Answers Chemistry, 12e (Brown, LeMay, Bursten, Murphy) chapter 7, 8 & 9

Chapter 7

1) The atomic radius of main-group elements generally increases down a group because __________.A) effective nuclear charge increases down a groupB) effective nuclear charge decreases down a groupC) effective nuclear charge zigzags down a groupD) the principal quantum number of the valence orbitals increasesE) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increasesAnswer: DDiff: 2 Page Ref: Sec. 7.3

2) Atomic radius generally increases as we move __________.A) down a group and from right to left across a periodB) up a group and from left to right across a periodC) down a group and from left to right across a periodD) up a group and from right to left across a periodE) down a group; the period position has no effectAnswer: ADiff: 1 Page Ref: Sec. 7.3

3) Atomic radius generally decreases as we move __________.A) down a group and from right to left across a periodB) up a group and from left to right across a periodC) down a group and from left to right across a periodD) up a group and from right to left across a periodE) down a group; the period position has no effectAnswer: BDiff: 1 Page Ref: Sec. 7.3

4) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?A) Mg > Na > P > Si > ArB) Ar > Si > P > Na > MgC) Si > P > Ar > Na > MgD) Na > Mg > Si > P > ArE) Ar > P > Si > Mg > NaAnswer: DDiff: 1 Page Ref: Sec. 7.3

5) Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr?A) Ca > K > As > Ge > KrB) Kr > Ge > As > K > CaC) Ge > As > Kr > K > CaD) K > Ca > Ge > As > KrE) Kr > As > Ge > Ca > KAnswer: DDiff: 1 Page Ref: Sec. 7.3

6) Which one of the following atoms has the largest radius?A) O

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B) FC) SD) ClE) NeAnswer: CDiff: 1 Page Ref: Sec. 7.3

7) Of the choices below, which gives the order for first ionization energies?A) Cl > S > Al > Ar > SiB) Ar > Cl > S > Si > AlC) Al > Si > S > Cl > ArD) Cl > S > Al > Si > ArE) S > Si > Cl > Al > ArAnswer: BDiff: 1 Page Ref: Sec. 7.4

8) Of the choices below, which gives the order for first ionization energies?A) Kr > Se > Br > Ga > GeB) Kr > Br > Se > Ge > GaC) Ga > Br > Ge > Kr > SeD) Ga > Ge > Se > Br > KrE) Br > Se > Ga > Kr > GeAnswer: BDiff: 1 Page Ref: Sec. 7.4

9) __________ have the lowest first ionization energies of the groups listed.A) Alkali metalsB) Transition elementsC) HalogensD) Alkaline earth metalsE) Noble gases Answer: ADiff: 1 Page Ref: Sec. 7.4

10) Which equation correctly represents the first ionization of phosphorus?

A) P (g) + e- → P- (g)

B) P (g) → P- (g) + e-

C) P (g) → P+ (g) + e-

D) P- (g) → P (g) + e-

E) P+ (g) + e- → P (g)Answer: CDiff: 1 Page Ref: Sec. 7.4

11) Which equation correctly represents the first ionization of calcium?

A) Ca (g) → Ca+ (g) + e-

B) Ca (g) → Ca- (g) + e-

C) Ca (g) + e- → Ca- (g)


D) Ca- (g) → Ca (g) + e-

E) Ca+ (g) + e- → Ca (g)Answer: ADiff: 1 Page Ref: Sec. 7.4

12) Which equation correctly represents the first ionization of copper?

A) Cu (g) → Cu+ (g) + e-

B) Cu (g) → Cu- (g) + e-

C) Cu (g) + e- → Cu- (g)

D) Cu- (g) → Cu (g) + e-

E) Cu+ (g) + e- → Cu (g)Answer: ADiff: 1 Page Ref: Sec. 7.4

13) Sodium is much more apt to exist as a cation than is chlorine. This is because __________.A) chlorine is a gas and sodium is a solidB) chlorine has a greater electron affinity than sodium doesC) chlorine is bigger than sodiumD) chlorine has a greater ionization energy than sodium doesE) chlorine is more metallic than sodiumAnswer: DDiff: 1 Page Ref: Sec. 7.5

14) Which equation correctly represents the electron affinity of calcium?

