+ NEET UG, ISEET: Chemistry MCQs

21 Pages·2012·0.31 MB·English

Chemistry MCQs for XI (Science) + NEET UG/ISEET
Written according to the New Text book (2012-2013) published by the Maharashtra State
Board of Secondary and Higher Secondary Education, Pune.

Std. XI Sci.
Triumph Chemistry

Prof. Santosh B. Yadav Prof. Anil Thomas
(M. Sc., SET, NET) (M.Sc., Chemistry)

Salient Features:
(cid:57) Exhaustive coverage of MCQs subtopic wise.
(cid:57) Each chapter contains three sections.
(cid:57) Section 1 contains easy level questions.
(cid:57) Section 2 contains competitive level questions.
(cid:57) Section 3 contains questions from various competitive exams.
(cid:57) Important formulae in each chapter.
(cid:57) Hints provided wherever relevant.
(cid:57) Useful for NEET and ISEET preparation.

g
Tar et
PUBLICATIONS PVT. LTD.
Mumbai, Maharashtra
Tel: 022 – 6551 6551
Website : www.targetpublications.org, www.targetpublications.in,
email : [email protected]
Std. XI

Triumph Chemistry

©
Target Publications Pvt Ltd.

Second Edition : August 2012

Price : ` 200/-

Printed at:
Anjum Binding Work
Worli

Published by
g
Tar et

PUBLICATIONS PVT. LTD.
Shiv Mandir Sabhagriha,
Mhatre Nagar, Near LIC Colony,
Mithagar Road,
Mulund (E),
Mumbai - 400 081
Off.Tel: 022 – 6551 6551
email: [email protected]
PREFACE

With the change in educational curriculum it’s now time for a change in Competitive Examinations.
NEET and ISEET are all poised to take over the decade old MHT-CET. The change is obvious not merely
in the names but also at the competitive levels. The state level entrance examination is ushered aside and the
battleground is ready for a National level platform. However, keeping up with the tradition, Target Publications
is ready for this challenge.
To be at pace with the changing scenario and equip students for a fierce competition, Target Publications
has launched the Triumph series. Triumph Chemistry is entirely based on Std XI (Science) curriculum of the
Maharashtra Board. This book will not only assist students with MCQs of Std. XI but will also help them
prepare for NEET and ISEET.
The content of this book has evolved from the State Board prescribed Text Book and we’ve made every
effort to include most precise and updated information in it. Multiple Choice Questions form the crux of this
book. We have framed them on every sub topic included in the curriculum. Each chapter is divided into 3
sections:
Section 1 consists of basic questions.
Section 2 consists of questions which can be asked at a competitive level.
Section 3 consists of questions compiled from various competitive examinations.
To end on a candid note, we make a humble request for students: Preserve this book as a Holy Grail even
after your first year in junior college. This book would prove as an absolute weapon in your arsenal for your
combat against Medical and Engineering entrance examinations.

Best of luck to all the aspirants!

Yours faithfully
Publisher
Contents

No. Topic Name Page No.
1 Some Basic Concepts of Chemistry 1
2 States of Matter 17
3 Structure of Atom 37
4 Periodic Table 71
5 Redox Reactions 91
6 Chemical Equilibrium 109
7 Surface Chemistry 148
8 Nature of Chemical Bond 171
9 Hydrogen 211
10 s-Block Elements 230
11 p-Block Elements (Groups 13 and 14) 250
Basic Principles and Techniques in
12 270
Organic Chemistry
13 Alkanes 292
14 Alkenes 309
15 Alkynes 326
16 Aromatic Compounds 338
17 Environmental Chemistry 355
Std. XI: Triumph Chemistry
TARGET Publications

01
Some Basic Concepts of Chemistry

Formulae
6. _____ pigment acts as a photosynthesizer in
1. General gas equation: PV = nRT plants.

