Question

Arrange the elements \(\mathrm{Na}, \mathrm{Si}\), and \(\mathrm{S}\) in the order of (a) decreasing atomic radius. (b) increasing first ionization energy. (c) decreasing electronegativity

Short answer

Question: Arrange the elements Sodium (Na), Silicon (Si), and Sulfur (S) in order of (a) decreasing atomic radius, (b) increasing first ionization energy, and (c) decreasing electronegativity. Answer: (a) Na > Si > S, (b) Na < Si < S, (c) S > Si > Na

Step-by-step solution

Identify the positions of the elements in the periodic table

Locate the positions of Sodium (Na), Silicon (Si), and Sulfur (S) in the periodic table. Na is in Group 1 (Alkali Metals) and Period 3; Si is in Group 14 and Period 3; S is in Group 16 and Period 3.

Arrange the elements based on decreasing atomic radius

As atomic radius decreases when moving from left to right across a period, the decreasing order of atomic radii will be: Na > Si > S

Arrange the elements based on increasing first ionization energy

Since ionization energy generally increases as we move left to right across a period, the increasing order of ionization energies will be: Na < Si < S

Arrange the elements based on decreasing electronegativity

Following the similar trend as ionization energy, electronegativity increases as we move left to right across a period, so the order in decreasing electronegativity will be: S > Si > Na To summarize the answers: (a) Decreasing atomic radius: Na > Si > S (b) Increasing first ionization energy: Na < Si < S (c) Decreasing electronegativity: S > Si > Na