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Chapter 9: Problem 2

For the following cases, what type of bonding is expected? (a) KCl molecule; (b) \(\mathrm{N}_{2}\) molecule.

Short Answer

Expert verified
(a) KCl molecule: Ionic bonding (b) \(\mathrm{N}_{2}\) molecule: Nonpolar covalent bonding

Step by step solution

01

Recall electronegativity values and bonding types

To determine the type of bond formed between the atoms in each molecule, we first need to recall the electronegativity values of the involved elements. We can use the Pauling electronegativity scale as a reference. Here are the electronegativity values for the elements in question: - Potassium (K): 0.8 - Chlorine (Cl): 3.16 - Nitrogen (N): 3.04 Next, we'll recall that bonds can be classified into the following types based on the difference in electronegativity (∆EN) values between the involved elements: - Ionic bond: ∆EN > 1.7 - Polar covalent bond: ∆EN = 0.4 - 1.7 - Nonpolar covalent bond: ∆EN < 0.4
02

Calculate electronegativity differences and bonding types

Now, let's calculate the electronegativity difference for each molecule and determine the type of bond formed: (a) KCl molecule ∆EN = |Electronegativity of Cl - Electronegativity of K| ∆EN = |3.16 - 0.8| ∆EN = 2.36 Since ∆EN > 1.7, the KCl molecule has ionic bonding. (b) \(\mathrm{N}_{2}\) molecule ∆EN = |Electronegativity of N - Electronegativity of N| ∆EN = |3.04 - 3.04| ∆EN = 0 Since ∆EN < 0.4, the \(\mathrm{N}_{2}\) molecule has a nonpolar covalent bonding.
03

Answer

(a) KCl molecule: Ionic bonding (b) \(\mathrm{N}_{2}\) molecule: Nonpolar covalent bonding

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