Std. 11, Chemistry MCQs, Maharashtra Board

25 Pages·2016·1.29 MB·English

by  Target Publications

Useful for all Agricultural, Medical, Pharmacy and Engineering Entrance Examinations

held across India.

STD XI Sci.
.

Triumph Chemistry

Based on Maharashtra Board Syllabus

Salient Features

• Exhaustive subtopic wise coverage of MCQs

• Quick Review and/or Important Formulae provided for all the chapters

• Hints included for relevant questions
  • Various competitive exams questions updated till the latest year
• Includes solved MCQs from JEE (Main), AIPMT / NEET P-I and P-II,

KCET 2015 and 2016

• Evaluation Test provided at the end of each chapter

Solutions/hints to Evaluation Test available in downloadable PDF format at

www.targetpublications.org/tp10145

  Printed at: Repro India Ltd., Mumbai

©  Target Publications Pvt. Ltd.
No part of this book may be reproduced or transmitted in any form or by any means, C.D. ROM/Audio Video Cassettes or electronic, mechanical

including photocopying; recording or by any information storage and retrieval system without permission in writing from the Publisher.

P.O. No. 30310

10145_10960_JUP
Preface

“Std. XI: Sci. Triumph Chemistry” is a complete and thorough guide to prepare students for
competitive level examinations. This book not only assists students with MCQs of Std. XI but also helps them to
prepare for JEE, AIPMT / NEET-UG, CET and various other competitive examinations.
The content of this book is based on the Maharashtra State Board Syllabus. Quick Review which
summarizes the important concepts of the entire chapter is provided for all the chapters. Formulae that form a
vital part of MCQ solving are provided for relevant chapters.
MCQs in each chapter are divided into three sections:
Classical Thinking: consists of straight forward questions including knowledge based questions.

Critical Thinking: consists of questions that require understanding of the concept and the applications of the
same.

Competitive Thinking: consists of questions from various competitive examinations like JEE, AIPMT / NEET-
UG, MH CET, KCET, CPMT, GUJ CET, AP EAMCET (Engineering, Medical), TS EAMCET (Engineering,
Medical), Assam CEE, BCECE, WB JEEM, etc.
Hints (i.e., complete solutions broken down to the simplest form possible) have been provided to the relevant
MCQs.
An Evaluation Test has been provided at the end of each chapter to assess the level of preparation of the
student on a competitive level.
In order to understand how chemistry plays an important role in our day to day life, we have made an
attempt to illustrate the same in the form of images/visuals in the related chapters.
The journey to create a complete book is strewn with triumphs, failures and near misses. If you think
we’ve nearly missed something or want to applaud us for our triumphs, we’d love to hear from you.
Please write to us at : [email protected]

Best of luck to all the aspirants!

Yours faithfully
Authors
Index

Sr. No. Topic Name Page No.
1 Some Basic Concepts of Chemistry 1
2 States of Matter (Gases and Liquids) 22
3 Structure of Atom 51
4 Periodic Table 85
5 Redox Reactions 103
6 Chemical Equilibrium 119
7 Surface Chemistry 165
8 Nature of Chemical Bond 186
9 Hydrogen 220
10 s-Block Elements 240
11 p-Block Elements (Group 13 and 14) 262
12 Basic Principles and Techniques in Organic Chemistry 290
13 Alkanes 330
14 Alkenes 351
15 Alkynes 369
16 Aromatic Compounds 387
17 Environmental Chemistry 405
Chapter 01: Some  Basic Concepts of Chemistry
01

Some Basic Concepts of Chemistry 

Subtopics

1.0 Introduction
Platinum alloy as an International Prototype
1.1 Importance and scope of chemistry of the Kilogram
1.2 Historical approach to particulate
nature of matter
1.3 Laws of chemical combination
1.4 Dalton’s atomic theory
1.5 Concepts of elements, atoms and
molecules
1.6 Atomic and molecular masses
1.7 Avogadro’s law, Avogadro’s number
and mole concept
1.8 Percentage composition and
empirical and molecular formula
1.9 Chemical reactions and
Have you ever wondered what is the reference for 1
kilogram???? It has been defined as the mass of the
stoichiometry
International Prototype of the Kilogram. The
prototype is made of platinum-iridium (Pt-Ir)

cylinder that is stored in an airtight jar at

International Bureau of Weights and Measures in

France. Pt-Ir was chosen because its mass remains

constant for an extremely long time and it is resistant

to the attack of different chemicals. This reference

standard is used to calibrate or standardize different
measuring devices such as analytical balances.

