(a) Why does the size of the atoms progressively become smaller when we move from sodium (Na) to chlorine (Cl) in the third period of the periodic table?
(b) Helium and neon are unreactive gases. What, if anything, do their atoms have in common?
(a) Why does the size of the atoms progressively become smaller when we move from sodium (Na) to chlorine (Cl) in the third period of the periodic table?
(b) Helium and neon are unreactive gases. What, if anything, do their atoms have in common?
(a) The size of atoms decreases progressively, on moving from sodium (Na) to chlorine (Cl) in the third period because the atomic number of the elements increases. Likewise, the number of electrons and protons in the atoms also increases. As the positive charges on the nucleus increase, the outermost electrons are held more tightly by the nucleus. Therefore, the size of the atom decreases.
(b) The atoms of helium and neon have their valence shells completely filled with electrons. The number of valence electrons is 8. So, they do not show any reactivity.
(a) The size of atoms decreases progressively, on moving from sodium (Na) to chlorine (Cl) in the third period because the atomic number of the elements increases. Likewise, the number of electrons and protons in the atoms also increases. As the positive charges on the nucleus increase, the outermost electrons are held more tightly by the nucleus. Therefore, the size of the atom decreases.
(b) The atoms of helium and neon have their valence shells completely filled with electrons. The number of valence electrons is 8. So, they do not show any reactivity.
