A) CONCEPT 1. Classification of Substances

www.tiwariacademy.in UNIT 1: SOME BASIC CONCEPTS OF CHEMISTRY

Concept Wise Handouts

Key Concepts

I. Classification of Substances II. SI Base units & Significant figures III. Laws of Chemical Combination IV. Mole Concept V. Concentration Terms

CONCEPT 1. Classification of Substances

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Mixtures Substances which have been combined such that Matter each substance retains its own chemical identity. Everything that has May be separated into pure substances mass and occupies space Three states: a solid, Pure Substances a liquid, or a gas. The same composition throughout Composition stays constant during a change of phase (going from a solid to a liquid to a gas or vice-versa)

Homogeneous Mixtures The same composition throughout. Components are indistinguishable. Composition can be varied. Homogeneous mixtures are solutions. MIXTURES Heterogeneous Mixtures Not the same composition throughout. Components are distinguishable. Composition can be varied.

Elements There are 88 naturally occurring elements. There are 118 current elements in the periodic table. PURE SUBSTANCE Compounds Contain two or more elements combined in definite proportions

ELEMENT COMPOUND

Metals Solids (except liquid mercury) Acids Good conductors of heat and Turn blue litmus paper red electricity

Metalloids Solids May conduct electricity. Neutral Substances Poor conductors of heat. No effect on litmus paper

Non-Metals Some gases, some solids, Bases one liquid (bromine). Turn red litmus paper blue Poor conductors of heat and electricity.

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Focus on free education www.tiwariacademy.in CONCEPT 2. SI Base units & Significant figures

S I BASE UNITS

Quantity Name Symbol

Length meter m

Mass kilogram kg

Time second s

Thermodynamic kelvin K temperature

Amount of Substance Mole Mol

S I DERIVED UNITS

Derived Quantity Name Symbol

Area square meter m2

Volume cubic meter m3

Speed ,velocity meter per second ms-1 acceleration meter per second square ms-2

Wave number reciprocal meter m-1

Rules for determining the number of significant figures i) All non-zero digits are significant ii) Zeros preceding the first non-zero digit are not significant iii) Zeros between two non-zero digits are significant. iv) Zeros at the end or right of the number are significant provided they are on the right side of the decimal point. But, if otherwise, the zeros are not significant.

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Focus on free education www.tiwariacademy.in CONCEPT 3. Laws of Chemical Combination a) Law of conservation of Mass [ Antoine Lavoisier]

MassReactant + MassReactant = MassProduct = MassProduct

Activity : Melting Ice – . Place a glass measuring cup of water, with a chunk of floating in it. . Point out the fact that most of the ice sits under the water, and only a small amount sticks up, above the surface. . Ask the students , what they thought was going to happen to the level of water, in the bowl, as the ice melted. Would the water level rise, stay the same, or go down ? They all will guess the water level would rise. . Wait & watch . After the ice melts completely , students can verify the Law of Conservation of Mass.

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Focus on free education www.tiwariacademy.in b) Law of definite proportion [Joseph Proust] – A given compound always contains elements in a certain proportion by mass.

Investigative activity Apparatus 0.1 M silver nitrate 0.1 M sodium chloride 0.1 M lead nitrate 0.1 M sodium iodide 0.1 M iron (III) chloride 0.1 M sodium hydroxide 9 large test tubes & 3 pipettes Reactions to be performed . Reaction 1: Prepare three test tubes with 5 ml, 10 ml and 15 ml of silver nitrate respectively. Using a clean pipette add 5 ml of sodium chloride to each one and observe what happens. . Reaction 2: Prepare three test tubes with 5 ml, 10 ml and 15 ml of lead nitrate respectively. Using a clean pipette add 5 ml of sodium iodide to each one and observe what happens. Write a balanced equation for this reaction. . Reaction 3: Prepare three test tubes with 5 ml, 10 ml and 15 ml of sodium hydroxide respectively. Add 5 ml of iron(III) chloride to each one and observe what happens. Observation & Conclusion Regardless of the amount of reactants added, the same products, with the same compositions, are formed (i.e. the precipitate observed in the reactions). However, if the reactants are not added in the correct ratios, there will be unreacted reactants that will remain in the final solution, together with the products formed. www.tiwariacademy.com

Focus on free education www.tiwariacademy.in iii) Law of Multiple Proportion [ John Dalton ]

When the same two elements combine to form more than one compound, the ratios of the mass of one element in the first compound to its mass in the second compound, (as it combines with the same mass of the other element), can always be expressed as ratios of small whole numbers( ex: 1:3 or 2:5).

For example Hydrogen and Oxygen combine to form water H2O and hydrogen peroxide

H2O2.

Two atoms of hydrogen combine with one atom of oxygen in the case of water, while two atoms of hydrogen combine with two atoms of oxygen in the case of hydrogen peroxide. The ratio of oxygen atoms combining with a fixed number of hydrogen atoms in these two compounds is 1:2.

