How many unpaired electrons are in the ground state electron configuration 4s23d9?
1 answer:
ANSWER
The number of the unpaired electrons is 1
STEP-BY-STEP EXPLANATION:
The electronic configuration of a particular element is given below as
From the electronic configuration above, you will see that the 4s-orbital has two electrons and the 3d-orbital has 9 electrons
According to Hund's Rule, it "states that electron goes into orbital singly before pairing commences."
To determine the number of unpaired electrons, we need to study the total number of electrons in the d-orbital as given by the question.
Note that, the <em>maximum number of electrons</em> that can enter into the d-orbital is 10
The next step is to fill in the electrons into the orbital
From the above structure, you will see that the number of paired electrons is 4 and the number of unpaired electrons is 1
Therefore, the number of the unpaired electrons is 1
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Answer:
(d) 3,7-dimethyl-4-nonyne.
Explanation:
Hello,
In this case, considering the attached picture on which you can see that the main chain has nine carbon atoms, one tripe bond at the fourth carbon and two methyl radicals at the third and seventh carbons respectively, by following the IUPAC rules, the name would be: (d) 3,7-dimethyl-4-nonyne since the chain must start at the side closest to the first triple bond due to its priority and subsequently considering the present radicals.
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