Question

Which of the following is CORRECT with respect to melting point of a transition element?

• A. V > Cr
• B. Cr > Mn
• C. Mn > Fe
• D. Ti > V

Answer 1

The Correct Option is B

We are comparing the melting points of transition elements based on their atomic structures and bonding characteristics. Generally, the melting points of transition elements are influenced by the number of unpaired electrons and the strength of metallic bonds.

Let's analyze the given options:

Option 1: V > Cr 

This is incorrect. Chromium (Cr) has a higher melting point than Vanadium (V), due to the unique electron configuration of Cr, which results in a more stable metallic bonding.

Option 2: Cr > Mn

This is correct. Chromium has a higher melting point than Manganese because Cr has a more stable electronic configuration and stronger bonding.

Option 3: Mn > Fe

This is incorrect. Manganese (Mn) has a lower melting point than Iron (Fe). Iron has a stronger metallic bond compared to Manganese.

Option 4: Ti > V

This is incorrect. Titanium (Ti) has a lower melting point than Vanadium (V), as the metallic bonding in Vanadium is stronger.

Conclusion:

The correct answer is: Option 2: Cr > Mn.

Answer 2

The melting points of transition elements depend on several factors, including the type of bonding and the atomic structure. In general, the transition metals with more unpaired d-electrons tend to have higher melting points due to stronger metallic bonding.

Looking at the transition elements listed:

1. Vanadium (V) has a melting point of 1910°C, while Chromium (Cr) has a higher melting point of 1907°C. So, V does not have a higher melting point than Cr.

2. Chromium (Cr) has a higher melting point compared to Manganese (Mn). This is due to the strong bonding in the body-centered cubic (BCC) structure of chromium, which gives it a high melting point of 1907°C, while manganese has a lower melting point of 1244°C.

Thus, Cr > Mn is the correct option.