Here, (a) is the most unstable and (d) is the most stable configuration. Accordi
ID: 700378 • Letter: H
Question
Here, (a) is the most unstable and (d) is the most stable configuration.
According to Pauli's exclusion principle, no two electrons can have the same set of quantum numbers. Hence, (a) is not a possible configuration. (b) on the other hand, has electrons with different spin qauntum number which makes the total spin zero and makes it more stable than (b). But (b) disobeys Hund's Rule which states that electrons in the orbitals of a sublevel are first singly occupied and with same spin before being doubly occupied.
Electrons in (c) are present in degenerate orbitals, have total spin zero, but the configuration doesn't obey the Hund's Rule. In (d) configuration also the electrons are present in degenerate orbitals but obey Hund's Rule and have parallel spin. Hence, the electrons would have a tendency to exchange their positions. The energy released in this process is called exchange energy and it increases stability.
(a), (b), (c) have zero exchange energy because in (a) and (b) electrons are present in same orbital and in (c) electrons don't have parallel spins. Hence, (d) is the most stable due to maximum exchange energy. (d) has the lowest energy.
So,
Explanation / Answer
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lle luentity of the element with this configuration? diamagnetic? element have? (b) Is a sample of the element paramagnetic or Pan (e) How many unpaired electrons does a 3t ion pf this Compare the configurations below with two electrons located in p orbitals. Which would be the most stable (have the lowest energy), which would be the least stable? Explain your answers. lit Goette op (a) f (b) F Draw a Lewis structure for each of the following molecules (a) chlorodifluoromethane, CHCIF