(A) Xanthophyll (B) Chlorophyll
2. Number of moles,
(C) Carotene (D) ATP
mass of substance
n =
7. Microprocessors used in computers are _____
molar mass of substance
chips developed by chemists.
3. Number of molecules (A) Carbon (B) Phosphate
= n × Avogadro number (N ) (C) Titanium (D) Silicon
A
4. Volume of gas at S.T.P. = n × 22.414 L 1.2 Historical Approach to Particulate Nature
of Matter
5. Molecular formula = n × Empirical formula,
8. If two or more phases are present in a mixture
Molecularmass
where n =
then it is called a _____ mixture.
Empiricalformulamass
(A) Heterogenous (B) Homogenous
6. At. mass of an element (C) Homologous (D) Heterologous

= mass of 1 atom of element × N
A 9. The arbitrarily decided and universally
accepted standards are called
SECTION - 1
(A) Fundamentals (B) Units

(C) Measures (D) Symbols
1.0 Introduction
10. Which out of the following is NOT a
1. Avogadro’s work was brought to light after his homogeneous mixture?
death, by (A) Air
(A) Cannizzaro (B) Dalton (B) Solution of salt in water
(C) Gay Lussac (D) Lord Kelvin
(C) Solution of sugar in water

(D) Smoke
2. Chemistry is a _____ science.

(A) Social (B) Central
11. Substances which cannot be decomposed into
(C) Fictional (D) Recent two different substances by chemical process

are called
3. The branch of chemistry that deals with the
(A) Atoms (B) Molecules
structure of matter, the energy changes and the
theories, laws and principles that explain the (C) Elements (D) Compounds

transformation of matter from one form to
12. Which of the following is a compound?
another is called _____ chemistry.
(A) Graphite (B) Brass
(A) Inorganic (B) Organic
(C) Milk (D) 22 Carat Gold
(C) Analytical (D) Physical

13. Mixture of all gases constitute _____ system.
4. _____ chemistry is the chemistry of the
(A) Homogeneous
substances consisting of living organisms.
(B) Heterogeneous
(A) Organic (B) Physical
(C) Element
(C) Inorganic (D) Bio
(D) Compound

1.1 Importance and Scope of Chemistry
14. Phenol−water system is a/an
5. Azidothymidine drug is used for treating (A) Element
_____ patients. (B) Compound
(A) Diabetes (B) AIDS (C) Homogeneous system
(C) Jaundice (D) Tuberculosis (D) Heterogeneous system
1
S ome Basic Concepts of Chemistry
Std. XI: Triumph Chemistry
TARGET Publications

15. Joseph Priestly found that the gas evolved on 23. In SO and SO , the ratio of the masses of
2 3
heating mercury oxide, supported vigorous oxygen which combine with a fixed mass of
burning. He named this gas as sulphur is 2:3. This is an example of the law of
(A) Oxygen (A) Constant proportion.
(B) Dephlogisticated air (B) Multiple proportion.
(C) Phlogisticated air (C) Reciprocal proportion.
(D) Gay Lussac.
(D) Hydrogen

24. Among the following pairs of compounds, the
16. There are _____ fundamental SI units.
one that illustrates the law of multiple
(A) 5 (B) 3
proportions is
(C) 12 (D) 7
(A) NH and NCl (B) H S and SO
3 3 2 2
17. The phlogiston theory was suggested for (C) CuO and Cu O (D) CS and FeSO
2 2 4
(A) neutralisation reaction.
1.4 Dalton’s Atomic Theory
(B) oxidation reaction.
(C) reduction reaction. 25. Greek philosopher _____ had suggested that
matter is composed of extremely small
(D) combustion reaction.
a-tomio.
18. Which one of the following is not a mixture? (A) Dalton (B) Aristotle
(A) Iodized table salt (C) Ptolemy (D) Democritus

(B) Gasoline
26. Dalton assumed that _____ are the smallest
(C) Liquefied Petroleum Gas (L. P. G.)
particles of compound.
(D) Distilled water.
(A) Atoms (B) Molecules

(C) Ions (D) Elements
1.3 Laws of Chemical Combination

1.5 Concepts of Atoms and Molecules
19. The law of definite composition was proposed
by 27. Atoms have a mass of the order
(A) Lomonosov (A) 10−26 kg (B) 10−15 kg
(B) Antoine Lavoisier (C) 10−26 g (D) 10−15 g

