{"id":37932,"date":"2022-06-09T11:30:38","date_gmt":"2022-06-09T06:00:38","guid":{"rendered":"https:\/\/www.cbselabs.com\/?p=37932"},"modified":"2022-06-09T12:10:29","modified_gmt":"2022-06-09T06:40:29","slug":"states-matter-cbse-notes-class-11-chemistry","status":"publish","type":"post","link":"https:\/\/www.cbselabs.com\/states-matter-cbse-notes-class-11-chemistry\/","title":{"rendered":"States of Matter Class 11 Notes Chemistry Chapter 5"},"content":{"rendered":"

Class 11 Chemistry Notes<\/a> students can refer to the States of Matter Class 11 Notes Chemistry Chapter 5 https:\/\/www.cbselabs.com\/states-matter-cbse-notes-class-11-chemistry\/ Pdf here. They can also access the CBSE Class 11 States of Matter Chapter 5 Notes while gearing up for their Board exams.<\/p>\n

States of Matter Class 11 Notes Chemistry Chapter 5<\/h2>\n

11th Chemistry States Of Matter Notes Chapter 5<\/strong><\/p>\n

\u2022 Intermolecular Forces<\/strong>
\nIntermolecular forces are the forces of attraction and repulsion between interacting particles
\nhave permanent dipole moments. This interaction is stronger than the London forces but is weaker than ion-ion interaction because only partial charges are involved.
\nThe attractive forces decrease with the increase of distance between dipoles. The interaction energy is proportional to 1\/r6<\/sup> where r is the distance between polar molecules.
\nIon-Dipole Interaction: This is the force of attraction which exists between the ions (cations or anions) and polar molecules. The ion is attracted towards the oppositely charged end of dipolar molecules.
\nThe strength of attraction depends upon the charge and size of the ion and the dipole moment and the size of the polar molecule.
\nFor example: Solubility of common salt (NaCl) in water.
\nStates Of Matter Class 11
\n\u2022 Ion-induced Dipolar Interactions<\/strong>
\nIn this type of interaction permanent dipole of the polar molecule induces dipole on the electrically neutral molecule by deforming its electronic cloud. Interaction energy is proportional to 1\/r6<\/sup> where r is the distance between two molecules.
\n\"States
\nState Of Matter Class 11 Notes
\n\u2022 London Forces or Dispersion Forces<\/strong>
\nAs we know that in non-polar molecules, there is no dipole moment because their electronic . charge cloud is symmetrically distributed. But, it is believed that at any instant of time, the electron cloud of the molecule may be distorted so that an instantaneous dipole or momentary dipole is produced in which one part of the molecule is slightly more negative than the other part. This momentary dipole induces dipoles in the neighbouring molecules. Thus, the force of attraction exists between them and are exactly same as between permanent dipoles. This force of attraction is known as London forces or Dispersion forces. These forces are always attractive and the interaction energy is inversely proportional to the sixth power of the
\ndistance between two interacting particles, (i.e. 1\/r6<\/sup> where r is the distance between two particles).
\nThis can be shown by fig. given below.
\n\"States
\nHydrogen bonding: When hydrogen atom is attached to highly electronegative element by covalent bond, electrons are shifted towards the more electronegative atom. Thus a partial positive charge develops on the hydrogen atom. Now, the positively charged hydrogen atom of one molecule may attract the negatively charged atom of some other molecule and the two molecules can be linked together through a weak force of attraction.
\n\"States
\nThermal Energy: The energy arising due to molecular motion of the body is known as thermal energy. Since motion of the molecules is directly related to kinetic energy and kinetic energy is directly proportional to the temperature.
\nStates Of Matter Notes
\n\u2022 The Gaseous State<\/strong>
\nPhysical Properties of Gaseous State
\n(i) ases have no definite volume and they do not have specific shape,
\n(ii) Gases mix evenly and completely in all proportions without any mechanical aid.
\n(iii) Their density is much lower than solids and liquids. :
\n(iv) They are highly compressible and exert pressure equally in all directions.
\nClass 11 Chemistry States Of Matter Notes
\n\u2022 Boyle\u2019s Law (Pressure-Volume Relationship)<\/strong>
\nAt constant temperature, the volume of a given mass of gas is inversely proportional to its pressure.
\n\"States
\nCharles\u2019 law:<\/strong> At constant pressure, the volume of a given mass of a gas is directly proportional to its absolute temperature.
\n\"States
\n\u2022 Gay Lussac\u2019s Law (Pressure-Temperature Relationship)<\/strong>
\nAt constant volume, pressure of a given mass of a gas is directly proportional to the temperature.
\n\"States
\n\"States
\n\u2022 Avogadro Law (Volume-Amount Relationship)<\/strong>
\nAvogadro’s law states that equal volumes of all gases under the same conditions of temperature and pressure contain equal number of molecules.
\nV \u03b1 n
\nWhere n is the number of moles of the gas.
\nAvogadro constant: The number of molecules in one mole of a gas
\n= 6.022 x 1023<\/sup>
\nIdeal Gas<\/strong>: A gas that follows Boyle’s law, Charles\u2019 law and Avogadro law strictly, is called an ideal gas.
\nReal gases follow these laws only under certain specific conditions. When forces of interaction are practically negligible.
\nChapter 5 Chemistry Class 11 Notes
\n\u2022 Ideal Gas Equation<\/strong>
\nThis is the combined gas equation of three laws and is known as ideal gas equation.
\n\"States
\n\"States
\n\u2022 Dalton\u2019s Law of Partial Pressure<\/strong>
\nWhen two or more non-reactive gases are enclosed in a vessel, the total pressure exerted by the gaseous mixture is equal to the sum of the partial pressure of individual gases.
