BRILLIANT PUBLIC SCHOOL, SITAMARHI (Affiliated up to +2 level to C.B.S.E., New Delhi) Class-XI IIT-JEE Advanced Chemistry Study Package Session: 2014-15 Office: Rajopatti, Dumra Road, Sitamarhi (Bihar), Pin-843301 Ph.06226-252314 , Mobile:9431636758, 9931610902 . Website: www.brilliantpublicschool.com; E-mail: brilliantpublic@yahoo com STUDY PACKAGE Target: IIT-JEE (Advanced) SUBJECT: CHEMISTRY-XI Chapters: 1. Mole Concept 2. Stoichiometry 3. Atomic Structure 4. Chemical Bonding 5. Periodic Table and Representative Element 6. Gaseous State 7. Chemical Equilibrium 8. Ionic Equilibrium 9. Thermodynamics 10. IUPAC Nomenclature 11. Hydrocarbons 12. Nitrogen Family STUDY PACKAGE Target: IIT-JEE(Advanced) SUBJECT: CHEMISTRY-XI TOPIC: 1. MOLE CONCEPT Index: 1. Key Concepts 2. Exercise I 3. Exercise II 4. Exercise III 5. Exercise IV 6. Answer Key 7. 34 Yrs. Que. from IIT-JEE 8. 10 Yrs. Que. from AIEEE CHEMISTRY – STUDY OF MATTER T P E Overview of Chemistry C N O C E L O M 4 2 of 2 e g a P Friends for you used in the sheet. 1. Teacher's advice → : Tips which can enhance your performance. 2. Student's query → : Arbit doubts which are generally developed among students. 3. Boost your confidence → : Some additional information. (cid:2) 4. Dangers → Take care of the general mistakes and crucial points. 2 KEY CONCEPTS T P E C 1. LAWS OF CHEMICAL COMBINATION N O 1.1 Law of conservation of mass [Lavoisier] C E 1.2 Law of constant composition [Proust] L O 1.3 Law of multiple proportions [Dalton] M 4 1.4 Law of reciprocal proportions [Richter] of 2 1.5 Gay Lussac law of combining volumes [Guess Who??] 3 e g a P "Wonder these laws are useful?" "These are no longer useful in chemical calculations now but gives an idea of earlier methods of analysing and relating compounds by mass." 2. MOLE CONCEPT 2.1 Definition of mole : One mole is a collection of that many entities as there are number of atoms exactly in 12 gm of C-12 isotope. or 1 mole = collection of 6.02 × 1023 species 6.02 × 1023 = N = Avogadro's No. A ` 1 mole of atoms is also termed as 1 gm-atom, 1 mole of ions is termed as 1 gm-ion and 1 mole of molecule termed as 1 gm-molecule. 2.2 Methods of Calculations of mole : Given no. (a) If no. of some species is given, then no. of moles = N A Given wt. (b) If weight of a given species is given, then no of moles = (for atoms), Atomic wt. Given wt. or = (for molecules) Molecular wt. (c) If volume of a gas is given along with its temperature (T) and pressure (P) PV use n = RT where R = 0.0821 lit-atm/mol-K (when P is in atmosphere and V is in litre.) 1 mole of any gas at STP occupies 22.4 litre. Gases do not have volume. What is meant by "Volume of gas"? (cid:2) Do not use this expression (PV = nRT) for solids/liquids. How would I calculate moles if volume of a solid is given? 3 2.3 Atomic weight:It is the weight of an atom relative to one twelvth of weight of 1 atom of C-12 T (cid:2) P E C Be clear in the difference between 1 amu and 1 gm. N O C (a) Average atomic weight = ∑ % of isotope X molar mass of isotope. E L (cid:2) O M The % obtained by above expression (used in above expression) is by number (i.e. its a mole%)24 of 4 2.4 Molecular weight : It is the sum of the atomic weight of all the constituent atom. e g a P ∑ n M i i (a) Average molecular weight = ∑ n i where n = no. of moles of any compound and m = molecular mass of any compound. (cid:2) i i Make yourselves clear in the difference between mole% and mass% in question related to above. Shortcut for % determination if average atomic weight is given for X having isotopes XA & XB. Average atomic weight −wt of XB % of XA = × 100 difference in weight of XA & XB Try working out of such a shortcut for XA, XB, XC 3. EMPIRICAL FORMULA, MOLECULAR FORMULA : 3.1 Empirical formula : Formula depicting constituent atom in their simplest ratio. Molecular formula : Formula depicting actual number of atoms in one molecule of the compound 3.2 Relation between the two : Molecular formula = Empirical formula × n Molecular mass n = Empirical Formula mass Check out the importance of each step involved in calculations of empirical formula. 