Question

The correct order of covalent radii of Si, Ge, Sn is:

• A. Ge \(<\) Si \(<\) Sn
• B. Sn \(<\) Si \(<\) Ge
• C. Si \(<\) Ge \(<\) Sn
• D. Sn \(<\) Ge \(<\) Si

Hint:

Remember, in the same group, the covalent radii increase as you go down the group due to the addition of electron shells.

Answer 1

The Correct Option is C

The trend of covalent radii in group 14 elements shows that as we move down the group, the size of the atoms increases. This is because the number of electron shells increases, leading to a greater atomic radius. - Silicon (Si) is located at the top of the group, and its atomic radius is smaller than that of germanium (Ge) and tin (Sn). - Germanium (Ge) is below silicon and has a larger atomic radius than silicon but smaller than tin (Sn). - Tin (Sn) is at the bottom of the group, and its atomic radius is the largest due to more electron shells. Therefore, the correct order of covalent radii is: \[ \text{Si}<\text{Ge}<\text{Sn} \] Thus, the correct answer is option (3).

Answer 2

Step 1: Understanding Covalent Radii Trend in Group 14 Elements
Covalent radius generally increases down a group in the periodic table due to the addition of electron shells.

Step 2: Elements in Question
- Silicon (Si) is in Period 3
- Germanium (Ge) is in Period 4
- Tin (Sn) is in Period 5

Step 3: Explanation of Trend
As we move down the group from Si to Sn, each element has an additional electron shell compared to the previous one, increasing the size of the atom.
Therefore, the covalent radius increases in the order:
Si < Ge < Sn.

Step 4: Conclusion
The correct order of covalent radii is Si < Ge < Sn.