Chemistry For Class IX (New Book ) - Chapter No. 1- Fundamentals of Chemistry - Multiple Choice Questions And Fill In The Blanks

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Chapter No.1 - Fundamentals of Chemistry
MCQs And Fill In The Blanks
Multiple Choice Questions

Tick Mark (✓) the correct answer
1. The branch of Chemistry which deals with hydrocarbons:
(a) Industrial chemistry
(b) Inorganic chemistry
(c) Organic chemistry ✓
(d) Physical chemistry

2. The atomic mass of an element expressed in gram is:
(a) Gram molecular mass
(b) Gram atomic mass ✓
(c) Gram formula mass
(d) Mole

3. Which of the following can be separated by physical means?
(a) Mixture ✓
(b) Element
(c) Compound
(d) Substance

4 The molar mass of H₂SO₄ is:
(a) 98 a.m.u
(b) 9.8 gm
(c) 98 gm ✓
(d) 9.8 a.m.u

5. The Molecule consist of two atoms is:
(a) Monoatomic molecule
(b) Polyatomic molecule
(c) Heteroatomic molecule
(d) Diatomic molecule ✓

6. A formula that indicates actual number and type of atoms in a molecule is called:
(a) Chemical formula
(b) Empirical formula
(c) Molecular formula ✓
(d) Formula mass

7. Ethyl alcohol was prepared by:
(a) Ibne-Sina
(b) Al-Razi ✓
(c) Al-Beruni
(d) Jaber bin-Hayan

8. which of the following is a homoatomic:
(a) H ✓
(b) NH₃
(c) H₂O
(d) CO₂

9. The Empirical formula of hydrogen peroxide is:
(a) H₂O₂
(b) HO ✓
(c) OH
(d) O₂H₂

10. A piece of matter in pure form is termed as:
(a) Radical
(b) Mixture
(c) Compound
(d) substance ✓

11. The word science comes from the word "Scientia" which is:
(a) Greek word
(b) Latin word ✓
(c) Persian word
(d) Arabic word

12. The Latin word "Scientia" means:
(a) process
(b) phenomenon
(c) knowledge ✓
(d) natural

13. In universal sciences chemistry purely deals with the:
(a) matter ✓
(c) chemical properties
(b) energy
(d) chemical reactions

14. Matter has:
(a) energy and occupy space
(b) weight and occupy space
(c) valency and occupy space
(d) mass and occupy space ✓

15. In nature, the matter changing:
(a) sometimes
(b) continuously ✓
(c) under certain conditions
(d) None of them

16. He proposed the idea of the atom.
(a) Aristotle
(b) Plato
(c) Democritus ✓
(d) Lavoisier

17. He invented experimental methods of nitric acid, hydrochloric acid, and white lead.
(a) Al-Razi
(b) Al-Beruni
(c) Ibne-Sina
(d) Jabir Ibn Hayyan ✓

18. He found the methods of extraction of metals from their ores and dyeing clothes.
(a) Jabir Ibn Hayyan ✓
(b) Al-Razi
(c) Ibne-Sina
(d) Al-Beruni

19. Densities of different substances was determined by:
(a) J. Priestley
(b) Al-Beruni ✓
(c) Al-Razi
(d) Gay Lussac

20. This Muslim scientist contributed to medicines, philosophy, and astronomy.
(a) Jabir Ibn Hayyan
(b) Al-Razi
(c) Ibne-Sina ✓
(d) Al-Beruni

21. The gaseous law was discovered by:
(a) Robert Boyle ✓
(b) John Dalton
(c) Mendeleev
(d) Eric Cornell

22. Oxygen, Sulphur dioxide, and hydrogen chloride were discovered by:
(a) J. Priestley ✓
(b) Cavendish
(c) Lavoisier
(d) Jacques Charles

23. Chlorine was discovered by:
(a) J. Priestley
(b) Cavendish
(c) Gay-Lussac
(d) Scheele ✓

24. Hydrogen was discovered by:
(a) J. Priestley
(b) Cavendish ✓
(c) Scheele
(d) J. Black

25. A French chemist discovered that oxygen is one-fifth of air.
(a) Arrhenius
(b) De Broglie
(c) Lavoisier ✓
(d) Avogadro

26. Atomic theory of matter was proposed by the English scientist:
(a) Jacques Charles
(b) Petit
(c) J.J. Berzelius
(d) John Dalton ✓

27. He discovered that water is composed of two parts hydrogen and one part oxygen by volume.
(a) Lavoisier
(b) J.J. Berzelius
(c) Scheele
(d) Gay-Lussac ✓

28. "Equal volumes of gases under constant temperature and pressure contain the equal number of molecules", is known as:
(a) Gas Law
(b) Avogadro's Law ✓
(c) Atomic Theory
(d) Acid-Base Theory

29. Gaseous law was described by a French scientist:
(a) Jacques Charles ✓
(b) Avogadro
(c) John Dalton
(d) De Broglie

30. Symbols, formula, and chemical equation were introduced by:
(a) Mendeleev
(b) J. J. Berzelius ✓
(c) Arrhenius
(d) De Broglie

31. This Russian chemist discovered the periodic arrangement of elements.
(a) Schrodinger
(b) Eric Cornell
(c) Rutherford
(d) Mendeleev ✓

