It largely concerns itself with the study of minerals found in the Earth’s crust. Zeros between two non-zero digits are significant. For example, 0.200 g has three significant figures. A mixture is a combination of two or more elements or compounds in any proportion (D) Application in Industry: for longer periods. 6. Some other substances having tinting property were kamplcica, pattanga and jatuka. so that the components do not lose their identity. Students can find the Important Questions of Class 11 Chemistry Chapter 1 Some Basic Concepts of Chemistry compiled here on this page. (i) Homogeneous mixtures: A mixture is said to be homogeneous if it has a uniform composition throughout and there are no visible boundaries of separation between the constituents. Free PDF download of Class 11 Chemistry revision notes & short key-notes for Chapter 12 - Organic Chemistry - Some Basic Principles and Techniques to score high marks in exams, prepared by expert Chemistry teachers from latest edition of CBSE(NCERT) books. According to this law when gases combine or are produced in a chemical reaction they do so in a simple ratio by volume provided all gases are at same temperature and pressure. 1. They are also called solutions. For a solution containing n2 moles of the solute dissolved in n1 moles of the solvent, With this study material, the chapter Some Basic Concepts of Chemistry can be simplified a great deal.These Notes of Chemistry Class 11 Chapter 1 further allow you to grasp any minute ⦠(A) Physical Classification: 1. The formula of the compound which gives the simplest whole number ratio of the atoms of yarious elements present in one molecule of the compound. The rapid industrialisation all over the world has resulted in lot of pollution. • Analytical Chemistry-This branch deals with the qualitative and quantitative analysis of various substances. Physics Wallah . Molecules are classified as homoatomic and heteroatomic. • Mass and Weight A few examples of mixtures are: milk, sea water, petrol, lime water, paint glass, cement, wood etc. For example, 16.0 has three significant figures, while 16.00has four significant figures. force of attraction, 4. arrangement of Solids: The particles are held very close to each other in an orderly fashion and there is not much freedom of movement. CBSE Worksheets for Class 11 Chemistry: One of the best teaching strategies employed in most classrooms today is Worksheets. 2. Molar mass of the solute X volume of the solution in liter. In case of even figure, the preceding digit remains unchanged. E.g. There are two ways of classifying the matter: For example, in 285 cm, there are three significant figures and in 0.25 mL, there are two significant figures. Law of Multiple Proportions Proposed by Dalton in 1803, this law states that:’ When two elements combine to form two or more compounds, then the differe nt masses of one element, which combine with a fixed mass of the other, bear a simple ratio to one another’. These properties can be classified into twocategories â physical properties and chemical properties.Physical properties are those properties which can be measured or observed without changing the identity or the composition of the substance. A compound is a pure substance made up of two or more elements combined in a definite proportion by mass, which could be split by suitable chemical methods. The final result has four decimal places. Mixtures are of two types, homogeneous and heterogeneous. The quantity of an element whose mass in grams is numerically equal to its atomic However, a popular unit of measuring volume, particularly in liquids is litre (L) but it is not in SI units or an S.I. Metric System was based on the decimal system. Topics Included are: The law states that, under similar conditions of temperature and pressure, whenever gases combine, they do so in volumes which bear simple whole number ratio with each other and also with the gaseous products. Zeros at the end of a number without decimal point are ambiguous. Molecular mass of the compound, An empirical formula represents the simplest whole number ratio of various atoms present in a compound. We can write 232.508 as 2.32508 x102 in scientific notation. In which any number can be represented in the form N × 10n Where n is an exponent having positive or negative values and N can vary between 1 to 10). Some elements such as sodium . Stoichiometry, thus deals with the calculation of masses (sometimes volume also) of the reactants and the products involved in a chemical reaction. They are polluting environment at an alarming rate. These particles may be atoms or molecules. 