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Chapter 5: Problem 37

Explain the structure of \(\mathrm{BeCl}_{2}\) with the help of hybridization.

Short Answer

Expert verified
Question: Based on the hybridization concept, describe the structure of \(\mathrm{BeCl}_{2}\). Answer: The structure of \(\mathrm{BeCl}_{2}\) is linear, with beryllium at the center forming single covalent bonds with two chlorine atoms at an angle of 180 degrees using its two \(\mathrm{sp}\) hybrid orbitals.

Step by step solution

01

Electron Configuration of Be and Cl

Determine the electron configuration of beryllium and chlorine. Beryllium has 4 electrons, and its electron configuration is \(1\mathrm{s}^{2}2\mathrm{s}^{2}\). Chlorine has 17 electrons, with an electron configuration of \(1\mathrm{s}^{2}2\mathrm{s}^{2}2\mathrm{p}^{6}3\mathrm{s}^{2}3\mathrm{p}^{5}\).
02

Type of Hybridization

Identify the type of hybridization in \(\mathrm{BeCl}_{2}\). In the case of \(\mathrm{BeCl}_{2}\), beryllium forms two single bonds with each of the chlorine atoms. To form these bonds, the two electrons in beryllium's 2s orbital get excited and hybridize with its vacant 2p orbitals. This results in the formation of two \(\mathrm{sp}\) hybrid orbitals.
03

The Structure of \(\mathrm{BeCl}_{2}\)

Determine the structure of \(\mathrm{BeCl}_{2}\) based on hybridization. The two \(\mathrm{sp}\) hybrid orbitals of beryllium are now available for bonding. The hybrid orbitals are arranged linearly at an angle of 180 degrees, resulting in a linear molecular structure for \(\mathrm{BeCl}_{2}\). The beryllium atom lies at the center with chlorine atoms on either side, forming single covalent bonds using their 3p orbitals.

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Most popular questions from this chapter

What are the factors on which the geometrical shapes of covalent molecules depend? Explain with suitable examples.

(a) The strength of a covalent bond depends on which factor/factors? (b) Classify covalent bonds depending on the strength. Compare those bonds.

In the formation of a \(\mathrm{Br}_{2}\) molecule, the overlapping of orbitals takes place.

How many new hybrid orbitals are formed in sp, \({ }^{s} \mathrm{p}^{2}\) and \(\mathrm{sp}^{3}\) hybridizations?

What would be the shape of \(\mathrm{XY}_{3}\) molecule if there is no lone pair on the central atom?
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