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For this problem, we first need to write the ground state electron configuration before we can get the number of unpaired electrons. We'll use the condensed noble-gas notation for this problem. This just means that we use the symbol of the nearest noble gas that comes before our element. We use this to represent the first part of the electron configuration.
A) For P(g), we start by finding the noble gas that we'll use and we'll see in the periodic table that it would be Ne. Now we still have to finish the electron configuration since we have more electrons in P. Also note that this is just a neutral element so no need to add or subtract electrons. There would be 5 electrons that would be in excess of Ne so we write the electron configuration as follows:
Write ground-state electronic configurations for the following atoms or ions and give the number of unpaired electrons:
P(g) ___ unpaired electrons
Ti(g) ___ unpaired electrons
Ni2+(g) ___ unpaired electrons
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Based on our data, we think this problem is relevant for Professor Johnson's class at UBC.