202110727-PERFORM-STUDENT-WORKBOOK-SCIENCE-G09-FY_Optimized

practice workbook science Grade 9 Name: Roll No: Section: School Name:

by classklap IMAX is India’s only customised content and educational assessment m. 610+ Published Books Team of IITians & PhDs IMAX Program has authored about 610+ Content development and automation are publications which are used by more than led by a team of IITians, data scientists and 4,50,000+ students. education experts Workshops Lakh Assessments IMAX Program has conducted IMAX Program has conducted more than teacher training workshops for more 85,00,000+ assessments across 17 states in the last 10 years. than 15,000+ teachers. Copyright © 2020 BGM Policy Innovations Pvt Ltd) All rights reserved. No part of this publication, including but not limited to, the content, the presentation layout, session plans, themes, key type of sums, mind maps and illustrations, may be reproduced, stored in a retrieval system or transmitted, in any form or by any means (electronic, mechanical, photocopying, recording or otherwise), without the prior, written permission of the copyright owner of this book. This book is meant for educational and learning purposes. The author(s) of the book has/ have taken all reasonable care to ensure that the contents of the book do not violate any copyright or other intellectual property rights of any person in any manner whatsoever. In the event the author(s) has/have been unable to track any source and if any copyright has been inadvertently infringed, please notify the publisher in writing for any corrective action. Some of the images used in the books have been taken from the following sources www.freepik.com, www.vecteezy.com, www.clipartpanda.com Creative Commons Attribution This book is part of a package of books and is not meant to be sold separately. For MRP, please refer to the package price.

This practice book is designed to support you in your journey of learning Science for class 9. The contents and topics of this book are entirely in alignment with the NCERT syllabus. For each chapter, a concept map, expected objectives and practice sheets are made available. Questions in practice sheets address different skill buckets and different question types, practicing these sheets will help you gain mastery over the lesson. The practice sheets can be solved with the teacher’s assistance. There is a self-evaluation sheet at the end of every lesson, this will help you in assessing your learning gap.



TABLE OF CONTENT • Assessment Pattern: 40 Marks • Assessment Pattern: 80 Marks • Syllabus & timeline for Assessment Page 1: 1. Matter In Our Surroundings Page 7: 2. Is Matter Around Us Pure Page 15: 3. Atoms And Molecules Page 23: 4. Structure Of The Atom Page 30: 5. The Fundamental Unit Of Life Page 37: 6. Tissues Page 45: 7. Diversity In Living Organisms Page 53: 8. Motion Page 60: 9. Force And Laws Of Motion Page 69: 10. Gravitation Page 75: 11. Work And Energy Page 82: 12. Sound Page 89: 13. Why Do We Fall Ill? Page 98: 14. Natural Resources Page 105: 15. Improvement In Food Resources







ASSESSMENT PATTERN Grade 9 / Science Max Internal PAPER: BEGINNER PAPER: PROFICIENT Mark Option Q.No Skill Level Difficulty Level Skill Level Difficulty Level Easy Medium Difficult Easy Medium Difficult Section A (Question Type: VSA) 11 Remembering • Remembering • 21 Understanding • Understanding • 31 Remembering • Remembering • 41 Understanding • Understanding • 51 Remembering • Remembering • 61 Remembering • Remembering • 7 1 • Remembering • Remembering • 81 Remembering • Remembering • 91 Understanding • Understanding • 10 1 • Understanding • Understanding • Section B (Question Type: SA) 11 3 • Remembering • Remembering • 12 3 Understanding • Understanding • Section C (Question Type: LA) 13 5 • Remembering • Remembering • 14 5 • Understanding • Understanding • 15 5 Applying • Applying • Section D (Question Type: LA) 16 3 Applying • Applying • 17 3 • Analysing • Analysing • 18 3 Analysing • Analysing • Beginner Paper: (Easy: 50%, Medium: 40%, Difficult:10%) Proficient Paper:(Easy: 40%, Medium: 40%, Difficult: 20%) Easy Question: Remembering questions directly from the text or from the given exercises. (Mostly from content of book or end of chapter exercise). Medium Difficulty Question: In-depth understanding of questions, not necessarily from the text. (Slightly modified concepts or end of chapter questions). Difficult Question: Question involving creativity like story writing, analysis question like character analysis, justification of title or extracts (mostly requires creative and thinking skills).

ASSESSMENT PATTERN Grade 9 / Science Max Internal PAPER: BEGINNER PAPER: PROFICIENT Mark Option Q.No Skill Level Difficulty Level Skill Level Difficulty Level Easy Medium Difficult Easy Medium Difficult Section A (Question Type: VSA) 11 Remembering • Remembering • 21 Remembering • Remembering • 31 Applying • Applying • 41 Remembering • Remembering • 51 Remembering • Remembering • 61 Remembering • Remembering • 71 Understanding • Understanding • 81 Understanding • Understanding • 91 Understanding • Understanding • 10 1 Understanding • Understanding • 11 1 • Remembering • Remembering • 12 1 Remembering • Remembering • 13 1 Remembering • Remembering • 14 1 Remembering • Remembering • 15 1 Applying • Applying • 16 1 Applying • Applying • 17 1 • Applying • Applying • 18 1 Applying • Applying • 19 1 • Understanding • Understanding • 20 1 Applying • Applying • Section B (Question Type: SA) 21 3 Remembering • Remembering • 22 3 Remembering • Remembering • 23 3 Understanding • Understanding • 24 3 • Understanding • Understanding • Section C (Question Type: LA) 25 5 Remembering • Remembering • 26 5 • Remembering • Remembering • 27 5 Remembering • Remembering • 28 5 • Remembering • Remembering • 29 5 Understanding • Understanding • 30 5 • Understanding • Understanding • Section D (Question Type: SA) 31 3 • Applying • Applying • 32 3 Applying • Applying • 33 3 • Analysing • Analysing • 34 3 Analysing • Analysing • 35 3 • Analysing • Analysing • 36 3 Analysing • Analysing •

SYLLABUS FOR ASSESSMENT Grade 9 / Science CHAPTERS PT-1 TE-1 PT-2 MOCK 1. Matter In Our Surroundings ✓ ✓ ✓ 2. Is Matter Around Us Pure ✓ ✓ ✓ ✓ 3. Atoms And Molecules ✓ ✓ ✓ 4. Structure Of The Atom ✓ ✓ 5. The Fundamental Unit Of Life ✓ ✓ ✓ 6. Tissues ✓ ✓ 7. Diversity In Living Organisms ✓ ✓ ✓ 8. Motion ✓ ✓ ✓ 9. Force And Laws of Motion ✓ ✓ ✓ 10. Gravitation ✓ ✓ 11. Work And Energy ✓ 12. Sound ✓ 13. Why Do We Fall Ill? ✓ 14. Natural Resources ✓ 15. Improvement In Food Resources ✓ Periodic Test-1 Assessment Timeline Term 1 Exam 1st July to 31st July Periodic Test-2 Term 2 Exam 23rd September to 21 October 16th December to 13th January 17th February to 9th March



LESSON WISE PRACTICE SHEETS (This section has a set of practice questions grouped into different sheets based on different concepts. By answering these questions you will strengthen your subject knowledge. A self-evaluation sheet is provided at the end of every lesson.)

