Write the electronic configuration of the O2− ion.

Expert Solution

In order to write a correct electronic configuration, one must keep in mind three rules, which are as follows:

Aufbau principle: This principle states that the orbitals are filled in the order of their energy, that is the orbitals with lower energy would be filled first.

Pauli's exclusion principle: This principle states that no two electrons should have the same set of all the 4 quantum numbers.

Hund's rule: This rule states that the electron pairing in an orbital in a subshell wouldn't happen until and unless all the orbitals in a subshell are half-filled.

Now, let's get to the problem at hand:

O2- could mean any of the two things: or

So let's start with :

The electronic configuration for is:

Now let's look at the configuration of :

is a molecule so, here, we're going to use molecular orbital theory to arrive at the electronic configuration:

So, the electronic configuration for is:

This configuration can be more plausibly seen in the image given below:

queen_honey_blossom answered 10 months ago

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