11. Bonding & Molecular Structure

Bond Energy

11. Bonding & Molecular Structure

Bond Energy

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Bond Energy Example 1

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Covalent Bonding: Bond Order, Bond Length, Bond Energy

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Covalent Bonding: Bond Order, Bond Length, Bond Energy

The Video Textbook Of Chemistry

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08:30

Bond Strength and Length

Bond Energy & Bond Length, Forces of Attraction & Repulsion - Chemistry

The Organic Chemistry Tutor

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14:49

Bond Strength and Bond Length

The Organic Chemistry Tutor

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06:42

Bond Length and Bond Energy

Bozeman Science

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Multiple Choice

Consider the following equation:

Determine the bond enthalpy value for the F–S bond.

Use the bond energies to estimate the enthalpy of reaction for the combustion of 5 moles of acetylene:

Calculate the enthalpy of the following reaction based on average bond enthalpies.

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Multiple Choice

Which of the following bonds is the strongest?

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Textbook Question

The graph shows how potential energy changes as a function of the distance between two atoms. (LO 7.2)

What is the length of the bond between the two atoms? (a) 3.4 angstroms (b) 3.8 angstroms (c) 6.0 angstroms (d) 8.0 angstroms

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Textbook Question

The following plot shows the potential energy of two Cl atoms as a function of the distance between them. (c) If the Cl2 molecule is compressed under higher and higher pressure, does the Cl–Cl bond become stronger or weaker?

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Textbook Question

Isomers are molecules that have the same chemical formula but different arrangements of atoms, as shown here for two isomers of pentane, C5H12.

(a) Do you expect a significant difference in the enthalpy of combustion of the two isomers? Explain.

What is the best prediction for the carbon–oxygen bond length in the carbonate anion, CO3 2-? (LO 7.14) Data for average carbon-oxygen bond lengths: (a) 143 pm (b) 132 pm (c) 121 pm (d) 118 pm

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Textbook Question

(b) Based on aver- age bond enthalpies, would you expect a photon capable of dissociating a C ¬ Cl bond to have sufficient energy to dis- sociate a C ¬ Br bond?

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Textbook Question

Explain the difference in the bond dissociation energies for the following bonds: (C-F, 450 kJ/mol), (N-F, 270 kJ/mol), (O-F, 180 kJ/mol), (F-F, 159 kJ/mol).

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Textbook Question

State whether each of these statements is true or false. (e) The longer the bond, the more energy is stored chemical bonds.

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

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Textbook Question

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)

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Textbook Question

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.)

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Textbook Question

Use bond enthalpies in Table 5.4 to estimate H for each of the following reactions: (a)

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Textbook Question

Consider the collection of nonmetallic elements: B, As, O, and I. (b) Which two would form the longest single bond?

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Textbook Question

The P¬P bond length in white phosphorus is 189 pm. The Cl¬Cl bond length in Cl2 is 199 pm. (b) What bond length is predicted for PCl3, using the atomic radii in Figure 7.7?

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Textbook Question

The P¬P bond length in white phosphorus is 189 pm. The Cl¬Cl bond length in Cl2 is 199 pm. (a) Based on these data, what is the predicted P¬Cl bond length in phosphorus trichloride, PCl3, in which each of the three Cl atoms is bonded to the P atom?

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Textbook Question

(a) The nitrogen atoms in an N2 molecule are held together by a triple bond; use enthalpies of formation in Appendix C to estimate the enthalpy of this bond, D(N‚N). (b) Consider the reaction between hydrazine and hydrogen to produce ammonia, N2H41g2 + H21g2¡2 NH31g2. Use enthalpies of formation and bond enthalpies to estimate the enthalpy of the nitrogen– nitrogen bond in N2H4. (c) Based on your answers to parts (a) and (b), would you predict that the nitrogen–nitrogen bond in hydrazine is weaker than, similar to, or stronger than the bond in N2 ?

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Textbook Question

Consider the reaction 2 H21g2 + O21g2¡2 H2O1l2. (a) Use the bond enthalpies in Table 5.4 to estimate H for this reaction, ignoring the fact that water is in the liquid state.

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Textbook Question

Two compounds are isomers if they have the same chemical formula but different arrangements of atoms. Use Table 8.3 to estimate H for each of the following gas-phase isomerization reactions and indicate which isomer has the lower enthalpy. (d) Methyl isocyanide Acetonitrile

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Textbook Question

If hydrogen were used as a fuel, it could be burned according to this reaction: H2( g) + 1 2 O2( g)¡H2O( g) Use average bond energies to calculate ΔHrxn for this reaction.

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Textbook Question

If hydrogen were used as a fuel, it could be burned according to this reaction: H2( g) + 1 2 O2( g)¡H2O( g) Use average bond energies to calculate ΔHrxn for the combustion of methane (CH4).

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Textbook Question

If hydrogen were used as a fuel, it could be burned according to this reaction: H2( g) + 1 2 O2( g)¡H2O( g) Which fuel yields more energy per mole?

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Textbook Question

If hydrogen were used as a fuel, it could be burned according to this reaction: H2( g) + 1 2 O2( g)¡H2O( g) Which fuel yields more energy per gram?

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Textbook Question

Calculate ΔHrxn for the combustion of octane (C8H18), a component of gasoline, by using average bond energies and then calculate it using enthalpies of formation from Appendix IIB. What is the percent difference between your results? Which result would you expect to be more accurate?

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Textbook Question

The heat of atomization is the heat required to convert a molecule in the gas phase into its constituent atoms in the gas phase. The heat of atomization is used to calculate average bond energies. Without using any tabulated bond energies, calculate the average C¬Cl bond energy from the following data: the heat of atomization of CH4 is 1660 kJ>mol, and the heat of atomization of CH2Cl2 is 1495 kJ>mol.

Calculate the heat of atomization (see previous problem) of C2H3Cl, using the average bond energies in Table 9.3.

Sulfur tetrafluoride 1SF42 reacts slowly with O2 to form sulfur tetrafluoride monoxide 1OSF42 according to the following unbalanced reaction: SF41g2 + O21g2¡OSF41g2 The O atom and the four F atoms in OSF4 are bonded to a central S atom. (c) Use average bond enthalpies (Table 8.3) to estimate the enthalpy of the reaction. Is it endothermic or exothermic?

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Textbook Question

(a) Compare the bond enthalpies (Table 8.3) of the carbon– carbon single, double, and triple bonds to deduce an average p@bond contribution to the enthalpy. What fraction of a single bond does this quantity represent?

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Textbook Question

Calculate an approximate heat of combustion for ethane (C2H6) in kilojoules by using the bond dissocation energies in Table 9.3. (The strength of the O'O bond is 498 kJ/ mol, and that of a C ' O bond in CO2 is 804 kJ/mol.)

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Textbook Question

(a) Use average bond enthalpies (Table 8.3) to estimate H for the atomization of naphthalene, C10H8:

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Textbook Question

Use the data in Table 9.3 to calculate an approximate ∆H° in kilojoules for the synthesis of hydrazine from ammonia: 2 NH3(g) + Cl2(g) → N2H4(g) + 2 HCl(g)

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Textbook Question

Use average bond enthalpies from Table 8.4 to estimate the enthalpies of the following gas-phase reactions: Reaction 1: HF1g2 + H2O1g2 Δ F-1g2 + H3O+1g2 Reaction 2: HCl1g2 + H2O1g2 Δ Cl-1g2 + H3O+1g2 Are both reactions exothermic? How do these values relate to the different strengths of hydrofluoric and hydrochloric acid?

(b) When subjected to high pressure and heated, polyvinyl chloride converts to diamond. During this transformation which bonds are most likely to break first?

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Textbook Question

(a) In polyvinyl chloride shown in Table 12.6, which bonds have the lowest average bond enthalpy?

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Textbook Question

The reaction S81g2 S 4 S21g2 has ΔH° = + 237 kJ (b) The average S ¬ S bond dissociation energy is 225 kJ/mol. Using the value of ΔH° given above, what is the S ' S double bond energy in S21g2?

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Textbook Question

The F ¬ F bond in F2 is relatively weak because the lone pairs of electrons on one F atom repel the lone pairs on the other F atom; Kp = 7.83 at 1500 K for the reaction F21g2 ∆ 2 F1g2. (c) Why is the F ¬ F bond in F2 weaker than the Cl ¬ Cl bond in Cl2?

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Textbook Question

Phosgene, COCl21g2, is a toxic gas used as an agent of warfare in World War I. (b) Using the table of bond dissociation energies (Table 9.3) and the value ΔH°f = 716.7 kJ>mol for C(g), estimate ΔH° f for COCl21g2 at 25 °C. Compare your answer to the actual ΔH° f given in Appendix B, and explain why your calculation is only an estimate.

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Open Question

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

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Open Question

Calculate the average molar bond enthalpy of the carbon–hydrogen bond in a CH₄ molecule.

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Open Question

Use average bond energies to calculate δHrxn for the following hydrogenation reaction: H₂C=CH₂(g) + H₂(g) → H₃C−CH₃(g)

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Open Question

Calculate δhrxn for the combustion of octane (C₈H₁₈) by using average bond energies.

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Open Question

Use average bond enthalpies to estimate the enthalpy δhrxn of the following reaction: 2 SF₄(g) + O₂(g) → 2 OSF₄(g)

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Open Question

Ethanol is a possible fuel. use average bond energies to calculate δH_rxn for the combustion of ethanol.

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Open Question

Predict whether the following reactions will be exothermic or endothermic.

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Open Question

Calculate δh° for the reaction using the given bond dissociation energies.

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Open Question

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

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Open Question

2 H₃C−CH₃(g) + 7O₂(g) → 4 CO₂(g) + 6 H₂O(g)

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11. Bonding & Molecular Structure

Bond Energy

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