1
Std. XI : Triumph Chemistry 

Quick Review

 Branches of chemistry:
Physical chemistry
 Deals with the structure of matter, the energy changes and the
theories, laws and principles that explain the transformation of
matter from one form to another.

Inorganic chemistry

 Deals with chemistry of elements other than carbon and of

Chemistry their compounds.

Study of the composition,

structure and properties of Organic chemistry

matter and the reactions by  Deals with the reactions of the compounds of carbon.

which one form of matter

may be converted into
Analytical chemistry

another form.
 Deals with the separation, identification and quantitative

determination of the compositions of different substances.

Biochemistry

 Deals with chemistry of compounds and processes occurring in

living organisms.

 Classification of matter:

Matter
 has mass
 occupies space

Pure substances Mixtures

 Fixed composition  Variable composition (that can be

separated bysimple physical methods)

Elements Compounds Homogeneous mixtures Heterogeneous mixtures
 Substances that cannot  Substances of definite  Composition is  Composition is not
be decomposed by a compositions which uniform. uniform.
simple chemical can be decomposed  All constituents  Two or more phases
process into two or into two or more present in one are present.
more different susbtances by a phase.  eg. phenol-water
substances. simple chemical
 eg. air, ethyl alcohol system, iron filings-
 eg. He (monoatomic), process.
and water sand system
H (diatomic)  eg. H O, NaCl
2 2

2
Chapter 01: Some  Basic Concepts of Chemistry
 Laws of chemical combination:

Law of conservation of mass

 First stated by Lomonosove (1765) and then by Antoine Laviosier (1783).

 Statement: The mass is neither created nor destroyed during chemical

combination of matter.

Law of definite composition/Law of definite proportion
 Stated by Joseph Proust.

 Statement: Any pure compound always contains the same elements in a

definite proportion by weight irrespective of its source or method of

preparation.

Law of multiple proportion
Laws of chemical  Stated by John Dalton.
combination  Statement: If two elements chemically combine with each other forming
two or more compounds with different compositions by mass then the
ratios of masses of two interacting elements in the two compounds are
small whole numbers.

Gay Lussac’s law of combining volumes of gases

 Stated by Gay Lussac.

 Statement: When gases react together to produce gaseous products, the
volumes of reactants and products bear a simple whole number ratio with
each other, provided volumes are measured at same temperature and
pressure.

Avogadro’s law

 Stated by Avogadro.

 Statement: Equal volumes of all gases under identical conditions of

temperature and pressure contain equal number of molecules.

Formulae 6. Number of molecules

= n  Avogadro number (N )
A
1
1. Atomic mass unit (1 amu) = th of a 12C-atom 7. Atomicity = number of atoms in a molecule

12
8. Total number of atoms in molecule
= 1.66  1027 kg
= n  N  Atomicity
A
2. 1 Mole = 6.022  1023 particles
9. Volume occupied by one mole of a gas at STP
(atoms/molecules/ions/electrons) = 22.4 L = 22.4 dm3

3. Number of moles (n)
10. Molecular formula = r  Empirical formula

Mass of thesubstance
= Molecularmass
Molar mass of thesubstance 11. r =

Empiricalmass
Atomicmass
4. Mass of an atom = 12. Average atomic mass
6.0221023
Sumof(Isotopicmassits%abundance)
=
Molecularmass 100
5. Mass of a molecule =
6.0221023
13. Avogadro’s law, V  n (At constant T and P)

