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Chapter 3: Problem 1

What do you mean by an ionic bond? Discuss the formation of an ionic bond and the necessary conditions.

Short Answer

Expert verified
An ionic bond is a type of chemical bond that forms through the electrostatic attraction between oppositely charged ions. It typically forms when a metal atom loses electron(s) to a non-metal atom such that both of them achieve a stable electronic configuration.

Step by step solution

01

Define Ionic Bond

An ionic bond is a type of chemical bond that involves the electrostatic attraction between oppositely charged ions. These ions represent atoms that have lost one or more electrons (known as cations) and atoms that have gained one or more electrons (known as anions). This bond is usually formed between a metal and a non-metal.
02

Explain Formation of Ionic Bond

Ionic bonds form when one atom gives up one or more electrons to another atom. For instance, when a sodium atom transfers one electron to a chlorine atom, forming a sodium cation \(Na^{+}\) and a chloride anion \(Cl^{-}\). The attraction between these oppositely charged ions forms an ionic bond.
03

Describe Necessary Conditions for Ionic Bond Formation

For an ionic bond to form, the outermost orbital of one atom (the valence shell) must lose electron(s) (usually a metal), while the other must gain those electron(s) in its valence shell (usually a non-metal). This ensures that both atoms gain a stable electronic configuration.

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Most popular questions from this chapter

(a) Neon molecule is monoatomic but Hydrogen molecule is diatomic. (b) The loss of an electron from a diatomic molecule results in decrease of its bond energy. (c) Bond length of NO is higher than that of \(\mathrm{NO}^{\circ}\) (d) Bond order of \(\mathrm{N}_{2}\) is higher than that of \(\mathrm{N}_{2}^{+}\).

Use MO diagram to compare bond length and bond order of following species: \(\mathrm{O}_{2}^{+}, \mathrm{O}_{2}, \mathrm{O}_{2}^{-}, \mathrm{O}_{2}^{2-}\).

Draw molecular orbital energy-level diagram for \(\mathrm{N}_{2}\) molecule.

Use MO diagram to predict the magnetic behaviour of the following molecules: (a) \(\mathrm{H}_{2}^{+}\) (b) \(\mathrm{B}_{2}\) (c) \(\mathrm{O}_{2}^{+}\) (d) \(\mathrm{N}_{2}^{2-}\)

Construct the wave functions for the \(s p\) and \(s p^{3}\) hybrid orbitals.
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