SUMMARY
Nickel (Ni) predominantly forms NiO with an oxidation state of +2, unlike other transition metals that exhibit a broader range of oxidation states. This behavior is similar to that of zinc (Zn) and copper (Cu), which are located adjacent to nickel in the periodic table. The underlying reason is the poor shielding effect of d-electrons from the nuclear charge, leading to an increase in effective nuclear charge as the number of d-electrons rises. Consequently, the energy of d-electrons decreases relative to valence s-electrons, limiting their participation in bonding as one moves across the period.
PREREQUISITES
- Understanding of transition metal chemistry
- Familiarity with oxidation states and their implications
- Knowledge of d-electron configurations
- Basic grasp of Slater's rules for effective nuclear charge
NEXT STEPS
- Research the oxidation states of transition metals in various compounds
- Study Slater's rules in detail to understand effective nuclear charge
- Explore the bonding characteristics of d-block elements
- Investigate the similarities and differences between nickel, zinc, and copper in terms of oxidation states
USEFUL FOR
Chemistry students, educators, and professionals interested in transition metal behavior and oxidation state variations.