Question

The correct order of metallic character is:

• A. Be > Ca > K
• B. Ca > K > Be
• C. K > Ca > Be
• D. K > Be > Ca

Answer 1

The Correct Option is C

To solve the question regarding the order of metallic character among the elements Be, Ca, and K, we need to understand the concept of metallic character. Metallic character refers to how readily an atom can lose electrons to form positive ions (cations). This characteristic increases as you move down a group in the periodic table and decreases as you move from left to right across a period.

The elements given are Beryllium (Be), Calcium (Ca), and Potassium (K). Let's analyze each:

1. Beryllium (Be): It is located in Group 2 and Period 2 of the periodic table. Beryllium has a small atomic size and holds its electrons tightly, thus having a lower metallic character.
2. Calcium (Ca): Calcium is also in Group 2, but in Period 4. As we move down the group from Beryllium to Calcium, the atomic size increases, leading to an increase in metallic character.
3. Potassium (K): Potassium is located in Group 1 and Period 4, which is to the left of Calcium in the same period. Group 1 elements have a greater metallic character than Group 2 elements in the same period because they can lose electrons more easily.

Therefore, comparing these elements based on their position in the periodic table and understanding that metallic character decreases across a period and increases down a group, the correct order of metallic character is:

K > Ca > Be

This is because Potassium, being a Group 1 element, has a higher tendency to lose its outer electron easily compared to Calcium and Beryllium. Hence, the correct answer is the option: K > Ca > Be.