d and f BLOCK ELEMENTS

Why is the E°(Cr3+/Cr2+) value relatively low, making Cr2+ a good reducing agent?

• Cr2+ is larger than Cr3+
• Cr3+ is more hydrated than Cr2+
• Cr3+ (d3) has a more stable electronic configuration than Cr2+ (d4)
• Cr2+ has a higher charge density

What is the typical geometry of a transition metal complex with a coordination number of 6?

• Tetrahedral
• Square planar
• Trigonal bipyramidal
• Octahedral

Which of the following is a characteristic feature of transition metals that allows them to exhibit variable oxidation states?

• They have low ionisation enthalpies
• They have high electronegativity
• They are all solids at room temperature
• The availability of electrons in both (n-1)d and ns orbitals for bonding

Why do transition metals readily form complex compounds?

• They have high melting points
• They are metals
• They have low electronegativity
• They have partially filled d orbitals that can accept electron pairs from ligands

What is the primary reason transition metal compounds often exhibit colours?

• They contain unpaired electrons
• They are ionic compounds
• They have high melting points
• d-d electronic transitions absorbing specific wavelengths of visible light