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| 4213212553 | Synthesis Reactions | When simple compounds are combined to form a single, more complex compound | 0 | |
| 4213212554 | Decomposition | The opposite of synthesis. A reaction where a single compound is split into two or more simple compounds, usually in the presence of heat. | 1 | |
| 4213212555 | Acid-base Reaction | A reaction when an evidence reacts with a base to form water and salt | 2 | |
| 4213212556 | Oxidation-Reduction reaction | A reaction that results in the change of the oxidation states of some precipitating molecules. | 3 | |
| 4213212557 | Precipitation | When yen aqueous solutions mix, sometimes a new cation/anion pairing can create an insoluble salt | 4 | |
| 4213212558 | Spectator ions | Ions that do not take part in the reaction They start out and end up as free ions | 5 | |
| 4213212559 | What are the two solubility rules you need to know for AP? | 1. Compounds with alkali metal cation or an ammonium cation are always soluble 2. Compounds with a nitrate anion are always soluble | 6 | |
| 4213212560 | Why do ionic substances dissolve in water? | The attraction of a h ions to the dipoles of the water molecules. | 7 | |
| 4213212562 | How to solve a stoichiometry | 1. Convert whatever you are given into moles. 2. The limiting reagent is not necessarily the reactant that you have the least of; it is the reactant that runs out first. 3. Use the balanced equation to determine how many moles of the desired product are generated. 4. Convert moles of product to the desired unit. | 8 | |
| 4213212563 | Enthalpy Change ΔΗ | The enthalpy of a substance is a measure of the energy that is released or absorbed by the substance when bonds are broken and formed during a reaction. | 9 | |
| 4213212564 | Basic Rules of Enthalpy | When bonds are formed energy is released. When bonds are broken energy is absorbed. | 10 | |
| 4213212565 | Enthalpy Change equation |  | 11 | |
| 4213212566 | Exothermic reaction | If the products have stronger bonds than the reactants, then the products have lower enthalpy than the reactants and are more stable; in this case energy is released by the reaction | 12 | |
| 4213212567 | Endothermic reaction | If the products have weaker bonds than the reactants, then the products have higher enthalpy than the reactants and are less stable; in this case, energy is absorbed by the reaction | 13 | |
| 4213212568 | Which is more likely to occur spontaneously? Endothermic or exothermic | Exothermic. All substances like to be in the lowest possible energy state, which gives them the greatest stability. | 14 | |
| 4213212569 | Endothermic reaction diagram |  | 15 | |
| 4213212570 | Exothermic Reaction Diagram |  | 16 | |
| 4213212571 | Activation Energy Ea | The amount of energy need to reach the transition state. (Find textbook definition) | 17 | |
| 4213212572 | Catalyst | Speeds up reaction by providing the reactants with an alternate pathway that has a lower activation energy. Lowers activation energy for both forward and reverse reactions so it has no effect on equilibrium conditions. | 18 | |
| 4213212573 | Oxidation state | Indicates the number of of electrons that it gains or loses when it forms a bond. | 19 | |
| 4213212574 | What are some important things to know when dealing with oxidation states? | 1. The oxidation state of an atom that is not bonded to an atom of another element is 0. That means either an atom that is not bonded to any other atom or an atom that is bonded to another atom or the same element (O2) 2. The oxidation numbers for all the atoms in a molecule must add up to 0. 3. The oxidation numbers for all atoms in a polyatomic ion must add up to the charge of the ion. | 20 | |
| 4213212575 | Oxidation number of alkali metals | +1 | 21 | |
| 4213212576 | Oxidation number of alkaline earth metals | +2 | 22 | |
| 4213212577 | Oxidation number of group 3A | +3 | 23 | |
| 4213212578 | Oxidation number of oxygen | -2 | 24 | |
| 4213212579 | Oxidation number of Halogens | -1 | 25 | |
| 4213212580 | Oxidation number of transition metals | Have several oxidation states which are differentiated from one another by a Roman numeral in the name of the compound. | 26 | |
| 4213212581 | Hydroxide formula | OH- | 27 | |
| 4213212582 | Nitrate Formula | (NO3)- | 28 | |
| 4213212583 | Acetate formula | (C2H3O2)- | 29 | |
| 4213212584 | Cyanide formula | CN- | 30 | |
| 4213212585 | Permanganate formula | (MnO4)- | 31 | |
| 4213212586 | Carbonate formula | (CO3)2- | 32 | |
| 4213212587 | Sulfate formula | (SO4)2- | 33 | |
| 4213212588 | Dichromate formula | (Cr2O7)2- | 34 | |
| 4213212589 | Phosphate formula | (PO4)3- | 35 | |
| 4213212590 | Ammonium formula | (NH4)+ | 36 | |
| 4213212591 | Oxidation-reduction reaction | Electrons are exchanged by the reactants, and the oxidation states of some of the reactants are changed over the course of the reaction. | 37 | |
| 4213212592 | Reduction | An atom gains electrons, oxidation number decreases | 38 | |
| 4213212593 | Oxidation | An atom loses electrons and the oxidation number increases | 39 | |
| 4213212594 | Half reactions | Oxidation and reduction formulas written separately | 40 | |
| 4213212595 | Every reaction has a ______________ , or voltage associated with it. | electric potential | 41 | |
| 4213212596 | How are electric potentials given? | reduction half reactions you can read them in reverse and flip the sign on the voltage to get oxidation potentials | 42 | |
| 4213212597 | How do you calculate electric potential? | add the potential for the oxidation half-reaction to the potential for the reduction half-reaction Never multiply the potential for the half reaction by the coefficient | 43 | |
| 4213212598 | What happens to the reduction potential when a solid is placed into a metallic solution and a new solid forms? | The reduction potential of the metal in solution is greater than that of the solid. | 44 | |
| 4213212599 | What happens to the reduction potential if a solid is placed into a metallic solution and no solid forms? | The reduction potential of the solid is higher. | 45 | |
| 4213212600 | Galvanic cell | also called voltaic cell a spontaneous redox reaction is used to generate a flow current | 46 | |
| 4213212601 | What happens in a galvanic cell? | Two half reactions take place in separate chambers and the electrons that are released by the oxidation reaction pass through a wire to the chamber where they are consumed in the reduction reaction | 47 | |
| 4213212602 | Current | defined as the flow of positive charge, so current is always in the opposite direction from the flow of electrons | 48 | |
| 4213212603 | Anode | where oxidation takes place | 49 | |
| 4213212604 | Cathode | where reduction takes place | 50 | |
| 4213212605 | What happens to the voltage of the cell under standard conditions? | the voltage of the cell is the same as the total voltage of the redox reaction. | 51 | |
| 4213212606 | Electrolytic Cells | An outside source of voltage is used to force a non-spontaneous redox reaction to take place. Most electrolytic cells occur in aqueous solutions which are created when a chemical dissolves in water. | 52 | |
| 4213212607 | What are the anodes and cathodes in electrolytic cells? | Metal bars that conduct current which do not take part in the reaction. | 53 | |
| 4213212608 | What are electrolytic cells are used? | Electroplating | 54 | |
| 4213212609 | What are the steps for electroplating? | 1. If you know the current and the time, you can calculate the charge in coulombs. 2.Once you know the charge in coulombs, you know how many electrons were involved in the reaction 3. When you know the number of moles of electrons and you know the half-reaction for the metal, you can find out how many moles of metal plated out. 4. Once you know the number of moles of meta, you can use what you know from stoichiometry to calculate the number of grams of metal. | 55 | |
| 4213212610 | Equation for current | I = q/t | 56 |
