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BJ Chem Ch 8 Vocab
BJ Chem Ch 8 Vocabulary Terms and Reaction Types
| Question | Answer |
|---|---|
| Represents the number of electrons that an atom in a compound must gain or lose to return to its netral state. | oxidation number |
| Covalently bonded groups of atoms that carry a charge. | polyatomic ion |
| IUPAC systematic way of naming compounds following rules | nomenclature |
| Covalent compounds made up of two (binary) elements. | binary covalent compound |
| Use of Greek prefixes to indicate the number of each of the atoms in a binary covalent compound. | Greek prefix system |
| Anions which contain oxygen and one other anion (e.g., ClO3- chlorate) | oxyanion |
| A compound made up of a cation and an anion where either or both is a polyatomic ion. | polyatomic ionic compound |
| Newer system of naming compounds containing metals with more than one oxidation state (e.g., iron II or iron III) | Stock system |
| Used for the stock system to indicate the oxidation state of the metal. | Roman numeral system |
| Compounds that hold a characteristic amount of water in their crystalline structure. | hydrate |
| Compounds without any water in their crystalline structure. | anhydrous |
| Acids containing hydrogen and one other element. | binary acid |
| Expressions which contain information on a reaction including reactants, products, etc. | chemical equation |
| Communicates all the substances involved in a chemical reaction but no information as to amounts. | word equation |
| Substances present before a reaction | reactant |
| Substances present after a reaction | product |
| Chemical equations that follow the law of mass conservation. | balanced chemical equation |
| Reactions which can occur forward or backward as indicated by a double arrow or a single arrow with two arrow heads. | reversible reaction |
| When a solid falls out of a solution it is called a ___________________. | precipitate |
| A substance that changes the rate of the reaction but does not undergo permanent changes themselves. | catalyst |
| Combine two or more substances: A + B --> C | synthesis reaction |
| Breaks down a substance into two or more substances: AB --> A + B | decomposition reaction |
| A reactive element replaces a less reactive element. AB + C --> AC + B | single replacement reaction |
| Two partners switch partners: AB + CD --> AD + BC | double replacement reaction |
| Ions which occur in both the reactants and products | spectator ion |
| The ionic equation minus spectator ions. It only shows the ions that react to form compound(s). | net ionic equation |
| Acid which has three elements: hydrogen, oxygen, and another nonmetal. | ternary acid |
| An equation which shows all the ions of both the reactants and products, including the spectator ions. | ionic equation |
| List of elements in order of reactivity | activity series |
| Li, K, Ba, SR, Ca, and Na are (more/less) reactive than Co, Ni, SN, and Pb | more |
| I2 is (more/less) than Cl2 | less |
| Alkali metals always have a ____ oxidation number. | +1 |
| Alkaline-earth metals always have a ____ oxidation number | +2 |
| Hydrogen usually has a ___ oxidation number when bonded to a nonmetal and a ___ oxidation number when bonded to a metal. | +1, -1 |
| Oxygen always has an oxidation number of -2 unless bonded to ________________ and in the peroxide ion. | flourine |
| Halogens generally have an oxidation number of _____ when bonded to metals. | -1 |
| The halogen which always has an oxidation number of -1 is ____________ | flourine |
| free atoms have an oxidation number of ____ | 0 |
| ions have an oxidation number equal to their ______ | charge |
| The sum of all oxidation numbers in compounds must equal ____ | zero |
| Reaction Type: Oxygen can be driven out of metal oxides and chlorates | decomposition |
| Reaction Type: Water is electrolyzed | decomposition |
| Reaction Type: Metal hydroxides release gaseous water when heated | decomposition |
| Reaction Type: Metal carbonates release carbon dioxide when heated | decomposition |
| Reaction Type: Some acids release carbon dioxide and water when heated | decomposition |
| Reaction Type: hydrates release heir water molecules when heated sufficiently | decomposition |
| Reaction Type: Atoms of active metals can replace less active ions from solutions and compounds | single replacement (cationic) |
| Reaction Type: Reactive halogens can replace less reactive halogens that are in solution | single replacement (anionic) |
| Reaction Type: Metals and nonmetals other than oxygen form compounds called salts. | synthesis |
| Reaction Type: Metals combine with oxygen to form metallic oxides | synthesis |
| Reaction Type: Nonmetals react with oxygen to form oxides | synthesis |
| Reaction Type: water and metal oxides form metal hydroxides | synthesis |
| water and nonmetal oxides combine to form oxyacids | synthesis |
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MArCHChemBJ
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