CBSE Class 11 Chemistry Revision Notes Set B

Download CBSE Class 11 Chemistry Revision Notes Set B in PDF format. All Revision notes for Class 11 Chemistry have been designed as per the latest syllabus and updated chapters given in your textbook for Chemistry in Class 11. Our teachers have designed these concept notes for the benefit of Class 11 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 Class 11 Chemistry for faster revision of difficult topics and get higher rank. After reading these notes also refer to MCQ questions for Class 11 Chemistry given on studiestoday

Revision Notes for Class 11 Chemistry All topics

Class 11 Chemistry students should refer to the following concepts and notes for All topics in Class 11. These exam notes for Class 11 Chemistry will be very useful for upcoming class tests and examinations and help you to score good marks

All topics Notes Class 11 Chemistry

REMEDIAL ACTION PLAN

L‐1 Some Basic Concepts of Chemistry

Chemistry deals with the composition, structure and properties of matter.

Anything that has mass and occupies space is called matter.

Matter mainly exists in three forms ‐ solid, liquid and gaseous forms. These forms are inter convertible

by changing the temperature and pressure.

SOLID <‐‐‐‐> LIQUID <‐‐‐‐> GAS

Solids have a definite volume and definite shape. The particles are closely attached and there is not much freedom of movement.

Liquids does not have a definite shape but have a definite volume. The particles are not so close and there is a freedom of movement.

Gases neither have definite shape nor have a definite volume. The particles are situated as far as they can and are able to move freely.

BASIC CLASSIFICATION OF MATTER

CBSE Class 11 Chemistry Revision Basic Concepts 1

Mixtures ‐ are the combination of two or more atoms which are combined in a ratio If the ratio is uniform throughout the mixture, then it is a homogeneous mixture If the ratio is not uniform throughout the mixture, then it is a heterogeneous mixture

Pure Substances ‐ consist of either one type of atoms or the combination of them in a fixed ratio. If only one type of atom is present in it, then it is called an element If more than one type is present, it is called a compound Molecules are are the combination of two or more atoms Physical Properties can be measured or identified without changing the composition of the substance. Chemical Properties occur due to a chemical change on the constituents.

Mass: It is the amount of matter present in a substance. It is independent of location. Weight: It is the amount of force excerted on an object by gravity. It changes according to the change in gravitational force.

Volume: It is the amount of space occupied by an object.

LAWS OF CHEMICAL COMBINATION

Law of Conservation of Mass (Antonie Lavoisier) ‐ Mass can neither be created nor be destroyed.

Law of Definite Proportions (Joseph Proust) ‐ A given compound always contains the same elements in the same proportion by mass.

Law of Multiple Proportions (John Dalton) ‐ When two or more elements combine to form more thanone compound, a fixed mass of one compound to a different mass of other always brings simple whole number ratios.

Gay Lussac's Law ‐ When gases combine or are produced in a chemical reaction, they do so in a simple ratio provided all gases are in the same temperature and pressure.

Avogadro's Law ‐ Equal Volumes of gases at the same temperature and pressure should contain equal number of molecules.

Scientific NotationIn which any number can be represented in the form N × 10n(Where n is an exponenthaving positive or negative values and N can vary between 1 to 10).e.g. We can write 232.508 as 2.32508 x102in scientific notation. Similarly, 0.00016can be written as 1.6 x 10–4

Precision refers to the closeness of various measurements for the same quantity.Accuracy is the agreement of a particular value to the true value of the result

Significant FiguresThe reliability of a measurement is indicated by the number of digits used torepresent it. To express it more accuratelywe express it with digits that are knownwith certainty. These are called as Significant figures. They contain all thecertaindigits plus one doubtful digit in a number. 

Rules for Determining the Number of Significant FiguresAll non‐zero digits are significant. For example,
6.9 has two significantfigures, while 2.16 has three significantfigures. The decimal place does notdetermine the number of significant figures.
 
A zero becomes significant in case it comes in between non zero numbers. Forexample, 2.003 has four significantfigures, 4.02 has three significant figures.
 
Zeros at the beginning of a number are not significant. For example, 0.002 hasone significant figure while 0.0045has two significant figures.
All zeros placed to the right of a number are significant. For example, 16.0 hasthree significant figures,while 16.00has four significant figures. Zeros at theend of a number without decimal point are ambiguous.
 
In exponential notations, the numerical portion represents the number ofsignificant figures. For example, 0.00045 isexpressed as 4.5 x 10‐4in terms of scientific notations. The number of significant figures in this number is 2,while in Avogadro's number (6.023 x 1023) it is four.The decimal point does not count towards the number of significant figures.For example, the number 345601 has sixsignificant figures but can be writtenin different ways, as 345.601
or 0.345601 or 3.45601 all having same numberofsignificant figures.
 
Atomic Mass ‐ It is defined as the mass equal to 1/12th the mass of a Carbon‐12 atom. It is represented by 'amu' (atomic mass unit) or 'u' (unified mass).
1 amu or 1 u = 1.66056 x 10‐24
 
Average Atomic Mass ‐ It is atomic mass of elements or compounds having isotopes. It is the sum of the product of the Relative Abundance and Atomic mass of the Isotopes.
Molecular Mass ‐ It is the sum of the atomic mass of the elements present in the molecule. Eg: CH4 ‐ (1 X 12) + (4 X 1) = 16 amu
 
Formula Mass ‐ It is used for measuring the molecular mass of the entities which does not exist in solid form. Eg: NaCl
Avogadro Number ‐ It is the amount of atoms or molecules present in one mole of a substance.
Avogadro Number(NA) = 6.023 X 1023
Molar Mass ‐ Mass of one mole of a substance.
Percentage Composition ‐ It is the Percentage of an element present in a compound.
%age of the element=mass of the element in the compound/molar mass of the compound X100
 
Empirical Formula ‐ It represents the simplest whole number ratio of various atoms present in a compound. It is calculated in following steps:
Convert the given amount to grams
Calculate the number of moles for each element
Divide the rest of the moles with the smallest one among them
Write the ratio with respect to elements
 
Molecular Formula ‐ It gives the exact number of various atoms in a given compound. It is calculated by:
Divide "Molar Mass" with "Empirical Formula"
Multiply the value with each element

Limiting Reagent ‐ It is the reactant which gets consumed and thus influence the amount of product formed.

Mass percentage‐
CBSE Class 11 Chemistry Revision Basic Concepts 2
Mole Fraction of A = number of moles of A/(number of moles of A + number of moles of B)
Mole Fraction of B = number of moles of B/(number of moles of A + number of moles of B)
 
Molarity:
CBSE Class 11 Chemistry Revision Basic Concepts 3
Molality:
CBSE Class 11 Chemistry Revision Basic Concepts

 
 

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Chapter 01 Some Basic Concepts of Chemistry
CBSE Class 11 Chemistry Basic Concepts Of Chemistry Notes

CBSE Class 11 Chemistry All topics Notes

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Notes for Chemistry CBSE Class 11 All topics

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All topics Notes for Chemistry CBSE Class 11

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All topics CBSE Class 11 Chemistry Notes

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Notes for CBSE Chemistry Class 11 All topics

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