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Chem
| Question | Answer |
|---|---|
| Cation | positively charged ion Forms when an atom loses electrons |
| anion | negatively charged ion Forms when an atom gains electrons |
| ionic bonds and Lattices | When positive and negative charges are near each other there is an attractive force described by Coulomb’s Law |
| Empirical formula | Gives the smallest whole number ratio of ions or atoms in the compound The smallest number of ions necessary to form a compound is a formula unit |
| Predicting formulas for ionic compounds | To form a neutral ionic compound the positive and negative charges of the cation and anion must be equal. |
| Hydrates | An ionic compound that has water molecules trapped in the crystal lattice is a hydrate. |
| covalent compounds | Form when two or more atoms share electrons to form bonds Water, H2O, is an example of a covalent compound. Molecular formulas are used to represent covalent compounds Molecular formulas provide the actual number of atoms in the molecule |
| Binary covalent compounds | Binary Covalent Compounds Contain atoms from two different elements Named the same way as ionic compounds Use the full name of the first atom and the stem name of the second atom with suffix -ide Use prefixes to indicate the number of atoms present |
| solute | Substance that is dissolved |
| solvent | Substance in which the solute is dissolved |
| solution | Refers to the solute and the solvent |
| Ionization | Occurs when ionic compounds dissolve in water; the ions dissociate from each other and become solvated by water molecules |
| Electrolyte solution | An electrically conducting solution; the separated cations and anions carry charge to form an electrically conducting solution |
| acids | molecular compounds that usually contain a hydrogen atom and a species that can form a stable anion Acids ionize when dissolved in water to produce a hydrogen cation, called the proton and a stable anion Form an electrolyte solution |
| Binary acids | Consist of the hydrogen atom and a single nonmetal atom, usually a halogen |
| oxoacids | Consist of the hydrogen atom (sometimes more than one) and an oxyanion |
| Elemental analysis | Technique for determining Elements in a compound Percent composition Empirical formula Empirical formula mass Mass spectrometry Determines the molecular formula mass |
| Mass spectrometry | determines molecular mass of compound Ionizing chamber converts molecule into ion Electric field accelerates ions Magnetic field deflects ion to an extent proportional to their mass; lighter |
| Balanced chemical equations | Represent chemical changes and include o Reactants o Reaction arrow o Products o Stoichiometric coefficients |
| Stoichiometric coefficients | Numbers before each species in the chemical reaction Used to balance chemical equations Shows law of conservation of mass has been followed relate amounts of reactants to amounts of products |
| Balancing equations | dd stoichiometric coefficients to a chemical equation to provide atom balance |
| Molecular equations | write ions together as compounds |
| ionic equations | show dissociated ions as separate species |
| precipitations reaction | two aqueous solutions combine to produce to create a solid product. |
| precipitate | The solid formed in the reaction |
| complete ionic equation | can be written when all of the ions are shown |
| spectator ions | an ion that is present in a solution but not directly involved in a chemical change |
| net ionic equations | an equation in which the only ions shown are those directly involved in the chemical change, and spectator ions are omitted |
| bases | a compound that produces OH- ions in water; a compound that accepts H+ ions |
| Neutralization reactions | A reaction in which an acid and a base combine to produce water and an ionic compound( called salt) |
| Metal displacement reaction | a reaction between two metals in which one metal is oxidized to its ionic form while the other metal ion is reduced to its elemental form. |
| activity series | a table that lists metals by their activity that is used to predict whether metal displacement reactions will occur. |
| Limiting reagent calculations | Identify limiting reagent Determine the maximum amount of product possible |
| Limiting reagent | Determines the amount of product that can be produced in a reaction completely consumed in the reaction |
| excess reagent | not completely consumed in the reaction |
| Molarity and Solution Stoichiometry | Relate molarity to moles of solute and volume of solution Solve stoichiometry problems that involve solution |
| Gravimetric Analysis | Technique for determining the concentration of ions in solution Use mass of precipitate in precipitation reaction to determine concentration of reactant |
| Theorietical yield | Maximum amount of product that can be obtained from the given amounts of starting materials |
| actual yield | Amount of product obtained from the reaction |
| percent yield | actual yield divided by theoretical yield times 100 |
| How to solve for molarity | M={moles of solute}\{liters of solution} Steps: 1. Find the moles of solute. 2. Convert mL to L by dividing by 1,000. 3. Divide moles by liters. |
| Solution Stoichiometry | Write and balance the equation. Make sure there are the same number of each type of atom on both sides. The coefficients give you the mole ratio. Convert mL to L. Divide milliliters by 1,000. Find moles using molarity. Multiply molarity by liters |
| Thermodynamics | study of relationship between energy and temperature changes |
| Thermochemistry | Part of thermodynamics that deals with chemical changes |
| Potential energy | stored energy Energy that results from position in a field of force |
| Kinetic energy | energy in motion |
| energy changes | work heat |
| exothermic reaction | system releases heat to surroundings 2C3H18(l)+25O2(g)--> 16CO2(g)+18H2O(g)+Heat |
| Endo thermic reaction | system absorbs heat from surroundings Heat+H2O(s)-->H2O(l) |
| system | reaction or process being studied |
| surroundings | everything around the system |
| pressure-volume work | w=-Pchange in V |
| enthalpy(H) | measure of the total heat content of a system |
| Change in enthalpy | gain or loss of heat energy as the result of a chemical or physical change |
| First law of thermodynamics | Energy can neither be created nor destroyed Energy that is lost by the system is gained by the surroundings Energy that is gained by the system is lost by the surroundings |
| Specific heat capacity | also called specific heat Amount of heat required to increase the temperature of one gram of a substance, 1 degree celcius |
| NH+4 | amonium ion |
| NO-2 | nitrite ion |
| NO-3 | nitrate ion |
| SO2-3 | sulfite ion |
| SO2-4 | sulfate ion |
| HSO- 4 | hydrogen sulfate |
| CO2-3 | Carbonate ion |
| PO3-4 | phosphate |
| HPO2-4 | hydrogen phosphate |
| H2PO-4 | dihydrogen phoshate |
| CrO2-4 | chromate ion |
| CrO2-7 | dichromate ion |
| MnO-4 | permanganate ion |
| C2H3O-2 | acetate ion |
| OH- | Hydroxide ion |
| CN- | cyanide ion |
| O2-2 | peroxide ion |
| CIO-4 | perchlorate |
| ClO-3 | chlorate |
| ClO-2 | chlorite |
| ClO- | hypochlorite |
| heat and temperature equation | q=mxsx^T Heat equals mass times specific heat times change in temp |
| First law of thermodynamics equation | ^E=q+w q heat, W work |
| pressure- volume work equation | w= -p^V |
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