Download free Chemistry Notes 9th Class

Chapter # 1
Important Board Questions from 2009 to 2019

1. State and explain the main branches of chemistry.
2. Define Chemistry and its Four branches of chemistry
3. Analytical, Bio chemistry and inorganic chemistry
4. Chemistry and contribution of Jabir IbnHayan in the field of chemistry.
5. Elements and compound with examples.
6. Differentiate element, compound and mixture with examples
7. Mixture and its types
8. What do you meant by atomic number? Give example.
9. Atomic number and mass number with example
10. What is atomic number of an element? How it differ from the mass number?
11. Chemical formula and empirical formula by giving examples.
12. Empirical and Molecular formula with examples.
13. Empirical and Molecular formula of a compound
14. Steps for determination of Empirical formula of a compound.
15. Molecular mass and formula mass with examples.
16. Gram atomic and gram molecular mass with examples.
17. Free radical with example
18. Difference between atom and ion
19. What is Hydrated ions?
20. Differentiate between homogeneous and heterogeneous mixture.
21. What is Percentage composition?
22. Classification of molecules with examples
23. Mole and Avogadro’s number with examples.
24. Molecular mass of a compound. How will you differentiate it from formula mass?
25. Give reasons to prove that atom is a neutral particle
26. How does molecule differ from an atom?
27. Why alloys are mixture but not compound?
28. NaCl is not a molecule but a formula unit. Why?
29. How many moles of CO₂ are present in 60g of CO₂?
30. What is the mass of 5 moles of ice?
31. Calculate the molecular mass of Glucose
32. Calculate the molecular mass of sugar.
33. Calculate the molecular mass of HNO₃
34. Calculate the number of moles in 550 grams of NaI
35. Calculate the moles in 10 grams of CO₂
36. How many moles of H₂O are present in 36gm of H₂O?
37. How many moles are of CO₂ are there in 7.5×10²⁴ molecules of the gas.
38. Calculate the number of molecules present in 5 moles of Glucose
39. Molecular mass of (atomic mass , )
40. How many moles of hydrogen are there in 8.9×10²³ hydrogen atom?
41. Calculate the number of molecules of 31.96 gm of oxygen atom
42. Find the number of protons, electrons and protons and neutrons in ,

Prepared by Hafiz Muhammad Uzair

1. The complete study of__________ is called matter.
(a) Matter
(b) Energy
(c) Frequency
(d) None of these
Show Answer

2. We all depend upon different ___________ , Which are necessary for our survival.
(a) Crucibles
(b) Chemicals
(c) Isotopes
(d) None of these
Show Answer

3. Chemistry has a wide range of _______________ which is serving the humanity.
(a) Applications
(b) Properties
(c) Techniques
(d) None of these
Show Answer

4. Petrochemicals, medicines, drugs, papers, soap, detergents, paints, colour, pigments etc are the inventions of ________________.
(a) Biology
(b) Physics
(c) Chemistry
(d) None of these
Show Answer

5. The study of chemistry also provides knowledge and techniques to improve our __________________.
(a) Stamina
(b) Appearance
(c) Health
(d) None of these
Show Answer

6. The Study of chemistry also helps us to explore and conserve the _____________resources.
(a) Artificial
(b) Natural
(c) Coilateral
(d) None of these
Show Answer

7. The Muslim period in science of chemistry was about _____________ years.
(a) 1000
(b) 800
(c) 1200
(d) None of these
Show Answer

8. The Egyptians, the Greeks and the ____________ contributed much to the science of chemistry.
(a) Muslims
(b) Babylonians
(c) Jews
(d) None of these
Show Answer

9. In this period, Muslim scientist focused on finding ways to change base metal such as Lead into______________.
(a) Mercury
(b) Gold
(c) Bronze
(d) None of these
Show Answer

10. Muslim scientist discovered ___________ elements like arsenic, antimony and bismuth etc.
(a) Few
(b) many
(c) five
(d) None of these
Show Answer

11. Many new chemicals processes were also introduced by Muslim scientists such as filtration, fermentation and ________etc.
(a) Ultra sonication
(b) Sedimentation
(c) Distillation
(d) None of these
Show Answer

12. The Period of Muslims is generally called the period of ___________ in the history of chemistry.
(a) Al-Chemists
(b) Elites
(c) Masters
(d) None of these
Show Answer

13. _________ is generally known as the “Father of chemistry”.
(a) Jabber Bin Haiyan
(b) Ibn-e-Sina
(c) Al-Beruni
(d) None of these
Show Answer

14. Who was the first scientist who has well- established laboratory?
(a) Zakriya Al Razi
(b) Jabber Ibn Haiyan
(c) Al Beruni
(d) None of these
Show Answer

15. Jabber bin Haiyan was the first to prepare.
(a) HCl
(b) HNO_3
(c) H_2SO_4
(d) All of them
Show Answer

16. Jabber Bin Haiyan was also known as ______ in the Europe.
(a) Geber
(b) Ibn-e-Sina
(c) Al-Razi
(d) None of these
Show Answer

17. Jabber Bin Haiyan’s Demise occur in ____________.
(a) 721 A.D
(b) 803 A.D
(c) 803 B.C
(d) None of these
Show Answer

18. Al-Razi wrote ________ books.
(a) 26
(b) 16
(c) 25
(d) 20
Show Answer

19. The most famous book of Al-Razi was _______________.
(a) Khayaban
(b) Mindeel
(c) Al-Asrar
(d) None of these
Show Answer

20. Al-Razi was the first scientist / Chemist to divide the chemical ________into four types .
(a) Isotopes
(b) Compound
(c) Solution
(d) None of these
Show Answer

21. Al-Razi prepared alcohol by ________.
(a) Fermentation
(b) Coagulation
(c) Filtration
(d) None of these
Show Answer

22. Al-Beruni was born in 973 AD and died in ______________.
(a) 1024 AD
(b) 1048 A.D
(c) 1072 AD
(d) None of these
Show Answer

23. Al-Beruni was the first chemist who determined the ________ of different substances.
(a) Frequencies
(b) Chemical Formula
(c) Densities
(d) None of these
Show Answer

24. Ibn-e-Sina was born in ___________ and died in 1037 A.D.
(a) 980 AD
(b) 980 B.C
(c) 985 A.D
(d) None of these
Show Answer

