Ch08_Testbank
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8.1 Multiple-Choice and Bimodal Questions1) There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom.A) 4, 2B) 2, 4C) 2, 3D) 4, 3E) 0, 3Answer: CDiff: 1Page Ref: Sec. 8.12) In the Lewis symbol for a fluorine atom, there are __________ paired and __________ unpaired electrons.A) 4, 2B) 4,1C) 2, 5D) 6, 1E) 0, 5Answer: DDiff: 1Page Ref: Sec. 8.13) Based on the octet rule, magnesium most likely forms a __________ ion.A) 2Mg+B) 2Mg-C) 6Mg-D) 6Mg+E) _MgAnswer: ADiff: 1Page Ref: Sec. 8.14) Based on the octet rule, phosphorus most likely forms a __________ ion.A) 3P+B) 3P-C) 5P+D) 5P-E) +PAnswer: BDiff: 1Page Ref: Sec. 8.15) Based on the octet rule, iodine most likely forms an __________ ion.A) 2I+B) 4I+C) 4I-D) I+E) I-Answer: EDiff: 1Page Ref: Sec. 8.16) There are __________ unpaired electrons in the Lewis symbol for an oxygen atom.A) 0B) 1C) 2D) 4E) 3Answer: CDiff: 1Page Ref: Sec. 8.17) How many unpaired electrons are there in the Lewis structures of a 3N- ion?A) 0B) 1C) 2D) 3E) This cannot be predicted.Answer: ADiff: 1Page Ref: Sec. 8.18) How many unpaired electrons are there in an 2O- ion?A) 0B) 1C) 2D) 3E) This cannot be predicted.Answer: ADiff: 1Page Ref: Sec. 8.19) The electron configuration of the phosphide ion (3P-) is __________.A) 2[Ne]3SB) 21[Ne]3S3PC) 23[Ne]3S3PD) 2[Ne]3PE) 26[Ne]3S3PAnswer: EDiff: 1Page Ref: Sec. 8.110) The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.A) 7, 4, and 6B) 1, 5, and 7C) 8, 2, and 3D) 7, 1, and 2E) 2, 7, and 4Answer: DDiff: 2Page Ref: Sec. 8.111) The only noble gas without eight valence electrons is __________.A) ArB) NeC) HeD) KrE) All noble gases have eight valence electrons.Answer: CDiff: 1Page Ref: Sec. 8.112) Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration?O Sr Na Se BrA) O, SeB) SrC) NaD) BrE) Sr, O, SeAnswer: BDiff: 1Page Ref: Sec. 8.113) Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration?O Sr Na Se BrA) BrB) SrC) NaD) O, SeE) Sr, O, SeAnswer: DDiff: 1Page Ref: Sec. 8.114) For a given arrangement of ions, the lattice energy increases as ionic radius__________ and as ionic charge __________.A) decreases, increasesB) increases, decreasesC) increases, increasesD) decreases, decreasesE) This cannot be predicted.Answer: ADiff: 1Page Ref: Sec. 8.215) The electron configuration of the 2S- ion is __________.A) 26[Ar]3S3pB) 22[Ar]3S3pC) 22[Ne]3S3pD) 26[Ne]3S3pE) 26[Kr]3S2p-Answer: DDiff: 1Page Ref: Sec. 8.216) The principal quantum number of the electrons that are lost when tungsten forms a cation is __________.A) 6B) 5C) 4D) 3E) 2Answer: ADiff: 1Page Ref: Sec. 8.217) Which one of the following species has the electron configuration4[Ar]3d?A) 2Mn+B) 2Cr+C) 3V+D) 3Fe+E) K+Answer: BDiff: 1Page Ref: Sec. 8.2Co+ ion?18) What is the electron configuration for the 2A) 16[Ar]4S3dB) 07[Ar]4S3dC) 05[Ar]4S3dD) 29[Ar]4S3dE) 210[Ne]3S3pAnswer: BDiff: 1Page Ref: Sec. 8.219) What is the electron configuration for the 2Fe ion?A) 06[Ar]4S3dB) 24[Ar]4S3dC) 08[Ar]4S3dD) 28[Ar]4S3dE) 62[Ar]4S3dAnswer: ADiff: 1Page Ref: Sec. 8.220) The formula of palladium(IV) sulfide is __________.A)Pd S24B)PdS4C)Pd S4D)PdS2E)Pd S22Answer: DDiff: 1Page Ref: Sec. 8.221) Elements from opposite sides of the periodic table tend to form __________.A) covalent compoundsB) ionic compoundsC) compounds that are gaseous at room temperatureD) homonuclear diatomic compoundsE) covalent compounds that are gaseous at room temperatureAnswer: BDiff: 1Page Ref: Sec. 8.222) Determining lattice energy from Born-Haber cycle data requires the use of__________.A) the octet ruleB) Coulomb's lawC) Periodic lawD) Hess's lawE) Avogadro's numberAnswer: DDiff: 2Page Ref: Sec. 8.223) How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell?A) 3B) 4C) 1D) 2E) 0Answer: BDiff: 1Page Ref: Sec. 8.324) A __________ covalent bond between the same two atoms is the longest.A) singleB) doubleC) tripleD) They are all the same length.E) strongAnswer: ADiff: 1Page Ref: Sec. 8.325) How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?A) 1B) 2C) 3D) 4E) 5Answer: DDiff: 1Page Ref: Sec. 8.326) A double bond consists of __________ pairs of electrons shared between two atoms.A) 1B) 2C) 3D) 4E) 6Answer: BDiff: 2Page Ref: Sec. 8.327) What is the maximum number of double bonds that a hydrogen atom can form?A) 0B) 1C) 2D) 3E) 4Answer: ADiff: 1Page Ref: Sec. 8.328) What is the maximum number of double bonds that a carbon atom can form?A) 4B) 1C) 0D) 2E) 3Answer: DDiff: 1Page Ref: Sec. 8.329) In the molecule below, which atom has the largest partial negative charge__________?A) ClB) FC) BrD) IE) CAnswer: BDiff: 1Page Ref: Sec. 8.430) 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: 1Page Ref: Sec. 8.431) Given the electronegativities below, which covalent single bond is most polar? Element: H C N OElectronegativity: 2.1 2.5 3.0 3.5A) C-HB) N-HC) O-HD) O-CE) O-NAnswer: CDiff: 1Page Ref: Sec. 8.432) Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.A) decreases, increasesB) increases, increasesC) increases, decreasesD) stays the same, increasesE) increases, stays the sameAnswer: CDiff: 1Page Ref: Sec. 8.433) A nonpolar bond will form between two __________ atoms of __________ electronegativity.A) different, oppositeB) identical, differentC) different, differentD) similar, differentE) identical, equalAnswer: EDiff: 1Page Ref: Sec. 8.434) The ionICI-has __________ valence electrons.4A) 34B) 35C) 36D) 28E) 8Answer: CDiff: 1Page Ref: Sec. 8.535) The ion NO-has __________ valence electrons.A) 15B) 14C) 16D) 10E) 12Answer: EDiff: 1Page Ref: Sec. 8.536) The Lewis structure ofAsH shows __________ nonbonding electron pair(s) on As.3A) 0B) 1C) 2D) 3E) This cannot be determined from the data given.Answer: BDiff: 1Page Ref: Sec. 8.537) The Lewis structure ofPF shows that the central phosphorus atom has __________3nonbonding and __________ bonding electron pairs.A) 2, 2B) 1, 3C) 3, 1D) 1, 2E) 3, 3Answer: BDiff: 1Page Ref: Sec. 8.538) The Lewis structure of HCN (H bonded to C) shows that __________ has __________ nonbonding electron pairs.A) C, 1B) N, 1C) H, 1D) N, 2E) C, 2Answer: BDiff: 2Page Ref: Sec. 8.539) The formal charge on carbon in the molecule below is __________.A) 0B) +1C) +2D) +3E) -1Answer: ADiff: 1Page Ref: Sec. 8.540) The formal charge on nitrogen inNO-is __________.3A) -1B) 0C) +1D) +2E) -2Answer: CDiff: 2Page Ref: Sec. 8.541) The formal charge on sulfur in 2SO-is __________, where the Lewis structure of the4ion is:A) -2B) 0C) +2D) +4E) -4Answer: BDiff: 2Page Ref: Sec. 8.542) In the Lewis structure of ClF, the formal charge on Cl is __________ and the formal charge on F is __________.A) -1, -1B) 0, 0C) 0, -1D) +1, -1E) -1, +1Answer: BDiff: 1Page Ref: Sec. 8.543) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is __________.A) 0B) +1C) -1D) +2E) -2Answer: BDiff: 1Page Ref: Sec. 8.644) How many equivalent resonance forms can be drawn for 2CO - (carbon is the