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Unit 4: Bonding
Chemical Bonding
Term | Definition |
---|---|
Cation | A positively charged ion |
Anion | A negatively charged ion |
ionic bond | Formed when one or more electrons are transferred from one atom to another |
covalent bond | A chemical bond that involves sharing a pair of electrons between atoms in a molecule |
ion | A charged atom |
octet rule | States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons |
polyatomic ion | a tightly bound group of atoms (covalently bonded) that behaves as a unit and has a positive or negative charge |
metallic bond | a bond formed by the attraction between positively charged metal ions and the electrons around them |
double covalent bond | a bond in which two atoms share two pairs of electrons |
triple covalent bond | a bond formed by sharing three pairs of electrons |
hydrogen bond | Attraction between a slightly positive hydrogen atom and a slightly negative atom. Strongest IMF. |
dipole-dipole interactions | Type of intermolecular force in which opposite poles of neighboring dipole molecules are drawn together. (+ and - attract) |
Lewis Dot Diagram | A method for representing an atom's valence electrons using dots around the element symbol. |
London dispersion forces | An IMF where the closer together the molecules are the stronger the forces of attraction. Larger mass also means stronger force of attraction. |
polar covalent bond | unequal sharing of electrons between two nuclei (no symmetry) |
nonpolar covalent bond | equal sharing of two electrons between two nuclei (symmetrical) |
multiple covalent bonds | a double or triple covalent bond - one pair of electrons for each bond |
chemical bond | the force that holds two atoms together |
Electronegativity | A measure of the ability of an atom in a chemical compound to attract electrons |