d and f BLOCK ELEMENTS

Why are the highest oxidation states of transition metals typically found in oxides and fluorides?

• Oxygen and fluorine are large atoms.
• Oxygen and fluorine are metals.
• Oxygen and fluorine are highly electronegative and can stabilize the high positive charge on the metal.
• They form weak bonds.

What is a consequence of the similar atomic radii of second and third-row transition elements (like Zr/Hf, Nb/Ta)?

• It increases their reactivity.
• It makes their compounds more ionic.
• It makes the separation of these elements more difficult.
• It decreases their melting points.

Why does the stability of the +2 oxidation state generally decrease from left to right across the first transition series?

• Atomic size increases.
• The number of d-electrons decreases.
• The sum of the first and second ionization energies generally increases across the series.
• Electronegativity decreases.

Which of the following gaseous ions, Mn3+, Cr3+, V3+, or Ti3+, is expected to be the most stable in aqueous solution based on electronic configuration?

• Mn3+
• Cr3+
• V3+
• Ti3+

How many unpaired electrons are present in a gaseous Ti3+ ion?

• 0
• 1
• 2
• 3