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CLASS 9

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KERALA SSLC

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EXAM

Based on Latest SCERT Textbook issued by Department of Education, Government of Kerala in 2016

Includes Onam Question Paper issued by Academic Council along with Scheme of Evaluation

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( 3 )

CONTENTS

*First Terminal Evaluation - 2016 with Scheme of Evaluation (Issued by Academic Council in November 2016) 5 - 8

th *NOTE : This is the November Examination Paper for class 9 issued by Academic council for District Education Office. It

contains questions from both Part I & Part II of the SCERT Textbook.This Oswaal Question Bank is exclusively based on

SCERT Textbook Part II. In order to purchase Oswaal Part I Question Bank contact your closest bookseller (refer to the

distributor list) or log on to www.oswaalbooks.com; flipkart.com; amazon.in.

5. ACIDS, ALKALIES AND SALTS 9 - 19

1 Acids and AlkaliesTopic :

SaltsTopic 2 :

6. COMPOUNDS OF NON-METALS 20 - 32

Ammonia—Preparation, Properties and UsesTopic 1 :

Topic 2 : Sulphuric acid–Preparation, Properties and Uses

Topic 3 : Hydrogen chloride and Nitric acid : Preparation, Properties and Uses

7. CARBON AND ITS COMPOUNDS 33 - 48

Topic 1 : Carbon and Its Allotropes

Topic 2 : Compounds of Carbon : Carbon dioxide, Carbon monoxide,

Carbonates and Bicarbonates

Topic 3 : Organic Compounds

qq

( 4 )

PREFACE

Malcolm Forbes said “Education's purpose is to replace an empty mind with an open one”

and this is something which is always followed by Government of Kerala, Department of Education,

whether through their education system framework or recent enhancement in their curriculum. The

aim of their Curriculum is not just to let learners obtain basic knowledge but to make them life-

long learners.

The purpose of this book is to nurture individuality and thus enhance one's innate potentials

which help in increasing the self-study mode for students. This book strengthens knowledge and

attitude related to subject. This book is designed in such a way that students can set their own goals

and can improve their problem solving and thinking skills.

This book is strictly as per the latest SCERT Kerala Textbook, introduced by SSLC Board in

2016. It follows the latest syllabus prescribed by the board. It contains all types of questions like

Textbook Questions, VSA Questions (Very Short Answer), SA Questions (Short Answer), MCQs

(Multiple Choice Questions) and LA Questions (Long Answer). A synopsis is given for every chapter

which contains important points from that chapter. Each chapter has high quality figures wherever

required for better, fast and clear understanding.

OSWAAL SSLC Question Bank is different and better in terms of High Quality Questions

which are developed by 'OSWAAL Expert Panel' which ensures success in examination. The Question

Bank is arranged ‘Topic-Wise’ where each topic from every chapter is explained in detail. High quality

figures and Flow charts are given to improve retention of concepts.

Through OSWAAL Books students are taught how to think, not what to think. We at

OSWAAL Books try to use quality content, standard language, creativity and high quality figures,

which makes readers to enjoy it because we believe if our readers don't enjoy reading our book then

there is no use in reading it at all. This is one of the reasons that the scope of this book extends from

students to teachers. Teachers can use this book as a perfect teaching guide and students can use

this book for good learning and practice.

At last we would like to thank our authors, editors, reviewers and specially students whom

we request to send suggestions regularly which will help in continuous improvement of this book

and will make this book “One of the Best”. Wish you all Happy Learning.

Why Topic Wise Question Banks are a Better Choice than Previous Year’s Papers ?

Question Banks Previous Years’ Papers

1. Chapter-wise and Topic –wise presentation

in Question Banks facilitates systematic

study.

2. Question Banks can be referred to by the

students throughout the year as well as at

the completion of each chapter in school.

3. Question Banks, take into account any

changes in syllabus or layout and hence are

fully updated and aligned as per the latest

specifications by the Board.

1. Year Wise presentation restricts

methodical flow of learning.

2. These can be referred to only after the

completion of the full syllabus in school.

3. Previous Years' questions cannot be

changed and hence fail to be adept with

the latest Board specifications

–Publisher

FIRST TERMINAL EVALUATION 2016CHEMISTRY

Standard : IX (Issued by Academic Council in November 2016) Score : 40

Time : 1½ hour

General Instructions : (i) First 15 minutes is given as cool off time. This time is to be used for reading and understanding the questions. (ii) Write down answers for all questions. (iii) The score for each questions is given along with the question.

