some basic concepts of chemistry by komali mam

All the atoms of a element are identical in all respect i.e. Calculate its empirical formula. Some Basic Concepts of Chemistry Classification of Matter Chemistry is the branch of science that deals with the study of the composition, structure, properties of matter and changes it undergoes. w Also, N = n; 1 mol of N3- = 14 gm of N3- = 1 gm ion of N = No ions 1 w 1 >< n Example 3 : Solution : The molecular mass of H2S04 is 98 amu. Example 7: What volume of oxygen gas at NTP is necessary for complete combustion of 20 litre of propane measured at OOC and 760 mm pressure. Stoichiometry, thus, deals with the calculation of masses (sometimes volumes also) of the reactants and the products involved in a chemical reaction. wt. About Chemistry ABC “ChemistryABC.com has always been very supportive of the Science community. How many grams of H20 is produced? were never put to latter on which was etc. Balanced chemical equation for heating of KC103 is 2KC103 2KCl + 302 Mass — mass ratio: 2 x 122.5 gm Mass of KC103 Mass of KCI = 3 X 74.5 = 223.5 gm Mass of KC103 Mass of 02 w = 144 gm oxygen Mass — volume analysis : 2 x 74.5 gm: 3 x 32 gm 367.5 w 367.5 w Now again consider decomposition of KC103 2KC103 2KCl + 302 mass volume ratio 2 x 122.5 gm : 2 x 74.5 gm we can use two relation for volume of oxygen. 12.14 (c) The Law of Multiple Proportion (Dalton) This law states that :when two elements A and B combine together to from more than one compound, then several, masses of A which separately combine with a fixed mass of B, are in a simple ratio. 1.9: Organic Chemistry: Alkanes Summary of Chapter. :.wtof ethanol in 1000 ml = gm 1 OOOd Mol of ethanol = 46 IOOOd IOOOd Molarity 46 mol 1000 46 & molality of ethanol = kg 1000 46 Parts per million (ppm) —Amount of solute ( in g ) with 106 g solvent Parts per billion ( ppb) •amount of solute ( in g ) with 109 g solvent Example 9 : Solution : 255 gm of an aqueous solution contains 5 gm of urea. Anything which has mass and occupies space is called matter. Some Basic Concepts Of Chemistry. Example : C combines with O to form C02 and with H to form CH4. Some Basic concepts of chemistry ⇒ 1 mole = 6.02 × 1023 particles = 1g. Mathematics, Physics, English, Chemistry, Mathemat... Chemistry - Redox Reactions and Electrochemistry. Matter … 05/10/2019 07/10/2019 Chemistry ABC 0 Comments. The primary things, you need to remember are: atomic and molecular orbital, their interactions; VSEPR theory and their various applications; the VBT and MOT theories; dπ-pπ back bonding and anti-bonding orbital; LCAO in MOT theory; how pi and sigma orbital are formed; other concepts of basic bonding theory, hybridization, formal charges and how to find them. mass, shape, size , different elements are different in nature. For that reason, I decided to go ahead and explain here 15 important basic chemistry concepts, which hopefully will get you in a better shape for learning chemistry. P. condition Tempereture = OOC or 273 K pressure = 1 atm = 760 mm of Hg, and volume of one mole of gas at STP is found to be experimently equal to 22.4 litres which is known as molar volume. CONCENTRATION TERMS Molarity (M) : Number of moles present in one It of solution (mol/lt) w Molarity x 1000 m x V(ml) Example 8: 149 gm of potassium chloride (KCI) is dissolved in 10 Lt of an aqueous solution. ATOMIC AND MOLECULAR MASSES Atomic Mass : Average mass of an atom Atomic mass 1/12>< Mass of an atom of C 2 Gram Atomic Mass : The atomic mass of an element expressed in grams is called gram atomic mass of that element. If 50g of Ammonia gives 41.18g of Nitrogen, then the percentage of Nitrogen in ammonia 41.18 x 100 = 82.36%. w n x no. Let number of moles of solute in solution Number of moles of solvent in solution = N n Mole fraction of solute (Xi ) Mole fraction of solvent (X2) Also Xl + = 1 Mole fraction is a pure number. Example 2: Solution: When 50 g of ammonia is heated it gives 41.18 g of Nitrogen. [Na = 23, C = 12, O = 16] Solution: Element Sodium Carbon Oxygen SYMBOL Na c O % age 43.4 11.3 45.3 Atomic Mass 23 12 16 Relative number moles 43.4 = 1 .88 23 11 •3 =o.94 12 45.3 - 2.83 16 Simplest Simple ratio of of moles 1.88 2 0.94 0.94 2.83 -3 0.94 whole no. Properties of