Chapter 7: Problem 62
What is the total number of electrons that can be held in all orbitals having the same principal quantum number \(n ?\)
Over 30 million students worldwide already upgrade their learning with Vaia!
All the tools & learning materials you need for study success - in one app.
Get started for free
For each of the following pairs of hydrogen orbitals, indicate which is higher in energy: (a) \(1 s, 2 s ;\) (b) \(2 p\), \(3 p ;\) (c) \(3 d_{x y}, 3 d_{y z};\) (d) \(3 s, 3 d ;\) (e) 4f, \(5 s.\)
Describe the shapes of \(s, p,\) and \(d\) orbitals. How are these orbitals related to the quantum numbers \(n, \ell\) and \(m_{\ell} ?\)
What is meant by the term "shielding of electrons" in an atom? Using the \(\mathrm{Li}\) atom as an example, describe the effect of shielding on the energy of electrons in an atom.
List all the possible subshells and orbitals associated with the principal quantum number \(n\), if \(n=5\).
The \(\mathrm{He}^{+}\) ion contains only one electron and is therefore a hydrogen-like ion. Calculate the wavelengths, in increasing order, of the first four transitions in the Balmer series of the \(\mathrm{He}^{+}\) ion. Compare these wavelengths with the same transitions in a \(\mathrm{H}\) atom. Comment on the differences. (The Rydberg constant for \(\mathrm{He}^{+}\) is \(\left.8.72 \times 10^{-18} \mathrm{~J} .\right)\)
What do you think about this solution?
We value your feedback to improve our textbook solutions.
