85) 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
86) 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.
87) 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.
88) 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
89) 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
90) 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.
91) 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.
92) 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)
93) 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.
94) B2O3 is the anhydride of
A) borous acid
B) diborane
C) tetraboric acid
D) boric acid
E) borax
95) 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).
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
5) 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
6) __________ has the lowest boiling point of any substance known.
A) Ne
B) He
C) Ar
D) Kr
E) Rn
7) The electron-pair geometry and molecular geometry of XeF2 are __________ and __________,
respectively.
A) trigonal bipyramidal; bent
B) trigonal bipyramidal; linear
C) trigonal bipyramidal; bent
D) octahedral; linear
E) octahedral; bent
8) 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
9) The number of electrons in the valence shell of Xe in XeF6 is __________
A) 10
B) 12
C) 14
D) 6
E) 8
10) What is the oxidation state of xenon in XeO2F2?
A) 0
B) +4
C) +8
D) +2
E) +6
11) What is the oxidation state of xenon in XeO4?
A) +8
B) +6
C) +4
D) +2
E) 0
12) Br2 can be prepared by combining NaBr with __________.
A) Cl2
B) HBr
C) HCl
D) NaCl
E) I2
13) The active ingredient in many liquid bleaches is __________.
A) NaCl
B) NaClO
C) NaClO2
D) NaClO3
E) NaClO4
14) Which halogen can react with fluorine to form the compound XF7?
A) bromine
B) fluorine
C) chlorine
D) iodine
E) astatine
15) Which halogen forms an oxyacid with the formula HXO2?
A) bromine
B) fluorine
C) chlorine
D) iodine
E) astatine
16) 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
17) Only the most active metals react with oxygen to form __________.
A) oxides
B) superoxides
C) peroxides
D) ozonides
E) water
18) The dissolution of 1.0 mol of __________ to 1.0 L of water at 25°C would yield the most acidic
solution.
A) SO3
B) CO2
C) CO
D) MgO
E) CaO
19) 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
20) 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
21) 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
22) The Haber process is used to make __________ from __________.
A) HNO3, N2
B) O2, KClO3
C) NH3, N2
D) NO2, O2
E) NO, N2
23) 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
24) The white allotropic form of __________ bursts into flame when exposed to air.
A) phosphorus
B) carbon
C) sulfur
D) selenium
E) oxygen
25) The two allotropic forms of phosphorus are __________ and __________.
A) black, red
B) white, black
C) white, yellow
D) white, red
E) black, yellow
26) 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
27) __________ is formed when wood is heated strongly in the absence of air.
A) Buckminsterfullerene
B) Carbon black
C) Sulfur dioxide
D) Coke
E) Charcoal
28) 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
29) 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
30) The compound whose formula is CaC2 is __________.
A) calcium carbide
B) carborundum
C) carbon calcide
D) calcium dicarbon
E) limestone
31) The addition of solid potassium cyanide to aqueous hydrochloric acid will produce __________.
A) H2O
B) HCN
C) NH3
D) K2CO3
E) K2C2
32) 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
33) What is the oxidation state of carbon in the carbonate ion?
A) +4
B) +2
C) 0
D) -2
E) -4
34) The correct name of H2CO3 is __________.
A) hydrogen carbide
B) hydrogen carbonate ion
C) carbonate ion
D) carbonic acid
E) carboxylic acid
35) The most common oxidation state of silicon is __________.
A) -4
B) +2
C) +6
D) -2
E) none of the above
36) Pyrex® glass is formed by adding an oxide of __________ to soda-lime glass.
A) lead
B) cobalt
C) boron
D) silver
E) phosphorous
37) SiO24- is the __________ ion.
A) orthosilicate ion
B) silicate ion
C) thiosilicate ion
D) silicon tetroxide ion
E) siliconate ion
38) The oxidation state of silicon in SiO24- is __________.
A) 0
B) +6
C) +2
D) +4
E) -4
39) The disilicate ion is __________.
A) Si2O88-
B) Si2O76-
C) Si2O84-
D) Si2O86-
E) Si2O72-
40) Glass is __________ whereas quartz is __________.
