chem notes 2
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| Amphoteric | can act as an acid or a base; H2O | ||||
| If we want the conjugate Base, then | H2O acting as an acid (proton donor); H20--> H+ + OH- (CB) | ||||
| If we want the conjugate Acid, then | H2O is acting as a base( proton acceptor) H20--> H3O+ (CA) | ||||
| Strong ACIDS::: 7 of them | HCl; HBr; HI; H2SO4; HNO3; HCLO4; HCLO3 | ||||
| Strong BASES:: 8 of them | LiOH; NAOH; KOH; RbOH; CsOH; ---> Group 1 & then Ca(OH)2; Sr(OH)2; Ba(OH)2 ----> Group 2 | ||||
| Ba(OH)2 | Barium Hydroxide | ||||
| Oxyacidic Trend: | More OXYGEN= more Acidic for Oxyacid i.e. HCLO<HCLO2 | ||||
| Oxyacidic Trend: | More ELECTRONEGATIVE the element= more Acidic ( stronger) ....NOT including H or O......I.e. HCLO3 > HBrO3 | ||||
| More acidic | more stable; larger; weaker conjugate base | ||||
| Kw of water= | 1X 10 ^-14 | ||||
| Kw= | [H+] [OH-] | ||||
| Ka*Kb= | Kw | ||||
| pH= | -log[H+] | ||||
| pOH= | -log[OH-] | ||||
| [H+]*[OH-]= | 1X 10^-14 | ||||
| pH+ pOH= | 14 | ||||
| H+= | 10^-pH | ||||
| OH- = | 10^-pH | ||||
| As -OH goes up (inc)....pOH goes ______? | DOWN (Dec) | ||||
| 1M HCL will have a pH of ?? | 0 | ||||
| 10 M HCL will have a pH of ??? and a pOH of ?? | pH= -1 and pOh= 15 | ||||
| weak acid _____ dissociated; Strong acid _____ dissociates | weak acid= partially dissociates; strong acids= fully dissociates | ||||
| Shortcut to find weak acid pH:: when Ka is given | [H3O+] = sqrt Ka*HA | ||||
| Shortcut to find weak base pOH:: when Kb is given | [OH-] = sqrt Kb*A- | ||||
| Moles and pH are ______ proportional | inversely | ||||
| Dissociation of a weak base | A- + H20= OH- + HA | ||||
| Dissociation of a weak acid | HA+ H20= H30 + A- | ||||
| HF + CL- ---> HCL + F- | HF= weak acid; CL- = weak conjugate base; HCL= strong acid; F- = strong conjugate base | ||||
| Equilibrium favors the ______ side in a dissociation rxn ??? | weaker side (side with weaker acid/ or base) | ||||
| INCREASE Ka= _____ pKa? | DECREASE ----> stronger acid | ||||
| INCREASE Kb= ______ pKb? | DECREASE ----> stronger base | ||||
| Cations (+)- neutral salt...8 conjugate acids | conjugate acid of strong bases....Li+, K+, Na+, Rb+, Cs+, Ca 2+, Sr 2+, Ba 2+ | ||||
| Anion (-) - neutral salt......7 conjugate bases | conjugate base of strong acid.....Cl-, Br-, I-, NO3-, CLO4-, CLO3-, HSO4- | ||||
| Anions | usually BASES w/ exception to the 7 conjugate bases of the strong acids | ||||
| Cations | usually ACIDS w/ exception to the 8 neutral conjugate acids of the strong bases | ||||
| More positively charged= the better the _____ | acid ( cation) | ||||
| To find out if a salt is acid or base...i.e. CsF | Cs is a neutral cation ( so its crossed out), and the F has a charge of -1 on table...so its basic ( anion) | ||||
| NaNO3 ( Sodium Nitrate) has a pH of?? | pH= close to 7 because both Na and NO3- are neutral species. | ||||
| Resists change in pH | buffer | ||||
| Buffer is a combination of.... | weak acid and its conjugate base.......OR.......weak base and its conjugate acid; BOTH needed in equal amounts | ||||
| Buffer can be _____ or ____ away from pH value... | +1, -1 | ||||
| Acid/ base pH is scaled based on powers of _____ | 10; i.e. pH of 2 is 1000 more acidic than pH of 5 | ||||
