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| 10635699831 | define solution | Homogeneous mixture of two or more substances | 0 | |
| 10635699832 | solvent vs solute | solvent - greatest quantity solute - smaller quantity, gets dissolved | 1 | |
| 10635699833 | When is a solution aqueous | the solvent is water | 2 | |
| 10635699834 | Is pure water conductive | no | 3 | |
| 10635699835 | define electrolyte | A substance that creates *aqueous* solutions that contains ions. It dissociates into Ion in the solution | 4 | |
| 10635699836 | define nonelectrolyte | A substance that creates *aqueous* solutions that does not contain ions. I does not break up into ions | 5 | |
| 10635699837 | which types of compounds create electrolytes/nonelectrolytes | Ionic compounds - electrolytes molecular compounds - nonelectrolyes | 6 | |
| 10635699838 | define dissociate | the act of a compound breaking apart into ions during the act of dissolving | 7 | |
| 10635699839 | Why is H2O good for dissolving (thus dissociating) ionic compounds | It's partial charges H ions are partial positive O ion is partial negative | 8 | |
| 10635699840 | define solvation/ solvated state | solvation is an interaction of a solute with the solvent, which leads to stabilization of the solute species in the solution. One may also refer to the solvated state, whereby an ion in a solution is surrounded or complexed by solvent molecules |  | 9 |
| 10635699841 | how to denote a solvated ion | Na+(aq) | 10 | |
| 10635699842 | What kinds of molecular compounds dissolved into ions | acids | 11 | |
| 10635699843 | Define ionize | convert (an atom, molecule, or substance) into an ion or ions, typically by removing one or more electrons | 12 | |
| 10635699844 | Strong electrolytes vs weak electrolyets | strong - exist almost completely as ions in aqueous solutions. All water soluble ionic compounds, few molecular compounds weak - exist mostly in the form of neutral molecules in aqueous solutions and only a small fraction dissociates into ions | 13 | |
| 10635699845 | define solubility | the amount to which a substance will dissolve at a given temperature | 14 | |
| 10635699846 | strong electrolyte != | high solubility | 15 | |
| 10635699847 | How to write the equation for an ionizing reaction (weak electrolytes) | The two arrows mean the reaction is happening in both directions. As AH dissociates A+ and H+ recombine to become AH again. This achieves chemical equalibrium |  | 16 |
| 10635699848 | define chemical equalibrium | number of each type of ion/molecule in a solution is constant | 17 | |
| 10635699849 | How to determine if a compound is an ionic compound | The presence of both metals and nonmetals except if an ion contains NH4+ | 18 | |
| 10635699850 | define precipitation reaction What happens during a precipitation reaction | when a reaction in a liquid solution creates a solid charged ions attract each other so strongly the create an insoluble solid | 19 | |
| 10635699851 | define precipitate | the solid formed by the precipitation reaction. | 20 | |
| 10635699852 | solubility less than __________ is insoluble | 0.01 mol/L | 21 | |
| 10635699853 | solubility rules | Understand then, don't need to memorize in BB | 22 | |
| 10635699854 | are double displacement (metathesis) reactions redox reactions? | Not a redox reaction |  | 23 |
| 10635699855 | How to balance an exchange reaction AKA double displacement reaction | 1. use the chemical formulas of the reactants to figure out which ions are present 2. write the chemical formulas of the products by combining the cation from one reaction with the anion of the other. Us the charges to determine the subscripts 3. check the solubilities. If one is insoluble it is a precipitation reaction 4. Balance the Equation | 24 | |
| 10635699856 | molecular equation | Does not show ionic character |  | 25 |
| 10635699857 | complete ionic equation for double displacement reaction | shows ionic character all soluble strong ions have their charges shown | | 26 |
| 10635699858 | define spectator ions for double displacement reaction | A spectator ion is an ion that exists in the same form on both the reactant and product sides of a chemical reaction. Thus it has no direct role in the reaction |  | 27 |
| 10635699859 | define net ionic equation for double displacement reaction | the equation consisting only of elements directly involved in the reaction to form: cross out anythin that doesn't change from left to right side What remains is your equation | | 28 |
