9701 · 28.1
General physical and chemical properties of the first row of transition elements, titanium to copper
This lesson explores the defining characteristics of the first-row d-block elements (Titanium to Copper), including their electronic configurations, variable oxidation states, formation of coloured ions, catalytic activity, and trends in physical properties. It establishes the formal definition of a transition element and explains why Scandium and Zinc are excluded.
Need to know
What you need to know
- Scandium (Sc) is in the d-block but is NOT a transition element. Its only stable ion is Sc³⁺, with the configuration [Ar] 3d⁰. The d-subshell is empty.
- Zinc (Zn) is also in the d-block but is NOT a transition element. Its only stable ion is Zn²⁺, with the configuration [Ar] 3d¹⁰. The d-subshell is full.
- Elements from Titanium (Ti) to Copper (Cu) all form at least one stable ion with a partially filled d-subshell (e.g., Ti³⁺ is 3d¹, V²⁺ is 3d³, Cr³⁺ is 3d³, Mn²⁺ is 3d⁵, Fe²⁺ is 3d⁶, Co²⁺ is 3d⁷, Ni²⁺ is 3d⁸, Cu²⁺ is 3d⁹).
Explanation
General physical and chemical properties of the first row of transition elements, titanium to copper
- Scandium (Sc) is in the d-block but is NOT a transition element. Its only stable ion is Sc³⁺, with the configuration [Ar] 3d⁰. The d-subshell is empty.
- Zinc (Zn) is also in the d-block but is NOT a transition element. Its only stable ion is Zn²⁺, with the configuration [Ar] 3d¹⁰. The d-subshell is full.
- Elements from Titanium (Ti) to Copper (Cu) all form at least one stable ion with a partially filled d-subshell (e.g., Ti³⁺ is 3d¹, V²⁺ is 3d³, Cr³⁺ is 3d³, Mn²⁺ is 3d⁵, Fe²⁺ is 3d⁶, Co²⁺ is 3d⁷, Ni²⁺ is 3d⁸, Cu²⁺ is 3d⁹).