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Chapter 5: Problem 42

Explain the structure of \(\mathrm{CH}_{4}\) with the help of hybridization.

Short Answer

Expert verified
Answer: The hybridization of the central carbon atom in methane (CH4) is sp³, resulting in a tetrahedral molecular geometry.

Step by step solution

01

Determine the central atom and its orbitals

In this exercise, the central atom is carbon, which has 6 electrons. Its electron configuration is 1s² 2s² 2p². Two electrons are in the 2s orbital, and two more are in the 2p orbitals.
02

Determine the hybridization of the central atom

In order to make four equivalent bonds with hydrogen atoms, carbon needs to have four unpaired electrons. This can be achieved by promoting one of the 2s electrons to the 2p orbital. The electron configuration of carbon becomes 1s² 2s¹ 2p³. Now, the 2s and three 2p orbitals mix or hybridize to form four equivalent hybrid orbitals known as sp³ hybrid orbitals.
03

Describe the bonding between central atom and surrounding atoms

The four hydrogen atoms, each with one electron in their 1s orbital, will bond with the four available unpaired electrons in the four sp³ hybrid orbitals of carbon. The overlap of the carbon sp³ hybrid orbitals and hydrogen 1s orbitals results in the formation of four sigma (σ) bonds.
04

Determine the molecular geometry of the molecule

The arrangement of the four sp³ hybrid orbitals in space is determined by minimizing electron repulsion, which results in a tetrahedral geometry. Each carbon-hydrogen bond is at an angle of 109.5° with respect to the others. Overall, the structure of methane (\(\mathrm{CH}_{4}\)) can be explained using hybridization: the central carbon atom undergoes sp³ hybridization, forming four sigma bonds with four hydrogen atoms, and resulting in a tetrahedral molecular geometry.

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Most popular questions from this chapter

"The orbitals of two different shells of an atom combine and form one hybrid orbital." State whether the statement is true or false and justify your answer.

Why do metals conduct electricity?

The number of \(\sigma\) bonds and \(\pi\) bonds in \(\mathrm{CO}_{2}\) molecule are \(\quad\) respectively.

(a) What is hybridization? (b) What are the conditions for an atom to undergo hybridization? (c) How can we explain the shapes and bond angles of \(\mathrm{BeCl}_{2}, \mathrm{BCl}_{3}\) and \(\mathrm{CH}_{4}\) with hybridization?

Which force opposes the interionic forces of attraction between the oppositely charged ions during the formation of an ionic crystal?
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