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what is Slater rule ?? Related: Introduction to the Periodic Table - ...
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Slater's Rules. The general principle behind Slater's Rule is that the actual charge felt by an electron is equal to what you'd expect the charge to be from a certain number of protons, but minus a certain amount of charge from other electrons
Slater's Rules:
1) Write the electron configuration for the atom using the following design;
(1s)(2s,2p)(3s,3p) (3d) (4s,4p) (4d) (4f) (5s,5p)
2) Any electrons to the right of the electron of interest contributes no shielding. (Approximately correct statement.)
3) All other electrons in the same group as the electron of interest shield to an extent of 0.35 nuclear charge units
4) If the electron of interest is an s or p electron: All electrons with one less value of the principal quantum number shield to an extent of 0.85 units of nuclear charge. All electrons with two less values of the principal quantum number shield to an extent of 1.00 units.
5) If the electron of interest is an d or f electron: All electrons to the left shield to an extent of 1.00 units of nuclear charge.
6) Sum the shielding amounts from steps 2 through 5 and subtract from the nuclear charge value to obtain the effective nuclear charge.
Examples:
Calculate Z* for a valence electron in fluorine.
(1s2)(2s2,2p5)
Rule 2 does not apply; 0.35 � 6 + 0.85 � 2 = 3.8
Z* = 9 – 3.8 = 5.2 for a valence electron.
Calculate Z* for a 6s electron in Platinum.
(1s 2)(2s 2,2p6)(3s2,3p6) (3d10) (4s2,4p6) (4d10) (4f14) (5s2,5p6) (5d8) (6s2)
Rule 2 does not apply; 0.35 � 1 + 0.85 � 16 + 60 � 1.00 = 73.95
Z* = 78 – 73.95 = 4.15 for a valence electron.
Shielding
The first ionization energy for hydrogen is 1310 kJ�mol–1 while the first ionization energy for lithium is 520 kJ�mol–1. The IE for lithium is lower for two reasons;
1) The average distance from the nucleus for a 2s electron is greater than a 1s electron;
2) The 2s1 electron in lithium is repelled by the inner core electrons, so the valence electron is easily removed.
For reason #2 the inner core electrons shield the valence electron from the nucleus so the outer most electron only experiences an effective nuclear charge. In the case of the lithium the bulk of the 1s electron density lies between the nucleus and the 2s
1 electron. So the valence electron `sees' the sum of the charges or approximately +1. In reality the charge the valence electron experiences is greater than 1 because the radial distribution show their is some probabilty of finding the 2s electron close to the nucleus.
Example:
Ruthenium atom: Ru: Z = 44
(1s2) (2s2 2p6) (3s2 3p6) (3d10) (4s2 4p6) (4d7) (5s1)
S(1s2) = 1 * 0.35 = 0.35
S(2s2 2p6) = 7 * 0.35 + 2 * 0.85 = 4.15
S(3s2 3p6) = 7 * 0.35 + 8 * 0.85 + 2 * 1.00 = 11.25
S(3d10) = 9 * 0.35 + 8 * 1.00 + 8 * 1.00 + 2 * 1.00 = 21.15
S(4s2 4p6) = 7 * 0.35 + 18 * 0.85 + 8 * 1.00 + 2 * 1.00 = 27.75
S(4d7) = 6 * 0.35 + 8 * 1.00 + 18 * 1.00 + 8 * 1.0 + 2 * 1.00 = 38.1
S(5s1) = 15 * 0.85 + 18 * 1.00 + 8 * 1.00 + 2 * 1.00 = 40.75
S(2s2 2p6) = 7 * 0.35 + 2 * 0.85 = 4.15
S(3s2 3p6) = 7 * 0.35 + 8 * 0.85 + 2 * 1.00 = 11.25
S(3d10) = 9 * 0.35 + 8 * 1.00 + 8 * 1.00 + 2 * 1.00 = 21.15
S(4s2 4p6) = 7 * 0.35 + 18 * 0.85 + 8 * 1.00 + 2 * 1.00 = 27.75
S(4d7) = 6 * 0.35 + 8 * 1.00 + 18 * 1.00 + 8 * 1.0 + 2 * 1.00 = 38.1
S(5s1) = 15 * 0.85 + 18 * 1.00 + 8 * 1.00 + 2 * 1.00 = 40.75
Zeff (electronic state) = Z - S(electronic state)
Zeff (1s2) = 44 - 0.35 = 43.7
Zeff(2s2 2p6) = 44 - 4.15 = 39.85
Zeff(3s2 3p6) = 44 - 11.25 = 32.75
Zeff(3d10) = 44 - 21.15 = 22.85
Zeff(4s2 4p6) = 44 - 27.75 = 16.25
Zeff(4d7) = 44 - 38.1 = 5.9
Zeff(5s1) = 44 - 40.75 = 3.25
Zeff(2s2 2p6) = 44 - 4.15 = 39.85
Zeff(3s2 3p6) = 44 - 11.25 = 32.75
Zeff(3d10) = 44 - 21.15 = 22.85
Zeff(4s2 4p6) = 44 - 27.75 = 16.25
Zeff(4d7) = 44 - 38.1 = 5.9
Zeff(5s1) = 44 - 40.75 = 3.25
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what is Slater rule ?? Related: Introduction to the Periodic Table - ...
