Question #c5557

1 Answer
May 21, 2015

Carbon uses #sp^3#, #sp^2#, and #sp# hybridization when it forms compounds.

Explanation:

Carbon uses #sp^3#, #sp^2#, and #sp# hybridization when it forms compounds.

#sp^3# Hybridization

When a carbon atom bonds to four other atoms, it mixes one #2s# and three #2p# orbitals to form four new energetically equivalent #sp^3# hybrid orbitals.

These orbitals are at angles of 109.5 ° to each other and point toward the corners of a tetrahedron.

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#sp^2# Hybridization

When a carbon atom bonds to three other atoms, it mixes one #2s# and two of the three #2p# orbitals to form three new energetically equivalent #sp^2# hybrid orbitals.

The #sp^2# orbitals are at angles of 120 ° to each other and point toward the corners of an equilateral triangle.

We say that they have a trigonal planar geometry.

The unhybridized #2p# orbital is perpendicular to the plane of the #sp^2# orbitals.

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#sp# Hybridization

When a carbon atom bonds to two other atoms, it mixes one #2s# and one of the three #2p# orbitals to form two new energetically equivalent #sp# hybrid orbitals.

The #sp# orbitals are at angles of 180 ° to each other and point directly away from each other in a straight line.

We say that they have a linear geometry.

The two unhybridized #2p# orbitals are perpendicular to each other and to the #sp# orbitals.

sp orbitals

The unhybridized p orbitals are used to make the π bonds in alkynes like ethyne.

Ethyne