A) Ca (g) + e- → Ca- (g)

B) Ca (g) → Ca+ (g) + e-

C) Ca (g) → Ca- (g) + e-

D) Ca- (g) → Ca (g) + e-

E) Ca+ (g) + e- → Ca (g)Answer: ADiff: 1 Page Ref: Sec. 7.5

15) Which of the following correctly represents the electron affinity of bromine?

A) Br (g) → Br+ (g) + e-

B) Br (g) + e- → Br- (g)

C) Br2 (g) + e- → Br- (g)

D) Br2 (g) + 2 e- → 2 Br- (g)

E) Br+ (g) + e- → Br (g)Answer: BDiff: 1 Page Ref: Sec. 7.5

16) Which of the following correctly represents the electron affinity of phosphorus?

A) P (g) → P+ (g) + e-


B) P (g) + e- → P (g)

C) P4 (g) + e- → P (g)

D) P4 (g) + 4 e- → 4 P- (g)

E) P+ (g) + e- → P (g)Answer: BDiff: 1 Page Ref: Sec. 7.5

17) Of the elements below, __________ is the most metallic.A) sodiumB) bariumC) magnesiumD) calciumE) cesiumAnswer: EDiff: 1 Page Ref: Sec. 7.6

18) Which one of the following is a metalloid?A) GeB) SC) BrD) PbE) CAnswer: ADiff: 1 Page Ref: Sec. 7.6

19) Which one of the following is a metal?A) GeB) SC) BrD) PbE) CAnswer: DDiff: 1 Page Ref: Sec. 7.6

20) The list that correctly indicates the order of metallic character is __________.A) B > N > CB) F > Cl > SC) Si > P > SD) P > S > SeE) Na > K > RbAnswer: CDiff: 1 Page Ref: Sec. 7.6

21) The list that correctly indicates the order of metallic character is __________.A) Sr > Ca > MgB) F > Cl > BrC) C > Ge > SiD) Li > Na > K


E) O > Se > SAnswer: ADiff: 1 Page Ref: Sec. 7.6

22) The element in the periodic table that looks like a metal, is a poor thermal conductor, and acts as an electrical semiconductor is __________.A) SnB) BC) AsD) SiE) GeAnswer: DDiff: 2 Page Ref: Sec. 7.6

23) Nonmetals can be __________ at room temperature.A) solid, liquid, or gasB) solid or liquidC) solid onlyD) liquid onlyE) liquid or gasAnswer: ADiff: 1 Page Ref: Sec. 7.6

24) Which of the following is not a characteristic of metals?A) acidic oxidesB) low ionization energiesC) malleabilityD) ductilityE) These are all characteristics of metals.Answer: ADiff: 1 Page Ref: Sec. 7.6

25) Consider the general valence electron configuration of ns2np5 and the following statements:(i) Elements with this electron configuration are expected to form -1 anions.(ii) Elements with this electron configuration are expected to have large

positive electron affinities.(iii) Elements with this electron configuration are nonmetals.(iv) Elements with this electron configuration form acidic oxides.

Which statements are true?A) (i) and (ii)B) (i), (ii), and (iii)C) (ii) and (iii)D) (i), (iii,) and (iv)E) All statements are true.Answer: DDiff: 2 Page Ref: Sec. 7.6, 7.7

26) Which of the following traits characterizes the alkali metals?A) very high melting pointB) existence as diatomic molecules


C) formation of dianionsD) the lowest first ionization energies in a periodE) the smallest atomic radius in a periodAnswer: DDiff: 1 Page Ref: Sec. 7.7

27) This element is more reactive than lithium and magnesium but less reactive than potassium. This element is __________.A) NaB) RbC) CaD) BeE) FrAnswer: ADiff: 1 Page Ref: Sec. 7.7

28) Alkali metals tend to be more reactive than alkaline earth metals because __________.A) alkali metals have lower densitiesB) alkali metals have lower melting pointsC) alkali metals have greater electron affinitiesD) alkali metals have lower ionization energiesE) alkali metals are not more reactive than alkaline earth metalsAnswer: DDiff: 1 Page Ref: Sec. 7.7

29) Which one of the following beverages originally contained lithium salts?A) Coca-Cola®B) Pepsi-Cola®C) Gatorade®D) Kool-Aid®E) Seven-Up®Answer: EDiff: 1 Page Ref: Sec. 7.7

30) All of the following are ionic compounds except __________.A) K2O

B) Na2SO4C) SiO2D) Li3N

E) NaClAnswer: CDiff: 1 Page Ref: Sec. 7.7

31) All of the halogens __________.A) exist under ambient conditions as diatomic gasesB) tend to form positive ions of several different chargesC) tend to form negative ions of several different chargesD) exhibit metallic characterE) form salts with alkali metals with the formula MX


Answer: EDiff: 1 Page Ref: Sec. 7.8

32) Hydrogen is unique among the elements because __________. 1. It has only one valence electron. 2. It is the only element that can emit an atomic spectrum. 3. Its electron is not at all shielded from its nucleus. 4. It is the lightest element. 5. It is the only element to exist at room temperature as a diatomic gas.A) 1, 2, 3, 4, 5B) 1, 3, 4C) 1, 2, 3, 4D) 2, 3, 4E) 3, 4Answer: EDiff: 2 Page Ref: Sec. 7.8

33) Most of the elements on the periodic table are __________.A) gasesB) nonmetalsC) metalloidsD) liquidsE) metalsAnswer: EDiff: 1 Page Ref: Sec. 7.6

34) Which periodic table group contains only metals?A) 8AB) 2AC) 6AD) 7AE) 5AAnswer: BDiff: 1 Page Ref: Sec. 7.8

Chapter 8 Basic Concepts of Chemical Bonding

1) The type of compound that is most likely to contain a covalent bond is __________.A) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic tableB) a solid metalC) one that is composed of only nonmetalsD) held together by the electrostatic forces between oppositely charged ionsE) There is no general rule to predict covalency in bonds.Answer: CDiff: 1 Page Ref: Sec. 8.3

2) Of the atoms below, __________ is the most electronegative.A) Si


B) ClC) RbD) CaE) SAnswer: BDiff: 1 Page Ref: Sec. 8.4

3) Of the molecules below, the bond in __________ is the most polar.A) HBrB) HIC) HClD) HFE) H2Answer: DDiff: 1 Page Ref: Sec. 8.4

4) Which of the following has the bonds correctly arranged in order of increasing polarity?A) BeF, Mg-F, N-F, O-FB) O-F, N-F, Be-F, Mg-FC) O-F, Be-F, Mg-F, N-FD) N-F, Be-F, Mg-F, O-FE) Mg-F, Be-F, N-F, O-FAnswer: BDiff: 1 Page Ref: Sec. 8.4

5) The Lewis structure of N2H2 shows __________.

A) a nitrogen-nitrogen triple bondB) a nitrogen-nitrogen single bondC) each nitrogen has one nonbonding electron pairD) each nitrogen has two nonbonding electron pairsE) each hydrogen has one nonbonding electron pairAnswer: CDiff: 2 Page Ref: Sec. 8.5

6) There are __________ valence electrons in the Lewis structure of CH3CH2Cl.A) 14B) 12C) 18D) 20E) 10Answer: DDiff: 3 Page Ref: Sec. 8.5

7) There are __________ valence electrons in the Lewis structure of CH3OCH2CH3.A) 18B) 20C) 26D) 32E) 36


Answer: CDiff: 3 Page Ref: Sec. 8.5

8) In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons.A) 2, 2B) 4, 2C) 2, 4D) 0, 6E) 5, 1Answer: BDiff: 2 Page Ref: Sec. 8.5

9) The Lewis structure of the COH32- ion is __________.

A)

B)

C)

D)

E)


Answer: ADiff: 2 Page Ref: Sec. 8.5

10) In the nitrite ion (NO2-), __________.