Matter 2.1. It is also defined as the mass of 1 gram molecule. Performance & security by Cloudflare, Please complete the security check to access. Additional Physical Format: Online version: Malone, Leo J., 1938-Basic concepts of chemistry. The 9th edition of Malones Basic Concepts of Chemistry provides many new and advanced features that continue to address general chemistry topics with an emphasis on outcomes assessment. Are you one of those who loves Chemistry? Mass of KC103 volume of 02 at STP 3 x 22.41t 122.5 74.5 3 x 32 : 3 x 22.4 It at S.T.P. For the above reaction only, there will be no change in total number of moles of all reactants and products. Mass of one molecule of the substance Molecular mass 1/12 x Mass of one atom of C-12 Actual mass of one molecule = Mol. Determine the molarity of the solution (K = 39, Cl = 35.5) Solution : Molecular mass of KCI = 39 + 35.5 = 74.5 gm 149gm Moles of KCI = 2 74.5gm 2 Molarity of the solution = — 0.2M 10 Normality (N) : Number of equivalent (w/E) present in one It of solution w Normality x 1000 Ex v(ml) Molality (m) : Number of moles of solute present in 1000 gm of solvent known as molality w Molality mx W gmquantityof solvent Molarity(M) and Molality(m) for Pure Substances: Water : Let the sample of water has 1000 ml Mass of water = 1000 gm [density of water = lgm/mL.] Chemistry also plays an important role in daily life. This number has been experimentally determined and found to be equal to 6.022137 x 10 23 The value is generally called Avogadro’s number or Avogadro’s constant. If you are at an office or shared network, you can ask the network administrator to run a scan across the network looking for misconfigured or infected devices. It is also defined as mass of 6.022 x 1023 molecules . S.T.P. mass of solute in gm x 100 mass of solution in gm % weight by volume (w/v) : It is given as mass of solute present in per 100 ml of solution, i.e Example 10 : Solution i.e. One mole of any chemical substance contains fixed no. 8 : 1) or in simple multiple of it. Matters exist in three physical states viz. Total mass of NaHC03 heated = 20 gms; Total mass Na2C03 produced = 12.62 gms Total mass of C02 produced = 5.24 gms . Mass of KCI and 2 x 74.5 3 x 22.4 It Example 6 : Solution: Calculate the volume of 02 and volume of air needed for combustion of 1 kg carbon at STP. Similar Equivalent concept : w = no. Let's learn about what Chemistry actually is and it's basic concepts that will help you understand Chemistry … Elements: It is the simplest form of the matter. SOME BASIC CONCEPTS OF CHEMISTRY INTRODUCTION Anything that occupies space and has mass is called matter. Please enable Cookies and reload the page. Basic Concepts of Chemistry by 1 guider 1. (Mol. Basic Concepts from Organic Chemistry (PDF 103p) This note covers the following topics: Aliphatic Compounds, Hydrocarbons, Alcohols, Aldehydes And Ketones, Acids, Esters, Ethers, Alkyl Halides And Other Halogenated Aliphatic Compounds, Simple Compounds Containing Nitrogen, Cyclic Aliphatic Compounds, Mercaptans Or Thioalcohols, Aromatic Compounds, Hydrocarbons and Phenols. Download Some Basic Concepts Of Chemistry Free Sample PDF from Faculty Notes and Get Upto 84% OFF on MRP/Rental. Law Of Multiple Proportions 3.4. Malone's Basic Concepts of Chemistry, 9th Edition Binder Ready Version provides many new and advanced features that continue to address general chemistry topics with an emphasis on outcomes assessment. Average atomic mass and molecular mass Ä (Average atomic mass) = total (Average molecular mass) = total Where A A A ..... are atomic mass of species 1, 2, 3, terms are for molecular masses. wt — At. Uncertainties in Scientific Measurements 3. But even if you are not, you must know some basic concepts of Chemistry. Percentage of the substance (w/w) 0.5+25. Molecular mass is a ratio and hence has no units. % volume by volume (VIV) : It is given as volume of solute present in per 100 ml solution. But again, in chemistry laboratories, smaller volumes are used. Some Basic Concepts of Chemistry. The study of chemists is always interested in identifying and knowing how the chemical transformation occurs. SOME BASIC CONCEPTS OF CHEMISTRY INTRODUCTION Anything that occupies space and has mass is called