Naming Compounds
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Created by:
CNikiGlenn on October 10, 2012
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146 terms
Terms | Definitions |
|---|---|
 H | hydrogen + cation |
| Li | lithium + cation |
| Na | sodiumd + cation |
| K | potassium + cation |
| Cs | cesium + cation |
| Be | beryllium +2 cation |
| mg | magnesium +2 cation |
| ca | calcium +2 cation |
| Ba | barium +2 cation |
| Al | aluminum +3 cation |
| Ag | silver + cation |
| Zn | zinc +2 cation |
| H- | hydride -1 anions |
| F | fluoride - anion |
| Cl | chloride- anion |
| Br | bromide - anion |
| I | iodide - anion |
| O | oxide -2 anion |
| S | sulfide -2 anion |
| AlCl3 | aluminum chloride |
| mgI2 | magnesium iodide |
| FeCl3 | iron(III) chloride |
| iron (III) | Fe +3 |
| iron(II) | Fe +2 |
| Copper(II) | Cu +2 |
| Copper (I) | Cu + |
| tin (IV) | Sn +4 |
| tin (II) | Sn +2 |
| lead (IV) | Pb (IV) |
| lead (II) | Pb +2 |
| Mercury (II) | Hg +2 |
| Mercury (I) | Hg2 +2 *Mercury (I) ions always occur bound together in pairs to form Hg2 +2 |
| Rules Type II Ionic Compounds | 1. The cation is always named first and the anion second. 2. Because the cation can assume more than one charge, the charge is specified by a Roman numeral in parentheses. |
| CuCl | copper chloride |
| HgO | mercury (II) oxide |
| Fe2O3 | iron (III) oxide |
| MnO2 | manganese (IV) oxide (4+)+2(-2)=0 |
| PbCl4 | lead (IV) chloride |
| CoBr2 | cobalt(II) bromide |
| Ca +2 | calcium chloride |
| Al2O3 | aluminum oxide |
| CrCl3 | Chromium (III) chloride |
| mono- | 1 |
| di- | 2 |
| tri- | 3 |
| tetra- | 4 |
| penta- | 5 |
| hexa- | 6 |
| hepta- | 7 |
| octa- | 8 |
| Type III Binary Compounds | 1.The first elememt in the formula is named first, and the full element name is used. 2. The second element is named as though it were an anion. 3. Prefixes are used to denote the numbers of atoms present. 4. The prefix mono- is never used for naming the first element. For example, CO is caled carbon monoxide, not monocarbon monoxide. |
| PCl5 | Phosphorus pentachloride |
| P4O6 | tetraphosphorus hexoxide |
| SF6 | Sulfur hexafluoride |
| SO3 | sulfur trioxide |
| SO2 | sulfur dioxide |
| N2O3 | dinitrogen trioxide |
| ammonium nitrate | NH4NO3 |
| Polyatomic ions | assigned special names that you must memorize in order to name the compounds containing them |
| ClO- | hypochlorite |
| ClO2- | chlorite |
| ClO3- | chlorate |
| ClO4- | perchlorate |
| NaOH | sodium hydroxide |
| OH- | hydroxide |
| NH4+ | ammonium |
| NO2- | nitrite |
| NO3- | nitrate |
| SO3-2 | sulfite |
| SO4-2 | sulfate |
| HSO4- | hydrogen sulfate (bisulfate is a widely used common name) |
| OH- | hydroxide |
| CN- | cyanide |
| PO4-3 | phosphate |
| HPO4-2 | hydrogen phosphate |
| H2PO4- | dihydrogen phosphate |
| CO3-2 | carbonate |
| HCO3- | hydrogen carbonate (bicarbonate is a widely used common name) |
| C2H3O2- | acetate |
| MnO4- | permangante |
| Cr2O7-2 | dichromate |
| CrO4-2 | chromate |
| O2-2 | peroxide |
| Na2SO4 | sodium sulfate |
| KH2PO4 | potassium dihydrogen phosphate |
| Fe(NO3)3 | iron (III) nitrate |
| Mn (OH)2 | manganise (II) hydroxide |
| Na2So3 | sodium sulfite |
| NH4ClO3 | ammonium chlorate |
| Na2CO3 | sodium carbonate |
| FeBr3 | iron (III) bromide |
| CsClO4 | cesium perchlorate |
| PCl3 | phosphorus trichloride |
| CuSO4 | copper (II) sulfate |
| HF | hydrofluoric acid |
| HCl | hydrochloric acid |
| HBr | hydrobromic acid |
| HI | hydroiodic acid |
| HCN | hydrocyanic acid |
| H2S | hydrosulfuric acid |
| HNO3 | nitric acid |
| HNO2 | nitrous acid |
| H2SO4 | sulfuric acid |
| H2SO3 | sulfurous acid |
| H3PO4 | phosphoric acid |
| HC2H3O2 | acetic acid |
| chemical reacton | a chemical change |
| chemical equation | chemicals present before the reaction are shown to the left of an arrow and the chemicals formed by the reactionare shown to the right of an arrow |
| reactant | shown left of an arrow |
| balancing a chemical equation | same # of each type of atom on the product side as on the reactant side of the arrow |
| coefficient | smallest integers (whole numbers) used to balanced equations |
| product | shown to right of the arrow |
| arrow | "yields" or "produces" |
| "driving forces" | formation of a solid, formation of water, transfer of electron, formation of a gas |
| Precipitation | one driving force for a chemical reaction is the formation of a solid |
| precipitate | the solid |
| Precipitation reaction | the reaction to a precipitate |
| strong electrolyte | each unit of a substance that dissolves in water produces separated ions |
| soluble solid | the solid "disappears" |
| Insoluble solid and slightly souluble solid | a solid where such a tiny amount dissolves in water that it is undetectable with the naked eye |
| molecular equation | shows the complete formulas of all reactants and products |
| Complete ionic equation | better represents the actual forms of the reactants and products in solutions |
| spectator ions | ions that do not participate directly in a reaction in a solution |
| net ionic equation | only those components that are directly involved in the reaction |
| acid | a substance that produces H+ ions (protons) when it is dissolved in water |
| strong acids | strong electrolytes that produce H+ ions |
| Arrhenius | aqueous solutions that exhibit basic behavior alway contain hydroxide ions |
| base | substance that produces hydroxide ions (OH-) in water |
| strong bases | strong electrolytes that contain OH- |
| strong acids and strong bases (hydroxides) mix | the fundamental chemical change that always occurs is that H+ ions react with OH- ions to form water |
| salt | ionic compound |
| oxidation-reduction reaction | a reaction that involves a transfer of electrons |
| precipation reaction | the formation of a solid when two solutios are mixed |
| double-displacement reaction | we sometimes call this reaction a double-exchange reaction |
| acid-base reactions | an H+ ion that ends up in the product water |
| oxidation-reduction reaction | electron transfer |
| combustion reactions | many chemical reactions that involve oxgen produce energy (heat) so rapidly that a flame result |
| synthesis or (combination) reaction | when a given compound formed from simpler materials |
| decomposition reactins | heating or by the application of an current |
| mole | the number equal to the number of carbon atoms in 12.01 grams of carbon |
| Avogadro's number | techniques for counting atoms very precisely have been used to determine this number to be 6.022* 10^23 |
| molar mass | any substance is the mass (in grams) of 1 mol of the substanc; is obtained by summing the masses of the component atoms |
| formula weight | molar mass for ionic compounds |
| mass percent | multiplying by 100 % |
| empirical formula | simplest formula |
| molecular formula | the one that gives the composition of the molecules that are present |
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