the behavior of gases in terms of molecular motion Volume then Pressure Temp then Volume moles is constant volume is directly proportional to moles P in atm V in L T in K for ratio 1 1 if not must change Actual Theoretical x 100 Percent Yield Limiting reagent mole A x ratio B ratio A mole B x ratio A ratioB mole B mole A B A then A limiting B A then B limiting Formulas Kinetic Molecular Theory E m v2 2 Boyle s Law P1V 1 P2V 2 Charles s Law V 1 T 1 P2V 2 T 2 Mole Fraction X a Density D m V Combined Gas Law V 1 n1 V 2 T2 P 1V 1 T 1 V 2 Avogadro s Law n2 Ideal Gas Law pV nRT Dilution of solution M 1V 1 M 2 V 2 mRT Molar Mass M n PV V P m V RT na ntotal Pa Partial Pressure X a PTotal Van Der Waals P nRT V nb a n 1 3 Radius r 1 4 Volume molecule V 4 3 Constants R 8 3144 Mole N a 6 02 x 1023 Standard molar Volume 22 414L mol if at STP STP P 760 torr 1 atm 101 325Pa T 273 15K 0C 32F C to F C F 32 1 8 1 Uncombined element 0 2 Sum of Ox in compound 0 3 Sum of Oz ion charge of ion 4 F 1 5 H 1 w nonmetals 1 w metals 6 O 2 7 halogens 1 8 Middle element pos neg X 0 0 08206 L atm mol K 2 b mol K r3 N a 2 v J 3 Carbonate Nitrite Chromate Phosphate Ammonium Chlorite Permanganate Sulfite Cyanide Peroxide 2 CO3 2 NO2 CrO4 PO4 3 NH4 ClO2 MnO4 SO4 2 CN O2 2 None None Soluble NO3 ClO4 Cl 2 Ag Hg2 Pb2 Ag Hg2 2 Pb2 2 Ca2 Ba2 Sr2 Hg2 Pb2 Ag None I SO4 Na K NH4 Electrolytes Strong HCL HNO3 HCLO4 H2SO4 NaOH Ba OH 2 Ionic compounds Week CH3COOH HF HNO2 NH3 H20 Strong Base Strong acid NaOH HI KOH HBr LiOH HClO4 RbOH HCl HClO3 CsOH 2 Insoluble CO3 PO4 3 OH Group IA NH4 Group IA NH4 Group IA Ca2 Ba2 Thermodynamics Constants U system U surrounding 0 U sys U su rr U q W w F x d w P V U qv constant V process q p U P V constant P process H U PV c 3 0 x 108m s Speed of light h 6 626 x10 34 j s Planck s constant M e 9 11 x10 31kg Mass of the electron Rh 2 18 x 10 18 j Type equation here Conversions Frequency 1 Hz 1 s 1 1 A 1 0 x10 10 100 pm H rxn np H p 1 nm 1 0 10 9 meters H kJ mol E H q mC s T Heat capacity J g C 1J kg m2 s2 2 39 x10 4 kcal nr H r 2 Einstein solved photoelectric effect 1 Planck explained the emission of radiation by heat solids 3 Bohr developed a model of hydrogen atom in which energy of its single electron is Light striking metal cause electron to eject amounts rather then over a continuous range a Quantum theory radiant energy is emitted by atoms and molecules in small i Relationship E hv as n up E up ii Energy is always emitted in whole numbers a b Light behaves like a stream of particles Photon c Resonace condition E of photon must match speracting energy level Quantum mechanics Light c E hv hc De Broglie equation h mv Energy h mv v h m En RH 1 n2 J g C H hv R H 1 X p h 4 Angler momentum a Electron is a De Broglie wave has particle like properties mvr nh b Therefore spatial coherence is needed for the electron orbits in a radius 2 c 2 r n a Orbit is well defined path have specific value b Absorbs photon E up 0 emission photon E down 0 c a Ground state electron most stable energy state b Excited state electron at higher energy level c Spectroscopic transition absorption and emission can be used to id molecules 5 What Bohr missed Correctly explan hydrogen ession spectrum failed elements with 1 electron 4 Bohr model an electron emits a photon when it drops from higher energy to lower limited to certain value Principal quantum number hydrogen emission spectrum ni2 1 ni2 i Only electrons with energies corresponding to integer values of the orbits circumference can travel in orbit this is why orbital energy are quantized d Because the they travel in a way that cant be found 6 De Broglie used Einstein s theory to develop h mv 7 Schrodinger describes motion and energy of subatomic particles a Particle probability theory where electrons might be b Beginning of new age in physics 8 Hunds rule most stable arrangement of electrons in a subshell is the one that has the greatest number of parallel spins 9 Aufbau principle provides guides lines for building up the elements Quantum Numbers 1 n principle quantum number a Identifies main energy level shell i K L M F 2 l Angular quantum number n 1 identifies shape of orbital a 3 ml Magnetic quantum number l 1 0 l 1 i s p d f 1 Law od energy be created 1st law of amount of universe is 2 a 3 State properties 4 State properties the state how state a in 5 Open exchange 6 Closed change Isolated neither 7 8 Expansion 0 w 0 a 9 work conservation of energy can not or destroyed thermodynamics energy in constant Can change form gained or lost by surrounding measurable function determined by regardless of was achieved Internal energy sum of all energy system system can mass and energy system can energy not mass can exchange work delta V Work done by system Compression delta V 0 w 0 a Work doe on system 10 Exothermic gives off heat to surrounding delta H 0 11 Endothermic system absorbs heat delta H 0 12 Specific heat amount of heat required to raise T of one g of substance by 1 degree 13 Calorimeter measurement of heat change H a Constant U deltaUsystem q w q p delta V q b Qp delta H 14 Standard enthalpy of formation is Dealt H of reaction where 1 mol of compound is formed from its elements at 1 atm 15 Standard enthalpy of reaction delta H of reaction at 1 atm 16 Hess Law change in enthalpy depends on reactants and products of reaction and does not rely on pathway or steps of e in orbital max 2 electrons per orbital of e in shell 2n2 2 8 18 n 1 2 3 Orbitals n2 number of orbitals l 0 ml 0 s 1 l 0 ml 0 s 1 l 1 ml 1 0 1 p 3 l 0 ml 0 s 1 l 1 ml 1 0 1 p …
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