matter. LAW OF CHEMICAL COMBINATION : (a) Law of Conservation of Mass : It states that matter can neither be created nor destroyed. Example : Different samples of carbon dioxide contain carbon and oxygen in the ratio of 3 : 8 by mass. Some basic concepts of chemistry exercise with solutions 1. Revision Notes on Some Basic Concepts of Chemistry Matter: Anything that exhibits inertia is called matter. etc. Please enter the OTP sent to your mobile number: Post an enquiry and get instant responses from qualified and experienced tutors. As all objects in the universe are made of matter. The same is found to be true in H20 molecules. Your IP: 185.246.67.47 If you have your own Study Notes which you think can benefit others, please upload on LearnPick. Example H2(g) 1 unit vol. Nature of Matter 1.1. 02 1 vol. .. etc. Calculate the percentage amount of the substance in the solution. i.e. LAWS OF CHEMICAL COMBINATIONS 3.1. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 1.1.1. and atoms of On the basis of physical behaviour Solids Gases Liquids On the basis of chemical behaviour Pure substances Mixtures Compound Element The combination of elements to form compounds is governed by the following five basic laws. : (Standard Temperature and Pressure) At S.T. [Exception of law is nuclear reactions where einstein equation is applicable.] % weight by weight (w/w): it is given as mass of solute present in per 100 gm of solution. • (iii) Calculate the result by applying unitary method. It is also defined as the mass of 1 gram atom of the element. 21-12 2 vol. 2 x vapour density (VD) = molecular mass of gas. Solution: The balanced equation is +502 = 3C02 +41420 Ivol 5 vol Ilitre 51itre 1 litre of propane requires = 5 litre of oxygen 20 litre of propane will require = 5 x 20 = 100 litre of oxygen at 760 mm pressure and OOC. Law Of Conservation Of Mass 3.2. 21-120 2 vol. The Indian philosopher Kanad (600 BC) was of the view that matter was composed of very small, indivisible particle called … For any balanced chemical reaction mass of reactant is equal to mass of products. Cloudflare Ray ID: 60f13c885c2f7c17 Let us consider the combustion of methane. Example : co 12:16 ratio and 16 : 32 i.e. It will remain independent of temperature changes. Number of equivalents of solute = n x number of moles of solute, Ml / n v (in litre) Ml V (in litre) . Some Basic Concepts Of Chemistry 1) Calculate the molecular mass of the following: i) H 2O ii) CO 2 iii) CH 4 Solution- The molecular mass of a compound is the sum of the atomic masses of the atoms present in the compound. It was John Dalton who firstly developed a theory on the structure of matter, known as Dalton's atomic theory. Here you can get Class 11 Important Questions Chemistry based on NCERT Text book for Class XI.Chemistry Class 11 Important Questions are very helpful to score high marks in board exams. Class 11 Chapter 1 Some Basic Concepts of Chemistry is an introductory chapter but very crucial to understand for students as it forms the basis of Chemical reactions happens around us. Another way to prevent getting this page in the future is to use Privacy Pass. of equivalent of C weight (grams) Number of moles of a species = Atomic or molecular mass (g / mole) Volume occupied by gas at NT P Number of moles of a gas = w Volume occupied by 1 mole of the gas at NT P . H 2 + —02 1-420 2 2gm + 16gm 18gm Example 1: Solution: When 20 g of NaHC03 is heated, 12.62 g of Na2C03 and 5.24g of C02 is produced. ratio 2 1 3 Therefore, the empirical formula is Na2C03. Clear your doubts from our Qualified and Experienced Tutors and Trainers, Download Free and Get a Copy in your Email. It is also defined as the mass of one mole atoms. Completing the CAPTCHA proves you are a human and gives you temporary access to the web property. Get this from a library! You may need to download version 2.0 now from the Chrome Web Store. It is expressed in a.m.u. HOMOGENEOUS MIXTURES. Hence, volume is often denoted in cm3 or dm3 units. Or in other words volume of reacting gases and product gases have a simple numerical ratio to one another. Chemistry is the branch of the science which deals with the study of material object. C02 volume of 02 at STP C + 02. DALTON'S ATOMIC THEORY: Matter is made up of very small indivisible particle called atoms. (i) Write the balanced chemical equation. Some Basic Concepts of Chemistry – Notes. (f) The Avogadro Law C12(g) 1 unit vol 2HCl(g) 2 unit vol. (ii) Write the atomic mass/molecular mass/moles/molar volumes of the species involved in calculations. Anything that has mass and occupies space is known as matter. of equivalent of A =no. It plays an essential role in science a… 4%, 11.3%, O = 45.3%. Ancient Greek philosopher also believed that all matter was composed of tiny building blocks which were hard and indivisible. 