1. Matter In Our Surroundings Learning Outcomes • Explain latent heat of vapourisation. • Explain latent heat of fusion. By the end of this unit, a student will be able to: • Define evaporation. • Define matter. • Distinguish between evaporation and boiling. • Enlist the characteristics of matter. • Explain the factors that affects the rate of • Differentiate between the states of matter. • Explain the effects of heat and pressure on states evaporation. • Explain how evaporation causes cooling. of matter. • Define various stages involved in interconversion of matter. Concept Map Matter Characteristics of matter States of matter Interconversion of states matter 1. Solid 1. Solidification 2. Liquid 2. Fusion 3. Gas 3. Vapourisation 4. Condensation 5. Sublimation Key Points moving more freely. This change in energy leads to change of state of matter. • All substances that are existing in this universe • The amount of heat energy that is required to is matter. Matter is anything that has mass and change 1 kg of a solid into liquid at atmospheric occupies space. Matter exists in three states i.e. pressure at its boiling point is known as the latent solid, liquid and gas. heat of fusion. • The temperature at which a liquid starts boiling at • Characteristics of matter- the atmospheric pressure is known as its boiling • Matter is made up of particles. Particles of matter point. • Boiling is a bulk phenomenon. Particles from the are called atoms, which cannot be seen by our bulk of the liquid gain enough energy to change naked eyes. into the vapour state. • Particles of matter are in continuous motion. • The amount of heat energy that is required to Therefore, particles possess certain amount of change 1 kg of a liquid into gas at atmospheric kinetic energy. pressure at its boiling point is known as the latent • Particles of matter have space between them. heat of vaporization. • Particles of matter attract each other. • Applying pressure and reducing temperature can • Interconversion of states of matter- On increasing liquefy gases. the temperature of solids, the kinetic energy of the • Evaporation is a surface phenomenon. particles increases. Due to the increase in kinetic • Particles from the surface gain enough energy energy, the particles start vibrating with greater to overcome the forces of attraction present in speed. The energy supplied by heat overcomes the liquid and change it into the vapour state. the forces of attraction between the particles. The particles leave their fixed positions and start 1

1. Matter In Our Surroundings This phenomenon of change of a liquid into vapours at any temperature below its boiling point is called evaporation. • The rate of evaporation depends upon the surface area exposed to the atmosphere, the temperature, the humidity and the wind speed. • The particles of liquid absorb energy from the surroundings to regain the energy, lost during evaporation. This absorption of energy from the surroundings make the surroundings cold. This is how evaporation causes cool- ing. Keywords: Latent heat of fusion, latent heat of vapourisation, condensation, evaporation, kinetic energy, fusion, diffusion, sublimation Work Plan CONCEPT CONCEPT COVERAGE PRACTICE SHEET SIMULATION Physical nature of • Matter is made up of Demonstration of matter particles. properties of Solids, Liquids & Gases • Particles of matter are in PS-1 continuous motion. Effect of change of • Particles of matter have temperature - Conversion space between them. PS-2 of Ice to Water • Particles of matter attract each other. States of matter • Solid • Liquid • Gas Effect of change of • Fusion Effect of change temperature and • Latent heat of fusion of temperature pressure • Solidification - Sublimation of • Vapourisation PS-3 Ammonium Chloride • Latent heat of vapourisation • Condensation • Sublimation Evaporation • Evaporation Factors Affecting • Factors affecting rate of Evaporation PS-4 evaporation Worksheet for “Matter in our Surroundings” PS-5 Evaluation with self- Self-evaluation check or Peer check* Sheet 2

PRACTICE SHEET - 1 (PS-1) I. State whether the following statements are III. Answer each of these questions. true or false. 1. What is matter? 1. Particles of matter cannot be seen by our 2. Volume of a solution does not increase when naked eyes. sugar dissolves completely in water. Why? 2. Particles of all matter have equal space 3. List out the characteristics of particles of between them. matter. 4. How is it possible for aquatic plants and II. Choose and circle the most appropriate option animals to breathe under water? for each of the following statements. 1. Particles in matter possess ______________. energy a. Kinetic energy b. Potential energy c. Mechanical energy d. Electrical energy 2. Ability of matter to be able to fit in a smaller space is called _____________. a Diffusion b. Compressibility c. Expansion d. Vibration 3. Particles possess certain amount of kinetic energy because ______________. a. They are in continuous motion. b. They have space between them. c. There are forces of attraction between them. d. They are too small in size. PRACTICE SHEET - 2 (PS-2) 1. State whether following statements are true or false. 1. Liquids are also known as fluids because of their ability to flow. 2. The movement of gas particles is in random direction. 3. Solids are highly compressible. 4. Density of solids is the highest amongst the three states of matter. 2. Answer each of these questions. 1. Why do solid particles have low kinetic energy? 2. Solids cannot be compressed. Why? 3. Gases are highly compressible. How is this property useful to us? 4. When a tea bag is placed in a cup of hot water, the colour of the water changes. Why? 3

PRACTICE SHEET - 3 (PS-3) I. Choose and circle the most appropriate option for each of the following statements. 1. The change of state from solid to gas without undergoing liquid state is called _______. a. Melting b. Evaporation c. Sublimation d. Freezing 2. An example of sublimable substance is __________________. a. Dry ice b. Sodium chloride c. Ice d Coal 3. The phenomenon of intermingling of particles is called ____________. a. Melting b. Evaporation c. Sublimation d. Diffusion 4. Boiling point of water in Kelvin scale is __________. a. 100K b. 273K c. 373K d. 0K 2. Answer each of these questions. 1. What is the latent heat of fusion? 2. Write two methods to liquefy a gas. 3. Define melting point. 4. Define latent heat of vapuorisation. 5. Why do particles of gas exert force on the container? PRACTICE SHEET - 4 (PS-4) 1. Fill in the blanks. 1. The phenomenon of change of a liquid into vapours at any temperature below its boiling point is called _______________. 2. The absorption of _________ from the surroundings make the surroundings cold during evaporation. 2. Answer each of these questions. 1. Explain the factors that affect rate of evaporation. 2. Why do we feel comfortable wearing cotton clothes in summer? 3. Why is evaporation a surface phenomenon? 4. Why is boiling a bulk phenomenon? 4

PRACTICE SHEET - 5 (PS-5) I. Choose the correct option 8. When a teaspoon of solid sugar is dissolved in a glass of water, what phase/phases are present 1. Which has the least energetic molecules? after mixing? a. Plasmas a. solid b. Liquids b. gas c. Solids c. solid and liquid d. gases d. only liquid 2. The standard room temperature is taken as: 9. Choose the correct matching. a. 100O C b. 20O C List – I List – II c. 298 K d. 273 K A. Increase in 1. Evaporation increases surfacearea 3. The force of attraction between the particles of matter is maximum in: B. Decrease in 2. Evaporation a. dry air temperature decreases b. iron rod c. kerosene oil C. Evaporation 3. Bulk phenomenon d. glycerine D. Boiling 4. Surface phenomenon 4. The rate of diffusion decreases: a. with decrease in temperature A BC D b. with increase in temperature a. 4 23 1 c. no effect of temperature b. 2 13 4 d. when the density of a solvent decreases c. 1 24 3 d. 1 43 2 5. Which of the following indicates the relative randomness of particles in the three states of 10. Which of these will not change the state of mat- matter? ter? a. gas > liquid > solid a. crushing a crystal b. Liquid < solid < gas b. pressure c. Liquid > gas > solid c. temperature d. solid > liquid > gas d. electricity 6. What colour of vapours are formed during the II. Short Answer Questions: sublimation of solid Iodine? 1. What is the effect of pressure on boiling point? a. Colourless 2. Why does it take more time for the clothes to b. Orange c. Black dry in monsoon season than in the dry season? d. Purple (violet) 3. Why do solids expand on heating? 7. If we add common salt in water, its freezing III. Long Answer questions: point: 1. State the various factors that affects the evapo- a. remains the same b. decreases ration. Explain. c. increases 2. a. Does rubbing ice on a burnt part of the body d. cannot be determined reduce pain? Give reasons. b. Why is the melting point of a substance very important? 5

