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Unit 3

Electrons and bonding

TermDefinition
Aufban Principle in the ground state of an atom or ion, electrons fill subshells of the lowest available energy, then they fill subshells of higher energy
Covalent Bond a chemical bond that involves the sharing of electron pairs between atoms.
Electron Affinity defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion.
Electron orbitals a mathematical function describing the location and wave-like behavior of an electron in an atom.
Hund's Rule A rule based on observation of atomic spectra.
Ion an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.
Lewis dot structure diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.
Metallic Bond chemical bonding that arises from the electrostatic attractive force between conduction electrons and positively charged metal ions.
Molecular Geometry three-dimensional arrangement of the atoms that constitute a molecule.
Octet Rule 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
Oxidation number a number assigned to an element in chemical combination which represents the number of electrons lost (or gained, if the number is negative), by an atom of that element in the compound.
Pauliexclusion Principle the assertion that no two fermions can have the same quantum number.
VSEPR Theory a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms
Created by: William Currie
 

 



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