d and f BLOCK ELEMENTS

What is a key difference in the electronic configurations of Lanthanoids and Actinoids?

• Lanthanoids fill the 5f orbitals, while actinoids fill the 4f orbitals.
• Lanthanoids primarily fill the 4f orbitals, while actinoids primarily fill the 5f orbitals.
• Lanthanoids fill the 4d orbitals, while actinoids fill the 5d orbitals.
• They have identical electronic configurations.

What is a characteristic property of Zinc (Zn) related to its common oxidation state?

• It commonly exhibits only the +1 oxidation state.
• It commonly exhibits +2 and +3 oxidation states.
• It commonly exhibits only the +2 oxidation state because losing two 4s electrons results in a stable, fully filled 3d10 configuration.
• It exhibits variable oxidation states like most transition metals.

What is the primary reason Scandium (Sc) shows only +3 as its stable oxidation state?

• It gains 1 electron to complete its d-subshell.
• It loses 2 electrons from the 4s orbital.
• It loses its 3 outermost electrons (2 from 4s and 1 from 3d) to achieve the stable, noble gas configuration of Argon.
• It forms covalent bonds exclusively.

In which type of compounds do transition metals commonly exhibit their highest oxidation states?

• Simple chlorides
• Simple sulfides
• Oxoanions
• Binary hydrides

Why do transition metals typically exhibit their highest oxidation states in oxides and fluorides?

• Oxygen and fluorine are large atoms.
• Oxygen and fluorine are highly electropositive elements.
• Oxygen and fluorine are highly electronegative elements that can effectively stabilize high oxidation states.
• They form ionic bonds easily.