Self-Evaluation Sheet Marks: 15 Time: 30 Mins 1. Answer these questions. (10 Marks) 2. Fill in the blanks. (5 Marks) 1. ___________ keeps the particles of matter A sample of liquid was heated in a test tube. The together. temperature of the solid was measured after 2. __________ particles tend to maintain their every 5 minutes. The results obtained are shown shape even when subjected to outside force. below. 3. The melting point of ice is ______K. Time in minutes Temperature in 0C 4. _____________ is the amount of water 00 vapour present in air. 5 20 5. The energy possessed by the particles in motion is _____ energy. 10 30 15 42 20 42 1. What is the boiling point of the liquid? Justify your answer. 2. An air bubble rises from the bottom of an ocean. As it rises, the bubble gets bigger. Why? 3. How is it possible to transport large volumes of CNG and LPG in cylinders? 4. Which is the correct method of storing dry ice? Why? 5. On heating, diffusion becomes faster. Why does this happen? 6

2. Is Matter Around Us Pure? Learning Outcomes • List out applications of - Evaporation, Centrifugation, Separating funnel, Sublimation, By the end of this unit, a student will be able to: Chromatography, Distillation, Crystallization • Define matter. • Classify mixture as suspension, colloids and • Differentiate between physical and chemical changes. solution. • Differentiate between suspension, colloids and • Define elements and compounds. • Classify elements as metals, metalloids and non- solution. • List out the properties of suspension, colloids and metals. • List out the physical properties of metals and solution. • Calculate the concentration of solution. non-metals. • Explain the following methods of separation - Evaporation, Centrifugation, Separating funnel, Sublimation, Chromatography, Distillation and Crystallization Concept Map Key Points • A solution has two components i.e. solvent and a solute. The component of the solution that • A mixture contains more than one substance dissolves the other component in it is called the (element and/or compound) mixed in any solvent. The component of the solution that is proportion. dissolved in the solvent is called the solute. A solution is a homogeneous mixture of solute and a • Mixture is further classified as homogeneous solvent. mixture and heterogeneous mixture. homogeneous mixture is formed when the • A solution becomes saturated when no more components of a mixture completely mix with solute can be dissolved in a solution at a given each other and are uniform throughout. While in temperature. The amount of the solute, present in Heterogenous mixture, the components of mixture the saturated solution at this temperature is called do not completely mix with each other and the its solubility. composition is not uniform throughout. 7

2. Is Matter Around Us Pure? • Below given are the ways of expressing the the sedimentation of heterogeneous mixtures. concentration of the solution. • Using separating funnel- A separating funnel is a Mass by mass percentage of a solution separation technique that is used for two liquids ‫݁ݐݑ݈݋ݏ݂݋ݏݏܽܯ‬ ‫ͲͲͳݔ‬ that do not dissolve in each other. ‫݊݋݅ݐݑ݈݋ݏ݂݋ݏݏܽܯ‬ • Sublimation process can be used to separate sublimable volatile substance from a non- Mass by volume percentage of a solution sublimable substance. • Chromatography is the technique used for ‫݁ݐݑ݈݋ݏ݂݋ݏݏܽܯ‬ ‫ͲͲͳݔ‬ separation of those solutes that dissolve in the ܸ‫݊݋݅ݐݑ݈݋ݏ݂݋݁݉ݑ݈݋‬ same solvent. This process depends on the difference in solubilities between two substances • A suspension is a heterogeneous mixture in which present in the mixture. the solute particles do not dissolve but remain • Distillation is used for the separation of suspended throughout the bulk of the medium. components of a mixture, containing two miscible • A colloid is a heterogeneous mixture in which very liquids that boil without decomposition and have small particles of one substance are distributed sufficient difference in their boiling points. evenly throughout another substance. The particle • Fractional distillation can be used to separate a size is relatively small as compared to that of mixture of two or more miscible liquids when the a suspension, thus the mixture appears to be difference in boiling points is less than 25 K. Air is a homogeneous. homogeneous mixture and can be separated into • As the size of particles is very small, we cannot see its components by fractional distillation. them with naked eyes. However, colloidal particles • Crystallisation is a process that separates a pure can easily scatter a beam of visible light. This solid in the form of its crystals from a solution. scattering of a beam of light is called the Tyndall • Physical change is a process in which the effect. substance experiences change in its physical • Colloidal solutions are made up of two properties like shape, size, colour, volume, components i.e. the dispersed phase and the appearance, state (i.e. solid, liquid, gas), etc., dispersion medium. The solute-like component without making any change in their molecular or the dispersed particles in a colloid, form the composition. These changes can be reversed dispersed phase, and the component in which using simple physical methods. Chemical change the dispersed phase is suspended is known as the is the process in which the atoms of one or dispersing medium. more substances are rearranged or combined • Heterogenous mixtures can be separated using to form a new substance. When a substance methods like handpicking, sieving and filtration. undergoes a chemical change, the chemical But when the size of the particles is very small properties of the substance changes and it is and they are uniformly suspended in the solution, transformed into a different substance with some of the following techniques should be used different chemical composition. Chemical change to separate them. can be characterized by evolution of energy, the • Evaporation- We can separate the volatile solvent formation of bubbles, change in odour, change in from its non-volatile solute by the method of temperature. evaporation. Keywords: Solution, Colloid, Tyndall Effect, • Centrifugation- Centrifugation is a process which Suspension, Centrifugation, Separating Funnel, involves the application of the centrifugal force for Sublimation, Chromatography, Fractional Distillation, Condenser, Crystallisation. 8

2. Is Matter Around Us Pure? Work plan CONCEPT CONCEPT COVERAGE PRACTICE SIMULATION SHEET Types of mixtures • Solution PS-1 Preparation of Mixtures • Suspension PS-2 (homo & hetero) • Colloids PS-3 Suspension, Colloidal Separation of • Evaporation PS-4 Solution and True Solution mixture • Separating funnel PS-5 Separation of a mixture of • Sublimation • Chromatography two Immiscible Liquids • Distillation Separation of Dyes in Black • Fractional Ink Using Chromatography Separating the Components distillation • Crystallisation of a Mixture Separation of a mixture Physical and • Examples of of two miscible liquids by chemical changes physical and chemical changes Distillation Fractional Distillation Pure substances • Elements • Compounds Working of Water • Solve PS 4 Purification System Worksheet for “Is Matter around us Pure?” Exercise and Self- evaluation 9