(C) Joseph Proust
28. A _____ is an aggregate of two or more atoms
(D) Dalton
of definite composition which are held
20. ___________ law of combining volumes together by chemical bonds.
states that “Whenever gases combine, they do (A) Ion (B) Molecule
so in simple ratio by volumes”. (C) Compound (D) Mixture

(A) Avogadro’s (B) Gay Lussac’s
29. Atoms have a radius of the order
(C) Dalton’s (D) Thomson’s (A) 10−26 m (B) 10−15 µm

(C) 10−15 mm (D) 10−15 m
21. The sum of the masses of reactants and
products is equal in any physical or chemical 1.6 Atomic and Molecular Masses

reaction. This is in accordance with
30. SI unit of mass is
(A) Law of multiple proportion
(A) kg (B) g
(B) Law of definite composition (C) m (D) m–1
(C) Law of conservation of mass
31. Mole is the SI unit of________.
(D) Law of reciprocal proportion
(A) Volume
22. Pure water can be obtained from various (B) Pressure
sources, but it always contains hydrogen and (C) Amount of substance
oxygen, combined in a ratio of 1:8 by weight. (D) Density

This is an example of 32. ________ is the sum of the atomic mass of all
(A) Law of conservation of mass the atoms as given in the molecular formula of
(B) Avogadro’s law the substance.
(C) Law of definite composition (A) Molecular mass (B) Empirical weight
(D) Gay Lussac’s law (C) Percentage weight (D) Percentage volume
2
Some Basic Concepts of Chemistry
Std. XI: Triumph Chemistry
TARGET Publications

33. The mass percentage of each constituent 43. One _____ is the collection of 6.022 × 1023
element present in 100 g of compound is atom /molecules/ions.
called its (A) kg (B) g
(A) Molecular composition. (C) mole (D) cm

(B) Atomic composition.
44. How many molecules are present in one gram
(C) Percentage composition.
of hydrogen?
(D) Mass composition.
(A) 6.02 × 1023 (B) 3.01 × 1023
34. Molar mass is a _____ quantity. (C) 2.5 × 1023 (D) 1.5 × 1023
(A) Vector (B) Imaginary
(C) Unitless (D) Useless 45. Avogadro’s number is

(A) number of atoms in one gram of element.
35. 1 amu is equal to
(B) number of millilitres which one mole of
1 1
(A) of C – 12 (B) of O – 16 a gaseous substance occupies at N.T.P.
12 14
(C) number of molecules present in one
(C) 1g of H2 (D) 1.66 × 10–23 kg gram molecular mass of a substance.
36. 10 dm3 of N gas and 10 dm3 of gas X at the (D) number of elements in one gram of
2
compounds.
same temperature contain the same number of

molecules. The gas X is
46. Which of the following law states that equal
(A) CO (B) CO2 volume of all gases contain equal number of
(C) H2 (D) NO molecules?
(A) Boyle’s law
37. In the reaction
(B) Charles’ law
2Na S O + I ⎯→ Na S O + 2NaI, the
2 2 3 2 2 4 6
(C) Avogadro’s law
equivalent weight of Na S O is equal to
2 2 3
(Molecular mass = M) (D) Gay Lussac’s law

(A) M (B) M/2
47. According to Avogadro’s law
(C) M/3 (D) M/4
1
(A) V ∝ (B) V ∝ T
38. A molal solution is one that contains 1 mole of P
a solute in
(C) V ∝ n (D) all of these
(A) 1000 g of the solvent
(B) One litre of the solvent 48. Avogadro’s law distinguishes between
(C) One litre of the solution (A) Cations and anions
(D) 22.4 litres of the solution (B) Atoms and molecules

(C) Atoms and ions
39. Recently the unit of atomic mass amu is
(D) Molecules and ions
replaced by
(A) u (B) mol 49. One mole of H O corresponds to
2
(C) g (D) kg (A) 22.4 litres at 1 atm and 25° C

