Definitions
1) Endothermic Reaction: heat is a reactant and is absorbed
2) Exothermic Reaction: heat is a product and is released
3) Lewis Dot Diagram: (electron dot diagram) – a chemical symbol surrounded by one to eight dots representing the valence electrons
4) Kernel: the nucleus of the atom as well as the non valence electrons, represented by the symbol of the element
5) Ions: when atoms have either a positive or negative charge due to the loss or gain of electrons
6) Metallic Bond: results from the attraction of mobile valence electrons for an atoms positively charged kernel
7) Malleability: a property of metals in that they can be hammered into shapes
8) Octet Rule: atoms will gain, lose or share electrons in order to have a complete octet of eight valence electrons (the configuration of a noble gas)
9) Non-Polar Covalent Bond: the equal sharing of electrons by two nonmetals
10) Polar Covalent Bond: the unequal sharing of electrons by two nonmetals (the atom with the higher electronegativity will have the stronger pull and act like the nonmetal)
11) Multiple Covalent Bond: when atoms share more than one pair of electrons
12) Molecule: a term used to describe anything that is covalently bonded
13) Symmetrical Molecules: molecules that have identical parts on all sides of an axis
14) Asymmetrical Molecules: molecules that lack identical parts on all sides of an axis
15) Polyatomic Ions: a covalently bonded group of atoms that have a net electric charge (when bonded to a metallic element also contain ionic bonds)
16) Ionic Bond: a bond formed by the complete transfer of electrons
17) Electronegativity: the ability to attract electrons
18) Intermolecular Forces: forces of attraction between molecules (covalently bonded)
19) Dipoles: polar molecules have positive and negative ends also known as dipoles (two poles)
20) Hydrogen Bond: an intermolecular bond between a hydrogen atom in one molecule and a F, O or N atom in another molecule
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