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MCAT Gen. Chem Ch. 4
| Term | Definition |
|---|---|
| Compounds | Substances composed of two or more elements in a fixed composition |
| Molecular Weight | Mass (amu) of the constituent atoms in a compound as indicated by the molecular formula |
| Molar Mass | Mass of one mole (Avogadro's number or 6.022 x 10^23 particles) of a compound measured in grams per mole |
| Gram Equivalent Weight | Measure of the mass of a substance that can donate one equivalent of the species of interest. |
| Normality | Ratio of equivalents per liter. It is related to molarity by multiplying the molarity by the number of equivalents present per mole of compound. |
| Equivalents | Moles of the species of interest. Equivalents are most often seen in acid-base chemistry (hydrogen ions or hydroxide ions) and oxidation-reduction reactions (moles of electrons or other ions) |
| Law Of Constant Composition | States that any pure sample of a compound will contain the same elements in the same mass ratio. |
| Empirical Formula | Smallest whole number ratio of the elements in a compound. |
| Molecular Formula | The same as or a multiple of the empirical formula. It gives the exact number of atoms of each element in a compound. |
| How To Calculate Percent Composition By Mass | Determine the mass of the individual element and divide by the molar mass of the compound |
| Combination Reactions | Occur when two or more reactants combine to form one product |
| Decomposition Reaction | Occur when one reactant is chemically broken down into two or more products. |
| Combustion Reactions | Occur when a fuel and an oxidant (typically oxygen) react to form the products water and carbon dioxide (if the fuel is a hydrocarbon) |
| Displacement Reactions | Occur when one or more atoms or ions of one compound are replaced with one or more atoms or ions of another compound |
| Single-displacement Reactions | Occur when an ion of one compound is replaced with another element. |
| Double-displacement Reactions | Occur when elements from two different compounds trade places with each other to form two new compounds. |
| Neutralization Reactions | Reactions in which an acid reacts with a base to form a salt (and usually water) |
| Steps To Balance Chemical Equations | Balance the least common atoms, balance the more common atoms (usually Hydrogen and Oxygen), and balance charge |
| Limiting Reagent | The reactant which will be consumed first in a chemical reaction |
| Theoretical Yield | Amount of product generated if all of the limiting reactant is consumed with no side reactions |
| Actual Yield | Typically lower than the theoretical yield |
| Percent Yield | Calculated by dividing the actual yield by the theoretical yield and converting to a percentage |
| -ous Endings Indicate: | Lesser charge |
| -ic Endings Indicate: | Greater charge |
| -ide Endings Indicate: | Monatomic anions |
| -ite Ending For An Oxyanion Indicates: | Contains a less amount of oxygen |
| -ate Ending For An Oxyanion Indicates: | Contains a greater amount of oxygen |
| Hypo- Ending For Oxyanion Series With 2+ Members Is Given To | Species with the fewest oxygens |
| Per- Ending For Oxyanion Series With 2+ Members Is Given To | Species with the most oxygens |
| Hydrogen / bi- Ending For Polyatomic Ions Containing Hydrogen Indicate | One hydrogen |
| Dihydrogen Ending For Polyatomic Ions Containing Hydrogen Indicate | Two hydrogens |
| Ionic Charges Are Predictable By (Representative Elements): | Group number and type of element (metal or nonmetal) for representative elements |
| Ionic Charges For Nonrepresentative Elements Are: | Generally not predictable |
| Electrolytes | contain equivalents of ions from molecules that dissociate in solution. |
| Solvation | Degree of dissociation, this determines the strength of an electrolyte. |
| Eq. 4.1: Moles From Mass | Moles = Mass of a sample / Molar mass |
| Eq. 4.2: Gram Equivalent Weight | GEW = Molar mass / n. n = number of particles of interest produced or consumed per molecule of the compound in the reaction. |
| Eq. 4.3: Equivalents From Mass | Equivalents = Mass of compound / Gram equivalent weight |
| Eq. 4.4: Molarity From Normality | Molarity = Molar mass / n. n = number of protons, hydroxide ions, electrons, or ions produced or consumed by the solute. |
| Eq. 4.5: Percent Composition | Percent composition = Mass of element in formula / Molar mass * 100% |
| Eq. 4.6: Percent Yield | % Yield = Actual yield / Theoretical yield * 100% |
Created by:
SamB91
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