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QuestionCompound 1:
Molecular orbital type: □\square Atomic orbitals in the sigma bond: □\square Atomic orbitals in the pi bond: □\square Compound 2:
Molecular orbital type: □\square Atomic orbitals in the sigma bond: □\square Atomic orbitals in the pi bond: □\square

Studdy Solution

STEP 1

1. The question involves understanding the molecular orbitals and the atomic orbitals involved in sigma and pi bonds.
2. Sigma bonds (σ\sigma) are formed by the end-to-end overlap of atomic orbitals.
3. Pi bonds (π\pi) are formed by the side-to-side overlap of atomic orbitals.
4. The carbon-carbon triple bond involves one sigma bond and two pi bonds.
5. The carbon-oxygen double bond involves one sigma bond and one pi bond.
6. The carbon-nitrogen single bond involves one sigma bond.

STEP 2

1. Determine the molecular orbital type and atomic orbitals involved for Compound 1's highlighted bond.
2. Determine the molecular orbital type and atomic orbitals involved for Compound 2's highlighted bond.

STEP 3

For Compound 1, identify the molecular orbital type for the highlighted carbon-oxygen double bond.
The molecular orbital type for a double bond is σ+π\sigma + \pi. Molecular orbital type: σ+π \text{Molecular orbital type: } \sigma + \pi

STEP 4

Determine the atomic orbitals involved in the sigma bond of the carbon-oxygen double bond in Compound 1.
The sigma bond is formed by the overlap of an sp2sp^2 hybrid orbital from carbon and an sp2sp^2 hybrid orbital from oxygen. Atomic orbitals in the sigma bond: sp2 (C)−sp2 (O) \text{Atomic orbitals in the sigma bond: } sp^2 \text{ (C)} - sp^2 \text{ (O)}

STEP 5

Determine the atomic orbitals involved in the pi bond of the carbon-oxygen double bond in Compound 1.
The pi bond is formed by the side-to-side overlap of unhybridized pp orbitals from both carbon and oxygen. Atomic orbitals in the pi bond: p (C)−p (O) \text{Atomic orbitals in the pi bond: } p \text{ (C)} - p \text{ (O)}

STEP 6

For Compound 2, identify the molecular orbital type for the highlighted carbon-nitrogen single bond.
The molecular orbital type for a single bond is σ\sigma. Molecular orbital type: σ \text{Molecular orbital type: } \sigma

STEP 7

Determine the atomic orbitals involved in the sigma bond of the carbon-nitrogen single bond in Compound 2.
The sigma bond is formed by the overlap of an sp3sp^3 hybrid orbital from carbon and an sp3sp^3 hybrid orbital from nitrogen. Atomic orbitals in the sigma bond: sp3 (C)−sp3 (N) \text{Atomic orbitals in the sigma bond: } sp^3 \text{ (C)} - sp^3 \text{ (N)}

STEP 8

There is no pi bond in the carbon-nitrogen single bond in Compound 2.
Atomic orbitals in the pi bond: None \text{Atomic orbitals in the pi bond: } \text{None}
Solution Summary: Compound 1: - Molecular orbital type: σ+π\sigma + \pi - Atomic orbitals in the sigma bond: sp2 (C)−sp2 (O)sp^2 \text{ (C)} - sp^2 \text{ (O)} - Atomic orbitals in the pi bond: p (C)−p (O)p \text{ (C)} - p \text{ (O)}
Compound 2: - Molecular orbital type: σ\sigma - Atomic orbitals in the sigma bond: sp3 (C)−sp3 (N)sp^3 \text{ (C)} - sp^3 \text{ (N)} - Atomic orbitals in the pi bond: None

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