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1 Some Basic Concepts of Chemistry Some Basic Concepts of Chemistry 1 1 Some Basic Concepts of Chemistry Matter – The three states of matter can be inter-converted by Anything which occupies space, has mass and which can be changing the conditions of temperature and pressure as felt by our senses is called matter. follows : Ev Liq Classification of Matter : Co GasGVa ap as uefacti n po orat tion ndensa – tion Physical Classification : io riza at io on n o tion tion Matter lim ndensa or r Deposi Co Sub or Solid Liquid Solid Liquid Solids Liquids Gases Definite shape Definite No definite Melting or Fusion Freezing or Crystallization and volume volume but no shape and Endothermic state changes Exothermic state changes definite shape volume – Chemical Classification : Matter Pure Substances Mixtures Fixed ratio of masses No fixed ratio of of constituents masses of constituents Elements Compounds Homogeneous Heterogeneous Consists of only one Composed of two Uniform composition Composition is not kind of atoms or more atoms of throughout uniform throughout different elements Solids at room temperature, high density, possess lustre, Metals good conductors of heat and Organic Inorganic electricity Compounds Compounds Originally obtained from Usually obtained from Brittle, do not possess animals and plants, contain minerals and rocks, do not lustre, poor conductors Non-metals carbon and few other elements contain C–H bonds of heat and electricity like H, O, S, N, X (halogens), Possess characteristics etc. having C–H bonds Metalloids of both metals and non- metals Units and Measurements Mass m kilogram kg Fundamental Units : The units which can neither be derived Time t second s from one another nor can be further resolved into any other Temperature T kelvin K units are called fundamental units or basic units. Electric current I ampere A The SI system has seven basic units : Luminous intensity Iv candela cd Physical quantity Symbol for Name of Symbol quantity unit for unit Amount of substance n mole mol Derived Units : The units for other quantities which can be Length l metre m derived from fundamental units are called derived units. 2 Chemistry – Physical Symbol Unit (S.I.) Symbol This can be done by method called factor label method or Quantity unit factor method. – Area A Square metre m2 This is done by using conversion factor (C.F.), which is a factor equal to one that converts a quantity in one unit Volume V Cubic metre m3 to the same quantity in another unit. Some conversion –3 Density r Kilogram per kg m factors are as follows : cubic metre Velocity v Metre per second ms–1 Conversion Factors –8 –10 –1 2 Force F Newton N = kg m s–2 1 angstrom (Å) = 10 cm = 10 m = 10 nm = 10 pm 1 inch = 2.54 cm Pressure P Pascal Pa = N m–2 1 cm = 0.3937 inch Energy E Joule J = N m 1 metre = 39.37 inch = kg m2s–2 1 km = 0.621 mile Frequency u Hertz Hz or s–1 1kg = 2.20 pounds (lb) Electric q Coulomb C = A s 1g = 0.0353 ounce charge –1 1 pound = 453.6 g Potential E° Volt V = J C –24 –27 –1 –1 1 atomic mass unit (amu) = 1.6605 × 10 g = 1.6605 × 10 kg difference = J A s –3 –10 2 –3 –1 ≡ 1.492 × 10 erg = 1.492 × 10 J = kg m s A = 3.564 × 1011 cal = 9.310 × 108 eV Precision : It refers to the closeness of various measurements for the same quantity. = 931.48 MeV 1 atmosphere (atm) = 760 torr = 760 mm Hg = 76 cm Hg Accuracy : It is the agreement of a particular value to the 5 true value of the result. = 1.01325 × 10 Pa 7 Significant figures : Significant figures are those digits in 1 calorie (cal) = 4.18 × 10 erg = 4.18 J a measured number that include all certain digits and one = 2.613 × 1019 eV doubtful digit. 1 erg = 10–7 J = 2.389 × 10–8 cal = 6.242 × 1011 eV 4 Rules for determining the number of significant figures : 1 faraday (F) = 9.6487 × 10 coulomb – All non-zero digits are significant. 1 dyne (dyne) = 10–5 N – A zero becomes significant when it comes in between 1 joule = 107 erg = 0.2390 cal two non-zero numbers. 1 litre = 1000 cc = 1000 mL = 1 dm3 – Zeros at the beginning of a number are not significant. = 10–3 m3 – All zeros to the right of a number are significant. 