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Can you explain slaters rules? Explain abount equation Effective nuclear charge = Nuclear charge – Screening constant? How to use it and exam poain of view.

  1. Can you explain slaters rules?
  2. Explain abount equation        Effective nuclear charge = Nuclear charge – Screening constant?  How to use it and exam poain of view.

Grade:11

2 Answers

Ramreddy IIT Patna
askIITians Faculty 49 Points
9 years ago
In quantum chemistry, Slater's rules provide numerical values for the effective nuclear charge concept. In a many-electron atom, each electron is said to experience less than the actual nuclear charge owing to shielding or screening by the other electrons. For each electron in an atom, Slater's rules provide a value for the screening constant(sigma).
Firstly, the electrons are arranged into a sequence of groups in order of increasing principal quantum number n, and for equal n in order of increasing azimuthal quantum number l, except that s- and p- orbitals are kept together.

[1s] [2s,2p] [3s,3p] [3d] [4s,4p] [4d] [4f] [5s, 5p] [5d] etc.

Each group is given a different shielding constant which depends upon the number and types of electrons in those groups preceding it.

The shielding constant for each group is formed as the sum of the following contributions:

An amount of 0.35 from each other electron within the same group except for the [1s] group, where the other electron contributes only 0.30.
If the group is of the [s p] type, an amount of 0.85 from each electron with principal quantum number n one less than that of the group, and an amount of 1.00 for each electron with principal quantum number two or more less.
If the group is of the [d] or [f], type, an amount of 1.00 for each electron "closer" to the atom than the group. This includes i) electrons with a smaller principal quantum number n and ii) electrons with an equal principal quantum number and a smaller azimuthal quantum number l.
Vineeth
19 Points
9 years ago
If the group is of the [d] or [f], type, an amount of 1.00 for each electron "closer" to the atom than the group. This includes i) electrons with a smaller principal quantum number n and ii) electrons with an equal principal quantum number and a smaller azimuthal quantum number l” an amount of 0.85 from each electron with principal quantum number n one less than that of the group, and an amount of 1.00 for each electron with principal quantum number two or more less..If the group is of the [s p] type, An amount of 0.35 from each other electron within the same group except for the [1s] group, where the other electron contributes only 0.30
Can you explain the darken and underlined statement
 

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