The bond energy of a C–C single bond averages 347 kJ mol⁻¹; that of a triple bond averages 839 kJ mol⁻¹. Explain why the triple bond is not three times as strong as a single bond.
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Chemistry 2e · 8.3 Multiple Bonds
Multiple Bonds: practice problems
5 problems from the book, with its answers. Check your working, or have any of them explained to you on the whiteboard.
Exercises 25
A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, H₃CCN. It is present in paint strippers.
(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.
(b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form σ bonds.
(c) Describe the atomic orbitals that form the π bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.
Exercises 27
Identify the hybridization of the central atom in each of the following molecules and ions that contain multiple bonds:
(a) ClNO (N is the central atom)
(b) CS₂
(c) Cl₂CO (C is the central atom)
(d) Cl₂SO (S is the central atom)
(e) SO₂F₂ (S is the central atom)
(f) XeO₂F₂ (Xe is the central atom)
(g) (Cl is the central atom)
Exercises 29
For each of the following molecules, indicate the hybridization requested and whether or not the electrons will be delocalized:
(a) ozone (O₃) central O hybridization
(b) carbon dioxide (CO₂) central C hybridization
(c) nitrogen dioxide (NO₂) central N hybridization
(d) phosphate ion central P hybridization
Exercises 31
Draw the orbital diagram for carbon in CO₂ showing how many carbon atom electrons are in each orbital.
Learn 8.3 on the whiteboard
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