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Solved: Calculate the energies needed to remove an
Chapter 7, Problem 144P(choose chapter or problem)
Calculate the energies needed to remove an electron from the n = 1 state and the n = 5 state in the \(\mathrm {Li}^{2+}\) ion. What is the wavelength (in nm) of the emitted photon in a transition from n = 5 to n = 1? The Rydberg constant for hydrogenlike ions is \((\mathrm {2.18 \times 10^{−18} J)Z^2}\), where Z is the atomic number.
Questions & Answers
QUESTION:
Calculate the energies needed to remove an electron from the n = 1 state and the n = 5 state in the \(\mathrm {Li}^{2+}\) ion. What is the wavelength (in nm) of the emitted photon in a transition from n = 5 to n = 1? The Rydberg constant for hydrogenlike ions is \((\mathrm {2.18 \times 10^{−18} J)Z^2}\), where Z is the atomic number.
ANSWER:Step 1 of 3
An electron from initial states 
The emitted energy calculated by the following formula;
Atomic number of Lithium - 3