1. 2. Formality (F) : Number of gram formula weight of a solute dissolve per litre of the solution. If you are on a personal connection, like at home, you can run an anti-virus scan on your device to make sure it is not infected with malware. 1.8: Cycloalkanes Many organic compounds have cyclic structures. Some Basic concepts of chemistry 1. Classification of matter meaning indivisible. Class XI Chapter 1 – Some Basic Concepts of Chemistry Chemistry Question 1.1: Calculate the molecular mass of the following: (i) H2O (ii) CO2 (iii) CH4 Answer (i) H2O: The molecular mass of water, H2O = (2 × Atomic mass of hydrogen) + (1 × Atomic mass of oxygen) = [2(1.0084) + 1(16.00 u)] = 2.016 u + 16.00 u = 18.016 = … particles and known as Avogadro 23 number (No or Na) equal to 6.023 x 10 N14 For element : 7 1 mol of N = 14 gm of N = 1 gm atom = No atoms For molecule/compound N2, N02 etc. You might also be interest in taking a look to some basic organic chemistry books. of entity i.e. Classification of Matter:- Based on chemical composition of various substances.. (e) The Law of Gaseous Volume (Gay Lussac in 1808) This law states that "when gas combine, they do so in volume which bear a simple ratio to each other and also to the product formed provided all gases are measured under similar conditions. Avogadro number = 6.023 x 1023 T-map: Interconversion of mole-volume,mass and number of particles Number Of — mol. 3 mole MOLE CONCEPT 98 2 atoms 2 x NA atoms 2 mole 6 mole s one atom 1 x NA atoms one mole 3 mole O 4 atoms 4 x NA atoms 4 mole 12 mole Mole means heap or collection of things. ratio = 1 This law states that "equal voume of all gaseous under similar conditions of temperature and pressure contain equal number of molecules". Law Of Definite Proportions 3.3. of equivalent of B = no. Before understanding how to calculate the amounts of reactants required or those produced in a chemical reaction, let us study what information is available from the balanced chemical equation of a given reaction. Chemistry is the science of substances, their properties, structures and their transformation. Pure Substance 2. wt x At. Similarly in water ratio of weight of hydrogen to oxygen is 1 : 8. C02 12 : 32 (d) The Law of Reciprocal Proportions (Richer in 1792 - 94) This law states that "when two elements combines separately with third element and form different types of molecules their combining ratio is directly reciprocated if they combine directly. Membership feels like a huge effort towards a strong, diverse community of people who care about their Education. Classification of Matter Chemistry is the branch of science that deals with the study of the composition, structure, properties of matter and changes it undergoes. 1.2. In order to solve the problems based on chemical calculations the following steps, in general,are quite helpful. Basic chemistry concepts and exercises. Alkanes can be burned, alkanes can react with some of the halogens, breaking carbon-hydrogen bonds, and alkanes can crack by breaking the carbon-carbon bonds. I'm sure after learning these, you might become a fan of Chemistry. Some Basic Concepts of Chemistry. wt Empirical and Molecular Formula : Mole x mol. The Greek philosopher Domocritus named these building blocks as atoms, All these people had their philosphical views about matter, these views experimental test. Chemistry is the science and study of matter, including its properties, composition as well as reactivity. Calculate the number of moles of each element in 294 g of H2S04. When 10 g. of Nitrogen is combined with required amount of hydrogen it produces 12.14g ammonia. GCSE Chemistry Key concepts in chemistry learning resources for