Understanding Shielding and Slater's Rule in Chemistry

Explore the concept of shielding and Slater's rule in chemistry, which explains how electrons in different energy levels affect the effective nuclear charge experienced by valence electrons. Learn how to estimate shielding extent using Slater's rules and calculate the effective nuclear charge for elements like Nitrogen and Copper.

• Chemistry
• Shielding
• Slaters Rule
• Effective Nuclear Charge
• Electron Configuration

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1. UNIT 2 Shielding and Slater's Rule By Hemanta Deka

2. Average radius of 2s orbital is greater than 1s. 2s electrons are repelled by 1s electrons.

3. Zeff (Effective Nuclear Charge)

4. Estimate the extent of shielding (): Slater s Rules Step 1- Write the electron configuration of the atom in the following order: (1s) (2s, 2p) (3s, 3p) (3d) (4s, 4p) (4d) (4f) (5s, 5p) ., etc Step 2- Identify the electron of interest and ignore all electrons in higher (higher energy levels) groups as the electrons in higher energy levels will not contribute to shielding of lower energy group electrons. Step 3- Slater's Rules are classified as follows A) Shielding experienced by an s and p electrons. All the electrons within same group shield 0.35. All the electrons within the n-1 group shield 0.85 All the electrons within the n-2 or lower groups shield 1.00 B) Shielding experienced by nd and nf valence electrons All the electrons within same group shield 0.35 All the electrons within the lower groups shield 1.00 Shielding constant can be calculated Zeff = Z-

5. Numerical Calculate the Zeff on valance electron of Nitrogen. Atomic number is 7. Electronic configuration-1s2,2s2, 2p3 S = (2 X 0.85) + (4 X 0.35) S= 3.10 Zeff= Z- Z= 7.0 - 3.1= 3.9 Calculate the Zeff on valance electron of Copper. Zeff= Z- = = = = Cu - (1s)2 (2s, 2p)8 (3s, 3p)8 (3d)10 4s1 Thus, = (n 1)s2p6 + (n 1)d10 + (n 2)s2p6 + (n 3)s2 8 0.85 1 10 8 1 2 1