PRACTICE SHEET - 1 (PS-1) I. State whether following statements are true II. Answer each of these questions. or false. 1. Write any two similarities between 1. Pure substances are further classified as suspension and colloid. homogeneous and heterogenous mixtures. 2. What are colloids? Write any three 2. Suspension shows tyndall effect. applications of colloids. 3. Solution is a homogenous mixture. 3. Mixture of sand in water is an example of 4. Particle size of colloid ranges from 1nm to suspension. Justify the statement. 1000nm. 4. What is a solution? List out the properties of solution. PRACTICE SHEET - 2 (PS-2) I. Answer each of these questions. 1. What is the principle of a separating funnel? How is a separating funnel used in metallurgy? 2. Write any two applications of centrifugation. 3. Gases are highly compressible. How is this property useful to us? 4. How would you separate the ammonium chloride from the mixture of ammonium chloride with sodium chloride? Draw a neatly labelled diagram to show the experiment. 5. Which method can be used for separating a mixture of ink and water? PRACTICE SHEET - 3 (PS-3) I. Choose and circle the most appropriate option 2. During distillation, the vapours are liquified for each of the following statements. in the _____. 1. Chromatography depends on one the following factors 3. A _____ is a mixture of two or more colours. (a) Colour of solute 4. We can separate the volatile solvent from its (b) Density of solution (c) Solubility of solute non-volatile solute by the method of ____. (d) Temperature of the solution III. Answer these questions. 2. A mixture of camphor powder and table salt can be separated by 1. Why is crystallisation method efficient than (a) Using separating funnel simple evaporation? (b) Sublimation process (c) Crystallisation 2. Observe the following diagram and identify (d) Magnetic separation the method of separation. Why has yellow 3. The separation method that crystallises out colour reached greater height as compared the pure solid from its solution is to other colours? Write any two applications (a) Filtration of this method of separation. (b) Crystallisation (c) Evaporation (d) Sedimentation II. Fill in the blanks. 1. ____________ is a tube packed with glass beads. 10

PRACTICE SHEET - 4 (PS-4) I. Write one/two words answers for each of these. 1. A form of matter that cannot be broken down by chemical reactions into simpler substances. 2. A solution that has dissolved as much solute as it is capable of dissolving at a given temperature. 3. A mixture of two or more metals. 4. A metal which is liquid at room temperature. 5. Elements which show properties of both metals and non-metals. II. Answer each of these questions. 1. Silicon is used as semi-conductors in electrical circuits. Why does silicon partially conduct electricity? 2. How is oxygen separated from the air? 3. Why is fractional distillation more efficient than simple distillation or what is the advantage of fractionating column in the process of fractional distillation? 11

PRACTICE SHEET - 45 (PS-45) I. Choose the correct option b. Can be a true solution or a colloidal solution c. A suspension 1. Brass contains d. A colloidal solution a. Zinc and silver b. Copper and silver 8. Which one of the following is correctly matched? c. Copper and zinc a. Emulsion – curd d. Gold and copper b. Foam – mist c. Aerosol – smoke 2. Which of the following upon shaking with water d. Solid sol – cake will not form a true solution? a. Alum 9. List-I List-II b. Common salt c. Sucrose A. Fog 1. Solid in gas d. Albumin B. Smoke 2. Solid in solid 3. Purity of a solid substance can be checked by its characteristic: C. Steel 3. Solid in liquid a. Melting point b. Boiling point D. Toothpaste 4. Liquid in gas c. Solubility in alcohol d. Solubility in water Code: 4. Which of the following will show Tyndall effect? ABCD List-II a. Copper sulphate solution a. 1 2 4 3 b. Starch solution b. 4 1 2 3 c. Sodium chloride solution c. 1 3 2 4 d. Sugar solution d. 1 4 3 2 5. Principle of chromatography is 10. List-I a. Rate of adsorption b. Rate of absorption A. Salt solution 1. Suspension c. Rate of diffusion d. None of these B. Blood 2. Colloid 6. A 15% alcohol solution means C. Smoke 3. True solution a. 15 ml water and 85 ml alcohol b. 15 ml alcohol and 85 ml water D. Chalk water 4. Emulsion c. 15 ml alcohol and 100 ml water d. 15 ml alcohol and 50 ml water Code: 7. A small amount of the sample of a soil was ABCD mixed with water in beaker. After stirring for a. 3 4 2 1 sometime, the beaker was allowed to stand. The b. 2 4 3 1 mud was found to settle down. The c. 4 2 1 3 liquid above the mud was carefully filtered. The d. 2 4 1 3 filtrate will be a. A true solution 12

PRACTICE SHEET - 5 (PS-5) II. Short Answer Questions: 1. Identify the following as either a physical or a chemical property. a. Soap is slippery. b. Gold does not rust. c. Water freezes at 0o C. d. Cooking gas burns in air to give a flame. e. Ice melts when kept outside the fridge 2. Assign reasons regarding salt solution as mixture. 3. In the following questions, a statement of assertion is followed by a statement of reason. Mark which is correct and incorrect. a. Assertion: In sublimation, a substance changes directly from solid to vapour without passing through liquid state and vice-versa. Reason: Distillation involves two processes i.e., vapourisation and condensation. III. Long Answer questions: 1. List few applications of colloids. 2. How will you justify that water is a compound? 13

Self-Evaluation Sheet Marks: 15 Time: 30 Mins I. Choose and circle the most appropriate option II. Answer these questions. (4 Marks) for each of the following statements.(4 Marks) 1. Brass is a 1. Why is it impossible to separate solution by a. Compound filtration method? b. Element c. Homogeneous mixture 2. It is advisable to extract sugar from c Heterogeneous mixture sugar solution through the process of crystallisation and not by evaporation. Why? 2. A colloid which has liquid in its dispersed phase as well as in dispersed medium is 1. State whether the following statements are a. Emulsion true or false. (3 Marks) b Aerosol c. Sol 1. A mixture of iron powder and sulphur powder d. Gel can be separated using a magnet. 3. Solubility of a solute in its solvent can be enhanced by one of the following factors a. Density b. Temperature c. Mass of solute d. Pressure 4. Colloidal solution being a heterogenous mixture, exhibits Tyndall effect because a. Particle moves at faster speed b. Particles are smaller in size c. Particles are larger in size d. Particles are stationary II. Answer these questions. (4 Marks) 2. Gemstone is an example of liquid -solid colloid. 1. 2g of dye is added to 25g of non-volatile 3. Solutions respond to Tyndall effect. alcohol to make 50 ml of ink. Find its concentration by mass and concentration by volume at this temperature. 14

3. Atoms And Molecules Learning Outcomes using criss-cross method. • Calculate molecular mass, formula mass, number At the end of this lesson, students will be able to: • State the law of chemical combination. of moles and number of particles. • State Dalton’s atomic theory. • Differentiate between an atom and molecule. • Write the symbols of various atoms. • Differentiate between a cation and an anion. • Predict the chemical formulae of compounds Concept Map Atoms And Molecules Laws Of Chemical ChemiFcoarlmSyumlabeol And MoleculaCroMnacsespAt nd Mole Combination Key Points • An ion is a charged particle and can be negatively or positively charged. A negatively • An atom is the smallest unit of matter that has charged ion is called an ‘anion’ and the the properties of constituent element. positively charged ion, a ‘cation’. • Law of conservation of mass states that mass • The molecular mass of a substance is the sum can neither be created nor destroyed in a of the atomic masses of all the atoms in a chemical reaction. molecule of the substance. • Law of definite proportions states that “In a • The mole is the amount of substance that chemical substance the elements are always contains the same number of particles (atoms/ present in definite proportions by mass”. ions/ molecules/ formula units etc.) as there are atoms in exactly 12 g of carbon-12. • According to Dalton’s atomic theory, all matter, whether an element, a compound or a mixture • The avogadro constant 6.022 × 1023 is defined is composed of small particles called atoms. as the number of atoms in exactly 12 g of carbon-12. • Chemical symbols are used to represent 15 elements which is approved by IUPAC. • Carbon-12 isotope was chosen as the standard reference for measuring atomic masses. • One atomic mass unit is a mass unit equal to exactly one twelfth (1/12th) the mass of one atom of carbon-12. • A molecule can be defined as the smallest particle of an element or a compound that is capable of an independent existence and shows all the properties of that substance.

