5- Carbohydrates worksheet.pdf - Rea De Guzman Name: Pd ... - Free Printable

Problem Analysis:

The task involves understanding and solving a problem related to chemical bonding and molecular geometry, specifically focusing on the molecule ethylene (C₂H₄). The image provided includes a molecular structure of ethylene, which is a planar molecule with a double bond between the two carbon atoms.

#### Key Points from the Image:
1. Molecular Structure: Ethylene (C₂H₄) has a planar structure with a double bond between the two carbon atoms.
2. Bonding Information:
- Each carbon atom forms a σ (sigma) bond with the other carbon atom.
- Each carbon atom also forms σ bonds with two hydrogen atoms.
- The double bond consists of one σ bond and one π (pi) bond.
3. Hybridization:
- Carbon atoms in ethylene are sp² hybridized.
- This results in trigonal planar geometry around each carbon atom.
4. Question: The question asks about the type of orbital overlap involved in the formation of the double bond between the two carbon atoms.

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Solution:

#### Step 1: Understand Orbital Overlap in Double Bonds
A double bond consists of:
1. One σ (sigma) bond: Formed by the head-on overlap of orbitals along the internuclear axis.
2. One π (pi) bond: Formed by the side-by-side overlap of orbitals perpendicular to the internuclear axis.

In ethylene:
- The σ bond is formed by the overlap of an sp² hybrid orbital from one carbon atom with an sp² hybrid orbital from the other carbon atom.
- The π bond is formed by the overlap of the unhybridized p orbital from one carbon atom with the unhybridized p orbital from the other carbon atom.

#### Step 2: Identify the Types of Overlap
- σ Bond Overlap: Head-on overlap of sp² hybrid orbitals.
- π Bond Overlap: Side-by-side overlap of unhybridized p orbitals.

#### Step 3: Answer the Question
The question asks specifically about the type of orbital overlap involved in the formation of the double bond. Since a double bond involves both σ and π bonds, the correct answer must include both types of overlap.

From the options provided in the question (not explicitly listed here but inferred from the context):
- The correct answer should mention both head-on overlap (for the σ bond) and side-by-side overlap (for the π bond).

#### Final Answer:
The type of orbital overlap involved in the formation of the double bond between the two carbon atoms in ethylene is:
- Head-on overlap for the σ bond.
- Side-by-side overlap for the π bond.

Thus, the correct choice would be the option that includes both types of overlap.

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Explanation of Hybridization and Geometry:

1. sp² Hybridization:
- Each carbon atom in ethylene uses one s orbital and two p orbitals to form three sp² hybrid orbitals.
- These sp² hybrid orbitals are arranged in a trigonal planar geometry.
- One sp² hybrid orbital from each carbon atom overlaps head-on to form the σ bond.
- The remaining unhybridized p orbitals from each carbon atom overlap side-by-side to form the π bond.

2. Planarity:
- The sp² hybrid orbitals lie in the same plane, making the molecule planar.
- All atoms (two carbons and four hydrogens) lie in the same plane.

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Conclusion:

The solution to the problem involves recognizing that a double bond consists of both σ and π bonds, formed by different types of orbital overlap. The final answer is:

\[
\boxed{\text{Head-on overlap and side-by-side overlap}}
\]