25. Ibn-e-Sina is generally known as the __________ of the Muslim’s world.
(a) Maximus
(b) Alexander
(c) Aristotle
(d) None of these
Show Answer

26. Ibn-e-Sina was the first one who rejected the idea that base metals can be converted into _____.
(a) Silver
(b) Gold
(c) Neon
(d) None of these
Show Answer

27. Ibn-e-Sina has written more than ________ books that are now taught in the Europe.
(a) 100
(b) 101
(c) 95
(d) None of these
Show Answer

28. Chemistry is the branch of ____________ science which includes the study of material and substances.
(a) Chemical
(b) Physical
(c) Historical
(d) None of these
Show Answer

29. ___________ Chemistry deal with the relationship between physical properties of substances along with chemical changes in them.
(a) Organic
(b) Inorganic
(c) Physical
(d) None of these
Show Answer

30. Hydrocarbon contains ________ elements only.
(a) C and H
(b) C,H,O
(c) C and O
(d) None of these
Show Answer

31. The study of ________ and their derivatives are called organic chemistry.
(a) Hydrocarbons
(b) Isotopes
(c) Chemical species
(d) None of these
Show Answer

32. Inorganic chemistry deals with all kind of elements and compounds, EXCEPT _________ and their derivatives.
(a) Organic compounds
(b) Chemical Compounds
(c) Biochemical
(d)
Show Answer

33. Analytical chemistry deals with qualitative and quantitative analysis of __________.
(a) Energy
(b) Quarks
(c) matter
(d) None of these
Show Answer

34. ___________ Chemistry deals with the study of techniques and chemical processes for the preparation of different industrial products.
(a) Environmental
(b) Industrial
(c) Nuclear
(d) None of these
Show Answer

35. Nuclear Chemistry concerned with the study of ____________, changes occurring in it and its properties.
(a) Nucleus
(b) Sub atomic particles
(c) Composition
(d) None of these
Show Answer

36. Biochemistry deals with the study of synthesis, composition, decomposition and chemical reaction of ______ factors.
(a) Abiotic
(b) Biotic
(c) Both a and b
(d) None of these
Show Answer

37. Anything that occupies space and having a mass is called ________________.
(a) Matter
(b) Mixture
(c) Substance
(d) None of these
Show Answer

38. Everything in the ________ is made of matter.
(a) Earth
(b) Mars
(c) Universe
(d) None of these
Show Answer

39. A piece of matter in _________ form is substance.
(a) Impure
(b) Pure
(c) Both a and b.
(d) None of these
Show Answer

40 Pure water is an example of a ____________.
(a) Substance
(b) Element
(c) Compound
(d) None of these
Show Answer

41. Element is a pure substance which cannot be _______ into other simpler substances by any physical or chemical process.
(a) Split up
(b) Combined up
(c) None
(d) All of These
Show Answer

42. The fundamental unit of an element is ______________.
(a) atom
(b) Electron
(c) Proton
(d) None of these
Show Answer

43. Scientists have discovered about _____ elements.
(a) 108
(b) 118
(c) 128
(d) None of these
Show Answer

44. There are __________ naturally occurring elements
(a) 92
(b) 94
(c) 96
(d) None of these
Show Answer

45. There are __________ artificial elements.
(a) 28
(b) 27
(c) 26
(d) None of these
Show Answer

46. Each element consists of ________kind of atoms.
(a) different
(b) Same
(c) None
(d) All of these
Show Answer

47. In 1814, ____________ suggested the system for representing element with symbol.
(a) Berzelius
(b) Max Plank
(c) Maximus
(d) None of these
Show Answer

48. The shortest name of an element is called __________.
(a) Representation
(b) Isotopes
(c) symbol
(d) None of these
Show Answer

49. B, C, F are the symbols of __________________.
(a) Compounds
(b) Elements
(c) Molecules
(d) None of these
Show Answer

50. Compound is a pure substance consists of two or more _________ types of elements chemically combined together in a fixed ratio by mass.
(a) Different
(b) Same
(c) Both a and b
(d) None of these
Show Answer

51. In the formation of a compound, the element must undergo __________changes.
(a) Physical
(b) Analytical
(c) Chemical
(d) None of these
Show Answer

52. In water (H_2O) molecule, the ratio of Hydrogen and oxygen is ____________.
(a) 1:2
(b) 2:1
(c) 2:2
(d) 1:1
Show Answer

53. A compound is always represented by ___________.
(a) Chemical formula
(b) Physical Formula
(c) None
(d) All of These
Show Answer

54. A _________ is made up of two or more substances that are not chemically combined.
(a) Compound
(b) Mixture
(c) Element
(d) None of these
Show Answer

55. The components of a mixture are not in a fixed __________.
(a) Ratio
(b) Composition
(c) Pattern
(d) None of these
Show Answer

56. Mixture can be separated by _______methods.
(a) Physical
(b) Analytical
(c) Chemical
(d) None of these
Show Answer

57. A homogenous mixture is one which has uniform __________ throughout its mass.
(a) Properties
(b) structure
(c) Composition
(d) None of these
Show Answer

58. Example of homogenous mixture is the solution of salt (NaCl) and ______________.
(a) Benzene
(b) Water
(c) chloroform
(d) None of these
Show Answer

59. A hetrogenous mixture is one which does not have _________composition throughout its mass.
(a) Uniform
(b) Semi Uniform
(c) Unformal
(d) None of these
Show Answer

60 Salad, dirt, sand and water etc are the example of ___________________.
(a) Homogenous mixture
(b) Compound
(c) Heterogeneous mixture
(d) None of these
Show Answer

61 The _______ of a compound is sharp and fixed.
(a) Freezing point
(b) Melting point
(c) Boiling point
(d) None of these
Show Answer

62. ____________ do not have sharp and fixed melting point.
(a) Mixture
(b) Molecules
(c) Isotopes
(d) None of these
Show Answer

63. When iron (Fe) and Sulphur (s) is strongly heated, it react with each other to form a compound.
(a) FeS
(b) Fe_2S
(c) FeS_2
(d) Fe_2S_2
Show Answer

