Question

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1
deduce the number of unpaired electrons rh would have in the d - sublevel. * (0.5 points)
7
3
5
2

Explanation:

Step1: Determine the electron configuration of Rh

Rhodium (Rh) has an atomic number of 45. Its electron configuration is \([Kr]4d^{8}5s^{1}\).

Step2: Analyze the d - sublevel electrons

The d - sublevel has 5 orbitals. According to Hund's rule, electrons fill orbitals singly first. For \(4d^{8}\), we first fill 5 orbitals with one electron each (total 5 electrons, all unpaired). Then we pair 3 of them. So the number of unpaired electrons in the d - sublevel is 1. Wait, no, let's correct. The electron configuration of Rh is \([Kr]4d^{8}5s^{1}\). For the \(4d\) sublevel: using Hund's rule (electrons occupy degenerate orbitals singly as far as possible). The \(4d\) sublevel has 5 orbitals. We have 8 electrons in \(4d\). First, 5 electrons occupy 5 orbitals (one in each, unpaired). Then the remaining 3 electrons pair up with 3 of the single - electron orbitals. So the number of unpaired electrons in \(4d\) is 2.

Answer:

2