Ionic, Covalent, and Metallic Bonds

Chemistry

Periodic table, trends, and bonding

Groups of the Periodic Table
Valence Electrons
Periodic Table Trends: Ionization Energy
Other Periodic Table Trends
Ionic, Covalent, and Metallic Bonds

Ionic, Covalent, and Metallic Bonds Introduction to ionic, covalent, polar covalent and metallic bonds.

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Ionic, Covalent, and Metallic Bonds

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Everything we've been dealing with so far has just been with the individual atoms.
But atoms bond or another way of saying is, they stick together.
'Cause if atoms didn't stick together then we'd all be, essentially just a collection of atoms
and this video wouldn't be being produced.
So atoms stick together and the form molecules
you take a bunch of atoms together and those stick togeher
and they'll form molecules,
and then obviously molecules will start building up
and you get other structures, then if we started talking about
Organic Chemistry you'de have a bunch of atoms
a lot of Carbons and Hydrogens and other things fitting together
and they'd be forming proteins and then proteins will fit together to form
organic structures and if you fit enough of those then you'll get
someone recording a YouTube video.
So this is where it all starts, atoms bond...
or they stick together and the purpose of this video
is kinda, think about the different types of ways that an atom an stick to another atom.
So the first and kind of the most powerful ways,
or I think of it as the most powerful ways
if you take and atom that really wants to give an electron, so really wants to give
wants to give
and then you have another atom that really wants to take and electron
We've talked about this before
An atom that wants to give an electron wants to give it because
it's trying to get to kind of a stable configuration in it's outer shell
everyone wants to look like a noble gas, we're all envious of the noble gases
Cause the noble gases have eight electrons in the outer shell
so who wants to give?
If you look at the periodic table, the people who want to give really badly
We've talked about this a bit
Are the alkali metals
These guys just really wanna off-load an electron
And there are other people who want to give 'em, but let's take the extreme example
So, these guys really want to offload an electron and who wants to take an electron?
Well, the halogens we've talked about it.
These guys love taking electrons.
They're not the only ones but they are some of the most electro...they have a very high electronegativity
They really wanna take electrons.
So if you put these around each other what happens?
Let's say, I don't know, let me make a sodium and chlorine.
Sodium and let's say we wanna flavor some of our food, sodium so you have some sodium and you have some
chlorine. So sodium, let me draw its valence shell.
Sodium's valence shell looks like this
its got 1 electron sitting their it would like to get ride of,
and then chlorine looks like this, Chlorine, its got 7 valence electrons.
1, 2, 4, 5, 6 ,7
so what happens is this guy wants to escape, this little blue electron wants to escape the sodium.
And essentially will move to the chlorine.
And obviously its not like a 1 for 1.

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At 5:31, how is the moon large enough to block the sun? Isn't the sun way larger?

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When naming a variable, it is okay to use most letters, but some are reserved, like 'e', which represents the value 2.7831...

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At 2:33, Sal says "double bonds" but should say "single bonds."

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