3. Atoms And Molecules Work Plan Concept Sub-Concept Practice Sheet Simulation PS-1 Matter and law of • Ancient theories of parti- PS-2 Activity to chemical combina- cles demonstrate law tion PS-3 • Law of conservation of of mass conservation of • Law of constant proportion mass • Dalton’s atomic theory Models • Definition of atom and molecule • Atomic size Concept of atom and • Chemical symbols molecule proposed by Dalton • Atomic mass • Molecules of elements • Molecules of compounds Chemical formulae, • Concept of ion Molecular mass and • Symbols and valences of mole concept cations and anions • Formulae of compounds • Calculation of molecular mass • Calculation of formula mass • Mole concept Worksheet for \"Atoms and Molecules\" PS- 4 Evaluation with self- Self-evaluation check or Peer check* Sheet 16

PRACTICE SHEET - 1 (PS-1) I. Choose and circle the most appropriate option for each of the following statements: 1. In ammonia, nitrogen and hydrogen are always present in the ______ ratio by mass. a. 14:3 b. 1:4 c. 3:4 d. 1:3 2. 3 g of carbon combines with ______ of oxygen to form CO. a. 3 g b. 10 g c. 4 g d. 5 g 3. Maharishi Kanad termed the smallest particle of matter as ___ a. Padarth b. Paramanu c. Kannu d. vasthu 4. In water, oxygen and hydrogen are always present in the ______ ratio by mass. a. 1:8 b. 8:1 c. 3:4 d. 1:7 5. _____ established two important laws of chemical combination. a. Maharishi Kanad b. Antoine L Lavoisier c. Democritus d. John Dalton II. State whether the following statements are true or false: 1. During a chemical reaction, the sum of themasses of the reactants and products change. 2. Dalton was the first scientist to use the symbols for elements in a very specific sense. 3. Dalton called the indivisible particles as atoms. III. Answer each of these questions: 1. State the laws of chemical combination. 2. Atoms combine in the ratio of small whole numbers to form compounds. Justify the statement giving an example. 17

PRACTICE SHEET - 2 (PS-2) I. Choose and circle the most appropriate option for each of the following statements: 1. Atomic radius is measured in ___________. a. millimetres b. nanometres c. centimetres d. inch 2. ___________ isotope was chosen as the standard reference for measuring atomic masses. a. carbon -14 b. carbon - 12 c. carbon -13 d. cobalt 3. Example of a diatomic molecule is _________. a. sodium b. calcium c. chlorine d. cobalt 4. A group of atoms carrying a charge is known as a ____________. a. cation b. anion c. polyatomic ion d. molecule 5. ________ is the smallest particle of the element that can exist independently and retain all its chemical properties. a. atom b. molecule c. ion d. radical II. Write the valencies of following ions: 1. Sodium 2. Potassium 3. Chloride 4. Iodide 5. Nitride 6. Sulphide 7. Hydrogen carbonate 8. Magnesium 9. Zinc 10. Oxide III. Answer each of these questions: 1. Define relative atomic mass. 2. Define molecular mass. 3. Give one point of difference between atoms and molecules. 18

PRACTICE SHEET - 3 (PS-3) I. Answer each of these questions: 1. Define one mole. 2. What does Avogadro number represent? 3. Give one point of difference between each of these- a. Atom and ion b. Anion and cation c. Molecular mass and formula mass 4. Calculate the molecular mass and formula mass of- a. gCe2Hn6=. (atomic weights – carbon = 12, hydro- 1) b. Hydrogen peroxide (atomic weights – oxy- gen = 16, hydrogen = 1) 5. Iron shows variable valency. Write the chemical formula of a compound which is formed by combining Iron (both valencies) with Chlorine. Calculate their molecular weight. (atomic weights – Iron=56, Cl=35.5) 6. How can we relate mole, Avogadro number and mass? 19

PRACTICE SHEET - 4 (PS-4) 8. All samples of carbon dioxide contain carbon and oxygen in the mass ratio 3:8. This is in I. Choose the correct option: agreement with the law of a. Constant proportions 1. Chemical formula of ferric oxide is b. Multiple proportions a. FeO c. Gaseous volumes b. Fe3O4 d. Conservation of mass c. Fe2O3 d. None of these 9. Directions for 9 and 10: In this section, each question has two matching 2. “All matter is made up of very small particles lists. Choices for the correct combination of ele- which cannot be further broken down. These ments from List-I and List-II are given as options particles are called atoms”. This statement is one (a), (b), (c) and (d) out of which one is correct. of the assumptions of (Hint: Atomic Mass) a. Rutherford’s nuclear theory b. Dalton’s atomic theory List-I List-II c. Kinetic theory of gases. A. Calcium 1. 14 d. Bohr’s theory B. Nitrogen 2. 16 C. Oxygen 3. 23 3. An atom is the D. Sodium 4. 40 a. Smallest particle of matter known CODE: b. Smallest particle of gas ABCD c. Smallest particle of an element that can take part a. 3 4 1 2 in a chemical change d. Radioactive emission b. 2 3 4 1 4. Molecular mass is defined as the c. 4 1 2 3 a. Mass of one molecule of any substance compared with the mass of one atom of C-12 d. 1 2 3 4 b. Mass of one atom compared with the mass of one molecule 10. List-I List-II c. Mass of one atom compared with the mass of one A. 52 g of He 1. 2 moles atom of hydrogen B. 8 g of O2 2. 1 mole d. None of the above C. 2 g of H2 3. 0.25 mole D. 56 g of N2 4. 13 mole 5. Molecules of ammonia and phosphorous are re- CODE: spectively ABCD a. Monoatomic and triatomic b. Tetratomic and tetratomic a. 4 3 2 1 c. Monoatomic and diatomic b. 1 4 3 2 d. Tetratomic and triatomic c. 2 3 1 4 d. 4 2 3 1 6. Number of moles of water present in 180 g of wa- ter will be II. Short Answer Questions: a. 18 b. 15 1. Give the chemical formula, for each of the c. 5 following acids: d. 10 a. Nitric acid – 7. Mass of 3 moles of NaOH in grams is b. Hydrogen bromide - a. 240g c. Carbonic acid – b. 120g d. Hypochlorous acid - c. 69g e. Iodic acid – d. 100g f. Sulphurous acid – 20

