Wednesday, October 16, 2013

Study Material IX Science Ch-3- Atoms and Molecules

The word atom is derived from the Greek word “Atomos” which means indivisible. John Dalton modeled atoms as hard indivisible spheres.
An Indian philosopher Maharishi Kanad, postulated that if we go on dividing matter (padarth), we shall get smaller and smaller particles. Ultimately, a time will come when we shall come across the smallest particles beyond which further division will not be possible. He named these particles Parmanu.
Ancient Greek philosophers – Democritus and Leucippus suggested that if we go on dividing matter, a stage will come when particles obtained cannot be divided further. Democritus called these indivisible particles atoms (meaning indivisible).
How and why elements combine and what happens when they combine. Antoine L. Lavoisier laid the foundation of chemical sciences by establishing two important laws of chemical combination.
(a) The Law of conservation of mass was stated by Antoine L. Lavoisier as” Mass can neither be created nor destroyed in a chemical reaction”
Verification of “Law of Conservation of mass”
 A solution of sodium chloride and silver nitrate are taken separately in the two limbs  of an 'H' shaped tube. The tube is sealed and weighed precisely. The two reactants   are made to react by inverting the tube.

The following reaction takes place.
 AgNO3(aq) + NaCl (aq) à AgCl (s) + NaNO3 (aq)
 The whole tube is kept undisturbed for sometime so that the reaction is complete.  When the tube is weighed again it is observed that:   Weight before the reaction = Weight after the reaction
(b) The law of constant proportions which is also known as the law of definite proportions was stated by Proust as “In a chemical substance the elements are always present in definite proportions by mass”.
E.g. In a compound such as water, the ratio of the mass of hydrogen to the mass of oxygen
is always 1:8, whatever the source of water. Thus, if 9 g of water is decomposed, 1 g of hydrogen and 8 g of oxygen are always obtained.
According to Dalton’s atomic theory, all matter, whether an element, a compound or a mixture is composed of small particles called atoms. The postulates of this theory may be stated as follows:
(i) All matter is made of very tiny particles called atoms.
(ii) Atoms are indivisible particles, which cannot be created or destroyed in a chemical reaction.
(iii) Atoms of a given element are identical in mass and chemical properties.
(iv) Atoms of different elements have different masses and chemical properties.
(v) Atoms combine in the ratio of small whole numbers to form compounds.
(vi) The relative number and kinds of atoms are constant in a given compound