A) both bonds are single bondsB) both bonds are double bondsC) one bond is a double bond and the other is a single bondD) both bonds are the sameE) there are 20 valence electronsAnswer: DDiff: 2 Page Ref: Sec. 8.6

11) Resonance structures differ by __________.A) number and placement of electronsB) number of electrons onlyC) placement of atoms onlyD) number of atoms onlyE) placement of electrons onlyAnswer: EDiff: 1 Page Ref: Sec. 8.6

12) To convert from one resonance structure to another, __________.A) only atoms can be movedB) electrons and atoms can both be movedC) only electrons can be movedD) neither electrons nor atoms can be movedE) electrons must be addedAnswer: CDiff: 1 Page Ref: Sec. 8.6

13) For resonance forms of a molecule or ion, __________.A) one always corresponds to the observed structureB) all the resonance structures are observed in various proportionsC) the observed structure is an average of the resonance formsD) the same atoms need not be bonded to each other in all resonance formsE) there cannot be more than two resonance structures for a given speciesAnswer: CDiff: 1 Page Ref: Sec. 8.6

14) Which of the following does not have eight valence electrons?A) Cl-B) Xe


C) Ti+4

D) Rb+1

E) Sr+1Answer: EDiff: 2 Page Ref: Sec. 8.7

15) The central atom in __________ does not violate the octet rule.A) SF4B) KrF2C) CF4D) XeF4

E) ICl4-

Answer: CDiff: 2 Page Ref: Sec. 8.7

16) The central atom in __________ violates the octet rule.A) NH3B) SeF2C) BF3D) AsF3E) CF4Answer: CDiff: 2 Page Ref: Sec. 8.7

17) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.A) NF3B) BeH2C) SO2D) CF4E) SO32-

Answer: BDiff: 1 Page Ref: Sec. 8.7

18) Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?A) NB) CC) HD) OE) BAnswer: EDiff: 1 Page Ref: Sec. 8.7

19) Bond enthalpy is __________.A) always positiveB) always negativeC) sometimes positive, sometimes negative


D) always zeroE) unpredictableAnswer: ADiff: 1 Page Ref: Sec. 8.8

20) Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform (CHBr3) is __________ kJ/mol.

A) 1241B) 689C) -689D) 1378E) -1378Answer: ADiff: 1 Page Ref: Sec. 8.8

21) Of the bonds C–C, C=C, and C≡C, the C–C bond is __________.A) strongest/shortestB) strongest/longestC) weakest/longestD) weakest/shortestE) intermediate in both strength and lengthAnswer: CDiff: 1 Page Ref: Sec. 8.8

22) Of the bonds C–N, C=N, and C≡N, the C–N bond is __________.A) strongest/shortestB) strongest/longestC) weakest/shortestD) weakest/longestE) intermediate in both strength and lengthAnswer: DDiff: 1 Page Ref: Sec. 8.8

23) A double bond consists of __________ pairs of electrons shared between two atoms.A) 1B) 2C) 3D) 4E) 6Answer: BDiff: 2 Page Ref: Sec. 8.3

24) A triple bond consists of __________ pairs of electrons shared between two atoms.A) 1B) 2C) 3D) 4E) 6Answer: CDiff: 2 Page Ref: Sec. 8.3


25) In the molecule below, which atom has the largest partial negative charge?

Cl |

F- C -Br | I

A) ClB) FC) BrD) IE) CAnswer: BDiff: 1 Page Ref: Sec. 8.4

26) The ability of an atom in a molecule to attract electrons is best quantified by the __________.A) paramagnetismB) diamagnetismC) electronegativityD) electron change-to-mass ratioE) first ionization potentialAnswer: CDiff: 1 Page Ref: Sec. 8.4

27) Given the electronegativities below, which covalent single bond is most polar?Element: H C N O Electronegativity: 2.1 2.5 3.0 3.5

A) C-HB) N-HC) O-HD) O-CE) O-NAnswer: CDiff: 1 Page Ref: Sec. 8.4

28) A nonpolar bond will form between two __________ atoms of __________ electronegativity.A) different, oppositeB) identical, differentC) different, differentD) similar, differentE) identical, equalAnswer: EDiff: 1 Page Ref: Sec. 8.4

29) The formal charge on nitrogen in NO3- is __________.


A) -1B) 0C) +1D) +2E) -2Answer: CDiff: 2 Page Ref: Sec. 8.5

30) The formal charge on sulfur in SO42- is __________, where the Lewis structure of the ion is:

A) -2B) 0C) +2D) +4E) -4Answer: BDiff: 2 Page Ref: Sec. 8.5

31) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is __________.