| 10635699860 | If every ion in an ionic equation is a spectator... | No reaction happens | 29 | |
| 10635699861 | What compounds are strong electrolyts | all ionic compounds, strong acids | 30 | |
| 10635699862 | What compounds are weak electrolytes | weak acids, weak bases | 31 | |
| 10635699863 | What compounds are nonelectrolytes | anything that is not an ionic compound, weak acids, or weak bases | 32 | |
| 10635699864 | Strong acids | HClO4 HClO3 H2SO4 HNO3 HCl HBr HI -ic acids are strong -ous acids are weak | 33 | |
| 10635699865 | Strong bases | LiOH NaOH KOH RbOH CsOH Ca(OH)2 Sr(OH)2 Ba(OH)2 Group A1 Group 2A | 34 | |
| 10635699866 | Define acids | Ionize in aqueous solutions to form H+(aq), hydrogen ions Hydrogen ions are essentially protons | 35 | |
| 10635699867 | what are hydrogen ions | just a proton (Hydrogen is just 1 proton and 1 electron) | 36 | |
| 10635699868 | Monoprotic vs diprotic | monoprotic - acid that yields 1 H+ ion diprotic - acid that yields 2 H+ ions | 37 | |
| 10635699869 | define base | substances that accept and react with H+ and produce OH- hydroxide ions when they dissolve A base does not have to have OH in it because it can often accept the O from the soultion | 38 | |
| 10635699908 | How to find out if a substance is a strong electrolyte, weak electrolyte, or a nonelectrolyte |  | 39 | |
| 10635699870 | Define neutralization action | when an acid and a base is mixed. The products do not have any of the characteristics of the reactants | 40 | |
| 10635699871 | What do neutralization reactions between metal hydroxides and acids produce? | salts and water You need to be able to recognize neutralization reactions. There may be questions that dont give a formula, but you can find it out yourself since you know the products of a neutralization reaction | 41 | |
| 10635699872 | define salt | any ionic compound whose cation comes from a base and it's anion comes from an acid | 42 | |
| 10635699909 | green text | 43 | ||
| 10635699873 | Oxidation reduction reactions | electrons are transferred from one reactant to another | 44 | |
| 10635699874 | Explain corrosion (redox reaction) | The conversion of a metal to a metal compound by a reaction betweeen the metal and some substance in it's enviornment i.e. the metals ions loose an election, becoming cat ions, and combines with anions in the envirnment to form an ionic compound | 45 | |
| 10635699875 | Define oxidized | when an atom, ion, or molecule has become more positive (looses electrons) | 46 | |
| 10635699876 | Define oxidation | the losing of electrons | 47 | |
| 10635699877 | define reduced | when an atom,ion, or molecule has gained electrons | 48 | |
| 10635699878 | define reduction | the gaining of electrons (becoming more negative`) | 49 | |
| 10635699879 | Oxidation is always followed by | reduction | 50 | |
| 10635699880 | define oxidation number what is it needed to identify | a number assigned to an element in chemical combination that represents the number of electrons lost (or gained, if the number is negative) by an atom of that element in the compound. Oxidation reduction reactions | 51 | |
| 10635699881 | what is the oxidation number for monatomic ions | its the same as their charge | 52 | |
| 10635699882 | what is the oxidation number for neutral molecules and polyatomic ions | a hypothetical charge determined by artificially dividing up the elections in the molecule/ion. | 53 | |
| 10635699883 | What are the rules for determining oxidation number Google it, find out oxygen ad hydrogen exceptions What the **** | 1. In elemental for the oxidation number is 0 (one element in the formula, no over all charge) 2. for a monatomic ion the oxidation number is equal to the charge of the ion (Al3+ redox number is +3) 3. nonmetals usually have negative oxidation numbers but not always a. Oxygen is -2 except in peroxides b. Hydrogen is usually +1 when bonded to nonmetals and -1 when bonded to metals c. fluorine is always -1 . The other halogens are usually -1 in most binary compounds But when bonded with oxygen (oxyanions) they are positive. Certain elements have same oxidation number in all/most of their compounds a. 1A metals are always +1 in compound b. 2A metals are always +2 in compound cl Fluorine is always -1 in compound 4. The sum of oxidation numbers in a neutral compound is zero. The sum of the oxidation numbers in a polyatomic ion equals said ion's charge. 5. Max oxidation number of group A is its group number (roman numeral) 6. For nonmetals the minimum oxidation number is group number minus 8. | 54 | |