1. In MgCl2, Magnesium and chlorine are held together by the attraction between anions and cations in it. Which is the anion present in it ? 1 2. Based on the symbol, 6

12C, identify the following : (a) Atomic number 1 (b) Mass number 1 (c) Number of protons 1 (d) Number of neutrons 1 3. The chemical bonding in Oxygen molecule is represented below.

O + O O O

Identify the nature of chemical bonding in this molecule. 1 4. In the table below, column A gives the names of scientists who are connected with the classification of elements

and column B gives their principles. Match A and B

A B

(a) Lavoisier(b) Chancourtoise(c) Newlands(d) Dobereiner

(a) Triads(b) Law of Octaves(c) Metals and Non-metals(d) Telluric helix

1111

5. The electronegativity values of certain elements are given below. Analyse the values and classify the following compounds into ionic and covalent systems.

Element Ca O F C K

Electronegativity 1.0 3.5 3.9 2.5 0.8

(a) Carbon monoxide (CO) 1 (b) Potassium oxide (K2O) 1 (c) Calcium flouride (CaF) 1 6. The electronic configuration of some elements are given below. (These are not actual symbols) Analyse the

configurations and answer the following questions. X – 2, 8, 6 Y – 2, 8, 8 Z – 2, 8, 1 (a) Which elements is chemically stable ? 1 (b) What is the atomic number of the element Z ? 1 (c) What is the nature of chemical bonding in the compound formed between the element Z with the element

X ? 1 7. Atoms of the same element having same atomic number but different mass numbers are called isotopes. (a) Draw the Bohr atom model of Tritium. 2 (b) Which is the fundamental particle present in Tritium, but not in Protium ? 1 (c) Write any one use for both Carbon–14 and Deuterium isotopes. 2

6 ] Oswaal Kerala SSLC Question Bank, CHEMISTRY PART–2, CLASS-IX

8. (A) The electronic configuration of two elements are represented below using dot diagrams. Analyse them and answer the following questions.

(a) Draw the electron dot diagram showing the compound formation between these two elements. 2 (b) Which is the cation ? 1 (c) Fluoride ion is formed from fluorine atom. Write the chemical equation for the reaction. 1

OR (B) (a) Illustrate the chemical bonding in CH4 using electron dot diagram (6C, 1H) . 2 (b) Write any two properties of compounds formed on the basis of such type of chemical bonding as

described above. 2 9. Analyse the following table and write the chemical formula of compounds formed by the combination of elements.

Element Valency

O 2

Zn 2

Cl 1

Ca 2

(a) Calcium (Ca) and Oxygen (O) 1 (b) Zinc (Zn) and Chlorine (Cl) 1 10. Some discoveries of certain scientists are given in the box and the statements corresponding to them are given

below. Match the suitable statements with the discoveries in the box and write down.

Law of definite proportions, Electromagnetic theory, Law of conservation of mass.

(a) A charged body in circular motion continuously emits energy as radiations. (b) There exists a simple whole number ratio between the masses of the combining elements in a compound. 2 11. Electronegativity difference is responsible for the polar nature of molecules. (a) Polar nature of Hydrogen fluoride is represented as Hd+ – Fd–. Which element is more electronegative ? 1 (b) How will you represent the polar nature of HCl ? (Electronegativity values : H–2.20, Cl–3.16) 1 12. Mg0 + 2H+1Cl–1 → MgxCl–1

2 + Hy2 Analyse the chemical reaction and answer the following questions.

(x and y are the oxidation numbers of respective atoms) (a) Identify x and y. 2 (b) Identify whether the above chemical reaction is a redox reaction. State the reason. 2 13. Identify the write the correct statements. (a) An atom has a central part called nucleus. (b) The negatively charged electrons are found inside the nucleus. (c) As distance from the nucleus increases, the energy of shells decreases. (d) The maximum number of electrons in a shell is 2n2. 2 14. Given below are some of the observations made by Rutherford on colliding alpha particles on a thin gold foil.

