Question

The correct increasing order of metallic character of the elements Si, Be, Mg, Na and P is

• A. P $<$ Si $<$ Be $<$ Mg $<$ Na
• B. Si $<$ P $<$ Be $<$ Mg $<$ Na
• C. Be $<$ P $<$ Si $<$ Na $<$ Mg
• D. Na $<$ Mg $<$ Be $<$ Si $<$ P

Hint:

The "bottom-left" corner of the periodic table is the most metallic. Sodium (Na) is the furthest left, making it the most metallic in this set. Phosphorus (P) is the furthest right, making it the least.

Answer 1

The Correct Option is A

Step 1: Understanding the Concept:
Metallic character is the ability of an atom to lose electrons.
- It increases down a group (due to increased radius).
- It decreases across a period from left to right (due to increased effective nuclear charge).
Step 2: Key Formula or Approach:
Identify the position of elements in the periodic table:
Group 1: Na (Period 3)
Group 2: Be (Period 2), Mg (Period 3)
Group 14: Si (Period 3)
Group 15: P (Period 3)
Step 3: Detailed Explanation:
1. Period 3 elements: Na (Metal) \(>\) Mg (Metal) \(>\) Si (Metalloid) \(>\) P (Non-metal). Order of metallic character: Na \(>\) Mg \(>\) Si \(>P \).
2. Group 2 elements: Be is above Mg. So, Mg is more metallic than Be.
3. Comparing Be and Si: Be is in group 2 and Si is in group 14. Be is more metallic than Si.
Combining these: P (least metallic) \(<\) Si \(<\) Be \(<\) Mg \(<\) Na (most metallic).
Step 4: Final Answer:
The order is P \(<\) Si \(<\) Be \(<\) Mg \(<\) Na.