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Chapter 3: Problem 19

Describe the type of bonding that exists in the \(\mathrm{Cl}_{2}(g)\) molecule. How does this type of bonding differ from that found in the HCl(g) molecule? How is it similar?

Short Answer

Expert verified
In Cl2(g), two chlorine atoms form a covalent bond by equally sharing electrons, resulting in a nonpolar covalent bond. In HCl(g), hydrogen and chlorine atoms also form a covalent bond by sharing electrons, but the electronegativity difference between the atoms causes an uneven electron distribution, resulting in a polar covalent bond. Therefore, the similarity between Cl2(g) and HCl(g) is that both involve covalent bonding between non-metal atoms, while the difference lies in the nature of the bond, with Cl2(g) being nonpolar and HCl(g) being polar.

Step by step solution

01

Identify the type of bonding in Cl2(g)

In Cl2(g), we have two chlorine atoms forming a bond. Since both atoms are non-metals, they share electrons to achieve a stable electron configuration, which means that Cl2(g) involves a covalent bond.
02

Identify the type of bonding in HCl(g)

In HCl(g), we have a hydrogen atom and a chlorine atom forming a bond. Both atoms are non-metals, and they also share electrons to achieve a stable electron configuration. Thus, the bonding in HCl(g) is also covalent.
03

Explain the differences in bonding between Cl2(g) and HCl(g)

The main difference between the covalent bonds in Cl2(g) and HCl(g) is related to their electronegativity. In Cl2(g), both chlorine atoms have the same electronegativity, which means they share electrons equally. This is called a nonpolar covalent bond. In HCl(g), the electronegativity of chlorine is higher than that of hydrogen, which means that chlorine attracts the shared electrons more strongly, creating an uneven distribution of electron density. This is known as a polar covalent bond.
04

Explain the similarity in bonding between Cl2(g) and HCl(g)

The primary similarity between the bonding in Cl2(g) and HCl(g) is that both molecules involve covalent bonds between non-metal atoms, where the atoms share electrons to achieve a stable electron configuration.

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