Question

Using the Bohr model, determine the lowest possible energy, in joules, for the electron in the He+ ion.

Answer 1

Answer:

$E=-8.72\times 10^{-18}\ Joules$

Explanation:

The expression for Bohr energy of the hydrogen-like species is:

$E_n=-Z^2\times \frac{2.179\times 10^{-18}}{n^2}\ Joules$

Where, Z is the atomic number of the element

For, $He^{2+}$, Z = 2

For lowest energy, n = 1

Thus, Applying the values as:-

$E=-2^2\times \frac{2.179\times 10^{-18}}{1^2}\ Joules$

$E=-8.72\times 10^{-18}\ Joules$