What are Isotopes? | Properties of Matter | Chemistry | FuseSchool

What are Isotopes? | Properties of Matter | Chemistry | FuseSchool

What are Isotopes? Find out in this video!

In a previous video we learnt about Isotopes. Here are a few more examples:

There are two isotopic forms of Chlorine: Chlorine 35 and Chlorine 37. Remember isotopes have the SAME number of protons, but a different number of neutrons. So, how many neutrons are in each of these isotopic forms of Chlorine?

Remember: Mass Number = Number of Protons + Number of Neutrons, and the number of protons for each isotope forms of elements is the same, so we can rearrange this formula to calculate the number of neutrons in each form: Neutrons = Mass Number - Protons

When we look at Chlorine on the periodic table, it has an atomic number of 17. Therefore it has 17 protons. Chlorine-35 has a mass of 35. Neutrons = Mass Number - Protons = 35 -17 = 18
18 neutrons. Chlorine-37 has a mass of 37. Neutrons = Mass Number - Protons = 37 -17 = 20. 20 neutrons. Chlorine-35 has 18 neutrons and Chlorine 37 has 20 neutrons.

Another example of an isotope is Lithium. Lithium has two stable isotopic forms.

The atomic number of Lithium is 3, therefore it has 3 protons.

The isotopes of Lithium have 3 neutrons and 4 neutrons respectively. How do we calculate each of the isotopes mass number? Remember, Mass Number = Number of Protons + Number of Neutrons. So for one isotopic form the mass number would be: 3 + 3 = 6. So, we would have Li-6. And for the other form, the mass number would be 3 + 4 = 7. So we would have Li- 7.

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