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Unit 3:A/B Review
Terms for Chemistry.
| Term | Definition |
|---|---|
| Evidence of a Chemical Reaction | Temperature Change (Hot or Cold); Creates a gas; Bubbles; Smell; Color change (Conditional) |
| Reactants | Substances you start with |
| Products | New substances created |
| Solid | (s) One of the states of matter, solidified |
| Liquid | (l) One of the states of matter, liquefied |
| Gas | (g) One of the states of matter, evaporated |
| Aqueous | (aq) Elements in water (H20) |
| Yields Arrow (-->) | Always go left to right; Always addition NOT subtraction; Represented by yields, reacts to form, creates, forms, combusts, etc. |
| Diatomic Elements | H2, O2, N2, Br2, Cl2, I2, F2 |
| Law of Conservation of Matter | Mass cannot be created or destroyed, It simply changes form |
| Most Common Driving Forces | Produces a solid, produces a gas, produces water, produces electricity (transfer of electrons.) |
| Synthesis | A + B --> AB |
| Decomposition | AB --> A + B |
| Single Displacement/Replacement | A + BC --> AC + B |
| Double Displacement/Replacement | AB + CD --> AD + CB |
| Combustion Reaction | Hydrocarbon + O2 --> CO2 + H2O |
| Precipitation Reaction | AB(aq) + CD(aq) --> AC(aq) + BC(s) |
| Acid/Base Reactions | acid + base --> salt (Metal & Halogen or Polyatomic ion) + water (H2O) |
| Molecular Equations | Complete reaction for all formulas of reactants & products |
| Ionic Equations | All parts show their ions |
| Spectator Ions | Ions that do not participate in the reactions: still in aqueous solutions |
| Net Ionic Equation | Shows only those components that are directly involved in the reaction |
| Oxidation Reduction (Redox) | Synthesis reactions of metals with non-metals (can be single displacement or another type on occasion.) Electrons are transferred from the metal to the non-metal |
| Oxidation | Losing electrons; oxidized (Remember OilRig!) |
| Reduction | Gaining electrons; reduced(Remember OilRig!) |
| Rules for Oxidation States/Numbers (1-3) | 1.) Sum of Oxidation #s in an ENTIRE compound must equal 0 2.) Sum of Oxidation #s in polyatomic ions equals the charge of the ion 3.) The oxidation state of uncombined elements and diatomic elements is 0 |
| Rules for Oxidation States/Numbers (4-7) | 4.) In ionic compounds the oxidation # equals the ionic charge 5.) Oxygen is almost always -2 6.) Hydrogen is 1+ except when paired with metals, then its -1 7.) Covalent compounds: most electronegative has the negative ox # |
| Stoichiometry | A branch of chemistry that deals w/ the relative quantity of reactants & products |
| The Mole/Avogadro's Number | 6.02 x 10^23 |
| Molar Mass/Formula Weight | The mass (in grams) of 1 mole if a substance based on its chemical formula. |
| Percent Composition | The % of a compound that is one element vs another |
| Empirical Formula | Provides info about the ration #s of atoms in the compound. Steps: Percent to mass, mass to mole, divide by small, multiply 'til whole |
| Meaning of Coefficient | Coefficients are the mole relationship for various reactants and products of a reaction. (Molar Ratio) |
| Mass to Mass | Mass A - Mole A Mole A - Mole B Mole B - Mass B |
| Hydrates/Hydrous | Molecule attached to water (H2O) |
| Anhydrous | No water molecules (H2O) |
| Limiting Reactant | The reactant that runs out first and stops the reaction |
| Excess Reactant | The leftover reactant(s) |
| Theoretical Yield | 100%; often called the "researched" yield |
| Actual Yield | >100%; often called the "experimental" yield |
| Percent Yield | Actual Yield/ Theoretical Yield x 100 |
Created by:
cbrock7086
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