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 10
Arrange the following bonds in order of increasing bond length: C–C, C=C, C≡C.
Describe how bond order affects both bond energy and bond length.
Describe how electronegativity difference between two atoms affects bond energy.
Describe the relationship between bond energy and bond length.
Explain why bond energies are usually given as average values.
Explain why the bond energy of a C–C bond is less than that of a C=C bond.
Explain why the bond energy of F–F is lower than that of Cl–Cl, even though fluorine is smaller than chlorine.
Explain why the bond energy of O=O is less than that of N≡N.
Explain why the bond length increases as the size of the bonded atoms increases.
If the bond energy of H–H is 436 kJ/mol, how much energy is needed to break 2 moles of H–H bonds?
The average bond energy of a C–H bond is 413 kJ/mol. How much energy is required to break all four C–H bonds in one mole of methane (CH₄)?
The bond energy of a C–C bond is 348 kJ/mol, and that of a C=C bond is 614 kJ/mol. What is the average bond energy per bond in C₂H₄ (ethene), which has one C=C and four C–H bonds (C–H = 413 kJ/mol)?
The bond energy of O=O is 498 kJ/mol. How much energy is required to break 0.5 moles of O=O bonds?
The bond length of C–H is 1.09 Å, and that of C–C is 1.54 Å. Which bond is stronger?
The bond length of H–F is 0.92 Å, and that of H–Cl is 1.27 Å. Which bond is stronger?
Which bond is stronger: a polar covalent bond or a nonpolar covalent bond, assuming the same atoms are involved?
A molecule of ethyne (C2H2) contains a triple bond between the two carbon atoms. If the bond energy of a C≡C bond is 839 kJ/mol and that of a C–H bond is 413 kJ/mol, calculate the total energy required to break all the bonds in one mole of ethyne molecules.
Describe how the presence of lone pairs on bonded atoms can affect bond length and bond energy, using water (H2O) as an example.
Explain why the bond energy of a C–F bond is higher than that of a C–I bond, even though both are single bonds between carbon and a halogen.
Explain why the bond energy of a C–N bond in methylamine (CH3NH2) is different from that in nitromethane (CH3NO2).