4. Pure substances can be further classified as (i) Elements (ii) Compounds figures. Homoatomic molecules are made up of the atoms of the same element and heteroatomic molecules are made The examples of chemical properties are characteristic reactions of different substances. have the same composition throughout the sample. Elements are further classified into metals, non-metals and metalloids. It is basically concerned with laws and theories of the different branches of chemistry. (i) Law of Conservation of Mass The reactant which is not consumed completely in the reaction is called excess reactant. CBSE Class 12 Chemistry , CBSE Class 12 Physics. rate of diffusion is very fast. Molecular mass of methane (CH4) The rounding off procedure is applied to retain the required number of significant It has greyish-yellow appearance and the two constituents, iron and sulphur, can be easily identified with naked eye. detergents, metal alloys and other inorganic and organic chemicals including new materials contribute in a big way to the national economy. negative values) are possible in Celsius scale but in Kelvin scale, negative temperature is not possible. categories – physical properties and chemical properties. These are stated below: • Atomic Mass •Atoms cannot be created, divided or destroyed during any chemical or physical change. He Provide The Education For Class 10th,Class 11th, Class 12th And For IIT Jee Students. • Uncertainty in Measurements This leads to y three types of [â¦] A 5 % (v/v) solution of ethyl alcohol contains 5 cm3 of alcohol in 100 cm3 of the solution, 3. NCERT Solutions for Class 6, 7, 8, 9, 10, 11 and 12. the following ways. SOME BASIC CONCEPTS OF CHEMISTRY. Where n is the common factor and also called multiplying factor. Molality- Molality is defined as the number of moles of solute dissolved per 1000 g (1 kg) of solvent. For example, let us carry out the addition of three numbers 3.52, 2.3 and 6.24, having different precisions or different number of decimal places. Ancient Indians had knowledge of various concepts from chemistry even before it emerged as a ⦠Compounds are formed when atoms of different elements combine in a fixed ratio. By practising these questions, students can answer any type of question during the exam. Anything which has mass and occupies space is called matter. 2. Volume of the solution in litre V, The Molarity of the solution can also be expressed in terms of mass and molar mass, Molarity of the solution = Mass of the solute Limiting Reactant/Reagent Physicswallahalakhpandey.com physics Alakh pandey ,alakhpandey notes,physicswallah ,notes of class 12 nd 11 ,IIT JEEE,NEET,AIMS, CAT, chemistry, 10. The word ‘stoichiometry’ is derived from two Greek words—Stoicheion (meaning element) and metron (meaning measure). In case n is 1, Molecular formula of a compound = Empirical formula of the compound. The components of such mixtures cannot be seen under a powerful microscope. A quantity of substance whose mass in grams is numerically equal to its molecular chemical change, are known as products, Limiting Reagent- The reactant which gets consumed first or limits the amount of product formed is known as limiting reagent. This is possible only when you have the best CBSE Class 11 Chemistry study material and a smart preparation plan. • Molecular Formula 3. Scientists are working day and night to develop substitutes which may cause lower pollution. A pure chemical compound always consists of the same elements combined together in a fixed proportion by weight. • Dimensional analysis: It helps to express the measured quantities in different systems of units. --Every substance has unique or characteristic properties. (iv) Law of Gaseous Volume (Gay Lussac’s Law) 1. For example, 6.9 has two significant figures, while 2.16 has three significantfigures. • Scientific figures: The uncertainty is taken care of by specifying the number of significant figures in which the observations are reported. Mole: It is the amount of substance which contains as many elementary entities as there are atoms in 0.012 kilogram of carbon -12. They completely occupy the container in which they are placed. mass. Second: It is the duration of 9192631, 770 periods of radiation which correspond to the transition between the two hyper fine levels of the ground state of caesium- 133 atom. Download CBSE Class 11 Chemistry Assignments in pdf covering all important topics with solutions developed as per CBSE and NCERT Syllabus for Chapters Of Chemistry. SI unit of mass is kilogram. then, 5 feet and 2 inch = 62 inch, 3. per mol or millilitre per mol, The mass percentage of each constituent element present in any compound is called Chemistry Notes , Chemistry Assignment , Chemistry Quiz , NCERT Solution Characteristics of solids: Solids have definite volume and definite shape. Metre: It is the length of the path travelled by light in vacuum during a time interval of 1/299792458 of a second. • Dalton’s Atomic Theory as compared to the mass of an atom of C-12 taken as 12. They all contain atoms of one type. For example: When iron filings and sulphur powder are mixed together, the mixture formed is heterogeneous. We have discussed the physical and chemical classification of matter. 