Question

Write the difference between ${}_6{}^{12}\mathrm{C}$ and ${}_6{}^{13}\mathrm{C}$. Justify how are they placed in the modern periodic table.

Answer 1

Isotopes:

• Isotopes are the atomic species of an element that have the same atomic numbers but different atomic mass numbers.
• In this, the atoms of an element possess the same number of protons and electrons but differ in the numbers of neutrons and are thus termed the isotopes of that element.
• All isotopes of an element share similar chemical properties since these properties are determined based on the number of protons and not the neutrons.

Isotopes of Carbon:

• Carbon has 3 isotopes- ${}_6{}^{12}\mathrm{C}$ ,${}_6{}^{13}\mathrm{C}$ and ${}_6{}^{14}\mathrm{C}$ among which carbon 12 and carbon 13 are stable and carbon 14 is unstable and radioactive in nature.

Difference between ${}_6{}^{12}\mathrm{C}$ and ${}_6{}^{13}\mathrm{C}$:

${}_6{}^{12}\mathrm{C}$	${}_6{}^{13}\mathrm{C}$
Carbon 12 consists of 6 electrons, 6 protons, and 6 neutrons.	Carbon 13 consists of 6 electrons, 6 protons, and 7 neutrons.
The mass number of carbon 12 is 12.	The mass number of Carbon 13 is 13.
It is mainly abundant in nature.	It is 1.1% abundant in nature.
Carbon 12 forms the building blocks of all biological systems. Also its allotropes graphite, diamond, and charcoal it is widely used in industrial applications	Carbon 13 isotope can be used in Nuclear Magnetic Resonance (NMR) research and diagnosis.

Position in the modern periodic table:

• The element carbon with atomic number 6 and atomic mass number 12 is placed in group 14 and period 2.
• The modern periodic table is arranged based on the atomic number of the elements.
• As isotopes of carbon have the same atomic number and electronic configuration they are not placed in different positions instead they belong to the same slot as that of carbon 12 which is group 14 and period 2.
• Carbon 12 is mentioned in the table and not the other isotopes as this form of carbon is the most stable and abundant form as compared to the others.