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Unit 3

TermDefinition
Aufbau 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 in which 2 atoms share some of their valence electrons
Electron Affinity The change in energy of neutral atom
Electron Orbitals Where electrons are most likely found in an atom
Hund's Rule Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied
Ion An atom or molecule with a net electric charge due to the loss or gain of 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 electrostatic attractive force between conduction electrons and positively charged ions
Molecular Energy The energy levels of electrons in atoms, ions, ad molecules
Molecular Geometry The geometry of where atoms are in relation to a central atom
Octect Rule Rule of thumb that reflects the theory that main group elements tend to bond such a way that each atoms has 8 electrons in its valence shell
Oxidation Number A number assigned to an element in a chemical combination which represents the number of lost electrons
Pauli Exclusion Principle No 2 electrons in the same atom can have identical values for all 4 of their quantum numbers
VSEPER 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: jg339431
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