| 10635699884 | define elemental form | A substance that cannot be broken down into simpler substances by chemical means. An element is composed of atoms that have the same atomic number, that is, each atom has the same number of protons in its nucleus as all other atoms of that element. | 55 | |
| 10635699885 | how to distinguish between charge and oxidation number | charge = 2+ oxidation number = +2 | 56 | |
| 10635699886 | the pattern of a reaction between a metal and an acid or metal salt | A + BX ---> AX + B | 57 | |
| 10635699887 | define displacement reaction | a chemical reaction in which a more reactive element displaces a less reactive element from its compound. Both metals and non-metals take part in displacement reactions. | 58 | |
| 10635699888 | define activity series | a list of metals arranged by ease of oxidation |  | 59 |
| 10635699889 | define active metals, which are they | metals that are most easily oxidized the alkali metals and alkaline earth metals (maybe more) | 60 | |
| 10635699890 | define noble metals, which are they | transition elements from groups 8B to 1B (maybe more) they have low reactivity | 61 | |
| 10635699891 | what can the activity series predict | the outcome single displacement reactions (Maybe double displacement???) | 62 | |
| 10635699892 | Which metals can be oxidized by which metals | Each metal on the activity series can be oxidized by metals lower than it on the table |  | 63 |
| 10635699893 | Anything under hydrogen on the activity series cannot... | react with acids to form H2 | 64 | |
| 10635699894 | define concentration | the amount of solute dissolved in a quantity of solvent The more solute the more concentrated | 65 | |
| 10635699895 | Define molarity molarity equation (aka how to find concentration) | The concentration of a solution by how many moles of a solute is in it. (M) MOLES OVER L |  | 66 |
| 10635699896 | What does 1.0 M Ca(NO3)2 mean? | 1.0 mol of Ca(NO3)2 per liter 1.0 mol Ca(NO3)2/L | 67 | |
| 10635699910 | Molarity problem |  | 68 | |
| 10635699897 | Two ways to express concentration of electrolytes | in terms of the compound used (1.0M of Na2SO4) In terms of the ions in the solution (2.0M Na+ and 1.0M of SO4^2-) | 69 | |
| 10635699911 | convert moles to volume using molarity???? | 70 | ||
| 10635699898 | define dilution | process of adding a concentrated version of a solution to another solution (usually water) gain a lower concentration of the concentrated solution. This is common for commonly used chemicals. | 71 | |
| 10635699899 | Dilution problem | It's basically algebraic manuipulation |  | 72 |
| 10635699900 | Moles of solute before dilution = | moles of solute after diultion | 73 | |
| 10635699912 | Equation for dilution (can only be used for a pure solvent) |  | 74 | |
| 10635699913 | Still need to do 4.6. Waiting to understand ch. 3 better | 75 | ||
| 10635699901 | What is special about the ferric ion in regards to Exchange (Metaphesis) reactions | Fe3 stays Fe3 when moving from products to reactants | 76 | |
| 10635699914 | Going from molecular formula to ionic formula to complete ionic formula | 77 | ||
| 10635699902 | Gas-forming reactions | some double displacement reactions don't give expected products When carbonate/bicarbonate.... |  | 78 |
| 10635699903 | Oxidizing agent vs reducing agent | oxidizing agent - substance that is reduced reducing agent- substance that is oxidized | 79 | |
| 10635699904 | define single replacement (single displacement) reaction are they redox reactions? | A + BC ---> AB + C are redox reactions | 80 | |
| 10635699915 | How to identify if a reaction is a redox reaction | 81 | ||
| 10635699916 | Using molarity in stoichiometry flow chart |  | 82 | |
| 10635699917 | Using molarity in stoichiometry problem |  | 83 | |
| 10635699918 | Titration flow chart |  | 84 | |
| 10635699919 | Single displacement reaction of halogens |  | 85 | |
| 10635699920 | Reactants and products of combustion reactions |  | 86 | |
| 10635699905 | what is H(OH) | H2O | 87 | |
| 10635699906 | Mass percent of solute (way of determining concentration other than molarity) | mass of solute/mass of solution x 100 | 88 | |
| 10635699921 | Exceptions |  | 89 | |
| 10635699907 | Carbonate charge Sulfate charge | CO3 2- SO4 2- | 90 | |
| 10635699922 | Oxidation number rules |  | 91 | |
| 10635699923 | How many liters of water must be added to dilute 250 mL of 12M HCl to 1M HCl |  | 92 | |
| 10635699924 | yep |  | 93 |
