Which of the following transition metals exhibits the highest number of oxidation states?

A. Iron (Fe)

B. Copper (Cu)

C. Manganese (Mn)

D. Zinc (Zn)

What is the primary reason for the formation of coloured compounds in transition metals?

A. Presence of f-orbitals

B. Incomplete d-orbitals

C. Complete s-orbitals

D. Presence of p-orbitals

Which of the following is NOT a property of transition metals?

A. High melting points

B. Formation of complex ions

C. Low electrical conductivity

D. Catalytic activity

Why is Zinc (Zn) not considered a typical transition element?

A. It has a complete d10 configuration

B. It forms coloured compounds

C. It has variable oxidation states

D. It forms complex ions

Which d-block element is commonly used as a catalyst in the Haber process?

A. Copper (Cu)

B. Iron (Fe)

C. Zinc (Zn)

D. Silver (Ag)

a) Explain the significance of variable oxidation states in transition metals. [3]

b) Why is zinc not considered a typical transition metal, despite being in the d-block? [2]

a) Describe the role of d-orbitals in the formation of complex ions. [3]

b) Why do transition metal compounds often appear coloured? [2]

a) How does the presence of d-electrons influence the catalytic activity of transition metals? [3]

b) Briefly explain the industrial significance of transition metals. [2]

a) Describe the relationship between the limit of convergence in atomic emission spectra and the first ionisation energy of an element. [3]

b) How does the nuclear charge influence ionisation energy? [2]

c) Explain the implications of electron shielding on atomic size. [3]

a) What is the significance of trends in successive ionisation energies for an element? [3]

b) How do these trends relate to electron configurations? [3]

c) Deduce the implications of these trends for an element's metallic or non-metallic character. [2]