(B) 6.02 × 1023 atoms of hydrogen and
40. The molecular mass of hydrogen peroxide is
34. What is the unit of molecular mass? 6.02 × 1023 atoms of oxygen
(A) g (B) mol (C) 18 g
(C) g mol−1 (D) mol g−1 (D) 1 g

1.7 Avogadro’s Law 50. The gram molecule of benzene is equal to
(A) 70 g C H (B) 72 g C H
6 6 6 6
41. The number of molecules in 16 g of oxygen is
(C) 10 g C H (D) 78 g C H
(A) 6.022 × 1023 (B) 3.011 × 1023 6 6 6 6
(C) 3.011 × 1022 (D) 1.5 × 1023 51. Under similar conditions, oxygen and nitrogen
are taken in the same mass. The ratio of their
42. N = _________ atoms mol−1. volumes will be_______.
A
(A) 6.021 × 1021 (B) 6.024 × 1024 (A) 7 : 8 (B) 3 : 5
(C) 6.051 × 1015 (D) 6.022 × 1023 (C) 6 : 5 (D) 9 : 2
3
S ome Basic Concepts of Chemistry
Std. XI: Triumph Chemistry
TARGET Publications

52. What is the mass of 0.5 mole of ozone molecule? 62. The starting material which takes part in
(A) 8g m (B) 16 g chemical reaction is called
(C) 24 g (D) 48 g (A) Product (B) Reactant

(C) Catalyst (D) Starter
53. Which one of the following pairs of gases
contains the same number of molecules 63. ________ is the quantitative relationship
(A) 16 g of O2 and 14 g of N2 between the reactants and products in a
(B) 8 g of O2 and 22 g of CO2 balanced chemical equation.
(C) 28 g of N and 22 g of CO
2 2 (A) Stoichiometry (B) Complexometry
(D) 32 g of O and 32 g of N
2 2 (C) Chemistry (D) Reactions

54. One mole of oxygen weighs______.
64. The _____ coefficients are the coefficients of
(A) 8g (B) 32g
reactants and products in the balanced
(C) 1g (D) 6.023 × 1023 g
chemical reaction.
55. The number of atoms present in a molecule of (A) balanced
a substance is called ________. (B) chemical
(A) Atomicity (B) Volume (C) stoichiometric
(C) Density (D) Mass
(D) molar

1.8 Percentage Composition and Molecular
Miscellaneous
Formula

65. Which of the following is correct?
56. The percentage composition of carbon in urea,
(A) 1 L = 1 dm3
[CO(NH ) ] is
2 2 (B) 1 L = 10 dm3
(A) 40% (B) 50%
(C) 10 L = 1 dm3
(C) 20% (D) 80%
(D) 1 L = 1 m3
57. _____ of a compound is the chemical formula
indicating the relative number of atoms in the 66. One mole of CO contains
2
simplest ratio. (A) 6.022 × 1023 atoms of C
(A) Empirical formula (B) 6.022 × 1023 atoms of O
(B) Molecular formula (C) 18.1 × 1023 molecules of CO
2
(C) Empirical mass
(D) 3 g atoms of CO
(D) Molecular mass 2

67. Chemical formula cannot be determined by
58. _____ indicates the actual number of
using
constituent atoms in a molecule.
(A) Raman Spectroscopy
(A) Empirical formula
(B) Nuclear magnetic resonance
(B) Molecular formula
(C) Empirical mass (C) Titration
(D) Molecular mass (D) X-ray diffraction method

59. Empirical formula of glucose is 68. Which of the following reactions has the ratio
(A) C H O (B) C H O of volumes of reacting gases and the product
6 12 6 6 11 6
(C) CHO (D) CH O as 1:2:2?
2
(A) 2CO + O ⎯→ 2CO
1.9 Chemical Reactions and Stoichiometry (g) 2(g) 2(g)
(B) O + 2H ⎯→ 2H O
2(g) 2(g) 2 (g)
60. _____ reactant is the reactant that reacts
(C) H + F ⎯→ 2HF
2(g) 2(g) (g)
completely but limits further progress of the
(D) N + 3H ⎯→ 2NH
reaction. 2(g) 2(g) 3(g)
(A) Oxidizing (B) Reducing 69. Volume occupied by 1 g molecular weight of
(C) Limiting (D) Excess any gas is called

(A) Gram molecular volume
61. _____ reactant is the reactant which is taken in
excess than the limiting reactant. (B) Gram atomic volume
(A) Oxidizing (B) Reducing (C) Gram molecular weight
(C) Limiting (D) Excess (D) Gram atomic weight
4
Some Basic Concepts of Chemistry
Std. XI: Triumph Chemistry
TARGET Publications

SECTION - 2 12. Which of the following contains only one
element?