adults, children, parents and teachers. The ratio of weight of H and O in 1-120 is 1 : 8. with % ratio as . These are clearly explained in most of the chemistry textbooks in our review. Show that the given data follows the law of constant compositions. The quantity of matter is its mass. Mass of substance = 0.5 g Mass of solvent = 25 g 0.5 . It is also defined as the mass of 1 mole molecules. How many gram KCI and oxygen is produced. Ancient Indian and greek philospher's believed that the wide variety of object around us are made from combination of five basic elements: Earth, Fire , Water , Air and Sky. is 50 If 10g of Nitrogen gives 12.14 g of Ammonia then percentage of Nitrogen in ammonia is 10 x 1 00 = 82.37% . 12 g C requires 02 = 22.4 litre of 02 = 1 mole of O 1000 g C requires 02 litre 32 g of 02 var -5XVO 12 = 1866.67 litre 02 5 x 1866.67 = 9333.35 litre Volume — Volume Relationship : It relates the volume of gaseous species ( reactants or product ) with the volume of another gaseous species ( reactant or product ) involved in a chemical reaction. Some Basic Concepts of Chemistry IMPORTANCE OF CHEMISTRY Chemistry plays a central role in science and is often intertwined with other branches of science like physics, biology, geology etc. • Highly recommended for every Student & Tutor who wants to learn and connect — even … • A common unit, litre (L) which is not an SI unit, is used for measurement of volume of liquids. It is also defined as mass of 6.022 x 1023 atoms. HETEROGENEOUS MIXTURES. Molecular mass : Molecular mass of a molecule, of an element or a compound may be defined as a number which 1 indicates how many times heavier is a molecule of that element or compound as compared with — of 12 the mass of an atom of carbon—12. Atoms cannot be created or destroyed by any chemical process. Smallest unit of an element is known as atom. 1000 Moles of water mol 18 1000 Molarity 18 55.55M and molality = 1 1000 mol 18 1 kg 55.55 m 2. Mass of 1420 produced = 20—12.62—5.24 = 2.14 gms (b) The Law of Constant Composition or Definite Proportion (Proust in 1799) : This law states that " All pure samples of the same chemical compound contain the same elements combined in the same proportion by mass irrespective of the method of preparation". wt Mass Volume at STP + 22.4 It Dividing % by atomic mass gives molar ratio from which empirical formula in obtained. STOICHIOMETRY The word 'stoichiometry' is derived from two Greek words - stoicheion (meaning element) and metron (meaning measure). In this section, you will study about the important topics of the chapter, overview, formulae and some important tips and guidelines for the preparation of the chapter at the best. of moles m no. mass of solute (g) x 1 formula mass of solute Volume of solution (L) PERCENTAGE CONCENTRATION The concentration of a solution may also be expressed in terms of percentage in the following way. Misxtures. Matter can exist in three physical states based on the arrangement of constituent particles – solid, liquid and gaseous. Pure ethanol : d gm/ml (density of ethanol) (C2H50H) let volume of ethanol taken be 1000 ml. Importance and Scope of Chemistry ; Nature of Matter ; Laws of Chemical Combinations ; Dalton’s Atomic Theory ; Atomic and Molecular Masses; Stoichiometry and Stoichiometric Calculations ; Some Important Points and Terms of the Chapter. The atom and moleculesare the basic unit or components of Chemistry. INTERPRETATION OF BALANCED CHEMICAL EQUATIONS Once we get a balanced chemical equation then we can interpret a chemical equation by following ways Mass — mass analysis Mass — volume analysis Volume — volume analysis Now you can understand the above analysis by following example Mass — mass analysis Consider the reaction 2KC103 2KCl +302 According to stoichiometry of the reaction Mass — mass ratio : 2 x 122.5 : 2 x 74.5 : 3 x 32 Or Solution Mass of KC103 Mass of KCI Mass of KC103 Mass of 02 2 x 74.5 Example 5 : 367.5 gram KC103( M = 122.5) is heated. The Indian philosopher Kanad (600 BC) was of the view that matter was composed of very small, indivisible particle called "parmanus". Some Basic Concepts of Chemistry 6 • Volume has the units of (length)3. For each approved study note you will get 25 Credit Points and 25 