64. The number of ______________ present in the nucleus of an atom of an element is called atomic number .
(a) Neutrons
(b) Electrons
(c) Protons
(d) None of these
Show Answer

65. An atom is electrically _______, because they have same number of electrons and protons.
(a) Cationic
(b) Neutral
(c) Anionic
(d) None of these
Show Answer

66. Elements are arranged in periodic table on the basis of number of ___________.
(a) Protons
(b) Quarks
(c) Electrons
(d) None of these
Show Answer

67. Atomic number is represented by _____________.
(a) z
(b) Z
(c) a
(d) A
Show Answer

68. The atomic number of carbon ( C ) is ______________.
(a) 5
(b) 7
(c) 6
(d) 8
Show Answer

69. Mass number is also called ____________number.
(a) Nucleon
(b) Neutron
(c) None
(d) All of these
Show Answer

70. The sum of number of protons and neutrons present in __________ of an atom is called mass number.
(a) Orbits
(b) Atom
(c) Nucleus
(d) None of these
Show Answer

71. Mass number is represented by _________________.
(a) a
(b) z
(c) A
(d) Z
Show Answer

72. The mass number of carbon (C) atom is _______________.
(a) 12
(b) 2
(c) 22
(d) 18
Show Answer

73. Electrons, protons and neutrons are collectively called as _________.
(a) Charges
(b) Unit
(c) Subatomic particle
(d) None of these
Show Answer

74. Relative atomic mass is the mass of an atom of an element relative to the mass of 1/12 of the mass of _________.
(a) C-12
(b) C-13
(c) C-14
(d) None of these
Show Answer

75. The atomic weight of C-12 is 12g which equal to ___________.
(a) 12 mol
(b) 1 mol
(c) 6.022 mol
(d) None of these
Show Answer

76. 1 mol of C-12 contain ______atoms.
(a) 6.023 \times 10^{23}
(b) 1.09 \times 10^{-11}
(c) 6.023 \times 10^{-23}
(d) None of these
Show Answer

77. Average atomic mass is the weighted average of the atomic masses of the naturally occurring ____________ of an element.
(a) Charges
(b) Isotopes
(c) Atomic Number
(d) None of these
Show Answer

78. An abbreviation used for the full name of a compound with the help of __________ is called chemical formula.
(a) Pattern
(b) Brails
(c) Symbols
(d) None of these
Show Answer

79. The formula tells us the type of atoms and ______ of the different atoms present in the compound.
(a) Ratio
(b) Atomic number
(c) Density
(d) None of these
Show Answer

80. The simplest formula which shows the _________ whole number ratio of the atoms of different elements present in a compound is called empirical formula.
(a) Largest
(b) Smallest
(c) Average
(d) None of these
Show Answer

81. The empirical formula for benzene (C_6H_6) is:
(a) CH_2
(b) C_2H
(c) C_2H_2
(d) CH
Show Answer

82. The molecular formula shows the _________numbers of atoms of different elements present in one molecule of a compound.
(a) Approximate
(b) Whole
(c) actual
(d) None of these
Show Answer

83. The smallest repeating unit of an ____________ compound showing the simple reaction between the ions is called formula unit.
(a) Ionic
(b) Covalent
(c) Metallic
(d) None of these
Show Answer

84. The __________ of the relative atomic masses of all the atoms present in the molecule is called molecular Mass.
(a) Subtraction
(b) Product
(c) Sum
(d) None of these
Show Answer

85. The sum of the atomic masses of __________ present in the formula unit of an ionic compound is called formula mas.
(a) Ions
(b) Isotopes
(c) atoms
(d) None of these
Show Answer

86. The atoms, molecules, ions etc that __________ in a chemical reaction is called chemical specie.
(a) Violate
(b) Hinder
(c) Take part
(d) None of these
Show Answer

87. The particle that carries an electrical charge, positive or negative due to the loss or gain of one or more _____ is called an ion.
(a) Protons
(b) Electrons
(c) Neutrons
(d) None of these
Show Answer

88. The positively charged specie is called ____________.
(a) Cation
(b) Free radical
(c) atom
(d) None of these
Show Answer

89. The negatively charged specie is called ___________________.
(a) Free radical
(b) Cation
(c) Anion
(d) None of these
Show Answer

90. The atom or group of atoms that has an __________ electron in an outer shell with no charge is called free radical.
(a) Unpaired
(b) Odd
(c) Both a and b
(d) None of these
Show Answer

91. A molecule is formed by ________ combination of atom.
(a) Chemical
(b) Physical
(c) Electrical
(d) None of these
Show Answer

92. Di-atomic molecules consist of _________ atoms i.e H_2 .
(a) 4
(b) 3
(c) 5
(d) 2
Show Answer

93. The ___________ are very big and large.
(a) Monoatomic
(b) Macro molecules
(c) Micro molecules
(d) None of these
Show Answer

94. _____________ is a macromolecule found in blood.
(a) Haemoglobin
(b) H_2O
(c) HCl
(d) None of these
Show Answer

95. Avogadro’s number is the collection of __________ particles.
(a) 1.0 \times 10^{-11}
(b) 6.023 \times 10^{23}
(c) 3 \times 10^8
(d) None of these
Show Answer

96. The amount of a substance which contains ____________ number is called mole.
(a) Avogadro’s
(b) Mass number
(c) Formula
(d) None of these
Show Answer

97. Mole is represented by _________________.
(a) NA
(b) mol
(c) amu
(d) None of these
Show Answer

98. Which one of the following can be broken into simpler substances.
(a) Ammonia
(b) Oxygen
(c) Sulphur
(d) None of these
Show Answer

99. The gram molecular mass of HNO_3 is .
(a) 60
(b) 100
(c) 63
(d) None of these
Show Answer

100. Which one is the example of triatomic molecule?
(a) O_2
(b) CO_2
(c) CH_4
(d) None of these
Show Answer

101. Which of the following is a homogenous mixture?
(a) Smoke
(b) air
(c) Fog
(d) Smog
Show Answer

Prepared by Hafiz Muhammad Uzair

1. A Greek philosopher “Democritus” suggested that all———— can be further divided into tiny particles.
(a) matter
(b) substances
(c) elements
(d) All of them
Show Answer

