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Hybridization of Carbon in Chemistry

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Questions and Answers

What is the main reason for carbon atom or compounds to hybridize its four second level atomic orbitals?

To form stronger bonds due to greater overlap and result in more stable lower energy molecules (correct)

To form nonpolar bonds due to absence of overlap and result in neutral energy molecules

To form weaker bonds due to lesser overlap and result in less stable higher energy molecules

To form ionic bonds due to complete transfer of electrons and result in charged molecules

In which type of hybridization does a carbon atom have four equivalent bonds to hydrogen, with each C-H bond having the same bond distance and a bond angle of 109.3 degrees?

No Hybridization

Sp3 Hybridization (correct)

Sp Hybridization

Sp2 Hybridization

When a carbon atom is bonded to another atom by a double bond, which type of hybrid state does it assume?

Sp3 Hybridization

Sp2 Hybridization (correct)

Sp Hybridization

No Hybridization

In which type of hybridization does a carbon atom join to only two other atoms, as in acetylene (C2H2)?

<p>Sp Hybridization</p> Signup and view all the answers

What is electronegativity (EN) a measure of?

<p>The ability of an atom to attract electrons</p> Signup and view all the answers

Study Notes

Carbon Hybridization

Carbon hybridizes its four second-level atomic orbitals to minimize energy and maximize stability in bonding with other atoms.

Tetrahedral Hybridization

During tetrahedral hybridization, a carbon atom forms four equivalent C-H bonds.
Each bond has an identical distance and a bond angle of 109.3 degrees.

Double Bond Hybrid State

When bonded to another atom via a double bond, carbon assumes a sp² hybrid state, typically involving one unhybridized p orbital.

Linear Hybridization

In linear hybridization, a carbon atom connects to only two other atoms, as demonstrated in acetylene (C₂H₂).
This involves sp hybridization, resulting in a bond angle of 180 degrees.

Electronegativity (EN)

Electronegativity measures an atom's ability to attract and hold onto electrons in a chemical bond.
It influences bond strength and polarity, impacting molecular structure and reactivity.

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Description

Test your knowledge on the hybridization of carbon atoms in chemistry. Understand why carbon behaves as a tetravalent element despite its electronic configuration suggesting it as a divalent element.