Calculate effective nuclear charge for the 4s electron of Chromium using Slater's rule
Calculate effective nuclear charge for the 4s electron of Chromium using Slater's rule
Ramzanraaz 29 , 7 Years ago
Grade 12th pass
Inorganic Chemistry> Calculate effective nuclear charge for th...
1 Answers
Arun
The formula to be used is:
Z* = Z - S
where:
Z* = effective nuclear charge
Z = atomic number of Cr = 24
S = shielding
Let us first calculate S using Slater's rule.
*Write the electronic configuration as follows: (1s)^2 (2s 2p)^8 (3s 3p)^8 (3d)^5 (4s)^1
*Electrons in an "s" or "p" orbit in the same shell as the electron for which you're solving contribute 0.35, electrons in an "s" or "p" orbital in the shell one energy level lower contribute 0.85, and electrons in an "s" or "p" orbital in shells two energy levels and lower contribute 1.
Therefore, the (4s)^1 do not contribute since we are focusing on the 3d orbital. Therefore,
S = (5 x 0.35) + (8 x 0.85) + (10 x 1) = 18.55
Thus,
Z* Z - S = 24 - 18.55 = 5.45
* Electrons in a "d" or "f" orbital in the same shell as the electron for which you're calculating contribute 0.35, and electrons in an "d" or "f" orbital in all lower energy levels contribute 1. Electrons in shells higher than the electron for which you're solving do not contribute to shielding.
Therefore, the (4s)^1 do not contribute since we are focusing on the 3d orbital. Therefore,
S = (4 x 0.35) + (18 x 1) = 19.4
Thus,
Z* = 24 - 19.4 = 4.6
Z* = Z - S
where:
Z* = effective nuclear charge
Z = atomic number of Cr = 24
S = shielding
Let us first calculate S using Slater's rule.
*Write the electronic configuration as follows: (1s)^2 (2s 2p)^8 (3s 3p)^8 (3d)^5 (4s)^1
*Electrons in an "s" or "p" orbit in the same shell as the electron for which you're solving contribute 0.35, electrons in an "s" or "p" orbital in the shell one energy level lower contribute 0.85, and electrons in an "s" or "p" orbital in shells two energy levels and lower contribute 1.
Therefore, the (4s)^1 do not contribute since we are focusing on the 3d orbital. Therefore,
S = (5 x 0.35) + (8 x 0.85) + (10 x 1) = 18.55
Thus,
Z* Z - S = 24 - 18.55 = 5.45
* Electrons in a "d" or "f" orbital in the same shell as the electron for which you're calculating contribute 0.35, and electrons in an "d" or "f" orbital in all lower energy levels contribute 1. Electrons in shells higher than the electron for which you're solving do not contribute to shielding.
Therefore, the (4s)^1 do not contribute since we are focusing on the 3d orbital. Therefore,
S = (4 x 0.35) + (18 x 1) = 19.4
Thus,
Z* = 24 - 19.4 = 4.6
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