Lennard-Jones potential
The chemical bond between two atoms results from the interaction between them.
Let us consider two atoms at a distance $r$. An empirical potential that describes the interaction between them is the potential Lennard-Jones,
$$ V(r) = D\left(\frac{R}{r}\right)^{12} - 2 \left(\frac{R}{r}\right)^6 $$
where $D, R$ are constants.
[This form of a potential describes Van der Waals bonds between atoms, that is, dipole-dipole interaction.]
Note that
$$ \begin{aligned} & V(r) \to \infty,\qquad \text{when}\;\; r\to 0 \\ & V(r) \to 0,\qquad\,\, \text{when}\;\; r\to \infty. \end{aligned} $$
The derivative is
$$ \frac{dV}{dr} = \frac{12}{r}\,\left[ \left(\frac{R}{r}\right)^6 - D \left(\frac{R}{r}\right)^{12} \right] $$
Solid line: Lennard-Jones potential. Dashed line: Parabolic approximation. (Values of parameters $D=1, R=5$.)
We have a minimum when
$$ \frac{dV}{dr}\Big|_{r=r_0} = 0 \Rightarrow r_0 = D^{1/6} R. $$
Its value is
$$ V(r=r_0) = -\frac{1}{D}. $$
[We also find $\frac{d^2V}{dr^2}(r=r_0) = \frac{72}{R^2 D^{4/3}} > 0$.]
Questions.
Solid line: Lennard-Jones potential. Dashed line: Parabolic approximation. (Values of parameters $D=1, R=5$.)