PRACTICE SHEET - 4 (PS-4) 2. What is the mass of 0.5 mole of water (H2O)? (Atomic masses : H = 1u, O = 16u) 3. a. Why does not the atomic mass of an element represent the actual mass of its atom? b. What happens to an element X if its atom gains two electrons? III. Long Answer questions: 1. What is the difference between the actual mass of a molecule and gram molecular mass? 2. Which amongst the following has a greater number of atoms? a. 11.5 g of sodium, or b. 15 g of calcium (Na = 23; Ca = 40) 21

Self-Evaluation Sheet Marks: 15 Time: 30 Mins I. Fill in the blanks: (3 Marks) 1. The number of atoms constituting a molecule is known as its _____________. 2. Ratio by mass of sodium chloride is _________. 3. Mass of 1 mole of a substance is called its _______. II. Answer each of these questions: 1. Why was oxygen considered as a reference for calculating atomic masses? (2 Marks) 2. Calcalute the number of molecules present in 108g of water molecule. (2 Marks) 3. Name each of these compounds – Mg3(PO4)2, Al2(CO3)3, NH4Br, H2CO3, CaH2, Zn(H(C3OM3a)2rks) 4. Write the postulates of Dalton’s atomic theory. (5 Marks) 22

4. Structure Of The Atom Learning Outcomes At the end of this lesson, students will be able to: • Define valency, atomic number and mass • State the postulates of each of these theories - number. Thomson’s model, Rutherford’s model, Bohr’s • Represent the atom in the correct notation. model, Chadwick’s theory. • Calculate the mass number and average atomic • Understand the reasons as to why some theories/ mass. models were discarded. • Define isotopes and isobars. • Explain the distribution of electrons in the • List out the applications of isobars. respective shells. Concept Map Structure of the atom Models/theoofraietosmon structure Valencym, aatsosmniucmnubmerber and Isotopes and Isobars Thomson’s model • Drawbacks of Rutherford’s model of the atom. Rutherford’s model The orbital revolution of the electron is not expected to be stable. Any particle in a circular Bohr’s model orbit would undergo acceleration. During J. Chadwick’s theory acceleration, charged particles would radiate energy. Thus, the revolving electron would lose Key Points energy and finally fall into the nucleus. • Dalton’s atomic theory suggested that the • Neil Bohr put forward the following postulates atom was indivisible and indestructible. But about the model of an atom: the discovery of two fundamental particles (electrons and protons) inside the atom, led » Only certain special orbits known as discrete to the failure of this aspect of Dalton’s atomic orbits of electrons, are allowed inside the theory. For explaining this, many scientists atom. proposed various atomic models. » While revolving in discrete orbits the • Thomson proposed that: electrons do not radiate energy. » An atom consists of a positively charged sphere and the electrons are embedded in » These orbits or shells are represented by it. the letters K, L, M, N… or the numbers, n = 1, » The negative and positive charges are equal 2,3,4.. in magnitude. So, the atom as a whole is electrically neutral. • J. Chadwick discovered another subatomic particle named neutron. It does not carry any • Rutherford concluded from the α-particle charge and mass is nearly equal to that of a scattering experiment that– Most of the space inside the atom is empty. The positive charge 23 of the atom occupies very little space. All the positive charge and mass of the gold atom were concentrated in a very small volume within the atom.

4. Structure Of The Atom proton. • The electrons present in the outermost shell of an atom are known as the valence electrons. Valency can be also known as combining capacity of an atom. • Atomic number is defined as the total number of protons present in the nucleus of an atom. It is denoted by the letter ‘Z’. • Protons and neutrons collectively are also called nucleons. • Isotopes are defined as the atoms of the same element, having the same atomic number but different mass numbers. • Atoms of different elements with different atomic numbers, which have the same mass number, are known as isobars.   Key words – Atom, molecule, valency, alpha particle, isotope, isobar, neutrons, protons, electrons 24

4. Structure Of The Atom Work Plan Concept Sub-Concept Practice Sheet Simulation PS-1 Models Charged particles in • Charged particles in matter PS-2 matter • Thomson’s model of an and the structure of PS-3 an atom atom PS-4 The structure of an • Rutherford’s model of an atom Isotopes atom • Bohr’s model of an atom • Discovery of neutrons • Distribution of electrons in different shells • Valency • Atomic number and mass number • Isotopes • Average atomic mass • Applications of isotopes • Isobars Worksheet for \"Structure Of The Atom\" Evaluation with self- check or Peer check* Self-evaluation Sheet 25

PRACTICE SHEET - 1 (PS-1) II. Answer each of these questions: I. Choose and circle the most appropriate option 1. Why did Rutherford choose gold foil for his for each of the following statements: experiment? 1. In Rutherford’s experiment, fast moving ___ particles were made to fall on a thin gold 2. Why is atom electrically neutral? foil. 3. Write the inferences for the following a. beta b. gamma observations. c. delta d. alpha Observations Inferences 2. The mass of an ______ is about 1/2000 times the mass of a hydrogen atom. Most of the fast moving a. Proton α-particles passed straight b. Neutron through the gold foil. c. Electron d. Proton + electron Some of the α-particles 3. Alpha particles are doubly charged _____. were deflected by the foil a. Hydrogen by small angles. b. Helium c. Carbon One out of every 12000 par- d. Chlorine ticles appeared to rebound. 4. Positively charged part at the centre in an atom is the _______. 4. Explain the conclusions obtained by a. Shells Rutherford experiment. b. Nucleus c. Proton 5. Write two properties each of anode rays and d. Electron cathode rays. PRACTICE SHEET - 2 (PS-2) 6. Why was Thomson’s model of a atom compared to watermelon? Explain with the I. Fill in the blanks: help of a neat labelled diagram. 1. Elements are defined by the number of ______ they possess. 4. State the maximum capacity of each shell to 2. The maximum number of electrons that can accommodate electrons. be accommodated in the outermost orbit is _______. 5. What happens to the energy of an electron 3. _________ is defined as the sum of the total when it jumps from lower to higher energy number of protons and neutrons present in level? the nucleus of an atom. 4. _________ is the number of protons of an atom. 5. The mass of an atom resides in its _______. II. Answer each of these questions: 1. Why does carbon share electrons instead of losing or gaining? 2. Valency of hydrogen, lithium and potassium is one. Justify. 3. Which kind of atoms are tend to lose electrons? Give an example. 26

PRACTICE SHEET - 3 (PS-3) I. Fill in the blanks: 1. Tritium is an isotope of ________. 2. Chlorine occurs in nature in two isotopic forms, with masses 35 u and ______ in the ratio of 3:1. II. Complete the following table : Element Symbol Mass Atomic Protons Neutrons Electrons Number Number 5 Boron B 65 Sodium Na 11 5 12 Copper Cu 11 35 Magnesium Mg 24 29 12 III. Answer each these questions: 1. Give one point of difference between isotopes and isobars. 2. Why are atoms of isotopes chemically same? 3. An atom contains 3 electrons, 3 protons and 4 neutrons. Calculate its mass number. What kind of ion will this element form? 4. The mass number of an element is 18. It contains 7 electrons. Predict the number of protons, neutrons and the name of the element. 5. Write any three applications of isotopes. 6. If nitrogen atom is available in the form of, say, two isotopes 14N(99.63%) and 15N (0.37%), calculate the average atomic mass of nitrogen atom. 7. Give an example of isobars.   27

