| Term | Definition |
|---|
| Compound | A pure substance that is composed of two or more elements in a fixed proportion. |
| Molecule | A combination of two or more atoms held together by covalent bonds. |
| n = m/M | Moles = mass/molar mass |
| Law of constant composition | Any sample of a given compound will contain the same elements in the identical mass ratio. |
| Empirical formula | The formula that gives the simplest whole number ratio of the elements in the compound. |
| Molecular formula | The formula that gives the exact number of atoms of each element in the compound and is usually a multiple of the empirical formula. |
| Percent Composition | = Mass of X in formula / Formula weight of compound x 100% |
| Combination Reactions | Reactions in which two or mor reactants form on product. |
| Decomposition Reactions | Reactions in which a compound breaks down into two or more substances. (usually with heat or electrolysis) |
| Single Displacement Reactions | Reactions in which an atom of one compound is replaced by an atom of another element. (Further classified as redox reactions) |
| Double Displacement Reactions | In what is also called metathesis reactions, elements from two different compounds displace each other to form new compounds. |
| Spectator ions | Ions that do not take place in the reaction, but remain in the solution throughout. |
| Net Ionic Equations | Ionic equations that show only the ions involved in the reaction. |
| Limiting Reactants | This is the reactant that is consumed fully in any reaction, thus stopping the reaction from continuing. |
| Excess Reactants | After a limiting reactant is used up, the left over reactants are called... |
| Yield | This characteristic of the reaction is the ammount predicted or obtained when the reaction is carried out. |
| Theoretical Yield | This is the ammount of product predicted from a balanced equation assuming that all of the limiting reactant has been used. |
| Percent Yield | = Actual Yield/Theoretical Yield x 100% |
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