2. The name of atom was given from the Greek word ————- which means indivisible.
(a) atomos
(b) atomics
(c) Halogens
(d) None of these
Show Answer

3. The word atom was first used —————.
(a) 400AD
(b) 400 BC
(c) 600AD
(d) 600BC
Show Answer

4. No further work on atom was done until the ————– century.
(a) 18th
(b) 20th
(c) 19th
(d) 21st
Show Answer

5. John Dalton, after a lot of experiments, concluded that all matter must be composed of tiny particles called —-.
(a) Atom
(b) Element
(c) isotope
(d) None of these
Show Answer

6. John Dalton states that an atom is ——————-.
(a) Invincible
(b) Indivisible
(c) Invisible
(d) None of these
Show Answer

7. John Dalton presented his own theory about atom in —————–.
(a) 1806
(b) 1906
(c) 1808
(d) 1908
Show Answer

8. ————–is composed of very small particles called atoms.
(a) Matter
(b) Energy
(c) Numbers
(d) All of these
Show Answer

9. Atom can neither be created nor ———————.
(a) Formulated
(b) Destroyed
(c) combined
(d) None of these
Show Answer

10. Atoms combine with each other in ————– number ratio.
(a) Integers
(b) Quadratic
(c) Whole
(d) None of these
Show Answer

11. Atoms of particular element are ———— in size shape, mass and also in other properties.
(a) Different
(b) Identical
(c) Atomic
(d) None of these
Show Answer

12. All chemical reactions occur due to the combination or ————— of atoms.
(a) Separation
(b) Distillation
(c) Filtration
(d) None
Show Answer

13. In———-, Rutherford performed an experiment to know the arrangement of electron and protons in an atom.
(a) 1910
(b) 1912
(c) 1911
(d) 1913
Show Answer

14. In Rutherford experiment which part of the atom has been discovered?
(a) Energy levels
(b) Nucleus
(c) Other
(d) None
Show Answer

15. ————— performed an experiment to determine the internal structure of the atom in 1911.
(a) J.J Thompson
(b) Max plank
(c) Rutherford
(d) None of these
Show Answer

16. In Rutherford experiment, what he has used?
(a) Gold foil
(b) Gold bar
(c) Silver foil
(d) Tin plates
Show Answer

17. He bombarded the ________ particles on gold foil from a radioactive source.
(a) Beta
(b) Alpha
(c) Gamma
(d) None of these
Show Answer

18. What radioactive source does Rutherford used?
(a) Polonium
(b) Thorium
(c) Radon
(d) None of these
Show Answer

19. This experiment showed that most of the volume occupied by the atom is —————.
(a) Bulky
(b) Small
(c) Empty
(d) None of these
Show Answer

20. From this experiment, Rutherford concluded that an atom contains a ———– portion i.e. nucleus.
(a) Negative
(b) Positive
(c) Neutral
(d) None of these
Show Answer

21. Similar charges ————–each other.
(a) Repel
(b) Attract
(c) Articulate
(d) All of these
Show Answer

22. On the basis of his conclusion drawn from the experiment, Rutherford proposed a new model at atom called ————-model.
(a) Planetary
(b) Universal
(c) Room & Cat
(d) None of these
Show Answer

23. Atom consists of positively charged nucleus which contains ———and neutrons.
(a) Electrons
(b) Protons
(c) Fundamental particles
(d) None of these
Show Answer

24. Electrons are ————around the nucleus just like the planets around the sun.
(a) Stand still
(b) Gathered
(c) Revolving
(d) None of these
Show Answer

25. The electrons around the nucleus would require ————- force.
(a) Centripetal
(b) Centrifugal
(c) Net
(d) Average
Show Answer

26. The size of the ————- is very small as compared to the size of atom.
(a) proton
(b) Neutron
(c) Nucleus
(d) All of them
Show Answer

27. Atom is ———— because electrons and protons will cancel the effect of each other.
(a) Negatively charge
(b) Neutral
(c) Positively charged
(d) None of these
Show Answer

28. Rutherford atomic model of an atom resembles our ________ system.
(a) Solar
(b) Universal
(c) Gravitational
(d) None of these
Show Answer

29. Rutherford model is applicable to neutral bodies and not on ————.
(a) Isotopes
(b) Energy
(c) Charged bodies
(d) None of these
Show Answer

30. According to which scientist, electrons are charged bodies revolving around the nucleus and emit energy.
(a) Rutherford
(b) Schrodinger
(c) Maxwell
(d) None of these
Show Answer

31. If electrons radiate energy continuously then the ———–spectrum will be obtained.
(a) Line
(b) Continuous
(c) Both
(d) None of these
Show Answer

32. Rutherford atomic model does not provide any explanation about ———— properties of elements.
(a) Chemical
(b) Physical
(c) Elemental
(d) None of these
Show Answer

33. In ————-, Neil Bohr proposed a new atomic theory to overcome the defects of Rutherford atomic model.
(a) 1901
(b) 1910
(c) 1915
(d) 1913
Show Answer

34. Bohr considered ———-atom as a model.
(a) Helium
(b) Hydrogen
(c) Thorium
(d) None of these
Show Answer

35. Electrons are revolving around the fixed circular path called ————-.
(a) Shells
(b) Orbits
(c) cycles
(d) Both a and b
Show Answer

36. Each shell has a —————– energy.
(a) Fixed
(b) variable
(c) No
(d) None of these
Show Answer

37. The farther the electron from the nucleus, the ———— will be the energy and vice versa.
(a) Lower
(b) Higher
(c) Intermediate
(d) None of these
Show Answer

38. The ________ of an object is fixed.
(a) Frequency
(b) Volume
(c) Energy
(d) None of these
Show Answer

39. ∆E=E_2-E_1=h \mu In ths equation what is “h”?
(a) Plank’s constant
(b) Max constant
(c) Variable
(d) None of these
Show Answer

40 Electrons can’t stay in ———shells.
(a) 1st
(b) 2nd
(c) Between
(d) None of these
Show Answer

41. Modern research show that an atom consist of ————— subatomic particles.
(a) 13
(b) 03
(c) 05
(d) None of these
Show Answer

