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Lecture 1
Inorganic Chemistry- Study of many elements
Periodic Table is a tabular arrangement of the elements
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1st draft by Mendeleev (1896)
• Predictions of properties of elements e
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gallium before they were discovered
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g
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Use Schrödinger Equation to solve for atoms containing more than one electron
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g
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Same system of quantum numbers as H
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Same angular function as H
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Same radical functions (distance from the nucleus) similar to H
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4
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As with H
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4th known as the spin quantum number (ms) must be ½ or -½
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1s 2s 2p 3s 3p 4s 3d
Hunds First Rule:
Electrons are placed as far apart as possible to minimise repulsion
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Electron Energies in Multi-electron systems
Energies of electrons depend on the principle and angular quantum number
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(probability of an electron being at distance r from the
nucleus)
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2s experiences less nuclear charge because the 1s
electron shields the 2s electron from the nucleus
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Electron Types
1
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These take part in chemistry
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Core Electrons- Low energy electrons in filled shells
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Effect of Shielding and Penetration:
1
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Hence, the electrons experience a nuclear charge less than the actual nuclear charge, called the effective
nuclear charge
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2
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A 2s electron will have more electron density near the nucleus than a 2p electron
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Depends on the principle (n) and angular quantum number (l)
Why is the 2s orbital filled before the 2p orbital?
Penetration seen from RDF graph for 2s and 2p orbitals
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So, 2s electrons penetrate the core electrons causing 2s to have a minor maximum
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Why is the 4s orbital filled before the 3d?
Both 3s and 3p orbitals are filled, addition of an electron in the 4s results in less shielding over the 3d
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