Question

The correct order of the metallic nature of the following elements is

• A. \(Si>Al>Na>Hg\)
• B. \(Na>Mg>Al>Si\)
• C. \(Al>Mg>Na>Si\)
• D. \(Mg>Na>Al>Si\)

Hint:

Metallic character decreases across a period (left to right) and increases down a group. Elements on the left side of the periodic table are more metallic than those on the right.

Answer 1

The Correct Option is B

Step 1: Understand metallic character and its periodic trends. Metallic character refers to the tendency of an element to lose electrons and form positive ions. It generally:
Decreases from left to right across a period
Increases from top to bottom in a group
Is related to lower ionization energy and electronegativity

Step 2: Analyze the positions of the given elements in the periodic table. Na (Sodium): Group 1, Period 3
Mg (Magnesium): Group 2, Period 3
Al (Aluminum): Group 13, Period 3
Si (Silicon): Group 14, Period 3
All these elements are in the same period (Period 3), so metallic character decreases as we move from left to right.
Step 3: Determine the correct order. Since all elements are in the same period and metallic character decreases from left to right, the correct order of decreasing metallic character is: Na>Mg>Al>Si Final Answer: \[ \boxed{\text{Na>Mg>Al>Si}} \]