central3atom)?A) 1B) 2C) 3D) 4E) 0Answer: CDiff: 1Page Ref: Sec. 8.645) How many equivalent resonance forms can be drawn forSO without expanding octet2on the sulfur atom (sulfur is the central atom)?A) 0B) 2C) 3D) 4E) 1Answer: BDiff: 1Page Ref: Sec. 8.646) How many equivalent resonance structures can be drawn for the molecule ofSO without having to violate the octet rule on the sulfur atom?3A) 5B) 2C) 1D) 4E) 3Answer: EDiff: 1Page Ref: Sec. 8.647) How many different types of resonance structures can be drawn for the ion2SO-where all atoms satisfy the octet rule?3A) 1B) 2C) 3D) 4E) 5Answer: ADiff: 2Page Ref: Sec. 8.648) Using the table of average bond energies below, the H∆for the reaction is __________Bond: C≡C C-C H-I C-I C-HD (kJ/mol): 839 348 299 240 413A) +160B) -160C) -217D) -63E) +63Answer: CDiff: 1Page Ref: Sec. 8.849) Using the table of average bond energies below, the H ∆for the reaction is __________ kJ.2H C C H (g) + H I (g)H C CHI (g)-≡--→=Bond: C≡C C=C H-I C-I C-HD (kJ/mol): 839 614 299 240 413A) +506B) -931C) -506D) -129E) +129Answer: DDiff: 1Page Ref: Sec. 8.850) Using the table of average bond energies below, the H ∆for the reaction is __________ kJ.23C O (g)+2H (g)H C O H (g) ≡→--Bond: C-O C=O C≡O C-H H-H O-HD (kJ/mol): 358 799 1072 413 436 463A) +276B) -276C) +735D) -735E) -116Answer: EDiff: 1Page Ref: Sec. 8.851) Using the table of bond dissociation energies, the H ∆ for the following gas-phase reaction is __________ kJ.A) -44B) 38C) 304D) 2134E) -38Answer: ADiff: 1Page Ref: Sec. 8.8reaction is __________ kJ.A) 291B) 2017C) -57D) -356E) -291Answer: CDiff: 1Page Ref: Sec. 8.8__________ kJ.222HCl (g)F (g)2HF (g)Cl (g)+→+A) -359B) -223C) 359D) 223E) 208Answer: ADiff: 1Page Ref: Sec. 8.88.2 Multiple-Choice Questions1) Which ion below has a noble gas electron configuration?A) 2Li +B) 2Be +C) 2B +D) 2C +E) 2N -Answer: BDiff: 1Page Ref: Sec. 8.12) Of the ions below, only __________ has a noble gas electron configuration.A) 3S+B) 2O+C) I+D) K-E) Cl-Answer: EDiff: 1Page Ref: Sec. 8.13) Which of the following has eight valence electrons?A) 4Ti+B) KrC) Cl-D) Na+E) all of the aboveAnswer: EDiff: 3Page Ref: Sec. 8.14) Which of the following does not have eight valence electrons?A) Ca+B) Rb+C) XeD) Br-E) All of the above have eight valence electrons.Answer: ADiff: 3Page Ref: Sec. 8.15) The chloride of which of the following metals should have the greatest lattice energy?A) potassiumB) rubidiumC) sodiumD) lithiumE) cesiumAnswer: DDiff: 2Page Ref: Sec. 8.26) Lattice energy is __________.A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phaseB) the energy given off when gaseous ions combine to form one mole of an ionic solidC) the energy required to produce one mole of an ionic compound from its constituent elements in their standard statesD) the sum of ionization energies of the components in an ionic solidE) the sum of electron affinities of the components in an ionic solidAnswer: ADiff: 1Page Ref: Sec. 8.27) In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii __________.A) increases, decrease, increaseB) increases, increase, increaseC) decreases, increase, increaseD) increases, increase, decreaseE) increases, decrease, decreaseAnswer: DDiff: 3Page Ref: Sec. 8.2The diagram below is the Born-Huber cycle for the formation of crystalline potassium fluoride.8) Which energy change corresponds to the electron affinity of fluorine?A) 2B) 5C) 4D) 1E) 6Answer: CDiff: 1Page Ref: Sec. 8.29) Which energy change