3.3 Vapour density : Vapour density : Ratio of density of vapour to the density of hydrogen at similar pressure and temperature. Molecular mass Vapour density = 2 Can you prove the above expression? Is the above parameter temperature dependent? 4 4. STOICHIOMETRY : Stoichiometry pronounced (“stoy – key – om – e – tree”) is the calculations of T P the quantities of reactants and products involved in a chemical reaction. E C This can be divided into two category. N O (A) Gravimetric analysis C E (B) Volumetric analysis (to be discussed later) L O M 4 4.1 Gravimetric Analysis : 2 of 4.1.1 Methods for solving : 5 e (a) Mole Method  Balance reaction required Pag (b) Factor Label Method  (c) POAC method } Balancing not required but common sense use it with slight caree. (d) Equivalent concept } to be discussed later 5. CONCEPT OF LIMITING REAGENT. 5.1 Limiting Reagent : It is very important concept in chemical calculation. It refers to reactant which is present in minimum stoichiometry quantity for a chemical reaction. It is reactant consumed fully in a chemical reaction. So all calculations related to various products or in sequence of reactions are made on the basis of limiting reagent. (cid:2) It comes into picture when reaction involves two or more reactants. For solving any such reactions, first step is to calculate L.R. 5.2 Calculation of Limiting Reagent : (a) By calculating the required amount by the equation and comparing it with given amount. [Useful when only two reactant are there] (b) By calculating amount of any one product obtained taking each reactant one by one irrespective of other reactants. The one giving least product is limiting reagent. (c) Divide given moles of each reactant by their stoichiometric coefficient, the one with least ratio is limiting reagent. [Useful when number of reactants are more than two.] actualyield ×100 6. PERCENTAGE YIELD : The percentage yield of product = thetheoreticalmaximumyield The actual amount of any limiting reagent consumed in such incomplete reactions is given by [% yield × given moles of limiting reagent] [For reversible reactions] For irreversible reaction with % yield less than 100, the reactants is converted to product (desired) and waste. 7. CONCENTRATION TERMS : 7.1 General concentraction term : Mass (a) Density = , Unit : gm/cc Volume Density of any substance (b) Relative density = Density of refrence substance 5 Density of any substance T P (c) Specific gravity = E Density of water at 4°C C N O Density of vapour at some temperature and pressure C E (d) Vapour density = L Density of H gas at same temperature and pressure O 2 M 4 2 (1) Which of these are temperature dependent. of 6 e g (2) Classify them as w/w, w/v, v/v ratio. a P 7.2 For solutions (homogeneous mixture) : What is solute and solvent in a solution. (cid:2) If the mixture is not homogeneous, then none of them is applicable. Classify each given ratio as w/w, w/v, v/v and comment on their temperature dependence.  w  wt.of solute (a) % by mass   : = × 100 W wt.of solution [X % by mass means 100 gm solution contains X gm solute ; ∴ (100 – X) gm solvent ] w wt.ofsolute (b) %  : = ×100[for liq. solution] V volumeofsolution w [X %   means 100 ml solution contains X gm solute ] V (cid:2) for gases % by volume is same as mole %  v  volumeofsolute (c) %  : = ×100 V volumeofsolution Molesof solute (d) Mole % : = ×100 Totalmoles Molesofsolute (e) Mole fraction (X ) : = a Totalmoles Mole of solute (f) Molarity (M) : = volume of solution in litre Molesofsolute (g) Molality (m) : = Massofsolvent(inkg) Massofsolute Mass of solute (h) Parts per million (ppm) : = ×106 ≅ × 106 Massofsolvent Mass of solution Get yourselves very much confortable in their interconversion. It is very handy. 