ________.

back 167

saltpeter

front 168

What is the primary commercial source of elemental nitrogen?

back 168

fractional distillation of liquid air

front 169

What group 5A element is the least metallic?

back 169

nitrogen

front 170

Low levels of arsenic consumption can lead to ________ or bladder cancer.

back 170

lung

front 171

Why does calcium carbonate dissolve in water containing carbon dioxide?

back 171

because the dissolved carbon dioxide makes the water slightly acidic

front 172

The balanced equation for the production of ethylene from calcium carbide is ________.

back 172

CaC2 + 2H2O → Ca(OH)2 + C2H2

front 173

What is an acetylide?

back 173

a carbide containing the C22- ion

front 174

What is meant by the term "composite"?

back 174

a combination of two or more materials

front 175

What are the principal components used in making soda-lime glass?

back 175

calcium oxide, sodium oxide, and silicon dioxide

front 176

What effect does substitution of K2O for Na2O in making soda-lime glass have in its properties?

back 176

increases hardness and melting point

front 177

Chains of silicate tetrahedra are called ________.

back 177

asbestos

front 178

Compounds containing only boron and hydrogen are called ________.

back 178

boranes

front 179

Air containing 4% H2 can be explosive.

back 179

true

front 180

The reduction of O2 by sodium hydride produces lye.

back 180

true

front 181

Xenon can have oxidation states of 2, 4, 6, and 8.

back 181

true

front 182

The instability of xenon fluorides is due to its negative enthalpy of formation.

back 182

false

front 183

Ozone is a pale blue poisonous gas with an irritating odor.

back 183

true

front 184

All oxides are ionic compounds.

back 184

false

front 185

Oxides can react with water to form acids or bases.

back 185

true

front 186

The reduction of metal oxides uses carbon monoxide.

back 186

true

front 187

Calcium carbide is a solid source of acetylene.

back 187

true

front 188

Explain why silicon does not form any allotropes with structures analogous to that of graphite or buckminsterfullerenes, even though it is in the same group as carbon.

back 188

Silicon is large enough to prevent efficient sideways-overlap of p orbitals required for π-bond formation.

front 189

Explain why hydrofluoric acid etches glass.

back 189

Hydrofluoric acid forms a soluble hexafluorosilic acid (H2SiF6), removing silicon from glass and, consequently, destroying it.

front 190

An aqueous solution of HF is considered a relatively ________ acid.

back 190

weak

front 191

What are the three steps in the Ostwald process of nitric acid synthesis?

back 191

1) oxidation of ammonia to NO and water, 2) oxidation of NO to NO2, 3) reaction of NO2 with water.

front 192

Photochemical decomposition of HNO3 produces small amounts of NO2 which causes the solution to sometimes become ________ in color.

back 192

yellow

front 193

Describe the major difference in the charge distribution in CH4 and SiH4.

back 193

Even though both C—H and Si—H bonds are polar, both CH4 and SiH4 are nonpolar due to their tetrahedral symmetry. Because carbon is more electronegative than hydrogen, bonding electrons are somewhat shifted towards carbon, leaving hydrogen atoms with positive partial charges. On the other hand, silicon is somewhat less electronegative than hydrogen and the bonding electrons are shifted towards hydrogen atoms, which adopt slightly negative charges.

front 194

Briefly explain why carbon and silicon can form oxides with such different physical properties, gaseous CO2 and solid SiO2.

back 194

Carbon atoms are small enough to form π bonds with oxygen due to the overlap of p orbitals, resulting in the formation of double C O bonds. Consequently, CO2 forms individual molecules that interact with each other via weak London dispersion forces. Silicon atoms are too large and form only single bonds with oxygen, four such bonds per each silicon atom, with each oxygen atom bridging between two silicon atoms, resulting in a covalent-network solid.