Ch.10 - Chemical Bonding I: The Lewis Model

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Tro 6th Edition

Ch.10 - Chemical Bonding I: The Lewis Model

문제 66a

Write the Lewis structure for each molecule or ion. a. H₃COCH₃

문제 67a

Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. a. SeO₂

문제 68

Write a Lewis structure that obeys the octet rule for each ion. Include resonance structures if necessary and assign formal charges to each atom. a. ClO₃^- b. ClO₄^- c. NO₃^- d. NH₄⁺

문제 70

Use formal charges to identify the better Lewis structure.

문제 71

How important is the resonance structure shown here to the overall structure of carbon dioxide? Explain.

문제 73

In N₂O, nitrogen is the central atom and the oxygen atom is terminal. In OF₂, however, oxygen is the central atom. Use formal charges to explain why.

문제 75

Draw the Lewis structure (including resonance structures) for the acetate ion (CH₃COO^-). For each resonance structure, assign formal charges to all atoms that have formal charge.

문제 76

Draw the Lewis structure (including resonance structures) for methyl azide (CH₃N₃). For each resonance structure, assign formal charges to all atoms that have formal charge.

문제 77

What are the formal charges of the atoms shown in red?

문제 78

What are the formal charges of the atoms shown in red?

문제 79b

Write the Lewis structure for each molecule (octet rule not followed). b. NO₂

문제 80

Write the Lewis structure for each molecule (octet rule not followed). a. BBr₃ b. NO c. ClO₂

문제 81

Write the Lewis structure for each ion. Include resonance structures if necessary and assign formal charges to all atoms. If necessary, expand the octet on the central atom to lower formal charge for the following ions: a. PO4^3- b. CN^- c. SO3^2- d. ClO2^-.

문제 82

Write Lewis structures for each molecule or ion. Include resonance structures if necessary and assign formal charges to all atoms. If you need to, expand the octet on the central atom to lower formal charge. a. SO4^2- b. HSO4^- c. SO3 d. BrO2^-

문제 83a

Write Lewis structures for each molecule or ion. Use expanded octets as necessary. a. PF₅

문제 84b

Write Lewis structures for each molecule or ion. Use expanded octets as necessary. b. AsF₆^-

문제 85a

Order these compounds in order of increasing carbon–carbon bond strength: HCCH, H₂CCH₂, H₃CCH₃.

문제 85b

Order these compounds in order of decreasing carbon–carbon bond length: HCCH, H₂CCH₂, H₃CCH₃.

문제 86

Which of the two compounds, H₂NNH₂ and HNNH, has the strongest nitrogen-nitrogen bond, and which has the shorter nitrogen-nitrogen bond.

문제 87

Hydrogenation reactions are used to add hydrogen across double bonds in hydrocarbons and other organic compounds. Use average bond energies to calculate ΔH_rxn for the hydrogenation reaction. H₂C=CH₂(g) + H₂(g) → H₃C–CH₃(g)

문제 88

Ethanol is a possible fuel. Use average bond energies to calculate ΔHrxn for the combustion of ethanol. CH₃CH₂OH(g) + 3 O2(g) → 2 CO₂(g) + 3 H₂O(g)

문제 89

Ethane burns in air to form carbon dixode and water vapor.

2 H3C¬CH3( g) + 7 O2( g)¡4 CO2( g) + 6 H2O( g)

Use average bond energies to calculate ΔHrxn for the reaction.

문제 90

In the Chemistry and the Environment box on free radicals in this chapter, we discussed the importance of the hydroxyl radical in reacting with and eliminating many atmospheric pollutants. However, the hydroxyl radical does not clean up everything. For example, chlorofluorocarbons—which destroy stratospheric ozone—are not attacked by the hydroxyl radical. Consider the hypothetical reaction by which the hydroxyl radical might react with a chlorofluorocarbon: OH(g) + CF₂Cl₂(g) → HOF(g) + CFCl₂(g) Use bond energies to explain why this reaction is improbable. (The C–F bond energy is 552 kJ/mol.)

문제 91

Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. a. BI3 c. HCFO b. K2S d. PBr3

문제 92b

Write an appropriate Lewis structure for each compound. Make certain to distinguish between ionic and molecular compounds. b. ClF₅

문제 93a

Each compound contains both ionic and covalent bonds. Write ionic Lewis structures for each, including the covalent structure for the ion in brackets. Write resonance structures if necessary. a. BaCO₃

문제 93b,c,d

문제 94

Does each compound contain both ionic and covalent bonds? Write ionic Lewis structures for each of them, including the covalent structure for the ion in brackets. Write resonance structures if necessary for the following: b. NH4Cl, d. Sr(CN)2, a. RbIO2, c. KOH.

문제 95

Carbon ring structures are common in organic chemistry. Draw a Lewis structure for each carbon ring structure, including any necessary resonance structures. a. C₄H₈ b. C₄H₄ c. C₆H₁₂ d. C₆H₆

문제 96

Amino acids are the building blocks of proteins. The simplest amino acid is glycine (H₂NCH₂COOH). Draw a Lewis structure for glycine. (Hint: The central atoms in the skeletal structure are nitrogen and the two carbon atoms. Each oxygen atom is bonded directly to the right-most carbon atom.)