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2. Electron counting - Wikipedia

   en.wikipedia.org/wiki/Electron_counting

   In chemistry, electron counting is a formalism for assigning a number of valence electrons to individual atoms in a molecule. It is used for classifying compounds and for explaining or predicting their electronic structure and bonding . [ 1 ]

3. Polyhedral skeletal electron pair theory - Wikipedia

   en.wikipedia.org/wiki/Polyhedral_skeletal...

   Electron count: 6 × Os + 18 × CO – 60 (for 6 osmium atoms) = 6 × 8 + 18 × 2 – 60 = 24 Since n = 6, 4n = 24, so the cluster is capped closo. Starting from a trigonal bipyramid, a face is capped. The carbonyls have been omitted for clarity. B 5 H 4− 5, hydrogen atoms omitted. Example: [11] B 5 H 4− 5

4. Electron configuration - Wikipedia

   en.wikipedia.org/wiki/Electron_configuration

   The various anomalies describe the free atoms and do not necessarily predict chemical behavior. Thus for example neodymium typically forms the +3 oxidation state, despite its configuration [Xe] 4f 4 5d 0 6s 2 that if interpreted naïvely would suggest a more stable +2 oxidation state corresponding to losing only the 6s electrons.

5. Periodic table (electron configurations) - Wikipedia

   en.wikipedia.org/wiki/Periodic_table_(electron...

   Note that these electron configurations are given for neutral atoms in the gas phase, which are not the same as the electron configurations for the same atoms in chemical environments. In many cases, multiple configurations are within a small range of energies and the small irregularities that arise in the d- and f-blocks are quite irrelevant ...

6. IUPAC numerical multiplier - Wikipedia

   en.wikipedia.org/wiki/IUPAC_numerical_multiplier

   The IUPAC numerical multiplier is a system of prefixes used in chemistry to indicate the number of atoms or groups in a molecule.

7. Octet rule - Wikipedia

   en.wikipedia.org/wiki/Octet_rule

   The bonding in carbon dioxide (CO 2): all atoms are surrounded by 8 electrons, fulfilling the octet rule.. The octet rule is a chemical rule of thumb that reflects the theory that main-group elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas.