Isotopes are really interesting!

They are different versions of the same element.

Each isotope has the same number of protons, but they have different numbers of neutrons.

This is important because it changes their atomic mass!

Let’s take a look at carbon as an example:

• Carbon-12 has 6 protons and 6 neutrons (6 + 6 = 12).
• Carbon-14 has 6 protons and 8 neutrons (6 + 8 = 14).

Even though both are carbon, their atomic masses are different because they have different numbers of neutrons.

Now, how does this connect to an element's atomic mass?

• Atomic Mass Calculation: The atomic mass you see on the periodic table is the average of all the isotopes that happen naturally.

This means the atomic mass is affected by how common each isotope is.

• Example Calculation: For carbon, about 98.9% is carbon-12, and only about 1.1% is carbon-14. So, the average atomic mass is closer to 12.

This cool connection between isotopes and atomic mass shows how complex and beautiful the elements we study can be! Isn’t that amazing?