Ch.8 Atomic Structure

First of all,  before we start the chapter, better do some REVIEW!

There is 3 different type of Subatomic Particles in an element

Proton: Large with positive chargeElectron: Small with negative chargeNeutron: Large with no charge

Moreover:

"# of Atomic number = # of Proton = # of Electron"

"# of Neutron =  Atomic mass - Atomic number/ Proton/ Electron"

Let's do some excerises:

Carbon:

Atomic number : 6  = Proton : 6 = Electron : 6  Atomic Mass: 12

Neutron: 12 - 6 = "6"

Rutherium:

Atomic number: 44 = Proton: 44 = Electron: 44 Atomic Mass: 101

Neutron: 101 - 44 = "57"

Bromine:

Atomic nimber: 18 = Proton: 18 = Electron: 18 Atomic Mass: 80

Neutron: 80 - 18 = "62"

Then now we can move over to Isotope,
Isotope is an atomic specie that has the same atomic number with different atomic mass.

let use Carbon as an example:

It has shown that Carbon has different Atomic mass as 12, 13, 14

So that we can indicate them as Carbon - 13, Carbon - 14

Why dont we take a look this video to see how's isotope practice works?