3
Std. XI : Triumph Chemistry 
10. The phlogiston theory was suggested for
Classical Thinking
_______ reaction.

(A) neutralisation (B) oxidation
1.0 Introduction
(C) reduction (D) combustion

1. _______ chemistry deals with the chemistry of
11. Substances which CANNOT be decomposed
elements other than carbon and of their
into two or more different substances by
compounds.
chemical process are called _______.
(A) Organic (B) Physical
(A) alloys (B) molecules
(C) Inorganic (D) Bio
(C) elements (D) compounds
2. The branch of chemistry which deals with the
separation, identification and quantitative 12. The arbitrarily decided and universally
determination of the composition of different accepted standards are called _______.
substances is called _______ chemistry. (A) fundamentals (B) units
(A) organic (B) inorganic (C) measures (D) symbols

(C) analytical (D) bio
13. There are _______ fundamental SI units.

1.1 Importance and scope of chemistry (A) 3 (B) 5
(C) 6 (D) 7
3. _______ pigment acts as a photosensitizer in
plants. 14. SI unit of temperature is _______.
(A) Xanthophyll (B) Chlorophyll (A) K (B) C
(C) Carotene (D) ATP
(C) F (D) D

4. _______ CANNOT be carried out in a lab.
15. SI unit of velocity is _______.
(A) Photosynthesis (B) Reduction
(A) km s1 (B) km hr1
(C) Oxidation (D) Hydration
(C) m s2 (D) m s1
5. Solar energy can be converted into electrical

energy using _______ cell. 1.3 Laws of chemical combination
(A) Daniel (B) lithium ion
(C) photovoltaic (D) nickel cadmium 16. The sum of the masses of reactants and

products is equal in any physical or chemical
6. In computers, _______ chips are used as
reaction. This is in accordance with law of
microprocessors.
_______.
(A) carbon (B) phosphorus
(A) multiple proportion
(C) titanium (D) silicon
(B) definite composition
1.2 Historical approach to particulate (C) conservation of mass
nature of matter (D) reciprocal proportion

7. Which one of the following is NOT a mixture?
17. If the law of conservation of mass was to hold
(A) Iodized table salt
true, then 20.8 g of BaCl , on reaction with
2
(B) Gasoline
9.8 g of H SO will produce 7.3 g of HCl and
2 4
(C) Liquefied Petroleum Gas (L.P.G.)
_______ of BaSO .
4
(D) Distilled water
(A) 11.65 g (B) 23.3 g
8. If two or more phases are present in a mixture (C) 25.5 g (D) 30.6 g

then it is called a _______ mixture.
18. Pure water can be obtained from various
(A) heterogeneous (B) homogeneous
sources, but it always contains hydrogen and
(C) homologous (D) heterologous
oxygen, combined in a ratio of 1:8 by weight.
9. Phenolwater system is a/an _______. This is an example of _______.
(A) element (A) law of conservation of mass
(B) compound (B) Avogadro’s law
(C) homogeneous system
(C) law of definite composition
(D) heterogeneous system
(D) Gay Lussac’s law

4
Chapter 01: Some  Basic Concepts of Chemistry
19. Two containers of the same size are filled 27. A/an _______ is an aggregate of two or more
separately with H gas and CO gas. Both the atoms in definite composition which are held
2 2
containers under the same T and P will contain together by chemical bonds.
the same _______. (A) ion (B) molecule
(A) number of atoms (C) compound (D) mixture

(B) weight of gas
1.6 Atomic and molecular masses
(C) number of molecules

(D) number of electrons 28. Every atom of an element consists of fixed

number of _______.
20. In SO and SO , the ratio of the masses of
2 3
(A) protons (B) neutrons
oxygen which combine with a fixed mass of
sulphur is 2:3. This is an example of the law of (C) electrons (D) all of these

_______.
29. The unit of atomic mass amu is replaced by
(A) constant proportion
_______.
(B) multiple proportion
(A) u (B) mol
(C) reciprocal proportion
(C) g (D) kg
(D) Gay Lussac
30. Mole is the SI unit of _______.
21. Which of the following reactions has the ratio
(A) volume
of volumes of reacting gases and the product
(B) pressure
as 1:2:2?
(C) amount of substance
(A) 2CO + O  2CO
(g) 2(g) 2(g) (D) density

(B) O + 2H  2H O
2(g) 2(g) 2 (g)
31. 1 amu is equal to _______.
(C) H + F  2HF
2(g) 2(g) (g)
1 1
(D) N + 3H  2NH (A) of C – 12 (B) of O – 16
2(g) 2(g) 3(g)
12 14
22. The volume of oxygen required for complete (C) 1 g of H (D) 1.66  10–23 kg
combustion of 0.25 cm3 of CH at S.T.P is 2
4
_______ cm3. 32. ________ is the sum of the atomic mass of all
(A) 0.25 (B) 0.5 the atoms as given in the molecular formula of
(C) 0.75 (D) 1 the substance.