PRACTICE SHEET - 4 (PS-4) I. Choose the correct option: 8. Which of the following statements does not form the part of Bohr’s model of hydrogen 1. Valency of oxygen is atom? a. The position and velocity of the electrons in the a. 1 orbit cannot be determined simultaneously. b. Electrons revolve in different orbits around the b. 3 nucleus. c. Energy of the electrons in the orbit is quantized. c. 4 d. The electron in the orbit nearest to the nucleus has the lowest energy. 2. d. 2 of neutrons in the element 94B is 9. Directions for Qns: 9 and 10. The number In each of the following questions, a statement a. 4 of Assertion is given, and a corresponding b. 9 statement of reason is given just below it. Of the statements, given below, mark the correct c. 5 answer as: a. If both Assertion and Reason are true and d. 13 Reason is the correct explanation of Assertion 3. Maximum number of electrons present in ‘N’ b. If both Assertion and Reason are true but Reason shell is a. 18 is not the correct explanation of Assertion b. 32 c. If Assertion is true but Reason is false c. 2 d. If both Assertion and Reason are false d. 8 Assertion : Cathode rays travel in straight lines. Reason: Cathode rays do not penetrate through 4. Which of the following elements contains only two electrons in the outermost shell? thin sheets a. Helium 10. Assertion: Isotopes are electrically neutral. b. Beryllium c. Magnesium Reason: Isotopes are species with same mass d. All of these number but different atomic numbers. 5. Isotopes have II. Short Answer Questions: a. Same chemical properties but different 1. What do you understand by ground state and physical properties b. Different chemical and physical properties excited state of an atom? c. Same chemical and physical properties 2. Calculate mass and charge on one mole of d. Same physical properties but different chemical properties electrons. 3. Justify the statement ‘atomic number of an 6. The number of electrons in the valence shell of calcium is element is equal to the number of electrons in a a. 4 neutral atom only and not in anion’. b. 2 c. 8 III. Long Answer questions: d. 6 1. List some important uses of isotopes. 7. Which of the following electronic configurations is wrong? 2. Most of the space in an atom is empty. Justify. a. Li (3) = 2,1 b. P (15) = 2,8,5 c. O (8) = 2,6 d. S (16) = 2,6,8 28

Self-Evaluation Sheet Marks: 15 Time: 30 Mins I. Write one/two words answer for each of the following questions: (5 Marks) a. Isotope of hydrogen with mass number 2. b. Sub-atomic particle carrying positive charge. d. Sodium (a metal) and chlorine (a non- c. Collective term for protons and neutrons. metal) both exhibit a valency 1. Justify the d. Smallest inert gas. statement. e. Sub-atomic particle carrying negative charge. II. Answer each of these questions: e. How does Bohr’s theory explain the emission ( 10 Marks) and absorption of energy? a. Give the actual mass of electron and proton in kg. b. How are X-rays produced? How are X-rays used in medical field? c. Percentage abundance of cobalt 35Co is 75.76% and that of 37Co is 24.24%. Calculate average atomic mass of cobalt. 29

5. The Fundamental Unit Of Life Learning Outcomes By the end of this unit, a student will be able to: • Differentiate between a plant cell and an animal • Define cell. cell • Give examples of various shapes of cell. • Explain the structure and function of plasma • Differentiate between a prokaryotic cell and a eukaryotic cell. membrane, cell wall, nucleus, cytoplasm, endoplasmic reticulum, golgi apparatus, • Explain the phenomenon of osmosis. ribosome, mitochondria, plastids and vacuoles. Concept Map Cell Structure of cell Cell organelles Plasma membrane ER Cell wall Golgi apparatus Nucleus Lysosomes Cytoplasm Mitochondria Plastids Vacuoles Key Points a selectively permeable membrane is called osmosis. It is the passage of water from a region • Cells are microscopic in size, they cannot be seen of high water concentration through a semi- by naked eyes. permeable membrane to a region of low water concentration. • Some organisms are made up of a single cell • The plasma membrane is flexible and is made up which are called as unicellular organisms. Ex- of organic molecules called lipids and proteins. ample- amoeba, paramecium, chlamydomonas, • Cell wall- Plant cells have another rigid outer bacteria, etc. Multicellular organisms are those covering called the cell wall. The cell wall lies which are made up of two or more cells. Example – outside the plasma membrane. The plant cell plants, animals, fungi, etc. wall is mainly composed of cellulose. Because of their walls, such cells can withstand much greater • Each cell is made up of various cell organelles. changes in the surrounding medium than animal These organelles together constitute the basic unit cells. called the cell. Shapes and size of cell may vary • Nucleus- The nucleus is situated at the centre of depending on their characteristics and functions. the cell which has a double layered covering called nuclear membrane. The nuclear membrane has • Plasma Membrane / Cell Membrane- This is the pores. outermost covering of the cell that separates the • Chromosomes contain information for inheritance contents of the cell from its external environment. of features from parents to next generation in the The plasma membrane allows or permits the entry form of DNA (Deoxyribose Nucleic Acid) molecules. and exit of some materials, in and out of the cell. Chromosomes are composed of DNA and protein. It also prevents movement of some other materi- • DNA molecules contain the information necessary als. The cell membrane, therefore, is called a selectively permeable membrane. • The movement of water molecules through such 30

5. The Fundamental Unit Of Life for constructing and organising cells. Functional into small pieces which enter the cell. During the segments of DNA are called genes. disturbance in cellular metabolism, for example, • Cytoplasm – The cytoplasm is the fluid content when the cell gets damaged, lysosomes may burst inside the plasma membrane which contains cell and the enzymes digest their own cell. Therefore, organelles. lysosomes are also known as the ‘suicide bags’ of • Endoplasmic Reticulum – It is a large network of a cell. membrane-bound tubes and sheets. There are two • Mitochondria – They are known as the power- types of ER– rough endoplasmic reticulum (RER) houses of the cell. The energy required for various and smooth endoplasmic reticulum (SER). RER chemical activities, needed for life is released by looks rough under a microscope because it has mitochondria in the form of ATP (Adenosine triph- particles called ribosomes attached to its surface. opshate) molecules. • The ribosomes, which are present in all active • Plastids – They are present only in plant cells. cells, are the sites of protein manufacture. ER There are two types of plastids – chromoplasts forms a network system throughout the cell to (coloured plastids) and leucoplasts (white or co- transport materials like proteins. lourless plastids). • Golgi apparatus – It consists of a system • Vacuoles – They are storage sacs for solid or liquid of membrane-bound vesicles, arranged contents. Animal cells have smaller vacuoles as approximately parallel to each other in stacks compared to the plant cells. called cisterns. Keywords: ER, Golgi apparatus, Lysosomes, • Lysosomes – They help to keep the cell clean by Mitochondria, Plastids, Vacuoles, Cell wall, Plasma digesting any foreign material as well as worn- membrane, Nucleus, Cytoplasm, hypotonic, out cell organelles. Lysosomes break foreign hypertonic, isotonic, osmosis, membrane materials such as bacteria, old organelles, etc. biogenisis, ATP 31