42. Election is ————— charged particle.
(a) Negatively
(b) Positively
(c) Neutral
(d) All of these
Show Answer

43. Mass of electron is ————–.
(a) 9.11 \times 10^{31} kg
(b) 9.11 \times 10^{-31} kg
(c) 6.023 \times 10^{23} kg
(d) All of these
Show Answer

44. Proton is a ———— charged particle.
(a) Negatively
(b) Positively
(c) Neutral
(d) None of these
Show Answer

45. Mass of proton is —————.
(a) 1.6726 \times 10^{-27} \ kg
(b) 9.11 \times 10^{-31} \ kg
(c) 1.37 \times 10^6 \ kg
(d) All of these
Show Answer

46. Proton is ———– times heavier than electron.
(a) 1847
(b) 1827
(c) 1837
(d) All of these
Show Answer

47. Neutron is a ————- particle because it has no charge.
(a) Negative
(b) Positive
(c) Neutral
(d) None of these
Show Answer

48. Neutron is ———– times Havier than proton.
(a) 05
(b) 15
(c) 50
(d) 150
Show Answer

49. The ———— of electrons around the nucleus in shells is called electronic configuration.
(a) Separation
(b) Distribution
(c) Catenation
(d) None of these
Show Answer

50. These shells are represented by ————.
(a) Alphabets
(b) Numeric
(c) Romans
(d) None of these
Show Answer

51. The maximum number of electrons in a particular shell is given by the formula ————.
(a) 4n^2
(b) 2n^3
(c) 4n^3
(d) 2n^2
Show Answer

52. How many electrons are there K-shell?
(a) 2
(b) 8
(c) 18
(d) 32
Show Answer

53. How many electrons are there in L-shell?
(a) 2
(b) 8
(c) 18
(d) 32
Show Answer

54. How many electrons are there in M-shell?
(a) 2
(b) 8
(c) 18
(d) 32
Show Answer

55. How many electrons are there in N-shell?
(a) 2
(b) 8
(c) 18
(d) 32
Show Answer

56. A shell or orbit is also is also called ———–.
(a) Energy level
(b) Hertz
(c) Atomic mass
(d) None of these
Show Answer

57. How many sub-shall are there in a shell?
(a) 14
(b) 10
(c) 04
(d) None of these
Show Answer

58. Which of them are sub-shell?
(a) s, p, d, f
(b) x, y, z
(c) K, L, M, N
(d) None of these
Show Answer

59. “s” sub –shell stands for ————-.
(a) Specific
(b) Sharp
(c) Sonic
(d) All of these
Show Answer

60 “p” sub-shell stands for —————
(a) Principal
(b) principle
(c) Para-magnetic
(d) None of these
Show Answer

61 “d” sub –shell stands for ————-.
(a) Drainage
(b) dissolved
(c) diffused
(d) All of these
Show Answer

62. “f” sub-shell stand for———–.
(a) Fermium
(b) fundamental
(c) Fencing
(d) None of these
Show Answer

63. “f” sub-shell can accommodate————- electrons.
(a) 2
(b) 6
(c) 10
(d) 14
Show Answer

64. Complete the electronic configuration of carbon atom i.e. 1s^2, 2S^2, ————-.
(a) 2p^2
(b) 2p^3
(c) 2p^4
(d) 2p^5
Show Answer

65. Atoms of the same element having same atomic number but different ———– is called isotopes.
(a) Density
(b) Mobility
(c) Mass number
(d) None of these
Show Answer

66. Atoms having same number of protons and electrons but differ number of neutrons are called ———–.
(a) Metallurgy
(b) Isotopes
(c) Surface area
(d) None of these
Show Answer

67. How many isotopes hydrogen has?
(a) 03
(b) 06
(c) 09
(d) 12
Show Answer

68. Protium, deuterium and tritium are the isotopes of ————-.
(a) carbon
(b) chlorine
(c) Hydrogen
(d) None of these
Show Answer

69. What is the most abundant isotope of hydrogen?
(a) Podium
(b) Deuterium
(c) tritium
(d) None of these
Show Answer

70. Which isotope of hydrogen is rarely found in nature?
(a) Protium
(b) Deuterium
(c) Tritium
(d) None of these
Show Answer

71. How many neutrons are there in tritium?
(a) 02
(b) 03
(c) 01
(d) None of these
Show Answer

72. Atomic number of carbon is ————-.
(a) 07
(b) 06
(c) 08
(d) None of these
Show Answer

73. Carbon is the first member of ————–.
(a) Group 1
(b) Group 7
(c) Group 4
(d) Group 6
Show Answer

74. How many isotopes of carbon are there in nature?
(a) 03
(b) 13
(c) 07
(d) 14
Show Answer

75. C -12, C -13 \ and \ C -14 are the isotopes of ————–.
(a) Iodine
(b) Radon
(c) Carbon
(d) none
Show Answer

76. Number of neutrons in Carbon-14 \ \left(_{14}C^6 \right) is —————.
(a) 7
(b) 8
(c) 9
(d) 10
Show Answer

77. Atomic number of chlorine is ——————–.
(a) 17
(b) 6
(c) 1
(d) 3
Show Answer

78. Chlorine is the second member of ————-
(a) Group 1
(b) Group 4
(c) Group 7
(d) Group 5
Show Answer

79. Group 7is also called ————-
(a) Alkali metals
(b) Halogens
(c) Nobles
(d) none
Show Answer

80. How many isotopes of chlorines are there in nature?
(a) 02
(b) 12
(c) 03
(d) 13
Show Answer

81. Cl -35 \ and \ Cl-37 are isotopes of ————–.
(a) Radon
(b) Krypton
(c) Chlorine
(d) Hydrogen
Show Answer

82. The abundance of Cl -35 is —————-.
(a) 75.53%
(b) 53.75%
(c) 73.55%
(d) 53. 66%
Show Answer

83. The abundance of Cl-37 is————- in nature.
(a) 24.47%
(b) 47.24%
(c) 74. 42%
(d) 54.26%
Show Answer

84. The number of neutrons in Cl-35 is 18 and Cl-37 is —————-.
(a) 20
(b) 40
(c) 02
(d) 04
Show Answer

85. Atomic number of uranium is —————.
(a) 82
(b) 92
(c) 28
(d) 29
Show Answer

86. How many isotopes of uranium in nature?
(a) 07
(b) 05
(c) 03
(d) 04
Show Answer

87. The most abundant isotope of uranium is —————.
(a) U -238
(b) U-235
(c) U-234
(d) U-236
Show Answer

88. The neutrons quantity in U-238 is ————–.
(a) 142
(b) 146
(c) 143
(d) 145
Show Answer

89. Iodine -131 is used for the cure of ————-.
(a) Pneumonia
(b) Cancer
(c) Goiter
(d) None of these
Show Answer

90. Cobalt -60 is used for the treatment of —————-.
(a) Cancer
(b) Diarrhea
(c) Tumor
(d) Treat less
Show Answer

91. Carbon -14 is used to trace the path of carbon in ————–.
(a) Respiration
(b) Photosynthesis
(c) Reduction
(d) None of these
Show Answer