corresponds to the first ionization energy of potassium?A) 2B) 5C) 4D) 3E) 6Answer: DDiff: 1Page Ref: Sec. 8.210) The electron configuration [Kr]4d10 represents __________.A) Sr+2B) Sn+2C) Te+2D) Ag+1E) Rb+1Answer: DDiff: 3Page Ref: Sec. 8.211) Fe+2 ions are represented by __________.A) [Ar]3d1B) [Ar]3d4C) [Ar]3d6D) [Ar]3d104s1E) [Ar]3d3Answer: CDiff: 4Page Ref: Sec. 8.213) 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: 1Page Ref: Sec. 8.314) In which of the molecules below is the carbon-carbon distance the shortest?A) 22H C CH =B) H C C H -=-C) 33H C CH -D) 22H C C CH ==E) 323H C CH CH ==Answer: BDiff: 1Page Ref: Sec. 8.315) Of the atoms below, __________ is the most electronegative.A) BrB) OC) ClD) NE) FAnswer: EDiff: 1Page Ref: Sec. 8.416) Of the atoms below, __________ is the most electronegative.A) SiB) ClC) RbD) CaE) SAnswer: BDiff: 1Page Ref: Sec. 8.417) Of the atoms below, __________ is the least electronegative.A) RbB) FC) SiD) ClE) CaAnswer: ADiff: 1Page Ref: Sec. 8.418) Which of the elements below has the largest electronegativity?A) SiB) MgC) PD) SE) NaAnswer: DDiff: 1Page Ref: Sec. 8.419) Of the molecules below, the bond in __________ is the most polar.A) HBrB) HIC) HClD) HFE)H2Answer: DDiff: 1Page Ref: Sec. 8.420) Of the bonds below, __________ is the least polar.A) Na, SB) P, SC) C, FD) Si, ClE) Na, ClAnswer: BDiff: 1Page Ref: Sec. 8.421) Which of the following has the bonds correctly arranged in order of increasing polarity?A) Be F, Mg F, N F, O F----B) O F, N F, Be F, Mg F----C) O F, Be F, Mg F, N F----D) N F, Be F, Mg F, O F----E) M gF, Be F, N F, O F----Answer: BDiff: 1Page Ref: Sec. 8.422) Which two bonds are most similar in polarity?A) O F -and Cl F -B) B F -and Cl F -C) Al Cl -and I Br -D) I Br -and Si Cl -E) Cl Cl -and Be Cl -Answer: ADiff: 2Page Ref: Sec. 8.423) The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e ) of the negative charge on I in HI?(301 debye = 3.3410 coulomb-meters -⨯; ;19e=1.6 10 coulombs -⨯)A) 191.610-⨯B) 0.057C) 9.1D) 1E) 0.22Answer: BDiff: 5Page Ref: Sec. 8.424) Which of the following names is/are correct for the compound 2TiO ?A) titanium dioxide and titanium (IV) oxideB) titanium (IV) dioxideC) titanium oxideD) titanium oxide and titanium (IV) dioxideE) titanium (II) oxideAnswer: ADiff: 1Page Ref: Sec. 8.425) Which of the following names is/are correct for the compoundSnCl?4A) tin (II) chloride and tin (IV) chlorideB) tin tetrachloride and tin (IV) chlorideC) tin (IV) tetrachlorideD) tin chlorideE) tin chloride and tin (II) tetrachlorideAnswer: BDiff: 1Page Ref: Sec. 8.426) The Lewis structure ofN H shows __________.22A) 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: 2Page Ref: Sec. 8.527) There are __________ valence electrons in the Lewis structure of CH3CH2Cl.A) 14B) 12C) 18D) 20E) 10Answer: DDiff: 3Page Ref: Sec. 8.528) 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: 2Page Ref: Sec. 8.529) The Lewis structure of the 2CO ion is __________.3A)B)C)D)E)Answer: ADiff: 2Page Ref: Sec. 8.5(NO) , __________.30) In the nitrite ion 2-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: 2Page Ref: Sec. 8.631) 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: 1Page Ref: Sec. 8.632) The oxidation number of phosphorus in PF3 is __________.A) -2B) +1C) +3D) +2E) -3Answer: CDiff: 2Page Ref: Sec. 8.633) 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: 1Page Ref: Sec. 8.634) 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 forms （观察到的是共振结构的平均形势）D) 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: 1Page Ref: Sec. 8.6For the questions that follow, consider the BEST Lewis structures of the following oxyanions:(i)2NO - (ii)3NO - (iii)23SO - (iv)24SO - (v)3BrO -35) There can be four equivalent best resonance structures of __________.A) (ii)B) (iii)C) (i)D) (iv)E) (v)Answer: DDiff: 2Page Ref: Sec. 8.5-8.736) In which of the ions do all X-O bonds (X indicates the central atom) have the same length?A) noneB) allC) (i) and (ii)D) (iii) and (v)E) (iii), (iv), and (v)Answer: BDiff: 1Page Ref: Sec. 8.6, 8.737) Of the following, __________ cannot accommodate more than an octet of electrons.A) PB) AsC) OD) SE) IAnswer: CDiff: 1Page Ref: Sec. 8.738) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.A)NF3B)IF3C)PF3SbFD)3E) 2So4Answer: BDiff: 2Page Ref: Sec. 8.739) Based on the octet rule, boron will most likely form a __________ ion.A) B3-B) B1+C) B3+D) B2+E) B2-Answer: CDiff: 2Page Ref: Sec. 8.740) Which of the following does not have eight valence electrons?A) Cl-B) XeC) Ti+4D) Rb+1E) Sr+1Answer: EDiff: 2Page Ref: Sec. 8.741) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.A) 3PO4B)SiF4C)CF4D)SeF4NFE)3Answer: DDiff: 3Page Ref: Sec. 8.742) The central atom in __________ does not violate the octet rule.A)SF4B)KrF2C)CF4D)XeF4E)ICl4Answer: CDiff: 2Page Ref: Sec. 8.743) The central atom in __________ violates（违反） the octet rule.A)NH3B)SeF2C)BF3D)AsF3E)CF4Answer: CDiff: 2Page Ref: Sec. 8.744) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.ClFA)3PClB)3SOC)3CClD)4COE)2Answer: ADiff: 1Page Ref: Sec. 8.745) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.A)NI3B)SO2C)ICl5D)SiF4E)CO2Answer: CDiff: 1Page Ref: Sec. 8.746) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.A)NF3B)BeH2C)SO2D)CF4E) 2SO3Answer: BDiff: 1Page Ref: Sec. 8.7BeCl?47) Why don't we draw double bonds between the Be atom and the Cl atoms in2A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom.B) There aren't enough electrons.C) That would result in more than eight electrons around beryllium.D) That would result in more than eight electrons around each chlorine atom.E) That would result in the formal charges not adding up to zero.Answer: ADiff: 2Page Ref: Sec. 8.748) Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?A) NB) CC) HD) OE) BAnswer: EDiff: 1Page Ref: Sec. 8.749) Bond enthalpy is _positive_________.A) always positiveB) always negativeC) sometimes positive, sometimes negativeD) always zeroE) unpredictableAnswer: ADiff: 1Page Ref: Sec. 8.850) 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(CHBr) is __________ kJ/mol.3A) 1241B) 689C) -689D) 1378E) -1378Answer: ADiff: 1Page Ref: Sec. 8.851) Of the bonds C-N,C N≡ , the C-N bond is __________.= , and C NA) strongest/shortestB) strongest/longestC) weakest/shortestD) weakest/longestE) intermediate in both strength and lengthAnswer: DDiff: 1Page Ref: Sec. 8.852) As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________.A) increases, increasesB) decreases, decreasesC) increases, decreasesD) decreases, increasesE) is unpredictableAnswer: DDiff: 1Page Ref: Sec. 8.853) Of the possible bonds between carbon atoms (single, double, and triple), __________.A) a triple bond is longer than a single bondB) a double bond is stronger than a triple bondC) a single bond is stronger than a triple bondD) a double bond is longer than a triple bondE) a single bond is stronger than a double bondAnswer: DDiff: 1Page Ref: Sec. 