Question

Use valence bond theory to write a hybridization and bonding scheme for CO2.

Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.

you can only use the following words:

two C(s)-O(s) ; two C(p)-O(p) ; trigonal planar ; two O(sp2)-C(sp) ; two O(sp)-C(sp2) ; carbon and oxygen ; sp2 ; a single and a double bond ; oxygen ; two single bonds ; linear ; tetrahydral ; carbon ; sp ; two double bonds ; sp3

Answer 1

Concepts and reason

Valence Bond Theory:

The Valence Bond Theory explains about covalent bond formations between two atoms and the shape of its geometry. It also assumes that all covalent bonds are localized.

Hybridization:

Hybridization is defined as the addition of different atomic orbitals to form a new hybrid orbital.

It is the concept of mixing atomic orbitals which have different shapes and energies to give an equal number of hybrid orbitals (to that of mixed orbitals), which have the same energy and shape. By using this concept, molecular geometry and bond angles can be explained for molecules.

VSEPR theory:

The Valance Shell Electron Pair Repulsion Theory (VSEPR) states that molecular geometry may alter due to the presence of repulsions between the lone pair of electrons and the bonded pair of electrons present in the molecule.

Fundamentals

Hybridization of the molecules can be found by counting the number of groups surrounding the central atom of the molecule.

Groups surrounded by the central atom	Hybridization	Molecular geometry
2		linear
3		Trigonal planar
4		tetrahedral
5		Trigonal bi-pyramidal

A lone pair of electrons is also considered as a group.

According to the VSEPR theory, molecular geometry may change due to the presence of repulsions between bonded pairs of electrons and lone pairs of electrons and they are arranged as follows.

Lewis Dot Structure of :

The central atom is Carbon.

The surrounding atoms are Oxygen.

Lewis Dot Structure of :

It is linear structure.

Structure of:

Carbon has two sp hybridized orbitals and two p atomic orbitals.

Oxygen has three sp² hybridized orbitals and one p atomic orbital.

Ans:

1. The Lewis structure for has a central carbon atom

attached to oxygen atoms through two double bonds.

2. Carbon dioxide has a linear electron geometry.

3. The carbon atom is hybridized.

4. Carbon dioxide has two C(p)-O(p) bonds and two O(p)-C(sp) bonds.