Hybridization of Carbon in Chemistry

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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

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

Carbon atoms hybridize their atomic orbitals to form stronger bonds with greater overlap, resulting in more stable molecules with lower energy.

In sp3 hybridization, a carbon atom has four equivalent bonds to hydrogen, each with the same bond distance (109.3 degrees).

When a carbon atom forms a double bond, it adopts an sp2 hybridization state.

In sp hybridization, a carbon atom forms only two bonds to other atoms, like in acetylene.

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Electronegativity (EN) is a measure of an atom's ability to attract electrons in a chemical bond.

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

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.

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

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 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.