Chapter 5: Problem 37

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

Short Answer

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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

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 \(1\mathrm{s}^{2}2\mathrm{s}^{2}2\mathrm{p}^{6}3\mathrm{s}^{2}3\mathrm{p}^{5}\).

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.

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

Short Answer

Step by step solution

Electron Configuration of Be and Cl

Type of Hybridization

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

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