(A) Marble (B) Diamond
1.0 Introduction
(C) Glass (D) Sand

1. _____ chemistry deals with the chemistry of
13. Which one of the following is not an element?
elements other than carbon and of their
(A) Diamond (B) Graphite
compounds.
(C) Silica (D) Ozone
(A) Organic (B) Physical
(C) Inorganic (D) Bio 14. The element similar to carbon is

(A) Mg (B) Mn
2. The branch of chemistry which deals with the
(C) Sn (D) Pb
separation, identification and quantitative
determination of the composition of different 1.3 Laws of Chemical Combination

substances is called _____ chemistry.
15. The law of multiple proportions is illustrated
(A) Organic (B) Inorganic
by
(C) Analytical (D) Bio
(A) Carbon monoxide and carbon dioxide
1.1 Importance and Scope of Chemistry
(B) Potassium bromide and potassium

chloride.
3. Solar energy can be converted into electrical
(C) Ordinary water and heavy water.
energy using
(D) Calcium hydroxide and barium
(A) Daniel cell (B) Lithium ion cell
hydroxide.
(C) Photovoltaic cell (D) Ni cell

16. Two elements, X (Atomic mass 16) and Y
4. _______ cannot be carried out in a lab.
(Atomic mass 14) combine to form
(A) Photosynthesis (B) Reduction
compounds A, B and C. The ratio of different
(C) Oxidation (D) Hydration
masses of Y which combine with fixed mass
5. The compound which is added to table salt for
of X in A, B and C is 1:3:5. If 32 parts by
maintaining proper health is
mass of X combine with 84 parts by mass of Y
(A) KCl (B) KBr
in B, then in C, 16 parts by mass of X will
(C) NaI (D) MgBr
2 combine with
1.2 Historical Approach to Particulate Nature (A) 14 parts by mass of Y
of Matter (B) 42 parts by mass of Y

(C) 70 parts by mass of Y
6. SI unit of velocity is
(D) 82 parts by mass of Y
(A) km s−1 (B) km hr−1
(C) m s−2 (D) m s−1 17. The volume of oxygen required for complete
combustion of 0.25 cm3 of CH at S.T.P is
4
7. SI unit of temperature is (A) 0.25 cm3 (B) 0.5 cm3
(A) K (B) °C (C) 0.75 cm3 (D) 1 cm3

(C) °F (D) D

18. How many litres of ammonia will be formed
8. Electrochemical equivalence has unit ____.
when 2 L of N and 2 L of H are allowed to
(A) kg m s−1 (B) kg m2 s−1 2 2
react?
(C) kg C−1 (D) kg m−1 s−2
(A) 0.665 (B) 1.0
9. Magnitude of ‘pico−’ is _____. (C) 4.00 (D) 1.33

(A) 10−12 (B) 10−15
19. Two elements, A and B, combine to form a
(C) 1012 (D) 1015
compound in which ‘a’ g of A combines with
10. One atmosphere is equal to ‘b ’ and ‘b ’g of B respectively. According to
1 2
(A) 101.325 K pa (B) 1013.25 K pa law of multiple proportion _____.
(C) 105 Nm (D) 107 Nm (A) b = b
1 2
(B) b and b bear a simple whole number
11. Which of the following elements of matter 1 2
ratio
would best convey that there is life on earth?
(A) Oxygen (B) Hydrogen (C) a1 and b1 bear a whole number ratio
(C) Carbon (D) Iron (D) No relation exists between b1 and b2
5
S ome Basic Concepts of Chemistry