| For a Buffer pH equation use :: | Henderson Hasselbach ::: pH= pKa+ log (A-)/ (HA) | ||||
| 10x more acid than base = | drop one unit from pKa value | ||||
| 100x more acid than base = | drop 2 unit from pKa value | ||||
| 10x more base than acid= | RAISE 1 unit from pKa value | ||||
| 100x more base than acid= | RAISE 2 unit from pKa value | ||||
| First Law of Thermodynamics | Energy can NOT be created nor destroyed | ||||
| Second Law of Thermodynamics | For a spontaneous process, ΔS universe> 0; ΔS system + Δ S surroundings > 0 | ||||
| Third Law of Thermodynamics | A perfect crystal at 0 K has ZERO entropy | ||||
| Change in work energy | ΔE= q + w ; q= change in heat energy & w= change in work energy | ||||
| System looses heat if q= | negative (-) | ||||
| System absorbes heat if q= | positive (+) | ||||
| System does work if w= | negative (-) | ||||
| System has work done on it if w= | positive (+) | ||||
| Gas expands then w= | negative (-) | ||||
| Gas compressed then w= | positive (+) | ||||
| w= | - PΔV | ||||
| locked piston = | constant volume | ||||
| As heat (Temp) increases, then ... | Pressure increase (P and T are directly related) | ||||
| Cool= | expanding gas | ||||
| Heat | compressing gas | ||||
| Isobaric | constant pressure; ΔP= 0 | ||||
| Isochoric | ΔV=0 & w= 0...think v0w isochoric | ||||
| Isothermal | constant temp; ΔT= 0, then ΔE=0 | ||||
| Adiabatic | NO heat allowed in or out; q=0 | ||||
| Altitude Change= State function= | doesnt matter the path taken ( independent) just matters start and finish | ||||
| Everything are State Functions EXCEPT: 2 of them | q and w ; Even though ΔE= state fx | ||||
| Path Dependent | q and w | ||||
| Solids have the _____ Entropy ( disorder) ΔS | Least amount out of a s,l,g | ||||
| Gasses have the ____ Entropy ( disorder) ΔS | MOST amount | ||||
| S--> L---> G ΔS=? | postitive | ||||
| G--->L---->S ΔS=? | negavite | ||||
| More moles of gas= ____ entropy | more | ||||
| in a rxn if we go left to right according to the number of moles of gas ( more moles of gas on right then left) | Δ S= positive | ||||
| If products + reactants have the same # of moles of gas ...then Entropy= | close to 0 or very small | ||||
| Enthalpy ΔH= | q x p | ||||
| ΔH<0 | Exothermic ( release heat) | ||||
| ΔH>0 | Endothermic ( absorb heat) | ||||
| if the soln is cold .... | endothermic rxn occuring | ||||
| if the soln if warm.... | exothermic rxn occuring | ||||
| Bond Enthalpy (D) | Amnt of energy needed to break a bond | ||||
| break bond= | ENDO ( energy needed in system) | ||||
| Make bond= | EXO ( release energy in a system) | ||||
| ΔH= | bonds broken- bonds formed | ||||
| Enthalpies of formation ΔHf= | products- reactants | ||||
| ΔHf for any element in it's standard state = | 0 ... i.e. Cl2 | ||||
| ΔHf= forms exactly ____ moles of any product & forms elements in their standard state | 1 M | ||||
| Hess's law: | Change in ΔH is same regardless of path taken | ||||
| Gibb's free energy (ΔG) | Energy that is free to do work | ||||
| ΔG<0 | Spontaneous | ||||
| ΔG>0 | non- spontaneous | ||||
| ΔG= 0 | equilibrium | ||||
| ΔG= | products- reactants | ||||
| ΔG= | ΔH-TΔS ; Get High Test Scores | ||||
