3.3Transition metal

Transition elements are defined as

• d block elements from Sc to Zn
• d block elements with electrons in d orbital
• d block elements with 3d orbitals
• d blocks elements with partially filled d orbitals

Electron configuration for Cr is 4s¹3d⁵ and NOT 4s²3d⁴. Why?

• Half filled 3d orbital is most stable
• Fully filled orbital is more stable
• 4s¹ is more stable than 4s²
• 3d⁵ is more stable than 3d⁴

Electron configuration for Cu is 4s¹3d¹⁰ and NOT 4s²3d⁹. Why?

• Half filled 3d orbital is most stable
• Fully filled 3d orbital is more stable
• Partially filled 3d orbital is more stable
• 4s¹ is more stable than 4s²

Sc and Zn are not transition elements. Why?

• 3d orbitals are empty
• 3d orbital are fully filled
• 3d orbitals are partially filled
• 3d orbitals are not partially filled

Which of the following is NOT a chemical property of transition metal?

• Formation of complex ion
• Variable oxidation states
• Different shapes
• Formation of coloured complexes

Formation of colour complexes is due to the following except

• Nature of transition element
• Oxidation states
• Different ligands
• 3d orbitals

Transition metal have variable oxidation states due to

• ability to lose electron from 3d and 4s
• ability to lose electrons from 4s
• ability to form complex ions
• ability to react with ligands

Complex metal ions shown in diagram below is made up of

• ligands
• transition metals
• different ligands
• ligands and transition metal

Which of the following is FALSE about complex ion shown in diagram below?

• Overall charge of 2-
• CI^- ion as ligands
• Cu²⁺ as transition metal ion
• Covalent bonding between Cu²⁺ and ligands

State the charge on the metal ion complex [Cu(Cl₂)]^- shown in diagram below.

• -1
• +1
• -2
• +2