92. Californium -252 is used to inspect airplane luggage for hidden —————-.
(a) Explosives
(b) Smoke detectors
(c) Carbon tracing
(d) None of these
Show Answer

93. The maximum number of electrons in third energy level is:
(a) 10
(b) 32
(c) 18
(d) 64
Show Answer

94. Mass of an atom is mostly due to its
(a) Nucleus
(b) Neutrons
(c) Electrons
(d) Protons
Show Answer

95. If Rutherford had used neutrons instead of alpha particles in his scattering experiment, the neutrons would
(a) Not deflect because they have no charge
(b) Have deflected more often
(c) Have been attracted to the nucleus easily
(d) Have given the same results
Show Answer

96. Electron in its ground state does not
(a) Spin
(b) Revolve
(c) Radiate energy
(d) Reside in orbit
Show Answer

97. Which statement about _6^{12}X \ and \ _6^{14}Y is false except
(a) They are isotopes
(b) They are the same elements
(c) They have the same number of electrons
(d) They have the same number of neutrons
Show Answer

98. The neutron particle
(a) Has a mass equal to that of an electron
(b) Has a mass approximately equal to that of a proton
(c) Has charge equal to but opposite to that of an electron
(d) Has a positive charge
Show Answer

99. Isotopes of the same element have
(a) The same number of protons
(b) The same number of neutrons
(c) Different number of electrons
(d) The same mass number
Show Answer

100. Which one is the lightest?
(a) An alpha particle
(b) A hydrogen atom
(c) An electron
(d) A proton
Show Answer

101. The nucleus of an atom has all of the following Characteristics except that
(a) Is positively charged
(b) Is very dense
(c) Contains nearly all of the atom’s mass
(d) Contains nearly all of the atom’s volume
Show Answer

102. L – shell has sub – shell (s)
(a) s
(b) s and p
(c) s, p, and d
(d) s, p, d and f
Show Answer

Prepared by Hafiz Muhammad Uzair

1. In the year 1800 , only ___________ elements were known.
(a) 34
(b) 38
(c) 42
(d) 46
Show Answer

2. By the year ___________ about 68 elements were known.
(a) 1800
(b) 1820
(c) 1840
(d) 1870
Show Answer

3. Till 1974, there were total ___________ elements present.
(a) 85
(b) 100
(c) 105
(d) 120
Show Answer

4. At present ___________ elements are known till date.
(a) 118
(b) 108
(c) 128
(d) 201
Show Answer

5. Out of 118 elements, ___________ were naturally occurring elements.
(a) 105
(b) 38
(c) 92
(d) 68
Show Answer

6. In periodic table, 26 elements are ___________.
(a) Natural
(b) Artificial
(c) None
(d) Complex
Show Answer

7. Many chemists, including Lavoisier (1787), Newlands (1864) attempted to classify the elements___________.
(a) systematically
(b) Vertically
(c) Originally
(d) Horizontally
Show Answer

8. In 1869, Russian chemist Mendeleev made the most successful classification based on ___________ of the element.
(a) Atomic number
(b) Atomic mass
(c) Radicals
(d) Masses
Show Answer

9. Initially, elements were divided into metals and ___________.
(a) Transition element
(b) Lanthanide series
(c) Non-metal
(d) Radical
Show Answer

10. In 1964, an English chemist J.Newland classified the elements in order of ___________atomic masses.
(a) Increasing
(b) Decreasing
(c) Constant
(d) Same
Show Answer

11. In 1869, Dimitri Mendeleev arranged _________elements in periods and groups.
(a) 65
(b) 68
(c) 75
(d) 63
Show Answer

12. The modern periodic table was put forward by:
(a) Mendeleev
(b) Newlands
(c) Henry Moseley
(d) Rutherford
Show Answer

13. Modern periodic table is based on _________.
(a) Atomic mass
(b) Atomic number
(c) Valency
(d) Last shell
Show Answer

14. The modern periodic law states that, “ the physical and chemical properties of elements are the periodic _________ of their atomic number”.
(a) Function
(b) Law
(c) Octave
(d) Valence
Show Answer

15. The _________rows of elements in periodic table are called periods.
(a) Vertical
(b) Horizontal
(c) Planner
(d) First
Show Answer

16. There are total _________periods in periodic table.
(a) 3
(b) 5
(c) 7
(d) 11
Show Answer

17. All the elements in the same period have the same number of electronic _________.
(a) Shells
(b) Orbit
(c) Energy levels
(d) All
Show Answer

18. The first period contain _________ electronic shell.
(a) 1
(b) 3
(c) 2
(d) 4
Show Answer

19. The second period contains _________electronic shells.
(a) 1
(b) 3
(c) 2
(d) 4
Show Answer

20. The third period contains ________ electronic shells.
(a) 1
(b) 3
(c) 2
(d) 4
Show Answer

21. The first period contain two elements i.e hydrogen and _________.
(a) Argon
(b) Lithium
(c) Helium
(d) Carbon
Show Answer

22. The first period is also called the _________ period of periodic table.
(a) Shortest
(b) Longest
(c) Average
(d) Constant
Show Answer

23. 2nd and 3rd period each contain _________elements and are called short periods.
(a) 18
(b) 8
(c) 17
(d) 7
Show Answer

24. The 4th and 5th periods have _________elements each.
(a) 18
(b) 8
(c) 17
(d) 7
Show Answer

25. In 4th and 5th period, 8 elements are called_________elements.
(a) Transition
(b) Representative
(c) Alkali
(d) Alkaline
Show Answer