1 coulomb (coul) = 2.9979 × 109 esu Scientific Notation : Numbers are represented in the term 1 curie (Ci) = 3.7 × 1010 disintegrations sec–1 N × 10n (where N lies between 1 to 10 and n is the exponent 1 electron volt (eV) = 1.6021 × 10–12 erg = 1.6021 × 10–19 J having positive or negative value). = 3.827 × 10–20 cal Dimensional Analysis : The expression of any particular –1 quantity in terms of fundamental quantity is known as = 23.06 kcal mol –10 dimensional analysis. 1 electrostatic unit (esu) = 3.33564 × 10 coul Illustration 1 (ii) 15.15 × 10–12 m or 1.515 × 10–11 m (a) Convert the following into basic units : –6 –6 (i) 28.7 pm (ii) 15.15 pm (iii) 25365 mg (iii) 25365 mg = 25365 × 10 kg [ 1 mg = 10 kg] –2 (NCERT Exemplar) = 2.5365 × 10 kg (b) How many significant figures are there in each of the (b) (i) two (ii) three following numbers? (iii) four (iv) two –3 (i) 17 (ii) 103 (iii) 1.035 (iv) 0.0010 (c) (i) 0.0048 = 4.8 × 10 5 (c) Express the following in the scientific notation. (ii) 234200 = 2.342 × 10 3 (i) 0.0048 (ii) 234200 (iii) 8008 (iv) 500.0 (iii) 8008 = 8.008 × 10 2 Soln.: (a) (i) 28.7 × 10–12 m or 2.87 × 10–11 m (iv) 500.0 = 5.000 × 10 Some Basic Concepts of Chemistry 3 Laws of Chemical Combination with the fixed weight of the other, bear a simple whole number ratio to one another. Law of Conservation of Mass : It states that during any physical or chemical change, total mass of products is equal Law of Reciprocal Proportions : It states that when two elements combine separately with a fixed mass of third to the total mass of reactants. element, then the ratio between their masses in which they Law of Definite or Constant Proportions : It states that a combine will be either same or simple multiple of the ratio compound always contains the same elements combined in in which they combine with each other. the same definite proportion by weight. Gay Lussac’s Law of Combining Volumes : It states that Law of Multiple Proportions : It states that when two or under similar conditions of temperature and pressure, more elements combine to form two or more compounds, whenever gases react together, the volumes of the reacting the different weights of one of the elements which combine gases as well as products bear a simple whole number ratio. Illustrations 2 A and B combines with each other to form X, Y, and Z. The 3 One volume of nitrogen combines with three volumes of following reactions take place in the formation of X, Y and Z. hydrogen to form two volumes of ammonia. 0.6 g A + 0.8 g B → 1.4 g X (a) What volumes of nitrogen and hydrogen are required to 9.0 g A + 24.0 g B → 33.0 g Y form 50 L of ammonia? 40.0 g A + 160.0 g B → 200.0 g Z (b) What volume of nitrogen will react completely with 30 L of Which law is illustrated by these data? hydrogen? What volume of ammonia will be formed? Soln.: On the basis of reactions given, 1 g of A reacts with Soln.: (a) N2 + 3H2 → 2NH3 different amounts of B, which are as follows : x L 3x L 2x L B 08. B 24.0 Given, 2x L = 50 L ⇒ x = 25 For X ⇒ = = 1.33 g; For Y ⇒ = = 2.66 g \ required volume of nitrogen = 25 L A 06. A 90. and volume of hydrogen required = 3 × 25 L = 75 L B 160 For Z ⇒ = = 4.0 g (b) Given, A 40 30 Thus, ratio of different amounts ofB , which react with 1 g of A. 3xx L = 30 L ⇒= = 10 = 1.33 : 2.66 : 4.0 = 1 : 2 : 3 3 Since, this is a simple ratio, so the above results illustrates law \ Required volume of nitrogen = x L = 10 L of multiple proportions. and volume of ammonia formed = 2x L = 2 × 10 L = 20 L Dalton's Atomic Theory It does not explain Gay-Lussac's law of combining gaseous Main postulates of Dalton's theory are as follows : volumes. Matter is made up of small indivisible particles called atoms. It does not give an idea about isotopes and isobars. Atoms can neither be created nor destroyed. It fails to explain why atoms of different elements show Atoms of a given element are identical in properties. different properties like mass, size, etc. Atoms of different elements differ in properties. It does not explain the difference between an atom and a Atoms of different elements combine in a fixed ratio to form molecule. molecule of a compound. Avogadro's Law : It states that equal volume of all gases Limitations of Dalton's Atomic Theory contain equal number of molecules at same temperature and pressure. It fails to explain the cause of chemical combination. Self Test 1 1. Which one of the following represents smallest quantity? B and C is 1 : 3 : 5.
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