\nLet P1<\/sub> ,P2<\/sub>, and P3<\/sub> be the pressure of three non reactive gases A, B, and C. When enclosed separately in the same volume and under same condition.
\nPTotal<\/sub> = P1<\/sub>+ P2<\/sub> + P3<\/sub>
\nWhere, PTotal<\/sub> = P is the total pressure exerted by the mixture of gases.
\nStates Of Matter Class 11 Notes Pdf
\n\u2022 Aqueous Tension<\/strong>
\nPressure of non reacting gases are generally collected over water and therefore are moist. Pressure of dry gas can be calculated by substracting vapour pressure of water from total pressure of moist gas.
\nP2Dry gas<\/sub>\u00a0= PTotal<\/sub> – Aqueous Tension
\n\u2022 Partial Pressure in terms of Mole Fraction<\/strong>
\nLet at the temperature T, three gases enclosed in the volume V, exert partial pressure P1<\/sub> , P2\u00a0<\/sub>and P3\u00a0<\/sub>respectively, then
\n\"States
\n\u2022 Kinetic Molecular Theory of Gases<\/strong>
\n(i) Gases consist of large number of very small identical particles (atoms or molecules),
\n(ii) Actual volume occupied by the gas molecule is negligible in comparison to empty space between them.
\n(iii) Gases can occupy all the space available to them. This means they do not have any force of attraction between their particles.
\n(iv) Particles of a gas are always in constant random motion.
\n(v) When the particles of a gas are in random motion, pressure is exerted by the gas due to collision of the particles with the walls of the container.
\n(vi) Collision of the gas molecules are perfectly elastic. This means there is no loss of energy after collision. There may be only exchange of energy between colliding molecules.
\n(vii) At a particular temperature distribution of speed between gaseous particles remains constant.
\n(viii) Average kinetic energy of the gaseous molecule is directly proportional to the absolute temperature.
\nChemistry Class 11 Chapter 5 Notes
\n\u2022 Deviation From Ideal Gas Behaviour<\/strong>
\nReal Gas:<\/strong> A gas which does not follow ideal gas behaviour under all conditions of temperature and pressure, is called real gas.
\nDeviation with respect to pressure can be studied by plotting pressure Vs<\/sub> volume curve at a given temperature. (Boyle’s law)
\n\"States
\nCompressibility factor (Z):<\/strong> Deviation from ideal behaviour can be measured in terms of compressibility factor, Z.
\n\"States
\n\"States
\n\u2022 van der Waals Equation<\/strong>
\n\"States
\nWhere V is a constant for molecular attraction while ‘V is a constant for molecular volume.
\n(a) There is no force of attraction between the molecules of a gas.
\n(b) Volume occupied by the gas molecule is negligible in comparison to the total volume of the gas.
\nAbove two assumptions of the kinetic theory of gas was found to be wrong at very high pressure and low temperature.
\nChapter 5 Class 11 Chemistry Notes
\n\u2022 Liquifaction of Gases<\/strong>
\nLiquifaction of gases can be achieved either by lowering the temperature or increasing the pressure of the gas simultaneously.
\nThomas Andrews plotted isotherms of C02<\/sub> at various temperatures shown in figure.
\n\"States
\nChemistry Class 11 States Of Matter Notes
\nCritical Temperature (Tc<\/sub>):<\/strong> It is defined as that temperature above which a gas cannot be liquified however high pressure may be applied on the gas.
\nTc<\/sub> = 8a\/27bR
\n(Where a and b are van der Waals constants)
\nCritical Pressure (Pc<\/sub>): It is the pressure required to Liquify the gas at the critical temperature.
\nPc = a\/27b2<\/sup>
\nThe volume occupied by one mole of the gas at the critical temperature and the critical pressure is called the critical volume (Vc<\/sub>).
\nFor Example. For C02<\/sub> to Liquify.
\nTc<\/sub> = 30.98\u00b0C
\nPc<\/sub> = 73,9 atm.
\nVc<\/sub> = 95-6 cm3<\/sup>\/mole
\nAll the three are collectively called critical constants.
\nState Of Matter Notes
\n\u2022 Liquid State<\/strong>
\n Characteristics of Liquid State<\/strong>
\n(i) In liquid, intermolecular forces are strong in comparison to gas.
\n(ii) They have definite volume but irregular shapes or we can say that they can take the shape of the container.
\n(iii) Molecules of liquids are held together by attractive intermolecular forces.
\nVapour Pressure:<\/strong> The pressure exerted by the vapour of a liquid, at a particular temperature in a state of dynamic equilibrium, is called the vapour pressure of that liquid at that temperature.
\nVapour Pressure depends upon two factors:<\/strong>
\n(i) Nature of Liquid (ii) Temperature
\n\"States
\nClass 11th Chemistry Chapter 5 Notes
\n\u2022 Surface Tension<\/strong>
\nIt is defined as the force acting per unit length perpendicular to the line drawn on the surface of liquid.
\nS.I. unit of Surface Tension = Nm-1<\/sup>
\nSurface Tension decreases with increase in temperature, because force acting per unit length decreases due to increase in kinetic energy of molecules.
\nChemistry Chapter 5 Class 11 Notes
\n\u2022 Viscosity<\/strong>
\nIt is defined as the internal resistance to flow possessed by a liquid.
\nThe liquids which flow slowly have very high internal resistance, which is due to strong intermolecular forces and hence are said to be more viscous.
\n\"States
\nWhen liquid flows, the layer immediately below it tries to retard its flow while the one above tries to accelerate.
\nThus, force is required to maintain the flow of layers.
\n\"States
\nNotes Of Chapter States Of Matter Class 11
\nEffect of Temp, on Viscosity:<\/strong> Viscosity of liquids decreases as the temperature rises because at high temperature, molecules have high kinetic energy and can overcome the intermolecular forces to slip past one another.
\n\u2022 Boyle\u2019s Law:<\/strong> It states that, under isothermal conditions pressure of a given mass of a gas is inversely proportional to its volume.
\n\"States<\/p>\n

