Oswaal CBSE Class 12 Mind Map Chemistry 2023 PDF

 2 ] MIND MAPS...

 2 ] MIND MAPS Learning MaDE SimpLE anytime, as frequency as you like till it becomes a habit! presenting words and When? To Unlock the imagination concepts as pictures!! and come up with ideas What? To Remember facts and MIND MAP Why? AN INTERACTIVE MAGICAL TOOL To Make clearer and better To know about more useful books click here notes To Concentrate and save time Result How? To Plan with ease and ace exams with a blank sheet of paper Learning made simple coloured pens and ‘a winning combination’ your creative imagination! What are Associations? It’s a technique connecting the core concept at the Centre to related concepts or ideas. Associations spreading out straight from the core concept are the First Level of Association. Then we have a Second Level of Association emitting from the first level and the chronology continues. The thickest line is the First Level of Association and the lines keep getting thinner as we move to the subsequent levels of association. This is exactly how the brain functions, therefore these Mind Maps. Associations are one powerful memory aid connecting seemingly unrelated concepts, hence strengthening memory. Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII  Cubic : (NaCl, Cu) a=b=c; primitive, bc, fc; === 90° Molecules held by Atoms /molecules held by Tetragonal : (SnO 2, T iO2) a=b  c; intermolecular forces weak dispersion Ions held by === 90°; primitive, BCT forces /London forces  (Ar, He) strong coulombic Orthorhombic :  (KNO 3, BaSO 4) Non-metals held Po forces  la a  b  c === 90°; primitive, BCO, FCO, by covalent bond r (NaCl, MgO) Hydro Hexagonal :  (ZnO, CdS) a=b  c;  (SiC, C) Molecules held by dipole-dipole ge n == 90° y =120°; primitive Metal atoms held interactions  (HCl, SO 2) Io bon Rhombohedral or Trigonal : by metallic bond n d Co ic  (Fe, Cu) ed (CaCO 3, HgS) va so len l id a=b=c; ==90°;primitive Me s talli cs t so lids Molecules held by hydrogen Monoclinic : (Monoclinic sulphur, zM olids bonding  (H2O(ice) Na2SO4.10H2O) == 90°   90°; Density = 3 a NA primitive, ec Triclinic : (K2Cr 2O 7, H3BO 3)   b  c ape (Cu, Al)  Overlapping / very small gap between it e sh      90°; primitive fin conduction and valence band de Oswaal CBSE Mind Maps, BIOLOGY, Class-XII ith (Polyethylene, clay)  Small energy gap between lw conduction and valence band s ta ry Body centred: One particle at its body centre ll c Smallest Unit a and at its cor n. (Si, Ge)  Very large gap sm Face centred: One particle at centre of each between conduction face and at its corner. of Semico nd and valence band End centred: One particle at centre of any two Electrical Properties uc to Crystal Lattice r s opposite faces and at its corner. n-type (negative charge) O O O O O O O O O O B O p-type (positive charge) To know about more useful books click here The Solid O O As O O O O O O O O O O O O O Packing Efficiency State O O O O Magnetic Properties Paramagnetic: weakly attracted  Unpaired electrons  (O2, Cu2+)  scp  AAA….type  52.4%  (Po) Imperfections Diamagnetic: weakly repelled  Paired electrons  (H2O, NaCl)  hcp  ABABAB…..type  74%  (Mg,Zn) Ferromagnetic: strongly attracted  domains in same direction  (Fe, Co)  ccp/fjcc  ABCABC….type  74%  (Cu, Ag) Po Antiferromagnetic: domain opposite and equal  (MnO)  bcc  square close packing  68%  (Li, Na) in Voids : Empty space At t de Ferromagnetic: domains unequal  (Fe3O4, MgFe2O4) between spheres a p fec oi t : nt s Three spheres in contact  Trigo 0.155 – 0.225 nal Im disturb Stoic Vacancy : Lattice sites vacant pu ri t h iom (non-ionic solids) etr yf or y ei Four spheres at the vertices of tetrahedron g n Interstitial : Particles occupy interstitial at  0.225 – 0.414 site (non -ionic solids) om sa re Six spheres at vertices of octahedron  0.414 – 0.732 Frenkel :Smaller ion dislocated to interstitial site (ZnS, AgCl) Metal Excess: Schottky: Equal number of ions Due to anionic Metal Deficiency: missing (NaCl, KCl) vacanci es (LiCl) Metal shows variable and presence of vacancy (Fe 2+, Fe3+) Trace the Mind Map extra cations (ZnO)    First Level Second Level Third Level [ 3  4 ] Partial pressure of gas in vapour phase is proportional to the mole fraction of gas in the solution. p =KHx Increases with decrease in temperature Normal molar mass = Abnormal molar mass Increases with increase in pressure Not significant  Osmotic pressure   = CRT K f × W2 ×1000  Depression in freezing point  Tf = M 2 ×W1 Abnormal molecular mass: Endothermic sol H > 0, Solubility increases molecular mass K ×1000 × W2 id  Elevation of boiling point  Tb = b different from expected value M 2 × W1 iq u Exothermic sol H < 0, Solubility decreases W ×M 1 P°1 - P1  Relative lowering of vapour pressure  2  M 2 ×W1 P1 Gas in L Colligative Gas – Gas  Mixture of O2 and N 2 properties Liquid – Gas  Chloroform with N2 Solubility s ou Solid – Gas  Camphor in N2 se a Minimum boiling azeotrope Vmix = positive G H mix = positive Gas – Liquid  O2 dissolved in water Ideal solution  (n-hexane and n-heptane) H mix = negative Liquid – Liquid  Ethanol dissolved in water Vmix = negative Raoult’s Law Solutions Types Solid – Liquid  Glucose dissolved in water To know about more useful books click here Gas – Solid  O2 in Pd Non-ideal solution  Liquid – Solid  Amalgam of Hg with Na (Mixture of chloroform and acetone) Maximum boiling azeotrope Different methods to express Solid – Solid  Cu dissolved in gold concentration of solution For any solution, the partial vapour pressure of each volatile component is directly proportional to its mole fraction. Mole fraction Normality: Number Molality: Number Molarity : Number Mass by volume p ercentage (w/v) of gram equivalents of moles of solute per of moles of solute of the solute dissolved kilogram of the solvent in 1L solution Mass percentage (w/w) in one litre of solution Parts per million : For trace quantities (Mass of solute(g) No. of moles of solute  100 No. of moles of component Mass of solvent in kg Mass of component in solution Volume of solution in mL)  100 Total no. of moles of all components Total mass of solution No. of gram equivalentof solute×100 No. of moles of solute Volume percentage (v/v) Volume of solution Volume of solution in litres No. of parts of components×10 6 Gram Equivalents of solute Volume of component Total no. of parts of components of solution Mass of solute  100 = Total volume of solution Equivalent weight Molecular mass Equivalent weight = Valency Trace the Mind Map    First Level Second Level Third Level Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII   1st Law  Amount of substance in a chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the quantity of electricity passed through electrolyte  W = Zit  2nd Law  Amount of different subst ances liberated by same quantity of rG° = –RT InK Galvanic cell that converts electricity passing through electrolytic solution are proportional energy of combustion of fuels to their chemical equivalent weights  …… W1 W2 W3 like H 2, CH4 directly into   rG° = –n FE°cell electrical energy E1 E2 E3 Painting, barrier protection, rust solutions Rusting of iron, tarnishing of silver Faraday’s laws of electrolysis Electrochemical phenomenon in which metal oxide of metal forms Relation between cell coating on metal surface. Fuel cells Mercury cell potential and Gibbs energy Products of electrolysis depends upon Leclanche cell (Dry cell) ot be reused) Corrosion an d cann Daniell Cell: cathode: Copper, Anode : Z inc; Salt o n ce (Lead storage battery, Oswaal CBSE Mind Maps, BIOLOGY, Class-XII Ni-Cd cell) bridge : Agar agar; electrolyte : KCN/KNO3 Batteries  Reduction : Cu2+ + 2e  Cu;Zn(s) Types of Oxidation : Zn2++2e– ;Zn|Zn2+(C1) || Cu 2+(C2)|Cu Cells 2.303RT [M] Nernst equation Ecell = E° cell – log n+ nT [M ] Electrochemistry 0.059 1 Resistance Ecell = E°cell – log n+ Half–cell  Mn+(aq) + ne–  M(s) n [M ] two portions of cell  nE° cell  V KC = Antilog   R= Unit : Ohm ()  0.0591  I 2.303 RT To know about more useful books click here E°cell = log K C Potential difference between Electrical resistance nF electrode and electrolyte. A chemical Electronic conductance: compound l Depends on:- Nature and that dissociates U shaped inverted R=  A structure of metal, Electrode potential when into ions and tube connecting  = Resistivity -Number of valence electrons per atom, ls concentration of all species in conducts electric two electrolytic -Temperature (Decreases current Unit : Ohm – Meter eta half cell is unity. solution Cathode  with increase in temperature) m Reduction takes place Electrode : Pt coated with Anode  Oxidation takes place Pt black, electrolyte : Electrolytic (Ionic) Conductance: Positive E° Weaker acidic solution pressure depends on:- reducing agent than H+/H2 1 bar Pt(s) |H2(g)| H+(aq) Conductivity  Nature of electrolyte added, Cell  Size of ions solvation Negative E°Stronger  Nature of solvent and its viscosity,  Concentration of electrolyte, reducing agent than  Temperature (increases with increase in H+/H2 Temperature) Two copper strips dipped in an aqueous solution 1 A Unit : Siemens (s) A series of half–cells arranged in increasing of CuSO4  Anode : Cu  Cu2+ + 2e– C= = standard oxidation potentials. cathode : Cu2+ + 2e–  Cu R l or ohm Increases on A = l dilution A  m = m; = V l Limiting molar conductivity :If molar conductivity reaches a limiting value when concentration Kohlrausch law of