= Solution
For a <hydrogen-like ion>, the <Coulomb potential> is stronger by the nuclear <atomic number> $Z$, and the <energy levels> scale as $Z^2$:
$$
\boxed{E_n=-\frac{Z^2R_H}{n^2},\qquad n=1,2,\ldots.}
$$
Here $Z$ is the number of <protons> in the <atomic nucleus>; the ion has exactly one <electron>, so its net <electric charge> is $(Z-1)e$. The zero of <energy> is a separated stationary <electron> and <atomic nucleus> at infinite distance. This is the nonrelativistic hydrogenic approximation using the supplied $R_H$; a more precise isotope-specific result also corrects the <reduced mass>.
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