16 July 2020- Surprise Topic No.4

Isotopes

Let's imagine a pair of identical twins. These twins have the same temperament, and since they're identical, it is very hard to tell them apart unless you examine them closely. When it is time for their annual physical, the twins need to step on a weighing scale, and when they do, one weighs slightly more than the other. In terms of chemistry, we can say that these twins are like isotopes of each other.

Atoms and elements are made of protons, neutrons and electrons. The nucleus is made of protons and neutrons, and the electrons surround the nucleus, as shown in the illustration below. The sum of the number of protons and the number of neutrons is equal to the atomic mass.

In a given element, the number of neutrons can be different from each other, while the number of protons is not. These different versions of the same element are called isotopes. Isotopes are atoms with the same number of protons but that have a different number of neutrons. Since the atomic number is equal to the number of protons and the atomic mass is the sum of protons and neutrons, we can also say that isotopes are elements with the same atomic number but different mass numbers.

Let us take a look at an example.

Isotopes of Hydrogen

The three are all isotopes of hydrogen. As you can see, they have the same atomic number, or number of protons, (number at the lower left of the element) but different atomic masses (number at the upper left of the element).

The number of neutrons can be calculated by calculating the difference between the atomic mass and atomic number. We can see that for the isotopes of hydrogen, they have varying number of neutrons. For protium, the number of neutrons is zero; for deuterium, the number of neutrons is one; and for tritium, the number of neutrons is two.

Going back to our comparison with identical twins, we can say that these three isotopes of hydrogen are like identical triplets of each other - they may appear to be identical outside, but they are different inside, and they also have different names.

Isotopes of Carbon

A very popular element, carbon, also has isotopes. There are three isotopes of carbon: carbon-12, carbon-13 and carbon-14. The numbers that are after the carbon refer to the atomic mass.

The most common and abundant isotope of carbon is carbon-12. Looking at the percentages below each carbon isotope, we see that almost 98.9% of the carbon that is found is in the form of carbon-12. The least abundant form of carbon is carbon-14, with an abundance of less than 0.0001%. If we calculate the number of neutrons for each carbon isotope, we can see that they differ from each other. For carbon-12, we have 6 neutrons; for carbon-13, we have 7 neutrons; and for carbon-14, we have 8 neutrons.

You may notice if we look at the atomic masses of elements in the periodic table that they are rarely ever whole numbers, just like for carbon where the atomic mass is 12.011. This is because the atomic mass of carbon is based on the average atomic masses of its isotopes and the abundance of each isotope.