In terms of masses also, every 2.016 g of hydrogen ( g.at. mass of hydrogen is 1.008g) combines with 15.999 g of oxygen to form water and 31.998g of oxygen to form hydrogen peroxide. Hence the ratio is 15.999 : 31.998 or 1:2 which is a simple ratio.

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Focus on free education www.tiwariacademy.in iv) Avogadro’s Law : “equal volumes of all gases under the same conditions of pressure and temperature contain the same number of molecules."

At standard temperature and pressure, 1 mole of the gas will occupy 22.4L and will contain 6.022 x 1023 particles of the matter.

“At STP 6.022 x 1023 particles of any gas will occupy 22.4L”

The Avogadro constant is named after the early nineteenth century Italian scientist Amedeo Avogadro.

v) Gay Lussac’s Law

Gay-Lussac's law is an ideal gas law where at constant volume, the pressure of anideal gas is directly proportional to its absolute temperature.

Pi/Ti = Pf/Tf where

Pi = initial pressure

Ti = initial temperature

Pf = final pressure

Tf = final temperature

The volume of gases taking part in a chemical reaction show simple whole number ratios to one another when those volumes are measured at the same temperature and pressure.

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Focus on free education www.tiwariacademy.in CONCEPT 4. Mole Concept

The mole (mol) is the amount of a substance that contains as many elementary entities as there are atoms in exactly 12.00 grams of 12C

I MOLE ≡ 6.O22 x 10 23 particles

Substance > Element ║ Compound Particles > Atom ║ Molecule

Ex. > ELEMENT - SODIUM - Na I MOLE > 23 u / 23g / 6.O22 x 10 23 atoms of sodium

Ex. > COMPOUND- WATER - H2O I MOLE > 18 u / 18 g / 6.O22 x 10 23 molecules of water

S.No. Symbol / formula of atom Atomic / 1mole Avogadro no. Molar mass / molecule molecular mass ( in g) ( g mol -1) ( u) 1. O 16 u 16 g 6.022 x 1023 atoms 16 g mol -1 23 -1 2. N2 28 u 28 g 6.022 x 10 molecules 28 g mol 3. HCl 36.5 u 36.5 g 6.022 x 1023 molecules 36.5 g mol - 1

www.tiwariacademy.com Focus on free education www.tiwariacademy.in GRAM MOLECULAR MASS Gram molecular mass is the mass in grams of one mole of a molecular substance.

Ex: The molecular mass of N2 is 28, so the gram molecular mass of N2 is 28 g.

ATOMIC MASS UNIT An atomic mass unit or amu is one twelfth of the mass of an unbound atom of carbon-12. It is a unit of mass used to express atomic masses and molecular masses.

Also Known As: Unified Atomic Mass Unit (u).

Ex: i) Convert 35 g of Al into mol. MASS A: Molar mass of Al= 27 g 27 g = 1mol 1mol = 35 g x ------Molarmass / 1mol 27 g = 1.3 mol of Al

1mol / Molar mass ii) How many grams of SiO2 are present in 0.8 mol ?

A: Molar mass of SiO2 = 60.1 g 1 mol = 60.1 g

60.1g of SiO2 MOLE = 0.8 mol of SiO2 x ------1mol of SiO2

= 48.1 g SiO2

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MOLE Ex . How many mol of CO2 are present in 55.5 L ?

A: 22.4 L = 1mol 1mol / 22.4 L 1mol = 55.5 L x ----- 22.4 L / 1mol 22.4 L = 2.48 mol of CO2.

VOLUME AT STP

MOLE Ex Calculate number of molecules in 200 g of N2O. Molar mass of N2O = 44 g

i ) to find number of moles:- 23 1mol / 6.02 X 10 44 g = 1 mol particles 6.02 X 10 23 particles / 1mol 1mol = 200 g x ------44.0 g

= 4.55 mol of N2O

ii) to find number of molecules 23 Number of 1 mol =6.02 x 10 molecules representative paticles 23 6.02 x 10 molecules N2O = ------1/ 4.55

24 = 2.74 x 10 molecules N2O

www.tiwariacademy.com Focus on free education www.tiwariacademy.in CONCEPT 5. Concentration terms

MOLARITY tells us the number of moles of solute in exactly one liter of a solution. (Note that molarity is spelled with an "r" and is represented by a capital M.)

We need two pieces of information to calculate the molarity of a solute in a solution:

 The moles of solute present in the solution.

 The volume of solution (in liters) containing the solute.

To calculate molarity we use the equation:

MOLALITY is the number of moles of solute dissolved in each kilogram of solvent. The unit for molality is a lower case m. Molality is used when the temperature varies during an experiment. Molarity will change slightly as the temperature changes because volume changes with temperature. The mass and moles in molality do not change with temperature. The equation for molality is:

MOLE FRACTION is the number of moles of one component divided by the total number of moles in solution. This concentration is similar to pph, but is based on moles instead of grams. There is no unit for mole fraction. The equation for mole fraction is :