(A) Molecular mass (B) Atomic weight
1.4 Dalton’s atomic theory
(C) Percentage weight (D) Percentage volume

23. Greek philosopher _______ had suggested that
1.7 Avogadro’s law, Avogadro’s number
matter is composed of extremely small
and mole concept
a-tomio.
(A) Dalton (B) Aristotle 33. N = _________ atoms mol1.
A
(C) Ptolemy (D) Democritus (A) 6.021  1021 (B) 6.024  1024

(C) 6.051  1015 (D) 6.022  1023
24. Dalton assumed that _______ are the smallest
particles of compound. 34. One _______ is the collection of 6.022  1023
(A) atoms (B) molecules
atoms /molecules/ions.
(C) ions (D) elements
(A) kg (B) g

1.5 Concepts of elements, atoms and (C) mole (D) cm

molecules
35. Avogadro’s number is ________.

25. Atoms have a mass of the order _______. (A) number of atoms in one gram of element.
(A) 1026 kg (B) 1015 kg (B) number of millilitres which one mole of
(C) 1026 g (D) 1015 g a gaseous substance occupies at N.T.P.
(C) number of molecules present in one
26. Atoms have a radius of the order _______. gram molar mass of a substance.
(A) 1026 m (B) 1015 m (D) number of elements in one gram of
(C) 1015 mm (D) 1015 m compounds.

5
Std. XI : Triumph Chemistry 
36. Which of the following law states that equal 45. 1 atom of an element weighs 1.792  10–22 g.
volume of all gases contain equal number of The atomic mass of the element is _______.
molecules? (A) 1.192 (B) 17.92
(A) Boyle’s law (C) 64 (D) 108

(B) Charles’ law
46. What is the mass of 0.5 mole of ozone molecule?
(C) Avogadro’s law
(A) 8 g (B) 16 g
(D) Gay Lussac’s law
(C) 24 g (D) 48 g
37. According to Avogadro’s law, ________.
47. The number of molecules in 16 g of oxygen
1
(A) V  (B) V  T gas is _______.
P
(A) 6.022  1023 (B) 3.011  1023
(C) V  n (D) all of these
(C) 3.011  1022 (D) 1.5  1023

38. Volume occupied by 1 g molecular weight of
48. Which of the following weighs the least?
any gas is called _______.
(A) 2.0 gram mole of CO
(A) gram molecular volume 2
(B) 0.1 mole of sucrose (C H O )
(B) gram atomic volume 12 22 11
(C) 1 gram atom of calcium
(C) gram molecular weight
(D) 1.5 mole of water
(D) gram atomic weight

49. Which one of the following pairs of gases
39. Avogadro’s law distinguishes between
contains the same number of molecules?
_______.
(A) cations and anions (A) 16 g of O2 and 14 g of N2
(B) atoms and molecules (B) 8 g of O2 and 22 g of CO2
(C) atoms and ions (C) 28 g of N2 and 22 g of CO2
(D) molecules and ions (D) 32 g of O2 and 32 g of N2

40. The number of atoms present in a molecule of 50. One mole of oxygen gas weighs _______.
a substance is called its ________. (A) 1 g (B) 8 g
(A) atomicity (B) volume (C) 32 g (D) 6.023  1023 g

(C) density (D) mass
51. Under similar conditions, same mass of
41. How many molecules are present in one gram oxygen and nitrogen is taken. The ratio of
of hydrogen gas? their volumes will be _______.
(A) 6.02  1023 (B) 3.01  1023 (A) 7 : 8 (B) 3 : 5
(C) 2.5  1023 (D) 1.5  1023 (C) 6 : 5 (D) 9 : 2