Write the inferences corresponding to the following observations. (a) Most of the alpha particles passed through the gold foil unaffected. 1 (b) Some alpha particles deviated in small angles. 1 (c) Only a small number of alpha particles bounced back. 1

SOLVED PAPER - 2016 [ 7

SOLUTIONS(Scheme of Valuation, 2016)

Q. No. Answer Marks

1. Cl– or Chloride ion 1

2. (a) 6 (b) 12 (c) 6 (d) 6 1 + 1 + 1 + 1

3. Double bond 1

4. (a) Lavoisier — Metals and Non metals (b) Chancourtoise — Telluric helix (c) Newlands — Law of Octaves (d) Dobereiner — Triads

1111

5. (a) Covalent (3.5 – 2.5=1) (b) Ionic (3.5 – 0.8=2.7) (c) Ionic (3.9 – 1.0=2.9)

111

6. (a) Y (b) 11 (c) ionic

111

7. (a)

1p2n

(b) Neutron (c) C–14 is used to determine the age of fossils and prehistoric objects. Deuterium is used in atomic reactor.

2

12

8.

(A) (a)

(b) Na+ or Sodium ion (c) F + 1e– → F–

OR

(B) (a)

(b) (Any two of the following) l Exists in solid, liquid and gaseous state l Generally insoluble in water, soluble in organic solvents like kerosene, benzene etc. l Low melting and boiling points l Generally not a conductor of electricity

211

2

1 + 1

9. (a) CaO (b) ZnCl2

11

8 ] Oswaal Kerala SSLC Question Bank, CHEMISTRY PART–2, CLASS-IX

10. (a) Electromagnetic Theory (b) Law of definite proportion

11

11. (a) F– (b) Hd+ –Cld–

11

12. (a) x__+ 2 y—0 (b) Here Mg undergoes oxidation and Hydrogen undergoes reduction. Thus oxidation and

reduction take place simultaneously in this reaction. So the above chemical reaction is a redox reaction.

2

2

13. Correct statements (a) An atom has a central part called nucleus. (b) The maximum number of electrons in a shell is 2n2.

11

14. (a) Most of the space in an atom is empty. (b) There are positively charged parts in an atom. These positively charged parts are

concentrated in a small space in atoms. (c) There is a small centre in an atom which consists of the entire mass and positive charge. The

positive charged alpha particles moving towards this centre reflects.

1

1

1

CHAPTER

5 ACIDS, ALKALIES AND SALTS

TOPIC-1Acids and Alkalies

QUICK REVIEW Acids are the compounds which give hydrogen ion in water solution. For

example, Hydrochloric acid (HCl), Sulphuric acid (H2SO4). HCl(aq) → H+ + Cl– Bases are the compounds which give hydroxide ion in water solution. For

example, Copper hydroxide, Cu(OH)2. Alkalies are the water soluble bases. For example, Sodium hydroxide

(NaOH), Potassium hydroxide (KOH). Metallic oxides are generally basic in nature. Amphoteric oxides are those metallic oxides which are both acidic as well as basic in character. They can react with

acids as well as bases. For example, Al2O3, ZnO. Properties of acids : l Form hydrogen ions in water. l Sour taste. l Turns blue litmus red. l React with carbonates to form carbon dioxide gas. l React with several metals like Mg and Fe releasing Hydrogen gas. l Act as electrolytes in solution. Types of acids : On the basis of strength : l Strong acids are the acids which ionize fully in water to produce large number of H+ ions. For example,

Hydrochloric acid (HCl), Sulphuric acid (H2SO4). l Weak acids are the acids which ionize partially in water to produce small number of H+ ions. For example,

citric acid (C6H8O7) and tartaric acid (C4H6O6). On the basis of occurrence : l Natural acids are the acids which are obtained from natural sources. For example, citric acid present in lime,

tartaric acid present in tamarind, lactic acid present in curd. These are usually weak acids. l Mineral acids are the acids which are prepared from mineral. For example, hydrochloric acid (HCl), sulphuric

acid. (H2SO4). They are strong acids. On the basis of number of H+ ions released by molecule : Monobasic, dibasic, tribasic. Properties of alkalies : l Form hydroxide ions in water. l Alkaline/bitter taste. l Turns red litmus blue. l Soapy to touch. l Act as electrolytes in solution. Carbonic acid is the solution obtained by dissolving carbon dioxide in water. CO2 + H2O → H2CO3 Soda water is the solution obtained by dissolving carbon dioxide in water under high pressure.

TOPIC - 1Acids and Alkalies .... P. 09

TOPIC - 2Salts .... P. 16

Oswaal Kerala SSLC Question Bank ForClass 9 Chemistry (Part-2) WithComplete Solutions For 2017

Examination

Publisher : Oswaal Books ISBN : 9788184818628 Author : Panel Of Experts

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