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Unit 3
Electrons and Bonding
Term | Definition |
---|---|
Aufbau Principle | states that 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 | 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. as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to f |
Electron Orbitals | a mathematical function describing the location and wave-like behavior of an electron in an atom. |
Hund's Rule | every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin. |
Ion | is a particle, atom or molecule with a net electrical charge. |
Lewis Dot Structure | are 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 | a type of chemical bonding that arises from the electrostatic attractive force between conduction electrons and positively charged metal ions. |
Molecular Geometry | is the three-dimensional arrangement of the atoms that constitute a molecule. |
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. |
Oxidation Number | describes the degree of oxidation of an atom in a chemical compound. |
Pauli Exclusion Principle | says that no two electrons can have the same set of quantum numbers; that is, no two electrons can be in the same state. |
VSEPR Theory | is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. |