A) hard, soft
B) crystalline, amorphous
C) amorphous, crystalline
D) pure SiO2, a mixture of SiO2 and carbonates
E) breakable, not breakable
41) What is the formula of borax?
A) H3BO3
B) H2B4O7
C) P5O8
D) B2O3
E) Na2B4O7∙10H2O
42) Which group 3A element is a metalloid?
A) B
B) Al
C) Ga
D) In
E) Tl
43) 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
44) Diborane is __________.
A) B10H14
B) B2O3
C) BH3
D) B2H6
E) B3BO3
45) Boric oxide is __________.
A) B2O
B) BO2
C) BO
D) B2O3
E) B2O4
46) The correct name for the BH4– ion is __________.
A) borate
B) boride
C) borohydride
D) borite
E) hydroboride
22.3 Short Answer
1) What are the three crystalline allotropes of carbon?
2) Of Li, K, P and Ne which is the least electronegative?
3) In a proton transfer reaction the weaker a Br∅nsted-Lowry acid the __________ is its conjugate.
4) D2O is known as __________.
5) H2 is reacted with __________ to produce methanol.
6) What noble gas is radioactive?
7) Of the non radioactive halogens which is the largest?
8) What halogen, other than astatine, is not usually found in seawater?
9) In a hypohalous acid the oxidation state of the halogen is __________.
10) Write the correctly balanced equation for the reaction between elemental fluorine and sodium
iodide.
11) Write the correctly balanced equation for the reaction between elemental iodine and sodium
bromide.
12) The acid and salts of which halogen-oxyanion are the most stable?
13) What anion containing Cl is used as a rocket fuel?
14) Astatine decays by __________.
15) What is the oxidation state of oxygen in the superoxide ion?
16) In a discussion of oxygen compounds, a disproportionation reaction is __________.
17) What process replenishes O2?
18) I am a highly polar, strongly hydrogen-bonded liquid with a density of 1.47 g/cm3. I can
decompose to form O2. Who am I?
19) If a metal forms more than one oxide, the acidic character of the oxide increases as the oxidation
state of the metal __________.
20) What sulfur gas is used to sterilize wine?
21) The electrical conductivity of __________ is low in the dark, but increases on exposure to light.
22) Write the balanced equation for the reaction of lithium nitride with water.
23) The danger from mixing ammonia with bleach is the production of __________.
24) KNO3 and NaNO3 are also known as __________.
25) What is the primary commercial source of elemental nitrogen?
26) What group 5A element is the most metallic?
27) Low levels of arsenic consumption can lead to __________ or bladder cancer.
28) Why does calcium carbonate dissolve in water containing carbon dioxide?
29) The balanced equation for the production of ethylene from calcium carbide is __________.
30) What is an acetylide?
31) What is meant by the term “composite”?
32) What are the principal components used in making soda-lime glass?
33) What effect does substitution of K2O for Na2O in making soda-lime glass have in its properties?
34) Chains of silicate tetrahedra are called __________.
35) Compounds containing only boron and hydrogen are called __________.
22.4 True/False Questions
1) Air containing 4% H2 can be explosive.
2) The reduction of O2by sodium hydride produces lye.
3) Xenon can have oxidation states of 2, 4, 6, and 8.
4) The instability of xenon fluorides is due to its negative enthalpy of formation.
5) Ozone is a pale blue poisonous gas with an irritating odor.
6) All oxides are ionic compounds.
7) Oxides can react with water to form acids or bases.
8) The reduction of metal oxides uses carbon monoxide.
9) Calcium carbide is a solid source of acetylene.
22.5 Essay Questions
1) 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.
2) Explain why hydrofluoric acid etches glass.
3) Explain why HF (aq) is a relatively weak acid compared to other hydrohalic acids.
4) What are the three steps in the Ostwald process of nitric acid synthesis?
5) Why are nitric acid solutions sometimes yellowish?
6) Describe the major difference in the charge distribution in CH4 and SiH4.
7) Briefly explain why carbon and silicon can form oxides with such different physical properties,
gaseous CO2 and solid SiO2.