Q. \(3d\) \(t_{2g}\)–\(2p\) \( \alpha\) \( \beta\)-hybridization.

Q: What is the hybridization of \mathrm{CO_3^{2-}} ?

\mathrm{CO_3^{2-}} has trigonal planar geometry, so the central carbon is sp^2 hybridized.

Q: Which orbitals form the pi bonds in \mathrm{CO_3^{2-}} ?

The unhybridized p orbital on carbon (perpendicular to the plane) overlaps with oxygen p orbitals to form the pi framework.

Q: What are the bond angles in \mathrm{CO_3^{2-}} ?

Trigonal planar means bond angles are about 120^\circ between the C–O bonds.

Answer

\( \mathrm{CO_3^{2-}} \) has 3 electron domains around the central carbon (two equivalent C=O bonds and one C–O single bond resonance). So the electron-group geometry is trigonal planar.

The central carbon must therefore be \( \mathrm{sp^2} \) hybridized (trigonal planar gives \( \mathrm{sp^2} \) with one unhybridized \(p\) orbital for \(\pi\) bonding).

Final result: \( \mathrm{CO_3^{2-}} \) (at carbon) is \( \mathrm{sp^2} \) hybridized.

Detailed Explanation

We need to determine the hybridization of the species with formula \(\mathrm{CO_3^{2-}}\) (carbonate). The key idea is to look at the electron geometry around each carbon atom.

Step 1: Identify the central atom and the bonding pattern

In \(\mathrm{CO_3^{2-}}\), carbon is the central atom. Carbon is bonded to three oxygen atoms.

So, around each carbon, there are three \(\sigma\)-bonds: \(\mathrm{C{-}O}\) (each between carbon and an oxygen).

Step 2: Determine the number of electron domains

Hybridization depends on the number of electron domains (regions of electron density) around the central atom.

For carbon in \(\mathrm{CO_3^{2-}}\):

\(\mathrm{3}\) bonding domains (three \(\mathrm{C{-}O}\) bonds)
\(\mathrm{0}\) lone-pair domains on carbon

Therefore, total electron domains \(= 3\).

Step 3: Match electron domains to the hybridization

Using VSEPR and hybridization rules:

\(3\) electron domains correspond to a trigonal planar geometry
Trigonal planar corresponds to \(\mathrm{sp^2}\) hybridization

Step 4: State the hybridization

Thus, the carbon in \(\mathrm{CO_3^{2-}}\) is \(\mathrm{sp^2}\) hybridized.

Final Answer

\(\mathrm{CO_3^{2-}}\): the central carbon atom is \(\mathrm{sp^2}\) hybridized (trigonal planar geometry around carbon).

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General Chemistry FAQs

What is the hybridization of \( \mathrm{CO_3^{2-}} \)?

\( \mathrm{CO_3^{2-}} \) has trigonal planar geometry, so the central carbon is \( sp^2 \) hybridized.

Why is \( \mathrm{CO_3^{2-}} \) trigonal planar?

There are 3 electron domains around carbon (three C–O sigma bonds) and no lone pairs on carbon, giving \( sp^2 \) and trigonal planar shape.

How do lone pairs affect hybridization in \( \mathrm{CO_3^{2-}} \)?

Since carbon has no lone pairs, electron-domain count stays 3. Thus carbon uses \( sp^2 \) rather than \( sp \) or \( sp^3 \).

How many sigma bonds and electron domains does \( \mathrm{CO_3^{2-}} \) have?

Carbon forms 3 sigma bonds to oxygen. Those are 3 electron domains, leading to \( sp^2 \) hybridization.

Does the resonance of \( \mathrm{CO_3^{2-}} \) change hybridization?

No. Resonance redistributes pi bonding, but geometry remains trigonal planar. Hybridization stays \( sp^2 \).

Which orbitals form the pi bonds in \( \mathrm{CO_3^{2-}} \)?

The unhybridized \( p \) orbital on carbon (perpendicular to the plane) overlaps with oxygen \( p \) orbitals to form the pi framework.

What are the bond angles in \( \mathrm{CO_3^{2-}} \)?

Trigonal planar means bond angles are about \( 120^\circ \) between the C–O bonds.

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