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Using the Bohr model, determine the lowest possible energy, in joules, for the electron in the ${Li}^{2+}$ ion.

$E=-1.961 \cdot 10^{-17} \mathrm{J}$

Chemistry 101

Chapter 6

Electronic Structure and Periodic Properties of Elements

Electronic Structure

Periodic Table properties

Drexel University

University of Kentucky

University of Toronto

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So this problem. We were asked to calculate the energy of a ground state electron on lithium to Plus don't do that. We're going to use the equation that I have written here and what it basically does is relates to the number of pro times on a given bore nucleus relative to the energy level in question and calculates the energy of an electron within that energy level. Keep in mind that the reason we're able to use this equation because let the M two plus is a bore like Adam, it only has one electron. So this equation directly applies to that single electron. So the only thing we really need to do here is to fill in our values because we're dealing with lithium has three protons. So this P is going to be three squared, multiplied by this constant negative 2.178 times 10 to the negative 18. Jules, the whole thing is going to be divided by the energy level of the electron in this case, because you want to look at the lowest energy state, we're going to be looking at the electron in its ground state, Oregon, and equal one So what we do? We multiply all this out. We end up with 1.961 times 10 to the negative 17 jewels.

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