26. In 4th and 5th period, 10 elements are called _________elements.
(a) Transition
(b) Representative
(c) Alkali
(d) Alkaline
Show Answer

27. The 6th period contains _________ elements.
(a) 64
(b) 32
(c) 25
(d) 20
Show Answer

28. In 6th period, there are _________ representative elements.
(a) 8
(b) 14
(c) 20
(d) 26
Show Answer

29. The 6th period have_________ transition elements.
(a) 8
(b) 14
(c) 10
(d) 20
Show Answer

30. In 6th period, the 14 elements of _________ series.
(a) Lanthanide
(b) Actinide
(c) Hydranite
(d) None
Show Answer

31. 7th period also has 8 representative elements, 10 transition elements and 14 elements of _________ series.
(a) Lanthanide
(b) Actinide
(c) Halogens
(d) None
Show Answer

32. The vertical column of elements in periodic table is called_______________.
(a) Periods
(b) traids
(c) Groups
(d) None of these
Show Answer

33. The groups in periodic table are numbered from:
(a) A to H
(b) I to VIII
(c) I to X
(d) A to G
Show Answer

34. Elements in the same group have same number of ___________in the outermost shell of the atom.
(a) electrons
(b) Proton
(c) Neutrons
(d) Mass number
Show Answer

35. Because of similarity in number of valance electrons, elements show resemblance in their ____________ properties in the same group.
(a) Physical
(b) Chemical
(c) Biological
(d) Electrical
Show Answer

36. The first group elements possess only __________valance electron.
(a) one
(b) Two
(c) Three
(d) Four
Show Answer

37. Group 1st elements are _________ .
(a) Less reactive
(b) Very reactive
(c) Non-reactive
(d) Constant
Show Answer

38. Group 1st elements are __________ in nature and show metallic character.
(a) Electropositive
(b) Electronegative
(c) Stable
(d) Electric field
Show Answer

39. Group 1st elements are also called_________________.
(a) Noble metals
(b) Alkali metals
(c) Transition
(d) Halogen group
Show Answer

40 Beryllium, Magnesium and calcium belongs to:
(a) Group V
(b) Group II
(c) Group VII
(d) Group III
Show Answer

41. Elements of group II are also called _____________ metals.
(a) Alkaline earth
(b) Alkali
(c) Nitrogen family
(d) Hydrogen family
Show Answer

42. Elements in group 2nd possess ____________ valance electrons.
(a) One
(b) Two
(c) Three
(d) Four
Show Answer

43. Group 2nd elements are ____________ electropositive than alkali metals.
(a) Same as
(b) More
(c) less
(d) Grater
Show Answer

44. Group III is called ____________ family.
(a) Carbon
(b) Boron
(c) Nitrogen
(d) Carbon
Show Answer

45. Elements of Group 3rd have ____________ valance electrons.
(a) One
(b) Two
(c) three
(d) Five
Show Answer

46. Group IV is called ____________ family, having four valance electrons.
(a) Carbon
(b) Metal
(c) Nitrogen
(d) Hydrogen
Show Answer

47. Group V is called ____________ family, having 5 valance electrons.
(a) Carbon
(b) Metal
(c) Nitrogen
(d) Helium
Show Answer

48. Group VI is called ____________family, having 6 valance electrons.
(a) Oxygen
(b) Metal
(c) Boron
(d) Iron
Show Answer

49. The seventh group in periodic table is ____________.
(a) Noble
(b) Halogens
(c) Alkali metals
(d) Carbon
Show Answer

50. Halogens have _____________ electrons in valance shell.
(a) Eleven
(b) Nine
(c) 7 seven
(d) Four
Show Answer

51. Halogens need ____________ electron to complete its octet.
(a) One
(b) Five
(c) Six
(d) Seven
Show Answer

52. Halogens are very ____________ and show non-metallic character.
(a) Electropositive
(b) Electronegative
(c) Mass number
(d) None
Show Answer

53. The 8th group is called _______ gases.
(a) Noble
(b) Hydrocarbon
(c) Lanthanide
(d) Actinide
Show Answer

54. They have two or __________ electrons in their valance shell.
(a) Two
(b) Five
(c) eight
(d) One
Show Answer

55. Group one and two elements are called ____________ elements.
(a) S-block
(b) P-block
(c) d-block
(d) b-block
Show Answer

56. All S-block and P-block elements are called ____________ elements.
(a) Transition
(b) Representative
(c) Traids
(d) None
Show Answer

57. Lanthanide and actinide series are called ____________ elements.
(a) f-block
(b) S-block
(c) P-block
(d) N-block
Show Answer

58. A pattern of repeating properties at regular interval is called ____________.
(a) Periodicity
(b) Aromaticity
(c) Electronegativity
(d) Electropositivity
Show Answer

59. The process by which there is __________ of properties in all group and periods after certain interval are called periodicity of properties.
(a) Repulsion
(b) repetition
(c) Exclusion
(d) Inclusion
Show Answer

60 The size of the atom is :
(a) Fixed
(b) Not fixed
(c) Constant
(d) Flexible
Show Answer

61 The distance between the nucleus and the valance shell of the atom is called____________.
(a) Atomic radius
(b) Atomic size
(c) Atomic mass
(d) Atomic number
Show Answer

62. The atomic radius is represented by ____________.
(a) R
(b) Ar
(c) r
(d) None
Show Answer

63. Atomic radius is ____________ proportional to no of shells.
(a) Directly
(b) Inversely
(c) Constant
(d) Indirect
Show Answer

64. Atomic radius is expressed in ____________.
(a) Dm,km
(b) nm, pm
(c) km, pm
(d) Qm, rm
Show Answer

65. Atomic radius ____________ in groups from top to bottom.
(a) Decrease
(b) No change
(c) increase
(d) None
Show Answer

66. Atomic radius decrease in period from ____________.
(a) Left to right
(b) Right to left
(c) Up to down
(d) Up to left
Show Answer

67. The decrease of atomic radius in periods is due to ____________ of electrons in same shell.
(a) Removal
(b) addition
(c) Variable
(d) Constant
Show Answer

68. The one half of the distance between nuclei of two similar atoms of same molecule containing ____________ covalent bond.
(a) Triple
(b) Double
(c) single
(d) Fourth
Show Answer

