Bond Energy and Bond Length
Chemistry ⇒ Chemical Bonding and Structure
Bond Energy and Bond Length starts at 10 and continues till grade 12.
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See sample questions for grade 11
Arrange the following bonds in order of increasing bond length: N≡N, N=N, N–N.
Describe how atomic radius affects bond length.
Describe the effect of multiple bonds on bond length and bond energy.
Explain the relationship between bond order and bond length.
Explain why bond energies are usually average values.
Explain why double bonds are stronger but not twice as strong as single bonds.
Explain why the F–F bond has a lower bond energy than the Cl–Cl bond, even though fluorine is smaller than chlorine.
Given the following bond energies: C–H = 413 kJ/mol, O=O = 498 kJ/mol, C=O = 799 kJ/mol. Calculate the enthalpy change for the reaction: CH4 + 2O2 → CO2 + 2H2O (use only the given bond energies).
If the bond energy of H–Cl is 431 kJ/mol, how much energy is required to break all the H–Cl bonds in 2 moles of HCl gas?
State the trend in bond length across a period for homonuclear diatomic molecules.
The average bond energy of O–H in water is 463 kJ/mol. Calculate the total energy required to break all O–H bonds in 3 moles of H2O.
The bond energy of Cl–Cl is 243 kJ/mol. If 729 kJ of energy is supplied, how many moles of Cl2 molecules can be dissociated?
The bond energy of H–H is 436 kJ/mol. Calculate the energy required to break 0.5 moles of H2 molecules.
A certain diatomic molecule has a bond length of 74 pm and a bond energy of 436 kJ/mol. If another diatomic molecule has a bond length of 110 pm, predict whether its bond energy is likely to be higher or lower, and justify your answer.
A molecule of ethene (C2H4) contains C–H and C=C bonds. If the average bond energy of C–H is 413 kJ/mol and C=C is 614 kJ/mol, calculate the total energy required to break all the bonds in one mole of ethene.
Consider the following molecules: CO, CO2, and C2H2. Arrange them in order of increasing C–O or C–C bond length and explain your reasoning.
Describe how the presence of lone pairs on bonded atoms can affect bond length and bond energy.
Explain why the bond energy of a C–F bond is higher than that of a C–I bond.
Given the following bond energies: H–H = 436 kJ/mol, Cl–Cl = 243 kJ/mol, H–Cl = 431 kJ/mol. Calculate the enthalpy change (ΔH) for the reaction: H2 + Cl2 → 2HCl.