1V 1V 2V All non-zero digits are significant. Some examples of physical properties are colour, odour, melting point, boiling point etc. E.g. • Industrial Chemistry-The chemistry involved in industrial processes is studied under this branch. For example, • Significant Figures Matter consists of indivisible atoms. The substances that react among themselves to bring about the chemical changes are known as reactants, whereas the substances that are produced as a result of the (B) Chemical classification • Mole Concept • Units of Measurement Kilogram: It is the unit of mass. Download Handwritten Notes on all the topics of Class XI Chemistry. So, SI unit of density can be obtained as follows: • Definitions of Basic SI Units Molecular formula = n x Empirical formula -> Thermometres with Fahrenheit scale are calibrated from 32°F to 212°F. 3. Since water contains hydrogen and oxygen, the percentage composition of both these elements can be calculated as follows: The Shapes of Carbon Compounds: In organic or carbon compounds, s and p orbitals are involved in hybridisation. These are called as Significant figures. 2. The value of n may be 1, 2, 3, 4, 5, 6 etc. or copper contain single atoms held together as their constituent particles whereas in some others two or more atoms combine to give molecules of the element. For example, 0.002 has one significant figure while 0.0045has two significant figures. For example, Average Atomic Mass The following experiments illustrate the truth of this law. It has given units of all the seven basic quantities listed above. It is usually represented by NA: (i) Law of Conservation of Mass (v) Avogadro’s Law: Avogadro proposed that, equal volumes of gases at the same temperature and pressure should contain equal number of molecules. (iii) The use of preservatives has helped to preserve food products like jam, butter, squashes etc. (iv) Gay Lussac’s Law of Gaseous Volumes 2. (B) Chemical Classification: • Balanced chemical equation: A balanced equation has the same number of atoms of each element on both sides of the equation. Matter can exist in three physical states: Molarity: It is defined as the number of moles of solute in 1 litre of the solution. According to this law equal volumes of gases at the same temperature and pressure should contain equal number of molecules. 1. (i) Calculation involving multiplication and division Mole fraction: It is the ratio of number of moles of a particular component to the total number of moles of the solution. = 16.043 u • Multiplication and Division of Significant Figures Filed Under: Chemistry, Class 11, Some basic concepts of chemistry Tagged With: Dimensional analysis, factor label method About Mrs Shilpi Nagpal Author of this website, Mrs Shilpi Nagpal is MSc (Hons, Chemistry) and BSc (Hons, Chemistry) from Delhi University, B.Ed (I. P. University) and has many years of experience in teaching. Chemistry Class 11: Syllabus and Important Notes. • Stoichiometry and Stoichiometric Calculations Now let us see how calculations are carried out with numbers expressed in scientific notation. Kelvin: It is the unit of thermodynamic temperature and is equal to 1/273.16 of the thermodynamic temperature of the triple point of water. (b) Combination between nitrogen and hydrogen: The two gases lead to the formation of ammonia gas under suitable conditions. The mass of a substance can be determined very accurately by using an analytical balance, Volume-- Volume has the units of (length)3. If the digit involved is less than 5, it is neglected and the preceding significant figure remains unchanged, 4.312 isrounded off to 4.31. e.g. It Liquids 3. • Dimensional Analysis 4. Pure Substances 2. The molecular formula shows the exact number of different types of atoms present in a molecule of a compound. structure and properties of matter. (a) When matter undergoes a physical change. determine the number of significant figures. mass and they occupy space. 4. Chemical reactions involve reorganisation of atoms. e.g. (i) Elements: An element consists of only one type of particles. consist of two or more parts (phases), which have different compositions. Significant figures are meaningful digits which are known with certainty. • All zeros placed to the right of a number are significant. The International System of Units (in French Le Systeme International d’Unites– (ii) It has helped to protect the crops from insects and harmful bacteria, by the use ‘ of certain effective insecticides, fungicides and pesticides. CBSE Class 12 Chemistry , CBSE Class 12 Physics. In the multiplication or division, the final result should be reported upto the same number of significant figures as present