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\nThe 18 Electron Rule for Transition Metal Complexes\n

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\n\nPublisher:\n\nProfessor Dave Explains\n\n\n
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\nOk, so we understand how ligands bond to metals to form transition metal complexes, but how many ligands will fit? Well, remember the octet rule from general chemistry? There is a similar concept that we can apply here, which is called...\nOk, so we understand how ligands bond to metals to form transition metal complexes, but how many ligands will fit? Well, remember the octet rule from general chemistry? There is a similar concept that we can apply here, which is called the 18 electron rule. 18 is bigger than 8 because transition metals have access to d orbitals. Let's see how this rule works now!\n
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Resource Details

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Media Length
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10:14
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Grade
9th - Higher Ed
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Subjects
Science
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Media Type
Instructional Videos
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Source:
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\nProfessor Dave Explains\n\n
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Date
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2022
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Language
English
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Audiences
For Teacher Use
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Fine Print: Educational Use
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Concepts

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transition metals, oxidation state, valence electrons, iron, electrons, carbon, alkyne
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Additional Tags

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18 electron rule, transition metal complex, octet rule, ligands, cyanide ions, lone pair, electron count, cyclopentadienyl anion, iron atom, electrons contributed, negative charge, metal atom, total count, common ligands, count, ligand, total, 18 electrons, simply, tungsten, charge, metal, complex, charges, minus
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