A) 0B) +1C) -1D) +2E) -2Answer: BDiff: 1 Page Ref: Sec. 8.6

32) How many equivalent resonance forms can be drawn for CO32-(carbon is the central atom)?

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


Diff: 1 Page Ref: Sec. 8.6

33) Using the table of average bond energies below, the ΔH for the reaction is __________ kJ.

Bond: C≡C C–C H–I C–I C–H

D (kJ/mol): 839 348 299 240 413

A) +160B) -160C) -217D) -63E) +63Answer: CDiff: 1 Page Ref: Sec. 8.8

34) Using the table of average bond energies below, the ΔH for the reaction is __________ kJ.

H–C≡C–H (g) + H–I (g) → H2CCHI (g)

Bond: C≡C C=C H–I C–I C–HD (kJ/mol): 839 614 299 240 413

A) +506B) -931C) -506D) -129E) +129Answer: DDiff: 1 Page Ref: Sec. 8.8

35) Using the table of average bond energies below, the △H for the reaction is __________ kJ.

C≡O (g) + 2H2 (g) → H3C–O–H (g)

Bond: C–O C=O C≡O C–H H–H O–HD (kJ/mol): 358 799 1072 413 436 463

A) +276B) -276C) +735D) -735E) -116Answer: EDiff: 1 Page Ref: Sec. 8.8

36) Using the table of bond dissociation energies, the ΔH for the following reaction is __________ kJ. 2HCl (g) + F2 (g) → 2HF (g) + Cl2 (g)


A) -359B) -223C) 359D) 223E) 208Answer: A

Chapter 9 Molecular Geometry and Bonding Theories

1) ClF3 has "T-shaped" geometry. There are __________ non-bonding domains in this molecule.A) 0B) 1C) 2D) 3E) 4Answer: CDiff: 4 Page Ref: Sec. 9.2

2) The electron domain and molecular geometry of BrO2- is __________.A) tetrahedral, trigonal planarB) trigonal planar, trigonal planarC) trigonal pyramidal, linearD) tetrahedral, bentE) trigonal pyramidal, seesawAnswer: DDiff: 4 Page Ref: Sec. 9.2

3) The electron-domain geometry of __________ is tetrahedral.A) CBr4B) PH3C) CCl2Br2D) XeF4E) all of the above except XeF4Answer: EDiff: 2 Page Ref: Sec. 9.2

4) The molecular geometry of the BrO3- ion is __________.

A) trigonal pyramidalB) trigonal planarC) bent


D) tetrahedralE) T-shapedAnswer: ADiff: 2 Page Ref: Sec. 9.2

5) The molecular geometry of the left-most carbon atom in the molecule below is __________.

A) trigonal planarB) trigonal bipyramidalC) tetrahedralD) octahedralE) T-shapedAnswer: CDiff: 1 Page Ref: Sec. 9.2

6) The molecular geometry of the right-most carbon in the molecule below is __________.

A) trigonal planarB) trigonal bipyramidalC) tetrahedralD) octahedralE) T-shapedAnswer: ADiff: 1 Page Ref: Sec. 9.2

7) The central iodine atom in the ICl4- ion has __________ nonbonded electron pairs and __________ bonded

electron pairs in its valence shell.A) 2, 2B) 3, 4C) 1, 3D) 3, 2E) 2, 4Answer: EDiff: 1 Page Ref: Sec. 9.2

8) The central iodine atom in IF5 has __________ unbonded electron pairs and __________ bonded electron

pairs in its valence shell.A) 1, 5B) 0, 5C) 5, 1D) 4, 1E) 1, 4


Answer: ADiff: 1 Page Ref: Sec. 9.2

9) The central Xe atom in the XeF4 molecule has __________ unbonded electron pairs and __________ bonded electron pairs in its valence shell.A) 1, 4B) 2, 4C) 4, 0D) 4, 1E) 4, 2Answer: BDiff: 1 Page Ref: Sec. 9.2

10) PCl5 has __________ electron domains and a __________ molecular arrangement.A) 6, trigonal bipyramidalB) 6, tetrahedralC) 5, square pyramidalD) 5, trigonal bipyramidalE) 6, seesawAnswer: DDiff: 3 Page Ref: Sec. 9.2

