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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?
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?
When a carbon atom is bonded to another atom by a double bond, which type of hybrid state does it assume?
In which type of hybridization does a carbon atom join to only two other atoms, as in acetylene (C2H2)?
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What is electronegativity (EN) a measure of?
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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 (Câ‚‚Hâ‚‚).
- 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.