5. The Fundamental Unit Of Life Work Plan CONCEPT SUB CONCEPT PRACTICE SIMULATION SHEET Types of cells • Shapes Observing • Size various cells • Unicellular organisms from the human • Multicellular organisms body PS-1 Structural organisation • Plasma membrane Plasma of a cell • Cell wall membrane or • Nucleus cell membrane - • Cytoplasm osmosis with an egg Cell organelles • Endoplasmic reticulum • Golgi apparatus PS-2 • Ribosome • Lysosome Structure of a • Mitochondria PS-3 plant cell • Vacuoles • Plastid Structure of an Worksheet for”Fundamental Unit of lIfe” animal cell PS-4 Evaluation with self- Self-evaluation check or Peer check* Sheet 32

PRACTICE SHEET - 1 (PS-1) I. Name the following. 1. The instrument used to observe cells. 2 The latin word for ‘little room’. 3. The scientist who designed the first microscope. II. Fill in the blanks. 1. The plant cell wall is mainly composed of ______. 2. The cell organelle that functions both as a passageway for intracellular transport and as a manufacturing surface is _____________. III. Answer each of these questions. 1. Why is a cell called the structural and functional unit of life? 2. What is the difference between unicellular and multicellular organisms? 3. How are plants able to survive the hypotonic conditions around them? 4. Absorption of water by roots is an example of diffusion. Justify the statement. PRACTICE SHEET - 2 (PS-2) I. Fill in the blanks. II. Answer these questions. 1. The nucleus has a double layered covering 1. What is the function of vacuoles in unicellular called _________. organisms? 2. Functional segments of DNA are called 2. What is ATP? Why is it known as energy ______. currency of the body? 3. Organisms having primitive nucleus are 3. Describe the structure of mitochondria. called ______. 4. Describe different types of plastids found in a 4. RER looks rough under a microscope because plant cell. it has ____ attached to its surface. 5. Cellular membrane system consists of ER and ______. II. Answer each of these questions. 1. Describe the nucleus of prokaryotes. 2. What are the functions of Golgi apparatus? PRACTICE SHEET - 3 (PS-3) I. Fill in the blanks. 1. The energy in the mitochondria is present in the form of ____. 2. ____ and ____ synthesise their own DNA. 3. ___ are called as suicide bags of the cell. 4. _____ are the storage sacs for solids and liquids in the cell. 5. The membranous layer of plastids are called as ___. 33

PRACTICE SHEET - 4 (PS-4) I. Choose the correct option a. Fats will not be stored b. Proteins will not be formed 1. Cell wall is present in c. Respiration will not take place a. Algal cell d. Carbon assimilation will not occur b. Plant cell c. Prokaryotic cell 8. A student put five raisins each in two beakers d. All of these A and B. Beaker A contained 50 ml of distilled water and beaker B had 50 ml of saturated sugar 2. Which of the following is useful for the synthesis solution. After sometime, the student would of proteins and enzymes? observe that a. Mitochondria a. Raisins in beaker A were more swollen than b. Rough endoplasmic reticulum those in beaker B c. Smooth endoplasmic reticulum b. Raisins in beaker A did not swell up at all d. Golgi complex c. Raisins in both beakers A and B were equally swollen 3. Main difference between animal cell and plant d. Raisins in beaker B were more swollen than cell is those in beaker A a. Respiration b. Growth 9. Directions for Qns: 9 and 10: c. Nutrition In each of the following questions, a d. Movement statement of Assertion is given and a corresponding statement of Reason is given 4. 4. A cell placed in a hypertonic solution will just below it. Of the statements, given below, a. Shrink mark the correct answer as: b. Swell up c. Show plasmolysis a. If both Assertion and Reason are true and d. No change in shape or size Reason is the correct explanation of Assertion 5. The undefined nuclear region of prokaryotes is b. If both Assertion and Reason are true but also known as Reason is not the correct explanation of a. Nucleic acid Assertion b. Nucleolus c. Nucleoid c. If Assertion is true but Reason is false d. Nucleus d. If both Assertion and Reason are false Assertion:Mitochondria are known as 6. Find out the incorrect statement. a. Osmosis is a slow process, occurs down the “powerhouse” of the cell. concentration gradient and does not expend Reason: Mitochondria are used to bring energy. about energy requiring activities of the cell b. Electron microscope uses very high voltage 10. Assertion: Larger cells are more efficient electricity. It uses electromagnets instead of Reason: Surface area ratio is more in larger cells glass lenses and beam of electrons instead of light. II. Short Answer Questions: c. Active transport of materials is rapid and usually occurs against the concentration 1. Why are lysosomes also known as “scavengers gradient involving carrier proteins and energy of the cells” ? in the form of ATP. d. A semipermeable membrane does not allow 2. In brief, state what happens when both solvent and solute molecules to pass a. Dry apricots are left for some time in pure through it. water and later transferred to sugar solution. b. Rheo leaves are boiled in water first and 7. If the ribosomes of a cell are destroyed, then then a drop of sugar syrup is put on it. c. Golgi apparatus is removed from the cell. 34

PRACTICE SHEET - 4 (PS-4) 3. If cells of onion peel and RBC are separately kept in hypotonic solution, what among the following will take place? Explain the reason for your answer. III. Long Answer questions: 1. What is the difference between diffusion and osmosis? 2. When amoeba is placed in a hypertonic medi- um, it shrinks. Why does this happen? Explain. 3. Describe the structure of ER and write one general function of ER. 35

Self-Evaluation Sheet Marks: 15 Time: 30 Mins I. Answer these questions.  (4 Marks) III. Write one/two-word answer for each of the following. (5 Marks) 1. In which cell organelle does complete breakdown of glucose occur? 1. The fundamental organisational unit of life. 2. Why is the size of vacuole bigger in plants? 2. The cell organelle that functions, both as a 3. Why is inner membrane of mitochondria passageway for intracellular transport and as a manufacturing surface. highly folded? 4. Nuclei are also called as ‘brains of cells’. Why? II. Answer these questions.  (6 Marks) 3. Plastids that contribute in photosynthesis. 4. Protein manufacturer of the cell. 1. A solution of 3% sucrose and a solution of 8% sucrose are kept separated by a semi-permeable membrane. What do you observe after one hour? 5. Membranous layers embedded in plastids. 2. Why are leucoplast colourless plastids? 3. Write any two differences between a prokaryotic and a eukaryotic cell. 36

6. Tissues • List out the functions of various plant tissues. Learning Outcomes • Explain the site, structure and constituents of At the end of this lesson, students will be able to: various animal tissues. • Define tissue. • List out the functions of various plant tissues. • List out the various types of plant and animal tissues. • Explain the site, structure and constituents of various plant tissues. Concept Map Tissue Plant Tissue Animal Tissue MerTisistesumeatic PeTrmissauneent EpTiitshseuleial CoTninsesucteive Nervous Tissue PeSTrmiimssapunleeent PCeTromimssapunleeexnt Key Points specific regions because the meristematic tissue is located only at these points. • A group of cells that are similar in structure • Cell formed by meristematic tissue take up a and/or work together to achieve a particular specific role and lose the ability to divide. They function forms a tissue. further form a permanent tissue. • Parenchyma- These form the basic packing • Tissues of plants and animals show tissue which are loosely packed. It consists of considerable difference in their characteristics, unspecialised. structure, shape, size and function. 37 • Plant tissues are of two types – meristematic tissue and permanent tissue. • The growth of plants occurs only in certain