The Slater's rules, named after John C. Slater, are a set of guidelines used to determine the effective nuclear charge experienced by an electron in a multi-electron atom. These rules help in understanding the electron configuration and predicting the periodic properties of elements.
The effective nuclear charge refers to the net positive charge experienced by an electron in an atom. It is not equal to the total number of protons in the nucleus because the repulsion between electrons reduces this charge. Slater's rules take into account the shielding effect of inner electrons on the outer electrons.
Here are the details of Slater's rules:
1. Screening or Shielding: The electrons in an atom are divided into groups based on their distance from the nucleus. Electrons in inner shells shield the outer electrons from the full nuclear charge. The shielding constant for each electron group is determined using empirical values.
2. Penetration: Electrons in outer shells can penetrate into inner shells, experiencing a greater effective nuclear charge. Electrons in the same group have different penetration abilities, with s-orbitals penetrating the most, followed by p-, d-, and f-orbitals.
3. Effective Nuclear Charge: The effective nuclear charge experienced by an electron in a particular orbital is calculated by subtracting the shielding constant of all closer electron groups from the nuclear charge. The shielding constants for each electron group are determined by Slater's empirical rules.
4. Order of Filling: Electrons fill orbitals in a specific order, following the Aufbau principle. The order is determined by the increasing energy of the orbitals.
By using Slater's rules, one can determine the effective nuclear charge experienced by an electron and predict various properties of elements, such as atomic size, ionization energy, electron affinity, and electronegativity. These properties are influenced by the effective nuclear charge and play a crucial role in understanding the periodic trends in the periodic table.
In summary, Slater's rules provide a framework to estimate the effective nuclear charge experienced by electrons in multi-electron atoms. These rules take into account the shielding effect of inner electrons, penetration of outer electrons into inner shells, and the order of filling orbitals. By utilizing Slater's rules, one can analyze and predict the periodic properties of elements in the periodic table.
The effective nuclear charge refers to the net positive charge experienced by an electron in an atom. It is not equal to the total number of protons in the nucleus because the repulsion between electrons reduces this charge. Slater's rules take into account the shielding effect of inner electrons on the outer electrons.
Here are the details of Slater's rules:
1. Screening or Shielding: The electrons in an atom are divided into groups based on their distance from the nucleus. Electrons in inner shells shield the outer electrons from the full nuclear charge. The shielding constant for each electron group is determined using empirical values.
2. Penetration: Electrons in outer shells can penetrate into inner shells, experiencing a greater effective nuclear charge. Electrons in the same group have different penetration abilities, with s-orbitals penetrating the most, followed by p-, d-, and f-orbitals.
3. Effective Nuclear Charge: The effective nuclear charge experienced by an electron in a particular orbital is calculated by subtracting the shielding constant of all closer electron groups from the nuclear charge. The shielding constants for each electron group are determined by Slater's empirical rules.
4. Order of Filling: Electrons fill orbitals in a specific order, following the Aufbau principle. The order is determined by the increasing energy of the orbitals.
By using Slater's rules, one can determine the effective nuclear charge experienced by an electron and predict various properties of elements, such as atomic size, ionization energy, electron affinity, and electronegativity. These properties are influenced by the effective nuclear charge and play a crucial role in understanding the periodic trends in the periodic table.
In summary, Slater's rules provide a framework to estimate the effective nuclear charge experienced by electrons in multi-electron atoms. These rules take into account the shielding effect of inner electrons, penetration of outer electrons into inner shells, and the order of filling orbitals. By utilizing Slater's rules, one can analyze and predict the periodic properties of elements in the periodic table.
Community Answer
what is Slater rule ?? Related: Introduction to the Periodic Table - ...
Ans.