Class 11 Chemistry Notes<\/a><\/h4>\n","protected":false},"excerpt":{"rendered":"

Class 11 Chemistry Notes students can refer to the States of Matter Class 11 Notes Chemistry Chapter 5 https:\/\/www.cbselabs.com\/states-matter-cbse-notes-class-11-chemistry\/ Pdf here. They can also access the CBSE Class 11 States of Matter Chapter 5 Notes while gearing up for their Board exams. States of Matter Class 11 Notes Chemistry Chapter 5 11th Chemistry States Of …<\/p>\n","protected":false},"author":29,"featured_media":164538,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"spay_email":""},"categories":[2],"tags":[],"yoast_head":"\nStates of Matter Class 11 Notes Chemistry Chapter 5 - CBSE Labs<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.cbselabs.com\/states-matter-cbse-notes-class-11-chemistry\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"States of Matter Class 11 Notes Chemistry Chapter 5\" \/>\n<meta property=\"og:description\" content=\"Class 11 Chemistry Notes students can refer to the States of Matter Class 11 Notes Chemistry Chapter 5 https:\/\/www.cbselabs.com\/states-matter-cbse-notes-class-11-chemistry\/ Pdf here. 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They can also access the CBSE Class 11 States of Matter Chapter 5 Notes while gearing up for their Board exams. 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