in the least precise number. molarity, the following equation is used: Class 11 Chemistry Chapter 1 notes are compiled by subject experts in compliance with the updated syllabus provided by CBSE.These notes for Class 11 Chemistry, are available online as free PDF downloads. • Scientific Notation abbreviated as SI) was established by the 11th General Conference on Weights and Measures (CGPM fromConferenceGenerale des Poids at Measures). These are given below: The chemistry class 11 syllabus aims to give the students an overall picture of what fundamentals of higher chemistry look like. In a mixture the constituents are not present in fixed ratio. Ionic compounds such as NaCl, KNO3, Na2C03 etc. In all physical and chemical changes, the total mass of the reactants is equal to that of the products. It is expressed as 3. • In exponential notations, the numerical portion represents the number of significant figures. For example, common salt, marble and limestone. CBSE Syllabus Class 12 Maths Physics Chemistry ... CBSE Syllabus Class 11 Mathematics biology chemistry ... CBSE Syllabus Class 10 Maths Science Hindi English ... CBSE Syllabus Class 9 Mathematics Science English Hindi ... Revised Syllabus for Class 12 Mathematics. Significant Figures For example, 0.03 has one significant figure and 0.0052 has two significant figures. Moreover, the properties of a compound are altogether different from the constituting elements. 1.5. Temperature: There are three scales in which temperature can be measured. unit. Chemistry Notes For Class 11 Chapter 1 SOME BASIC CONCEPTS Download In Pdf, Chemistry is the branch of science that deals with the composition, In order to express its empirical formula, we have to take out a common factor 2. The atomic mass of an element is the number of times an atom of that element is heavier than an atom of carbon taken as 12. up of the atoms of the different element have different atomicity (number of atoms in a molecule of an element) like monoatomic, diatomic, triatomic and polyatomic. If the digit coming after the desired number of significant figures happens to be more than 5, the precedingsignificant figure is increased by one, 4.317 is rounded off to 4.32. It has the units of (length)3. Molecular Mass This unit is quite large and a chemist often expresses density in g cm3 where mass is expressed in gram and volume is expressed in cm3. Hence, a convenient system of expressing the number in scientific notation is used. According to the rule the final result = 0.024 Types of mixtures: Mixtures are of two types: Using stoichiometric calculations, the amounts of one or more reactants required to produce a particular amount of product can be determined and vice-versa. Mass % of the element=Mass of element in 1 molecule of the compound x 100 Inorganic compounds are those, which areobtained from non-living sources such as minerals. All the organic compounds have been found to contain carbon as their essential constituent. CHEMISTRY HANDWRITTEN NOTES CLASS 11 & 12 FOR NEET/JEE ASPIRANTS. 1. • Biochemistry-This branch deals with the chemical changes going on in the bodies of living organisms; plants and animals. For example, the formula of hydrogen peroxide is H202. It is also known as unified mass. They all contain carbon. Burning of Mg-ribbon in air. • Stoichiometry: The quantitative study of the reactants required or the products formed is called stoichiometry. This law was proposed by Louis Proust in 1799, which states that: Zeros preceding to first non-zero digit are not significant. An element is the simplest form of matter that cannot be split into simpler substances A balanced equation for this reaction is as given below: of moles of the solute = n The chemical equation is These questions cover all the important topics and are designed exclusively for students exam preparation. is taken’. Mass percent: It is obtained by using the following relation: element as compared to the mass of an atom of carbon -12 taken as 12. All of them have been calibrated. have been prepared artificially. It is equal to the mass of the international prototype Common factor = 6 Therefore, the atomic mass of an element must be its average atomic mass and it may be defined as the average relative mass of an atom of an element as compared to the mass of carbon atoms (C-12) taken as 12w. 1. Weight of substance may vary from one place to another due to change in gravity. mass is called gram molecular mass. The combination of elements to form compounds is governed by the following five basic laws. • Matter can also be classified into elements, compounds and mixtures. (B) In Health and Sanitation: A few Mass percent or weight percent (w/w%) CBSE Class 11 Basic Concepts of Chemistryâ Get here the Notes for CBSE Class 11 Basic Concepts of Chemistry. 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