Slater's Rules. The general principle behind Slater's Rule is that the actual charge felt by an electron is equal to what you'd expect the charge to be from a certain number of protons, but minus a certain amount of charge from other electrons
Slater's Rules:
1) Write the electron configuration for the atom using the following design;
(1s)(2s,2p)(3s,3p) (3d) (4s,4p) (4d) (4f) (5s,5p)
2) Any electrons to the right of the electron of interest contributes no shielding. (Approximately correct statement.)
3) All other electrons in the same group as the electron of interest shield to an extent of 0.35 nuclear charge units
4) If the electron of interest is an s or p electron: All electrons with one less value of the principal quantum number shield to an extent of 0.85 units of nuclear charge. All electrons with two less values of the principal quantum number shield to an extent of 1.00 units.
5) If the electron of interest is an d or f electron: All electrons to the left shield to an extent of 1.00 units of nuclear charge.
6) Sum the shielding amounts from steps 2 through 5 and subtract from the nuclear charge value to obtain the effective nuclear charge.
Shielding
The first ionization energy for hydrogen is 1310 kJ�mol–1 while the first ionization energy for lithium is 520 kJ�mol–1. The IE for lithium is lower for two reasons;
1) The average distance from the nucleus for a 2s electron is greater than a 1s electron;
2) The 2s1 electron in lithium is repelled by the inner core electrons, so the valence electron is easily removed.
For reason #2 the inner core electrons shield the valence electron from the nucleus so the outer most electron only experiences an effective nuclear charge. In the case of the lithium the bulk of the 1s electron density lies between the nucleus and the 2s
1 electron. So the valence electron `sees' the sum of the charges or approximately +1. In reality the charge the valence electron experiences is greater than 1 because the radial distribution show their is some probabilty of finding the 2s electron close to the nucleus.
Example:
Ruthenium atom: Ru: Z = 44
(1s2) (2s2 2p6) (3s2 3p6) (3d10) (4s2 4p6) (4d7) (5s1)
S(1s2) = 1 * 0.35 = 0.35
S(2s2 2p6) = 7 * 0.35 + 2 * 0.85 = 4.15
S(3s2 3p6) = 7 * 0.35 + 8 * 0.85 + 2 * 1.00 = 11.25
S(3d10) = 9 * 0.35 + 8 * 1.00 + 8 * 1.00 + 2 * 1.00 = 21.15
S(4s2 4p6) = 7 * 0.35 + 18 * 0.85 + 8 * 1.00 + 2 * 1.00 = 27.75
S(4d7) = 6 * 0.35 + 8 * 1.00 + 18 * 1.00 + 8 * 1.0 + 2 * 1.00 = 38.1
S(5s1) = 15 * 0.85 + 18 * 1.00 + 8 * 1.00 + 2 * 1.00 = 40.75
S(2s2 2p6) = 7 * 0.35 + 2 * 0.85 = 4.15
S(3s2 3p6) = 7 * 0.35 + 8 * 0.85 + 2 * 1.00 = 11.25
S(3d10) = 9 * 0.35 + 8 * 1.00 + 8 * 1.00 + 2 * 1.00 = 21.15
S(4s2 4p6) = 7 * 0.35 + 18 * 0.85 + 8 * 1.00 + 2 * 1.00 = 27.75
S(4d7) = 6 * 0.35 + 8 * 1.00 + 18 * 1.00 + 8 * 1.0 + 2 * 1.00 = 38.1
S(5s1) = 15 * 0.85 + 18 * 1.00 + 8 * 1.00 + 2 * 1.00 = 40.75
Zeff (electronic state) = Z - S(electronic state)
Zeff (1s2) = 44 - 0.35 = 43.7
Zeff(2s2 2p6) = 44 - 4.15 = 39.85
Zeff(3s2 3p6) = 44 - 11.25 = 32.75
Zeff(3d10) = 44 - 21.15 = 22.85
Zeff(4s2 4p6) = 44 - 27.75 = 16.25
Zeff(4d7) = 44 - 38.1 = 5.9
Zeff(5s1) = 44 - 40.75 = 3.25
Zeff(2s2 2p6) = 44 - 4.15 = 39.85
Zeff(3s2 3p6) = 44 - 11.25 = 32.75
Zeff(3d10) = 44 - 21.15 = 22.85
Zeff(4s2 4p6) = 44 - 27.75 = 16.25
Zeff(4d7) = 44 - 38.1 = 5.9
Zeff(5s1) = 44 - 40.75 = 3.25
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