independent migration of ions approaches zero. C  0, m = m 1. Calculate °m for any electrolyte from ° of individual ions 2. Determine value of dissociation constant for weak electrolytes Strong electrolyte Weak electrolyte m = m – Ac½ (KCl) Ù  = m (acetic acid) Ù°m Limiting molar conductivity of an electrolyte can be represented as Trace the Mind Map sum of individual contribution of anions and cations of the electrolyte    First Level Second Level Third Level °m = v+°++v–°– [ 5  6 ] Ea and proper orientation of the molecules Number of collisions determine the criteria for an effective collision. Rate = PZAB e–Ea/RT per unit volume of P is Steric or Probability reaction mixture Appearance of products or disappearance of factor Rate = ZAB e–Ea/RT reactants over a long time interval. d [P] cy rav = dt = slope en u –d [R] Collision in which molecules collide with sufficient eq rav = = –slope Effective Collision Fr dt kinetic energy and proper orientation for breaking on lisi of bonds and formation of new bonds. Col Number of reacting species taking Rate of change in concentration of part in an elementary reaction colliding reactant/product at a particular time to bring out a reaction. ate rinst= –d[R] =+d[P] R dt dt ge Activation Energy, Ea Sum of powers of ra : Energy required to form an intermediate called activated complex (C) ve concentration of Rate of disappearance of R Ea= Threshold energy - Average Kinetic energy of reacting molecules A the reactants in Decease in concentration of R – [R] Molecularity of a = = the rate law. Time taken t Reaction Collision Theory: Rate of Change in concentration of k = Ae–Ea/RT Ea reaction depends on the Order of a Reaction reactants or products in unit Rate of appearance of P log k = log A – collision frequency and 2.303RT effective collisions. time; Unit : mol L-1 s-1 or atm s-1 Increase in concentration of P + [P] = = Ea T2 –T1 Time taken t log k2 = Rate of Chemical r k1 2.303RT T1T2 [ [ Reaction Fa ate I Arrhenius Equation nf Concentration : Higher the concentration cto of l rs r of reactants, faster is the rate of reaction. To know about more useful books click here ea uen ct c ion ing Temperature : Increases with increase in Integration of differential rate equation to temperature. Becomes almost double with give a relation between concentrations at Integrated Rate 10°C rise. different times and rate constant. Chemical Equation Presence of Catalyst : Increases with a catalyst. Kinetics Surface Area : Greater is the surface area, faster Expression in which reaction is the rate of reaction. Order Integrated Straight Unit rate in given in terms of molar Activation Energy : Lower the activation energy, Rate Law Plot (k) concentration of reactants with faster is the reaction. each term raised to power which 0 kt =[R]0-[R] [R] vs t mol L-1 s-1 Pseudo First may or may not be same as Order Reaction stoichiometric coefficient of In[R] 1 kt =In {[R]-0/[R]} s-1 reactants in a balanced chemical vs t equation. aA + bB  cC + dD Half-life of A Reaction a d [R] Rate = k [A] [B]b = dt Not truly of first order but under certain conditions behave, c d [C] [D] as first order reaction. k= In such reaction, one reactants is in excess. [A]a–[B]b  Acid hydrolysis of ethyl acetate Time in which the concentration of a  Inversion of sugar reactant is reduced to one half of its initial concentration. Unit Order –1 0 mol L s –1 First Order Zero Order 1 s–1 Trace the Mind Map 0.693 [R]0 mol–1L s–1    First Level Second Level Third Level t1/2 = t1/2 = 2 k 2k Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII Oswaal CBSE Mind Maps, BIOLOGY, Class-XII [ 7 To know about more useful books click here 8 ] Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII To know about more useful books click here Oswaal CBSE Mind Maps, BIOLOGY, Class-XII [ 9 To know about more useful books click here 10 ] Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII To know about more useful books click here Oswaal CBSE Mind Maps, BIOLOGY, Class-XII [ 11 To know about more useful books click here 12 ] Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII To know about more useful books click here Oswaal CBSE Mind Maps, BIOLOGY, Class-XII [ 13 To know about more useful books click here 14 ] Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII To know about more useful books click here Oswaal CBSE Mind Maps, BIOLOGY, Class-XII [ 15 To know about more useful books click here 16 ] Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII To know about more useful books click here Oswaal CBSE Mind Maps, BIOLOGY, Class-XII [ 17 To know about more useful books click here 18 ] Oswaal CBSE Mind Maps, CHEMISTRY, Class-XII To know about more useful books click here