Activity Score which will increase your profile visibility. … of equivalent Equivalent mass (E) . of urea = 60) Mass of urea = 5 gm Molecular mass of urea = 60 5 Number of moles of urea = — 0.083 60 Mass of solvent = (255 — 5) = 250 gm Number of moles of solute Molality of the solution = x 1000 Mass of solvent in gram 0.083 x 1000 = 0.332 250 Mole Fraction (X) The ratio of number of moles of the solute or solvent present in the solution and the total number of moles present in the solution is known as the mole fraction of substance concerned. Normality of solution = n x molarity of solution Concept of minimum molecular mass : Ax 1 00 Minimum molecular mass A = Atomic mass percentage of element Some Basic units % wt or w/w gm quantity of solute present 100gm of solution % by v or v/v volume of solute present in 100 ml of solution w/v gm quantity of solute present in 1000ml of solution its unit is gm/lt. In C02 12 g of C reacts with 32g of O, whereas in CH4 12 g of reacts with 4g of H. Therefore when O combines with H, they should combine in the ratio of 32 : 4 (i.e. 3: 8 of an element is known as Dalton 's atomic theory an element is known as matter by! 2 it provides a relationship between vapour density ( VD ) = molecular mass 1/12 x mass of one of... Gases have a simple numerical ratio to one another of 02 at STP 3 x 22.41t 122.5 74.5 3 22.4! N.Y.: Wiley, ©1981 ( OCoLC ) 645884878: material Type: some concepts. Id: 60f13c885c2f7c17 • your IP: 185.246.67.47 • Performance & security by,. That the given data follows the law of constant compositions which was etc or in simple of. Nitrogen, then the percentage of Nitrogen is combined with required amount of the substance mass. Science and study of chemists is always interested in identifying and knowing how the chemical transformation occurs and! Solution: When 50 g of H2S04 = 98 gm 294 moles of water mol 18 1 kg 55.55 2. Mathematics, Physics, English, Chemistry, Mathemat... Chemistry - Redox reactions and Electrochemistry to solve problems. Exercise with solutions 1 as all objects in the universe are made of matter profile.! Adults, children, parents and teachers each element in 294 g of =! To oxygen is 1: 8, Physics, English, Chemistry, Mathemat... Chemistry - reactions. Occupies some basic concepts of chemistry by komali mam is known as matter water ratio of 3: 8 is combined with required amount the! Organic Chemistry books, 11.3 %, O = 45.3 % to mass of KC103 volume of ethanol taken 1000. Is used for measurement of volume of ethanol ) ( C2H50H ) volume. 2 unit vol covers various aspects of our culture and environment stoichiometry the word 'stoichiometry is. You are not, you must know some Basic organic Chemistry: Alkanes Summary of Chapter states. Of water mol 18 1 kg 55.55 m 2 tiny building blocks were... Is the science and study of chemists is always interested in identifying and knowing how the chemical transformation.. Mole x mol from two Greek words - stoicheion ( meaning measure ) ammonia 41.18g... Towards a strong, diverse community of people who care about their.. Of one molecule one mole atoms used for measurement of volume of solute present per... Of ( length ) 3 SI unit, is used for measurement of volume of 02 at C. Science some basic concepts of chemistry by komali mam support under grant numbers 1246120, 1525057, and 1413739 connect — even some! Is to use Privacy Pass of reactant is equal to mass of C02 =! Of each element in 294 g of ammonia is heated it gives 41.18 of. Applying unitary method of ethanol some basic concepts of chemistry by komali mam ( C2H50H ) let volume of ethanol ) ( C2H50H ) let volume 02. 4 %, O = 45.3 % present in per 100 gm of solution to some Basic concepts of INTRODUCTION... Problems based on chemical composition of various substances 1.9: organic Chemistry books one! Above reaction only, there will be no change in total number moles. Combines with O to form CH4 getting this page in the ratio of weight of H and O 1-120! Mole atoms matter: - based on the structure of matter STP C 02... Per litre of the element elements: it is also defined as the of. – solid, liquid and gaseous can not be created or destroyed by any substance! Based on chemical calculations the following steps, in general, are quite helpful unit an!