69. The general formula of covalent radius is :
(a) d/2
(b) 2 / d
(c) 1/ 2 D
(d) 3/ 2
Show Answer

70. Covalent radii of F_2 molecule is ;
(a) 199 pm
(b) 143pm
(c) 228pm
(d) 271pm
Show Answer

71. The minimum energy required to remove the valance electron from valence shell to form ____________ is called ionization energy.
(a) Positive ion
(b) Negative ion
(c) Radical
(d) Constant
Show Answer

72. When the electron is completely removed from valance shell, the process is called____________.
(a) Fractionation
(b) Distillation
(c) ionization
(d) Filtration
Show Answer

73. The process of ionization needs____________.
(a) Matter
(b) energy
(c) Electron affinity
(d) Electrical positivity
Show Answer

74. Ionization energy of an elements is measured in:
(a) Joules
(b) Frequency
(c) Hertz
(d) Galvin
Show Answer

75. The first ionization energy of sodium is:
(a) +1450 kj/mol
(b) +496 kj/mol
(c) +738 kj/mol
(d) +630 kj/mol
Show Answer

76. Ionization energy depends upon all Except:
(a) Atomic radius
(b) Nuclear charge
(c) Shielding effect
(d) Dative bond
Show Answer

77. Ionization energy ____________ as we move down the group.
(a) Decrease
(b) Increase
(c) Constant
(d) Equal
Show Answer

78. Ionization energy_________ in period from left to right.
(a) Decrease
(b) Increase
(c) Constant
(d) Equal
Show Answer

79. The minimum amount of energy released when an electron is added to valance shell of the atom to form _________ is called electron affinity.
(a) Anion
(b) Radical
(c) Cation
(d) None
Show Answer

80. Electron affinity is expressed in _________.
(a) E
(b) A
(c) E.A
(d) A.E
Show Answer

81. Electron affinity is represented by _________.
(a) dm^3
(b) kj/mol
(c) N_A
(d) M_N
Show Answer

82. Electron affinity means love for _________electrons.
(a) Keeping
(b) Donating
(c) Accepting
(d) Losing
Show Answer

83. The electron affinity of “Cl” is _________kj/mol.
(a) -348 kj/mol
(b) +348 kj/mol
(c) -843 kj/mol
(d) -748 kj/mol
Show Answer

84. The electron affinity _________ in a group from top to bottom.
(a) Increase
(b) decreases
(c) No change
(d) Equal
Show Answer

85. The electron affinity _________in a period from left to right.
(a) increase
(b) Decrease
(c) No change
(d) Equal
Show Answer

86. Electrons in an atom are distributed in _________.
(a) Same shell
(b) Different shell
(c) Nucleus
(d) Last shell
Show Answer

87. The inner electrons shield the outer electron from the nuclear charge and reduce hold of the nucleus on these valance electrons. This effect is called_________.
(a) Shielding effect
(b) Screening effect
(c) Allotropy
(d) Both a and b
Show Answer

88. The shielding effect _________, when we move from left to right in a period.
(a) increase
(b) Decrease
(c) Remains same
(d) None
Show Answer

89. The ability of an atom to ________ shared pair of electron towards itself is called electronegativity.
(a) Repel
(b) attract
(c) Share
(d) Gain
Show Answer

90. The attraction of shared pair electron in electronegativitywill occur in _________ bond.
(a) Ionic
(b) Metallic
(c) covalent
(d) Organic
Show Answer

91. In a covalent bond, two atoms involve in _________, mutually share their electrons.
(a) Bond formation
(b) Electron donation
(c) Nucleons
(d) Protons
Show Answer

92. Electronegativity is represented by_________.
(a) E
(b) E
(c) E.N
(d) none
Show Answer

93. The following factors affect electronegativity Except:
(a) Mobility
(b) Nuclear charge
(c) Shielding effect
(d) Atomic radius
Show Answer

94. The electronegativity _________ in groups from top to bottom.
(a) Increase
(b) decrease
(c) Constant
(d) None
Show Answer

95. Electronegativity _________ in periods form left to right.
(a) Increase
(b) Decrease
(c) Constant
(d) None
Show Answer

96. The most electronegative element in periodic table is_________.
(a) Chlorine
(b) cesium
(c) Fluorine
(d) None
Show Answer

97. The least electronegative element in periodic table is:
(a) Chlorine
(b) Cesium
(c) Fluorine
(d) None
Show Answer

98. The electronegativity of fluorine is
(a) 4.0
(b) 0.7
(c) 3.0
(d) 0.8
Show Answer

99. The electronegativity of Cesium is:
(a) 4.0
(b) 0.7
(c) 3.0
(d) 0.8
Show Answer

100. Which one has the largest ionization energy?
(a) Na
(b) Al
(c) H
(d) He
Show Answer

101. Which of the following elements is in the same family as fluorine:
(a) Silicon
(b) Antimony
(c) iodine
(d) Arsenic
Show Answer

102. Which of the following would have the smallest ionization energy:
(a) K
(b) P
(c) S
(d) Ca
Show Answer

103. An element has configuration 2, 8, 1. It belongs to, _________:
(a) Group I and III period
(b) Group III and I period
(c) Group I and VII period
(d) Group VII and III period
Show Answer

104. Which of the following elements would be most similar to carbon:
(a) Nitrogen
(b) Boron
(c) Oxygen
(d) silicon
Show Answer

105. s-block elements are:
(a) metals
(b) Non-metal
(c) Metalloids
(d) Transition
Show Answer

106. Which of the following would have the largest ionization energy:
(a) Na
(b) Al
(c) H
(d) He
Show Answer

107. Elements in a _________ have similar chemical properties:
(a) Period
(b) group
(c) Both a and b
(d) Neither a nor b
Show Answer

108. An element has 8 electrons in its valence shell. It is a member of:
(a) Alkali family
(b) Halogen family
(c) Noble family
(d) Carbon family
Show Answer

109. The modern periodic table is based on:
(a) Atomic number
(b) Mass number
(c) Neutron number
(d) Isotope number
Show Answer

110. Shielding effect is due to:
(a) Neutron
(b) Proton
(c) Proton and neutron
(d) electron
Show Answer