Which statement(s) is/are false? Check all that apply.A π bond restricts rotation about the bond axisBonds formed from the overlap of atomic s orbitals are always σ bondsTwo σ bonds comprise a double bondEnd-to-end overlap of orbitals results in a bond with electron density above and below the bond axisNone of the above
Question
Which statement(s) is/are false? Check all that apply.A π bond restricts rotation about the bond axisBonds formed from the overlap of atomic s orbitals are always σ bondsTwo σ bonds comprise a double bondEnd-to-end overlap of orbitals results in a bond with electron density above and below the bond axisNone of the above
Solution
The false statements are:
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"Two σ bonds comprise a double bond" - This is false because a double bond is made up of one σ bond and one π bond, not two σ bonds.
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"End-to-end overlap of orbitals results in a bond with electron density above and below the bond axis" - This is false because end-to-end overlap of orbitals results in a σ bond, which has electron density along the bond axis, not above and below it. Above and below the bond axis electron density is characteristic of a π bond, which results from side-to-side overlap of orbitals.
The other statements are true:
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"A π bond restricts rotation about the bond axis" - This is true because π bonds involve the overlap of parallel p orbitals, which restricts rotation.
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"Bonds formed from the overlap of atomic s orbitals are always σ bonds" - This is true because s orbitals can only overlap directly, forming σ bonds.
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"None of the above" - This is false because there are false statements in the list.
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