NEET Chemistry Mole Concept Revision Notes

Chemistry
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Download NEET Chemistry Mole Concept Revision Notes in PDF format. All Revision notes for Full Course Mole Concept have been designed as per the latest syllabus and updated chapters given in your textbook for Mole Concept in Full Course. Our teachers have designed these concept notes for the benefit of Full Course students. You should use these chapter wise notes for revision on daily basis. These study notes can also be used for learning each chapter and its important and difficult topics or revision just before your exams to help you get better scores in upcoming examinations, You can also use Printable notes for Full Course Mole Concept for faster revision of difficult topics and get higher rank. After reading these notes also refer to MCQ questions for Full Course Mole Concept given on studiestoday

Revision Notes for Full Course Mole Concept Mole Concept

Full Course Mole Concept students should refer to the following concepts and notes for Mole Concept in Full Course. These exam notes for Full Course Mole Concept will be very useful for upcoming class tests and examinations and help you to score good marks

Mole Concept Notes Full Course Mole Concept

Matter:
 
Anything that exhibits inertia is called matter.
The quantity of matter is its mass.
 
Classification of Matter:-
 
Based on chemical composition of various substances..
 
NEET Chemistry Mole Concept Revision Notes
 
 
Measurement of Temperature
 
Three scales of temperature
 
• Kelvin scale (K)
• Degree Celsius scale (oC)
• Degree Fahrenheit scale (oF)
Relations between the scales:
• oF = 9/5(oC) + 32
• K = oC + 273
0 K temperatures is called absolute zero.
 
Dalton’s Atomic Theory:
 
• Every matter consists of indivisible atoms.
• Atoms can neither be created nor destroyed.
• Atoms of a given element are identical in properties
• Atoms of different elements differ in properties.
• Atoms of different elements combine in a fixed ratio to form molecule of a compound.
 
Laws of Chemical Combination:
 
Law of conservation of mass:
“For any chemical change total mass of active reactants are always equal to the mass of the product formed”
 
Law of constant proportions:
“A chemical compound always contains same elements in definite proportion by mass and it does
not depend on the source of compound”.
 
Law of multiple proportions:
“When two elements combine to form two or more than two different compounds then the different masses of one element B which combine with fixed mass of the other element bear a simple ratio to one another”
 
Law of reciprocal proportion:
“ If two elements B and C react with the same mass of a third element (A), the ratio in which they do so will be the same or simple multiple if B and C reacts with each other”.
 
Gay Lussac’s law of combining volumes:
“At given temperature and pressure the volumes of all gaseous reactants and products bear a simple whole number ratio to each other”.
 
Atomic and Molecular Masses:
Atomic Mass:
• Mass of an atom.
• Reported in atomic mass unit “amu” or unified mass “u”
• One atomic mass unit i.e. amu, is the mass exactly equal to one-twelfth the mass of one carbon- 12 atom.
 
Molecular Mass:
• Mass of a molecule of covalent compound.
• It is equal to the sum of atomic masses of all the elements present in the molecule.
 
Formula Unit Mass
• Mass of a molecule of an ionic compound
• It is also equal to the sum of atomic masses of all the elements present in the molecule
 
Mole Concept:
Mole:
• Unit of amount of substance.
• One mole amount of substance that contains as many particles or entities as there are atoms in exactly 12 g of the 12C isotope.
 
Molar mass:
• Mass of one mole of a substance in gram
• Molar mass in gram in numerically equal to atomic/molecular/formula mass in amu or u.
 
Mole fraction:-
Ratio of the moles of one component of the solution to the total number of moles of solution
Total mole fraction of all the components of a solution is equal to 1.
For binary solutions having two components A and B
 
Mole fraction of A
XA = (nA)/(nA+nB)]
Mole fraction of B
XB = (nB)/(nA+nB)]
or XB = 1- XA
Molarity(M):-
 
Number of moles of solute per 1000 mL of the solution.
M = (Number of moles of solute)/(Volume of solution in L)
 
Molality(m):-
number of moles of solute per 1000 gram of the solvent.
m = (Number of moles of solute)/(Weight of solvent in kg)
 
 
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NEET Full Course Mole Concept Mole Concept Notes

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Notes for Mole Concept NEET Full Course Mole Concept

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Mole Concept Notes for Mole Concept NEET Full Course

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Mole Concept NEET Full Course Mole Concept Notes

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