d and f BLOCK ELEMENTS

What is the electronic configuration of the Zn²⁺ ion?

• [Ar] 3d⁸
• [Ar] 3d⁹
• [Ar] 3d¹⁰
• [Ar] 3d¹⁰ 4s²

What is the electronic configuration of the Cu⁺ ion?

• [Ar] 3d⁹
• [Ar] 3d¹⁰
• [Ar] 3d¹⁰ 4s¹
• [Ar] 3d⁸ 4s²

What is the electronic configuration of the Fe²⁺ ion?

• [Ar] 3d⁶
• [Ar] 3d⁶ 4s²
• [Ar] 3d⁵ 4s¹
• [Ar] 3d⁴ 4s²

Why do later transition metals (like Cu, Zn) tend to have fewer common oxidation states compared to early ones (Sc, Ti, V)?

• Because they are less reactive
• Because their d-orbitals are more filled, making it harder to remove d-electrons or less favorable energetically
• Because they have higher atomic numbers
• Because they are located on the right side of the periodic table

What is the relationship between the number of d-electrons and the maximum oxidation state for early transition metals?

• Maximum oxidation state equals the number of d-electrons
• Maximum oxidation state often equals the number of valence electrons (d + s electrons)
• Maximum oxidation state is always +2
• Maximum oxidation state equals the atomic number