Noble gases, also known as the group 18 elements on the periodic table, have the smallest atomic radius of any element. These elements, which include helium, neon, argon, krypton, xenon, and radon, have unique chemical and physical properties that set them apart from other elements.
One of the main reasons for their small atomic radius is their fully filled valence electron shells. The valence shell is the outermost electron shell of an atom, and it plays a crucial role in determining an atom’s chemical properties. In the case of noble gases, their valence electron shells are completely filled with electrons, giving them a stable and unreactive nature.
This stability is due to the principle of octet rule, which states that atoms will tend to lose, gain or share electrons to achieve a full octet of electrons in their outermost shell. As the noble gases have 8 electrons in their outermost shell, they are stable and do not need to react with other elements to attain a full outer shell.
Additionally, the small atomic radius of noble gases is also due to the presence of a strong shielding effect. The shielding effect refers to the ability of inner electrons to shield the outer electrons from the full effect of the positively charged nucleus. In the case of noble gases, their fully filled valence shells provide an effective shielding effect, which results in a smaller atomic radius.
In conclusion, the small atomic radius of noble gases is a result of their fully filled valence electron shells and the strong shielding effect provided by these electrons. These properties give noble gases their unique and unreactive nature, making them useful in a variety of industrial and medical applications such as lighting, refrigeration, and medical imaging.