The introduction of matter wave concept by de Broglie, the principle of uncertainty by Heisenberg etc., paved the way for modern atomic theory
MODERN ATOMIC THEORY - Modern atomic theory are as follows.
v Atom is considered to be a divisible particle.
v Atoms of the same element may not be similar in all respects.                             eg: Isotopes (17Cl35,17Cl37 )
v  Atoms of different elements may be similar in some respects eg. Isobars (18Ar 40 , 20Ca 40 )
v  Atom is the smallest particle which takes part in chemical reactions.
v The ratio of atoms in a molecule may be fi xed and integral but may not be simple e.g., C12H22O11 is not a simple ratio (Sucrose)
v Atoms of one element can be changed into atoms of other element by transmutation.
v The mass of an atom can be converted into energy. This is in accordance with Einstein’s equation E = mc2
Atom: It is the smallest particle of an element which may or may not have independent existence. The atoms of certain elements such as hydrogen, oxygen, nitrogen, etc .do not have independent existence whereas atoms of helium, neon, argon, etc. do have independent existence. Thus we can say that all elements are composed of atoms.
IUPAC (International Union of Pure and Applied Chemistry) approves names of elements. Many of the symbols are the first one or two letters of the element’s name in English. The first letter of a symbol is always written as a capital letter (uppercase) and the second letter as a small letter (lowercase)
For example :  (i) hydrogen, H (ii) aluminium, Al and not AL (iii) cobalt, Co and not CO.
Symbols of some elements are formed from the first letter of the name and a letter, appearing later in the name. Examples are: (i) chlorine, Cl, (ii) zinc, Zn etc.
Other symbols have been taken from the names of elements in Latin, German or Greek. For example, the symbol of iron is Fe from its Latin name ferrum, sodium is Na from natrium, potassium is K from kalium. Therefore, each element has a name and a unique chemical symbol.
Molecule: A molecule is the smallest or the simplest structural unit of an element (or) a compound which contains one (or) more atoms. It retains the characteristics of an element. A molecule can exist freely and it is a combined form of bonded units whereas an atom is a singular smallest form of non bonded unit.
Molecules are of two types, namely homo atomic molecules and hetero atomic molecules.
Homo atomic molecules: These are the molecules which are made up of atoms of the same element. For example hydrogen gas consists of two atoms of hydrogen (H2).Similarly oxygen gas consists of two atoms of oxygen (O2).
HETERO ATOMIC MOLECULES : The hetero atomic molecules are made up of atoms of different elements. They are also classified as diatomic, triatomic, or polyatomic molecules depending upon the number of atoms present. H2O, NH3, CH4, etc., are the examples for hetero atomic molecules.
Atomicity:   The number of atoms present in one molecule of an element is called the atomicity of an element. Depending upon the number of atoms in one molecule of an element, molecules are classified into monoatomic, diatomic, triatomic or poly atomic molecules containing one, two, three, or more than three atoms respectively.
Mon atomic molecules: Helium (He) Neon (Ne) Metals
Di atomic molecules:   Hydrogen H2 Chlorine Cl2
Tri atomic molecules: Ozone (O3)
Poly atomic molecules: phosphorous P4 Sulphur S8
Atomicity = Molecular Mass/Atomic mass
Isotopes  These are the atoms of same element with same atomic number (Z) but different mass number (A). Example (17Cl35,17Cl37 )
Isobars   These are the Atoms of the different element with same mass number but different atomic number. Example (18Ar40, 20Ca 40 )
 Isotones These are the atoms of different elements with same number of neutrons Example : (6C13, 7N14 )
AVOGADRO’S HYPOTHESIS  : Amedeo Avogadro put forward hypothesis and is based on the relation between number of molecules and volume of gases that is “volume of a gas at a given temperature and pressure is proportional to the number of particles”.
Avogadro’s Law: Equal volumes of all gases under the same conditions of temperature and pressure. contain the equal number of molecules.
 (a) Find the atomicity of chlorine if its atomic mass is 35.5 and its molecular mass is 71 
(b) Find the atomicity of ozone if its atomic mass is 16 and its molecular mass is 48
An ion is a charged particle and can be negatively or positively charged.
A negatively charged ion is called an ‘anion’ and the positively charged ion, a ‘cation’. For example, sodium chloride  (NaCl). Its constituent particles are positively charged sodium ions (Na+) and negatively charged chloride ions (Cl–).
Ions may consist of a single charged atom or a group of atoms that have a net charge on them.
A group of atoms carrying a charge is known as a polyatomic ion e.g. Calcium oxide (Ca+2 O-2)
Ionic compound A compound which consist of ions is called ionic compound like NaCl (Na+1  Cl-1)
Relative atomic mass of an element is the ratio of mass of one atom of element to the 1/12th  part of mass of one atom of carbon. Relative atomic mass is a pure ratio and has no unit. If the atomic mass of an element is expressed in grams, it is known as gram atomic mass.
e.g., Gram atomic mass of hydrogen = 1g ;             
Gram atomic mass of carbon = 12g
Gram atomic mass of nitrogen = 14g ;                     
Gram atomic mass of oxygen = 16g
Atomic mass is expressed in atomic mass unit (amu). One atomic mass unit is defi ned as 1/12th part of the mass of one atom of carbon.
Chemical Formulae: The chemical formula is a symbolic representation of a compound of its composition.
Valency : The combining power (or capacity) of an element is known as its valency. Valency can be used to find out how the atoms of an element will combine with the atom(s) of  another element to form a chemical compound.
RELATIVE MOLECULAR MASS (RMM) : The relative molecular mass of an element or a compound is the ratio of mass of one molecule of the element or a compound to the mass of 1/12 th part of mass of one atom of carbon. Relative Molecular mass is a pure ratio and has no unit. If the molecular mass of a given substance is expressed in gram, it is known as gram molecular mass of that substance.
Molecular mass is the sum of the masses of all the atoms present in one molecule of the compound or an element.
Test your numerical skill:
Problem:    Find the gram molecular mass of water (H2O)
Solution:  Þ 2(H) = 2 x 1 = 2  and   1(O) = 1 x 16 = 16  
Gram molecular mass of H2O = 2 + 16 = 18g
Problem:  Find the gram molecular mass of carbon dioxide
Solution:  Þ  (CO2) 1(C) = 1 x 12 = 12 and  2(O) = 2 x 16 = 32
 Gram molecular mass of CO2 = 12 + 32 = 44 g
While performing a reaction, to know the number. of atoms (or) molecules involved, the concept of mole was introduced. The quantity of a substance is expressed in terms of mole.
Definition of mole :  Mole is defined as the amount of substance that contains as many specifi ed elementary particles as the number of atoms in 12g of carbon-12 isotope.
One mole is also defined as the amount of substance which contains Avogadro number (6.023 x 1023) of particles.
Avogadro number: Number of atoms or molecules or ions present in one mole of a substance is called Avogadro number. Its value is 6.023 x 1023.
Therefore, one mole of any substance =  6.023 x 1023 particles may be atoms, molecules, ions
For  e g.  One mole of oxygen atoms represents 6.023 x 1023 atoms of oxygen and 5 moles of oxygen atoms contain 5 x 6.023x1023 atoms of oxygen.
To find the number of moles, the following formulae are useful
(a) Number of moles = Given Mass /atomic mass = Given Mass /molecular mass
(b) Number of moles = No.of atom/(6.023 x 1023) = No. of molecules/(6.023 x 1023)