42. One mole of CO contains _______. 1.8 Percentage composition and empirical
2
(A) 6.022  1023 atoms of C and mol ecular formula

(B) 6.022  1023 atoms of O
52. Chemical formula CANNOT be determined
(C) 18.1  1023 molecules of CO2 by using _______.
(D) 3 g atoms of CO2 (A) Raman spectroscopy

(B) nuclear magnetic resonance
43. One mole of H O corresponds to _______.
2
(C) Titration
(A) 22.4 litres at 1 atm and 25 C
(B) 6.02  1023 atoms of hydrogen and (D) ultraviolet spectroscopy

6.02  1023 atoms of oxygen 53. The mass percentage of each constituent
(C) 18 g of H2O element present in 100 g of a compound is
(D) 1 g of H O called its _______.
2

(A) molecular composition
44. The gram molecule of benzene is equal to
(B) atomic composition
_______ g C H .
6 6
(C) percentage composition
(A) 70 (B) 72
(D) mass composition
(C) 10 (D) 78

6
Chapter 01: Some  Basic Concepts of Chemistry
54. _______ of a compound is the chemical 64. _______ reactant is the reactant that reacts
formula indicating the relative number of completely but limits further progress of the
atoms in the simplest ratio. reaction.
(A) Empirical formula (A) Oxidizing (B) Reducing
(B) Molecular formula (C) Limiting (D) Excess

(C) Empirical mass
65. _______ reactant is the reactant which is taken
(D) Molecular mass
in excess than the limiting reactant.

55. The percentage composition of carbon in urea, (A) Oxidizing (B) Reducing
[CO(NH ) ] is _______. (C) Limiting (D) Excess
2 2
(A) 20% (B) 40%
66. The _______ coefficients are the coefficients
(C) 50% (D) 80% of reactants and products in the balanced

chemical reaction.
56. What is the % of H O in Fe(CNS) 3H O?
2 3 2
(A) balanced (B) chemical
(A) 19 (B) 25
(C) stoichiometric (D) molar
(C) 30 (D) 45

Miscellaneous
57. The percentage of oxygen in NaOH is
_______. 67. Which of the following relations for expressing
(A) 8 (B) 10 volume of a sample is NOT correct?
(C) 40 (D) 60 (A) 1L = 103 ml (B) 1dm3 = 1L

(C) 1L = 103m3 (D) 1L = 103 cm3
58. A compound made of two elements A and B
are found to contain 25% A (Atomic mass 68. Which out of the following is NOT a
12.5) and 75% B (Atomic mass 37.5). The homogeneous mixture?
simplest formula of the compound is _______. (A) Solution of glucose in water.
(A) AB (B) AB (B) Solution of salt in water.
2
(C) AB (D) A B (C) Mixture of glucose solution and salt
3 3

solution.
59. _______ indicates the actual number of
(D) Mixture of oil and water.
constituent atoms in a molecule.
(A) Empirical formula 69. The molecular mass of hydrogen peroxide is
(B) Molecular formula 34. What is the unit of molecular mass?
(C) Empirical mass (A) g (B) mol
(D) Molecular mass (C) g mol1 (D) mol g1

Synthetic fabrics
60. Which of the following has same molecular

formula and empirical formula?

(A) CO2 (B) C6H12O6
(C) C2H2 (D) C2H2O4

61. Empirical formula of glucose is _______.

(A) C H O (B) C H O
6 12 6 6 11 6

(C) CHO (D) CH O
2
1.9 Chemical reactions and stoichiometry

62. The starting material which takes part in

chemical reaction is called _______.

(A) product (B) reactant

(C) catalyst (D) starter

63. ________ is the quantitative relationship
Synthetic fabrics like nylon, terylene, etc., are man-
between the reactants and products in a
made fabrics. They are very elastic and dry quickly
balanced chemical equation.
after washing. They are mainly popular because of
(A) Stoichiometry (B) Complexometry their crease free nature i.e., they don’t need to be
(C) Chemistry (D) Reactions ironed !!!

7