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-_, | Short Formula (Chemistry), , Heisenberg’s uncertainty principle :, Ap > if ny a AX.A’ 5, Ax.Ap> 4> oF mAx.Av> 4 or xAV> ZO, , Quantum Numbers :, , * Principal quantum number (n) = 1, 2, 3, 4 .... to 2,, “ x , — oh, * Orbital angular momentum of electron in any orbit = Dn, * Azimuthal quantum number (¢) = 0, 1, ..... to (n-1)., * Number of orbitals in a subshell = 2¢ + 1, * Maximum number of electrons in particular subshell = 2 x (2/ + 1), * q hoe net, Orbital angular momentum L = On LUG =n [e+ ss, STOICHIOMETRY, Mi f it f li it, eo Relative atomic mass (R.A.M) = ——e— rrr = Total Number of nucleons, qo *mass of one carbonatom, o Y-map, ¢ at Volume at STP, = a, t i, + mol. wt.| | x mol. wt., + At. wt. x At. wt., Density:, . | density of the substance, Specific gravity = “Gensity of water at 4°C, For gases:, , Molar mass of the gas PM, , Molar volume of the gas = Bi rer, , Absolute density (mass/volume) = RT, , das PMgasier — Myas Mg, Vapour density V.D= dy, = PMy, et & Ms, =>, , , , , , , , Mog = 2 V.D.
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| Short Formula (Chemistry), , Mx1000, 6. Molarity into Molality m = 4999, 000 p—-MM,, , M, and M, are molar masses of solvent and solute. p is density of solution (gm/mL), M = Molarity (mole/lit.), m = Molality (mole/kg), x, = Mole fraction of solvent, x, = Mole fraction of solute, Average/Mean atomic mass :, , 4X4 FAK 2 tov FAX, 100, Mean molar mass or molecular mass :, , AS, , nyM, +n2M, +, 0 ny+ng+., , , , Calculation of individual oxidation number :, Formula : Oxidation Number = number of electrons in the valence shell — number of electrons left after bonding, , Concept of Equivalent weight/Mass :, , Atomic weight, , For elements, equivalent weight (E) = Valency -factor, , M, , For acid/base, E=———___, Basicity/ Acidity, , Where M = Molar mass, M, , For O.A/R.A, —E=——_—___—__—_—_, 10. of moles of e~ gained/lost, , , , Atomic or moleculear weight, , Equivalent weight (E) = TF, , (v.f. = valency factor), , Concept of number of equivalents :, , Wt w_WwW, No. of equivalents of solute = Eq. wt. = Mn, , No. of equivalents of solute = No. of moles of solute * v.f., , Normality (N) :, , Number of equivalents of solute, , Normality (N) = ~Vojume of solution (in litres), , Normality = Molarity x v.f., , Calculation of valency Factor:, n-factor of acid = basicity = no. of H* ion(s) furnished per molecule of the acid., n-factor of base = acidity = no. of OH" ion(s) furnised by the base per molecule., At equivalence point :, , NV, = NAV,, , n.M,V, = n.MLV,,, , , , "
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| Short Formula (Chemistry), , Volume strength of H,0,:, 20V H,O, means one litre of this sample of H,O, on decomposition gives 20 It. of O, gas at S.T.P., , Valume, strength of HO., , Normality of H,0, (N) = ee, , Volume strength of H,O,, , Molarity of H,O, (M) = 11.2, Measurement of Hardness :, , mass of CaCO,, Total mass of water, , Hardness in ppm = 3, , Calculation of available chlorine from a sample of bleaching powder :, , 3.55xxx V(mL), %ofCl,= yg) ___ Where x= molarity of hypo solution and v = mL.. of hypo solution used in titration., , Temperature Scale :, , C-O _ K-273 _ F-32. ___R-R(O), , 700-0 373-273 212-32" R(100) RO) where R = Temp. on unknown scale., , , , Boyle’s law and measurement of pressure :, 1, , At constant temperature, Vo P, PY, = PW,, Charles law :, At constant Vat Mi Me, constant pressure, or a, , “ Tp, , Gay-lussac’s law:, , At constant volume, Pat, Py Py, , 7, ~ T, ~ temp on absolute scale, 1 2, , Ideal gas Equation :, PV=nRT, , d, pv= RT ore = © RTorPm=dRT, m m, Daltons law of partial pressure :, MRT Bete, v v, Total pressure = P, + P,+P,+...., , , , PR