11) Of the molecules below, only __________ is polar.A) SbF5B) AsH3C) I2D) SF6E) CH4Answer: BDiff: 2 Page Ref: Sec. 9.3

12) Of the molecules below, only __________ is nonpolar.A) CO2B) H2O

C) NH3D) HClE) TeCl2Answer: ADiff: 1 Page Ref: Sec. 9.3

13) Of the molecules below, only __________ is polar.A) CCl4B) CH4C) SeF4D) SiCl4Answer: CDiff: 1 Page Ref: Sec. 9.3


14) Of the molecules below, only __________ is nonpolar.A) BF3B) NF3C) IF3D) PBr3E) BrCl3Answer: ADiff: 1 Page Ref: Sec. 9.3

15) The molecular geometry of the BeCl2 molecule is __________, and this molecule is __________.

A) linear, nonpolarB) linear, polarC) bent, nonpolarD) bent, polarE) trigonal planar, polarAnswer: ADiff: 1 Page Ref: Sec. 9.3

16) The molecular geometry of the PF3 molecule is __________, and this molecule is __________.

A) trigonal planar, polarB) trigonal planar, nonpolarC) trigonal pyramidal, polarD) trigonal pyramidal, nonpolarE) tetrahedral, unipolarAnswer: CDiff: 2 Page Ref: Sec. 9.3

17) The molecular geometry of the BCl3 molecule is __________, and this molecule is __________.A) trigonal pyramidal, polarB) trigonal pyramidal, nonpolarC) trigonal planar, polarD) trigonal planar, nonpolarE) trigonal bipyramidal, polarAnswer: DDiff: 1 Page Ref: Sec. 9.3

18) The sp2 atomic hybrid orbital set accommodates __________ electron domains.A) 2B) 3C) 4D) 5E) 6Answer: BDiff: 1 Page Ref: Sec. 9.5

19) The hybridizations of nitrogen in NF3 and NH3 are __________ and __________, respectively.

A) sp2, sp2


B) sp, sp3

C) sp3, sp

D) sp3, sp3

E) sp2, sp3

Answer: DDiff: 1 Page Ref: Sec. 9.5

20) The hybridization of the oxygen atom labeled y in the structure below is __________. The C-O-H bond angle is __________.

A) sp, 180°B) sp2, 109.5°C) sp3, 109.5°D) sp3d2, 90°E) sp, 90°Answer: CDiff: 2 Page Ref: Sec. 9.5

21) There are __________ unhybridized p atomic orbitals in an sp-hybridized carbon atom.A) 0B) 1C) 2D) 3E) 4Answer: CDiff: 1 Page Ref: Sec. 9.5

22) There are __________ unhybridized p atomic orbitals in an sp2-hybridized carbon atom.A) 0B) 1C) 2D) 3E) 4Answer: BDiff: 1 Page Ref: Sec. 9.5

23) Valence bond theory does not address the issue of __________.A) excited states of moleculesB) molecular shapeC) covalent bondingD) hybridization


E) multiple bondsAnswer: ADiff: 2 Page Ref: Sec. 9.5

24) The carbon-carbon σ bond in ethylene, H2C=CH2, results from the overlap of __________.

A) sp hybrid orbitalsB) sp3 hybrid orbitalsC) sp2 hybrid orbitalsD) s atomic orbitalsE) p atomic orbitalsAnswer: CDiff: 1 Page Ref: Sec. 9.6

25) The π bond in ethylene, H2C=CH2, results from the overlap of __________.

A) sp3 hybrid orbitalsB) s atomic orbitalsC) sp hybrid orbitalsD) sp2 hybrid orbitalsE) p atomic orbitalsAnswer: EDiff: 1 Page Ref: Sec. 9.6

26) A typical triple bond consists of __________.A) three sigma bondsB) three pi bondsC) one sigma and two pi bondsD) two sigma and one pi bondE) three ionic bondsAnswer: CDiff: 1 Page Ref: Sec. 9.6

27) A typical double bond consists of __________.A) three sigma bondsB) three pi bondsC) one sigma and two pi bondsD) one sigma and one pi bondE) three ionic bondsAnswer: DDiff: 1 Page Ref: Sec. 9.6


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Answers Chemistry, 12e (Brown, LeMay, Bursten, Murphy) chapter 7, 8 & 9