6 7.3 Some typical concentration terms : T P (a) Oleum : Labelled as '% oleum' (for e.g. 102% oleum), it means maximum amount of H SO E 2 4C that can be obtained from 100 gm of such oleum (mix of H SO and SO ) by adding sufficientN 2 4 3 O water. C E L O Work out what are the maximum and minimum value of the % M 4 2 (b) H O : Labelled as 'volume H O (for e.g. 20V H O ), it means volume of O (in litre) at STPof 2 2 2 2 2 2 2 7 that can be obtained from 1 litre of such a sample when it decomposes according to e g a P 1 H O → H O + O 2 2 2 2 2 Work out a relationship between M and volume H O and remember it 2 2 8. SOME EXPERIMENTAL METHODS : 8.1 For determination of atomic mass : (a) Dulong's and Petit's Law : (cid:2) Atomic weight × specific heat (cal/gm°C) ∝≅ 6.4 Gives approximate atomic weight and is applicable for metals only. Take care of units of specific heat. mv2 B (b) Mass spectrometry : = qvB r d B is the magnitude of magnetic field r = d/2 m is mass of ion, v is velocity of ion, r is the distance where the ions strikes, q is the charge on the ion. 8.2 For molecular mass determination : (a) Victor Maeyer's process : (for volatile substance) Procedure : Some known weight of a volatile substance (w) is taken, converted to vapour and collected over water. The volume of air displaced over water is given (V) and the following expressions are used. w w M = RT or M = RT PV (P−P')V If aq. tension is not given If aq. tension is P' Aqueous tension : Pressure exerted due to water vapours at any given temperature. This comes in picture when any gas is collected over water. Can you guess why? (b) Silver salt method : (for organic acids) Basicity of an acid : No. of replacable H+ atoms in an acid (H contained to more electronegative atom is acidic) Procedure : Some known amount of silver salt (w gm) is heated to obtain w gm of while 1 2 shining residue of silver. Then if the basicity of acid is n, molecular weight of acid would be w 1  2 × ×M =w and molecular weight of acid = M – n(107) 108 n salt 1 salt This is one good practical application of POAC. 7 (c) Chloroplatinate salt method : (for organic bases) T P Lewis acid : electron pair acceptor E C Lewis base :electron pair donor N O Procedure : Some amount of organic base is reacted with H PtCl and forms salt known asC 2 6 E chloroplatinate. If base is denoted by B then salt formed L O (i) with monoacidic base = B H PtCl M 2 2 6 4 (ii) with diacidic base = B (H PtCl ) 2 2 2 6 2 of (iii) with triacidic base = B (H PtCl ) 8 2 2 6 3 e The known amount (w gm) of salt is heated and Pt residue is measured. (w gm). If acidity of base is 'n'ag 1 2 P w 1 M −n(410) then  2 × ×M =w and M = salt 195 n salt 1 base 2 8.3 For % determination of elements in organic compounds : All these methods are applications of POAC Do not remember the formulas, derive them using the concept, its easy. (a) Liebig's method : (Carbon and hydrogen) ∆ (w)OrganicCompound→(w )CO +H O(w ) 1 2 2 2 CuO w 12 % of C = 1× ×100 44 w w 1 % of H = 2 × ×100 18 w where w = wt. of CO produced, w = wt. of H O produced, 1 2 2 2 w = wt. of organic compound taken (b) Duma's method : (for nitrogen) ∆ (w) Organic Compound → N → (P, V, T given) CuO 2 use PV = nRT to calculate moles of N , n. 2 n×28 ∴ % of N = ×100 w w = wt of organic compound taken (c) Kjeldahl's method : (for nitrogen) (w)O.C.+H SO → (NH ) SO NaOH→ NH + H SO → (molarity and volume (V ) 2 4 4 2 4 3 2 4 1 consumed given) MV ×2×14 ⇒ % of N = 1 ×100 w where M = molarity of H SO . 2 4 8