d and f BLOCK ELEMENTS

Which element among the following is NOT typically considered to have a typical metallic structure at normal temperatures?

• Iron
• Chromium
• Titanium
• Mercury

Which of the following best explains why the enthalpies of atomisation for transition metals are generally high?

• Weak interatomic forces in the solid.
• The presence of only s electrons in bonding.
• The involvement of multiple d and s electrons in strong metallic bonds.
• Complete electron pairing which reduces bonding strength.

According to the text, what is the general trend for the melting points of transition metals within a series (excluding anomalies)?

• They decrease steadily from left to right.
• They increase steadily from left to right.
• They remain constant across the series.
• They rise to a maximum near the d⁵ configuration and then decrease.

Which physical property listed is NOT generally associated with the typical metallic nature of transition elements?

• High tensile strength
• Ductility
• Low electrical conductivity
• Malleability

Why do transition metals (excluding Zn, Cd, Hg) generally exhibit high boiling points?

• Due to weak van der Waals forces.
• Due to the presence of large atomic radii.
• Due to strong metallic bonding involving multiple electrons (d and s) in the lattice.
• Due to their complete d electron shells.