SUMMARY
The effective nuclear charge (Zeff) of an atom is influenced by the loss or gain of electrons. When an atom loses an electron, the shielding effect diminishes, resulting in an increase in Zeff. For example, in neutral helium (He), the Zeff is between 1 and 2, while in the helium ion (He+), the Zeff is exactly 2. This demonstrates that ionization alters the effective nuclear charge experienced by the remaining electrons.
PREREQUISITES
- Understanding of effective nuclear charge (Zeff)
- Familiarity with Slater's rules for calculating Zeff
- Basic knowledge of atomic structure and electron configuration
- Concept of shielding effect in multi-electron atoms
NEXT STEPS
- Study Slater's rules for calculating effective nuclear charge
- Explore the concept of shielding effect in detail
- Investigate the differences in Zeff for various ions
- Examine case studies of Zeff in different elements
USEFUL FOR
Students of chemistry, educators teaching atomic structure, and anyone interested in the principles of effective nuclear charge and ionization effects.