8.854) Most explosives are compounds that decompose rapidly to produce __________ products and a great deal of __________.A) gaseous, gasesB) liquid, heatC) soluble, heatD) solid, gasE) gaseous, heatAnswer: EDiff: 1Page Ref: Sec. 8.855) Dynamite consists of nitroglycerine mixed with __________.A) potassium nitrateB) damp KOHC) TNTD) diatomaceous earth or celluloseE) solid carbonAnswer: DDiff: 1Page Ref: Sec. 8.856) Dynamite __________.A) was invented by Alfred NobelB) is made of nitroglycerine and an absorbent such as diatomaceous earthC) is a much safer explosive than pure nitroglycerineD) is an explosiveE) all of the aboveAnswer: EDiff: 1Page Ref: Sec. 8.88.3 Short Answer Questions1) The electron configuration that corresponds to the Lewis symbol, is __________.Answer: 25[Ne]3S 3pDiff: 2Page Ref: Sec 8.12) Write the balanced chemical equation for the reaction for which H rxn ∆︒ is the lattice energy for potassium bromide.Answer: KBr (s)K (g)Br (g)++→+Diff: 1Page Ref: Sec. 8.23) Using the noble gas shorthand notation, write the electron configuration for Fe +3.Answer: [Ar]3d 5Diff: 2Page Ref: Sec. 8.24) Give the electron configuration of 2Cu +.Answer: 9[Ar]3dDiff: 2Page Ref: Sec. 8.25) Which halogen, bromine or iodine, will form the more polar bond with phophorus?Answer: bromineDiff: 1Page Ref: Sec. 8.46) Draw the Lewis structure of ICl2+.Answer:Diff: 1Page Ref: Sec. 8.57) Alternative but equivalent Lewis structures are called __________.Answer: resonance structuresDiff: 1Page Ref: Sec. 8.68) Benzene is an __________ compound with __________ equivalent Lewis structures. Answer: aromatic, twoDiff: 3Page Ref: Sec. 8.69) In a reaction, if the bonds in the reactants are stronger than the bonds in the product, the reaction is __________.Answer: endothermicDiff: 1Page Ref: Sec. 8.710) In compounds of __________ and __________, the octet rule is violated due to the presence of fewer than eight valence electrons.Answer: boron and berylliumDiff: 2Page Ref: Sec. 8.711) Polyatomic ions with an odd number of electrons will __________ the octet rule. Answer: fail or violateDiff: 2Page Ref: Sec. 8.712) The strength of a covalent bond is measured by its __________.Answer: bond enthalpy （键焓）Diff: 1Page Ref: Sec. 8.813) To produce maximum heat, an explosive compound should have ____weak______ chemical bonds and decompose to molecule with _____strong_____ bonds. Answer: weak, strongDiff: 4Page Ref: Sec. 8.814) Calculate the bond energy of C-F given that the heat of atomization of CHFClBr is 1502 kJ/mol, and that the bond energies of C-H, C-Br, and C-Cl are 413, 276, and 328 kJ/mol, respectively.∆=-+-+-+-Answer: H[D (C H) D (C F) D (C Cl) D(C Br)] atomization-=∆--+-+-D(C F)H[D(C H)D(C Cl)D(C Br)]atomization= [1502 - (413 + 276 + 328)] kJ/mol= 485 kJ/molDiff: 1Page Ref: Sec. 8.815) The reaction below is used to produce methanol:23CO(g) 2H (g)CH OH (l)+→ H 128KJ rxn ∆=-(a) Calculate the C-H bond energy given the following data:(b) The tabulated value of the (C-H) bond energy is 413 kJ/mol. Explain why there is a difference between the number you have calculated in (a) and the tabulated value.Answer:(a) H =D(C O) 2 D(H H)[3 D(C H)D(C O)D(O H)]rxn∆≡+---+-+- 3 D(C H) H D(C O) 2 D(H H)D(C O)D(O H)rxn -=-∆+≡+----- D(C-H) = (128 + 1072 + 2(436) - 358 - 463)/3 = 417D(C-H) = 417 kJ/mol(b) Tabulated values, like those in Table 8.4, are averaged from many bond energies measured for C-H bonds in many different molecules.Diff: 2Page Ref: Sec. 8.8。
