we have already talked about electron configuration

and now in this video

we're going to extend that understanding

by thinking about the electron configuration of ions.

These are going to be charged atoms.

Let's just start looking at some examples.

Let's say we are dealing with fluorine.

Now, we know what a neutral fluorine atom's

electron configuration would be.

In fact, if you want a little bit of practice,

try to pause this video

and think about what is the electron configuration

of a neutral fluorine atom?

All right, now let's work through this together.

A neutral fluorine atom has nine electrons,

and we could just use our Periodic Table of Elements.

So first, we're going to have two electrons in 1s.

So we'll have 1s two.

And then we're going to go to the second shell.

So then we go to 2s two.

So far we have filled in four electrons.

And next we got to the 2p sub-shell.

And we are going to have,

we're talking about a neutral fluorine,

we are going to have one two three four five electrons

in that 2p sub-shell.

So it's 2p five.

So if that's the electron configuration for fluorine,

what do you think the electron configuration

for fluoride would be?

This is just the anion that has one extra electron.

It is a negatively charged ion.

Pause this video and try to figure it out.

Well, here you're now going to have one extra electron.

The fluorine has nabbed an electron from someplace

and so where will that extra electron go?

Well our 2p sub-shell has space for one more electron.

So that's where it will go.

So the fluoride anion is going to have

an electron configuration of 1s two, 2s two, 2p,

now it's going to have an extra electron here, 2p six.

2p six.

Now let's do another example.

Let's say we wanted to figure out the electron configuration

of a part positively charged calcium ion.

So calcium, let's make it two plus.

It has a positive charge of two.

You could do this as a neutral calcium

that has lost two electrons.

What would be its electron configuration?

Pause this video and try to figure that out.

All right, well one way to figure this out is

first we could figure out the electron configuration

of a neutral calcium atom

and then from that, we can take two

of the highest energy electrons away.

And so neutral calcium, you could view it,

actually let's do it in noble gas configuration.

Neutral calcium, the noble gas that comes

right before calcium is argon.

So it's going to have the electron configuration of argon

and then we are going to have two electrons

for that fourth shell.

It's going to fill in the 4s sub-shell.

And so we're going to have argon

and then we're going to have, let me do this in a new color,

let's call this 4s two.

Now what do you think is going to happen

if we were to lose two electrons?

Well those two electrons in that 4s sub-shell,

in the fourth shell, are gonna go away.

And so the electron configuration here

for calcium with a positive two charge,

this calcium cation, is going to be

the electron configuration of argon and no 4s two.

So it's actually going to have

the exact same electron configuration as argon.

So I will leave you there, just a couple of examples.

And I encourage you, if you're in the mood,

just pick any of these atoms, any of these elements,

and think about what would happen

if they gained or lost an electron

and what their electron configurations might be.