1. When the mass of the substance is given:  Use this formula : Number of moles = given mass/ atomic mass
(a). Calculate the number of moles in  (i) 81g of aluminium ii) 4.6g sodium  (iii) 5.1g of Ammonia  (iv) 90g of water  (v) 2g of NaOH
Solution:   (i) Number of moles of aluminium = given mass of aluminium / atomic mass of aluminium = 81/27 = 3 moles of aluminium [Rest Question do yourself]
(b) Calculate the mass of 0.5 mole of iron
Solution: mass = atomic mass x number of moles = 55.9 x 0.5 = 27.95 g
Do yourself :  Find the mass of 2.5 mole of oxygen atoms [ Mass = molecular mass x number of moles]
2. Calculation of number of particles when the mass of the substance is given:
 Number of particles =( Avogadro number x given mass)/gram molecular mass
Problem: Calculate the number. of molecules in 11g of CO2
Solution: gram molecular mass of CO2 = 44g
Number of molecules = (6.023 x 1023 x 11) / 44 = 1.51 x 1023 molecules
Do yourself: Calculate the number of molecules in 360g of glucose
3. Calculation of mass when number of particles of a substance is given:
Mass of a substance = (gram molecular mass x number of particles)/6.023 x 1023
Problem: Calculate the mass of 18.069 x 1023 molecules of SO2
Solution: Gram molecular mass SO2 = 64gm
The mass of 18.069 x 1023 molecules of SO2 = (64x18.069 x 1023)/ (6.023 x 1023) = 192 g
Do yourself: (a) Calculate the mass of glucose in 2 x 1024 molecules (b) Calculate the mass of 12.046 x 1023 molecules in CaO
4. Calculation of number of moles when you are given number of molecules:
Problem:  Calculate the number moles for a substance containing 3.0115 x 1023 molecules in it.
Solution: Number of moles = [Number of molecules/(6.023 x 1023)]
                                             = ( 3.0115 x 1023)/( 3.0115 x 1023) =0.5 moles
Do yourself: (a) Calculate number of moles in 12.046x 1022 atoms of copper (b) Calculate the number of moles in 24.092 x 1022 molecules of water.
More to solve:
Problem: Calculate the number of aluminum ions present in 0.051 g of aluminum oxide. (Hint: The mass of an ion is the same as that of an atom of the same element. Atomic mass of Al=27 u)
Solution: Mass of the 1 mole of Al2 O3  = 2x27 + 3x16 = 102gm
The number of ions present in 102 gm of aluminum oxide = 6.023 x 1023 ion
The number of ions present in 0.051g of aluminum oxide 
= (6.023 x 1023 ion x 0.051g)/ 102 gm 
= 6.023 x 1023 ion x0.0005 = 3.0115 x 1020 ions
In Al2 O3, Aluminium and oxygen are in ratio 2:3
So, the number of aluminum ions present (Al3+) in 0.051g of aluminum oxide = 2 x 3.0115 x 1020 ions =6.023 x 1020 ion

Problem: What is the percent composition of sulfuric acid?

Solution: Find the atomic masses of all the elements and multiply each mass by the number of atoms in the compound, then add. 
H: 1.00 × 2 = 2.00 
S: 32.1 
O: 16.0 × 4 = 64.0 
2.00 + 32.1 + 64.0 = 98.1 grams 
Take the masses of each element and divide it by the total mass. Change the final answer to a percent. 
H: 2.00 ÷ 98.1= 0.020 = 2.0% S: 32.1 ÷ 98.1= 0.327 = 32.7% O: 64.0 ÷ 98.1= 0.652 = 65.2% 
There is 2.0% of hydrogen, 32.7% of sulfur, and 65.2% of oxygen in Sulfuric acid.

Volume occupied by one mole of any gas at STP is called molar volume. Its value is 22.4 litres 22.4 litres of any gas contains 6.023 x 1023 molecules.

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