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chadchem2
chem notes 2
| Question | Answer |
|---|---|
| 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 (+) |
Created by:
zrsoori
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