| Room temp = | 25 degrees C standard conditions | ||||
| ΔH= - .......ΔS= + | Spontaneous for all temp | ||||
| ΔH= + .......ΔS= - | Non spontaneous for all temp | ||||
| ΔH= - .......ΔS= - | Spontaneous at low temp | ||||
| ΔH= + .......ΔS= + | Spontaneous at High temp | ||||
| Oxidation State Rules...Get their typical oxidation states | #1 Group 1 or 2 Metals ; #2 H+ is +1 except when bonded to a metal; #3 More electronegative elements get their typical oxidation states | ||||
| Permangenate | MnO4- | ||||
| Iodide | I- | ||||
| SOdium Azide | NaN3 | ||||
| In Redox Reactions... if #e- is on the product side | oxidation | ||||
| In Redox Reactions... if #e- is on the reactant side | reduction ( think reactant reduction RR) | ||||
| In finding E for the reduction potential rxns... | dont worry about coefficients, just change sign if reverse is needed | ||||
| The standard electrode reduction potential E for H= | 0v | ||||
| shift right= E cell Increases= | spontaneous | ||||
| shift left= E cell dencreasses= | non spontaneous | ||||
| E cell= cell potential or | EMF | ||||
| for E cell shifting... only ____ matter not s or L | aq | ||||
| add more reactant, shift to the | left | ||||
| add more product , shift to the | right | ||||
| add more solid or Liquid, shift to the | NO shift because s and L are not counted | ||||
| Increase pH ( loosing H+ and becomes more basic) , shift to the | the side with more H+ ions | ||||
| Decrease pH ( adding H+ and becomes more acidic), shift to the | the side with less H+ ions | ||||
| Nerst :: | E= E - [.0592/ n] log Q ; where n= number of moles transfered in rxn; and Q= products/ reactant | ||||
| strongest oxidizing agent= gets reduced | most positive v | ||||
| strongest reducing agent = gets oxidized | most negative v ( think RAN....reducing agent negative) | ||||
| In a redox rxn if sum = NEGATIVE ...then rxn is | not spontaneous | ||||
| In a redox rxn if sum = POSITIVE ...then rxn is | spontaneous | ||||
| For Spontaneous rxns;; ΔG=___; Ecell = ____; Q___K | negative; positive; Q<K If one is true then all is true | ||||
| Electrolysis= | Destruction of electricity; consumes electricity; have to have moving ions; | ||||
| molten electrolysis= | melt salt | ||||
| NaBr (liguid)= | molten b/c its a liquid | ||||
| Grams made by electrolysis:: | (AMPS) ( t in seconds) ( mw) / ( n) ( Faraday= 96,000) | ||||
| Reductant= | gets oxidized | ||||
| Oxidant= | gets reduced | ||||
| Galvanic/ Voltaic Cells | Spontaneous | ||||
| Cell potential/ EMF= E>0; ΔG<0 | Galvanic/ Voltaic Cells | ||||
| Produces electricity | Galvanic/ Voltaic Cells | ||||
| RED CAT & AN OX | Galvanic/ Voltaic Cells | ||||
| e- go from ANODE ---> CATHODE | Galvanic/ Voltaic Cells | ||||
| ions float in and out of bridge; keep solns neutral; necessary for battery; | SALT bridge | ||||
| In a salt bridge....anions go to _____ & cations go to _____ | anode; cathode | ||||
| NON- spontaneous/ consumes energy | ELectrolytic cell | ||||
| E<0 ; ΔG>0 for _____ cells | Electrolytic cell | ||||
| In a electrolytic cell, anode is ____ & cathode is ____ | +; - | ||||
| In a electrolytic cell electrons move from | ANODE (-)----> Cathode (+) |
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Created by:
zrsoori
on 2010-06-01