Orbital Overlap Diagram of Ethyne - Acetylene

TL;DR

Acetylene has an SP hybridized carbon atom with overlapping S and SP orbitals in the CH bond, and overlapping SP orbitals in the triple bond.

Transcript

65. draw the orbital picture of acetylene so first let's start with the Lewis structure of acetylene now what is the hybridization at this carbon this carbon has two groups attached to it so it's going to be s1p1 hybridized one plus one is two hydrogen is simply an S orbital it's not really a hybrid orbital it's just pures when you have a hybrid yo... Read More

Key Insights

• ♏ Acetylene's carbon atom is SP hybridized, meaning it has one S and one P orbital in its hybrid orbital.
• 🎅 The CH bond in acetylene has an overlap between an SP orbital of carbon and an S orbital of hydrogen.
• 🫀 The triple bond in acetylene has an overlap between two SP orbitals on adjacent carbon atoms.
• 😀 Acetylene has two empty P orbitals remaining in its SP hybrid carbon atom.
• 💁 The sigma bond in the triple bond is formed by the overlap of two SP orbitals.
• 💁 The first pi bond in the triple bond is formed by the overlap of two empty P orbitals in the Y direction.
• 😴 The second pi bond in the triple bond is formed by the overlap of two empty P orbitals in the Z direction.

Questions & Answers

Q: How is acetylene's carbon atom hybridized?

Acetylene's carbon atom is SP hybridized, meaning it uses one S and one P orbital to form the SP hybrid orbital.

Q: What type of orbital overlap is found in the CH bond of acetylene?

The CH bond in acetylene has an overlap between the SP orbital of carbon and the S orbital of hydrogen.

Q: How many empty P orbitals does an SP hybrid carbon have?

An SP hybrid carbon has two empty P orbitals remaining, as it used one of its three P orbitals to form the SP hybrid orbital.

Q: What type of orbital overlap is found in the triple bond of acetylene?

The triple bond in acetylene has an overlap between two SP orbitals on the adjacent carbons.

Summary & Key Takeaways

• Acetylene's Lewis structure shows an SP hybridized carbon with two hydrogen atoms attached.

• The carbon atom takes one S orbital and one of its three P orbitals to form the SP hybrid orbital.

• In the triple bond, there are two SP orbitals overlapping, while in the CH bond, an SP orbital overlaps with an S orbital.