Organic Chemistry
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Explain why the indicated C―C bond in butan-2-ylium is shorter than the indicated C―C bond in butane.
Determine whether the σ bond or the π bond has the more effective orbital overlap in a carbon—carbon double bond.
Sort the indicated bond lengths from shortest to longest.
Determine which of the following bonds will be longer and which will be stronger.
Arrange the indicated bonds in terms of increasing bond length. Explain the ranking.
Explain why the S−H bond in ethanethiol is longer than the O−H bond in ethanol if the S and O in the mentioned compounds are both sp3 hybridized.
Determine the number of s bond orbitals that can overlap with the empty p orbitals in the given compound.
Consider the partial structure below wherein the σ bonds are shown:
Provide the complete structure by adding one π bond, and indicate the orientation of the p orbitals used (x, y, or z-axis).
Predict which of the following bonds will be longer and which will be stronger.
Explain why the indicated C―N bond in N-methylethenamine is stronger than the indicated C―N bond length in N-methylethanamine.
Predict which of the given bonds will be longer and which will be stronger.
Consider the structure shown below where only the σ bond is shown. Draw the missing π bonds and specify the orientation of the p orbitals used.
Determine the number of s-orbitals that can overlap with the vacant p-orbital in the following ions:
(i) tert-butyl cation
(ii) n-pentyl cation
(iii) sec-pentyl cation