For an Na+ - Cl- ion pair, attractive and repulsive energies EA and ER, respectively,
depend on the distance between the ions r, according to

=−1.436

=7.32×10−6
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For these expressions, energies are expressed in electron volts per Na+ - Cl- pair, and r
is the distance in nanometers. The net energy EN is just the sum of the preceding two
expressions.

a. Superimpose on a single plot EN, ER, and EA versus r up to 1.0 nm (Use an Excel
worksheet).
b. On the basis of this plot, determine (i) the equilibrium spacing r0 between the Na+
and Cl- ions, and (ii) the magnitude of the bonding energy E0 between the two
ions.

The amount of energy required to separate the atoms forming a molecular bond into free atoms is known as bond energy, and it serves as a gauge of the strength of a chemical connection.

For Na⁺ and Cl⁻ ion pair, the attractive and repulsive energies are E(A) and E(R). The energies depend on the distance between the ions r.

We have,

E(A) = ( -1.436 / r )

E(R) = ( 7.32 × 10⁻⁶ / r⁸ )

(a) The plot for E(N), E(R), and E(A) versus r up to 1 nm is attached below.

(b) From the plot,

r(0) = 0.24 nm

E(0) = 5.3 eV

Hence, the equilibrium spacing r(0) between Na⁺ and Cl⁻ ions is 0.24 nm and the bonding energy is 5.3 eV.

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