32. Acid Base Theory and ions dissociation were proposed by:
(a) Mendeleev
(b) Rutherford
(c) Arrhenius ✓
(d) Petit

33. He contributed to the study of electromagnetism and electrochemistry.
(a) J.J. Thomson
(b) Schrodinger
(c) M. Faraday ✓
(d) Carl Wieman

34. The electron was discovered by:
(a) J.J. Thomson ✓
(b) M. Faraday
(c) Rutherford
(d) Albert Einstein

35. This British scientist proposed a theory for the hydrogen atom based on quantum theory.
(a) Rutherford
(b) Satyendra Nath Bose
(c) Carl Wieman
(d) Neil Bohr ✓

36. The nuclear structure of the atom was postulated by:
(a) Neil Bohr
(b) J.J. Thomson
(c) Rutherford ✓
(d) J.J. Berzelius

37. He discovered alpha and beta rays and proposed the laws of radioactive decay.
(a) De Broglie
(b) Rutherford ✓
(c) Schrodinger
(d) Carl Wieman

38. Quantum mechanical model of the atom was proposed by:
(a) Schrodinger ✓
(b) Rutherford
(c) J.J. Thomson
(d) Albert Einstein

39. The hypothesis about wave-particle duality nature of electron was proposed by:
(a) Schrodinger
(b) Eric Cornell
(c) De Broglie ✓
(d) Neil Bohr

40. Fourth state of matter was proposed by:
(a) Satyendra Nath Bose
(b) Albert Einstein
(c) Both of them ✓
(d) None of them

41. The first Bose-Einstein Condensate was synthesized by:
(a) De Broglie
(b) Eric Cornell ✓
(c) Carl Wieman
(d) Schrodinger

42. The first Bose-Einstein Condensate was produced by:
(a) De Broglie
(b) Eric Cornell
(c) Carl Wieman ✓
(d) Schrodinger

43. Chemistry also deals with the changes involved in the:
(a) matter ✓
(b) mass
(c) energy
(d) properties

44. The branch of chemistry which deals with the laws and principles governing the combination of atoms and molecules:
(a) Inorganic chemistry
(b) Biochemistry
(c) Physical chemistry ✓
(d) Analytical chemistry

45. The gasoline, plastics, detergents, dyes, food additives, natural gas, and medicines are studied in the:
(a) Industrial Chemistry
(b) Physical Chemistry
(c) Inorganic Chemistry
(d) Organic Chemistry ✓

46. The branch of Chemistry which deals with the study of all elements and their compound except hydrocarbons is:
(a) Industrial Chemistry
(c) Inorganic Chemistry ✓
(b) Physical Chemistry
(d) Organic Chemistry

47. It is the branch of chemistry that deals with the compounds of living organisms.
(a) Organic chemistry
(b) Inorganic chemistry
(c) Physical chemistry
(d) Biochemistry ✓

48. This branch of chemistry helps us to understand how living things obtain energy from food.
(a) Inorganic chemistry
(b) Biochemistry ✓
(c) Organic chemistry
(d) Medicinal chemistry

49. It is used in chromatography, electrophoresis, and spectroscopy.
(a) Analytical Chemistry ✓
(b) Quantum Chemistry
(c) Industrial Chemistry
(d) Biochemistry

50. The branch of Chemistry that deals with synthetic organic chemistry, pharmacology, and various biological specialities.
(a) Nuclear chemistry
(c) Analytical chemistry
(b) Biochemistry
(d) Medicinal chemistry ✓

51. The branch of Chemistry that deals with the application, mechanics, and experiments of physical models in a chemical system.
(a) Physical chemistry
(b) Inorganic chemistry
(c) Quantum chemistry ✓
(d) Green chemistry

52. The main purpose of this branch is to use waste material efficiently and improvement of energy efficiency in the chemical industry.
(a) Analytical chemistry
(b) Environmental chemistry
(c) Biochemistry
(d) Green chemistry ✓

53. It is considered the fourth state of matter.
(a) energy
(b) plasma ✓
(c) wave
(d) quanta

54. The different states of matter are due to the:
(a) difference of specific gravity
(b) difference of mass
(c) difference of chemical properties
(d) difference of energy ✓

55. Matter is made up of the smallest particle which is known as:
(a) atom ✓
(b) molecule
(c) radical
(d) ion

56. They are the basic units of matter and define structure of elements.
(a) atom ✓
(b) molecule
(c) radical
(d) ion

57. The smallest particle in a chemical element or compound that has the chemical properties of that element or compound is called:
(a) atom
(b) molecule ✓
(c) radical
(d) ion

58. He, Ar and Kr are the examples of:
(a) monoatomic elements ✓
(b) diatomic molecules
(c) polyatomic molecules
(d) heteroatomic molecules

59. O₂, Cl₂ and N₂ are the examples of:
(a) monoatomic elements
(b) diatomic molecules ✓
(c) polyatomic molecules
(d) heteroatomic molecules

60. Examples of polyatomic molecules are:
(a) Br₂ & O₃
(b) I₂ & P₄
(c) Xe & S₈
(d) P₄ & S₈ ✓

61. It is a substance made up of same type of atoms:
(a) Molecule
(b) Compound
(c) Element ✓
(d) Radical

62. Number of elements has been discovered so far is:
(a) 105
(b) 108
(c) 118 ✓
(d) 120

63. It is an abbreviation to represent the name of elements.
(a) Symbol ✓
(b) Formula
(c) Equation
(d) Expression

64. Na is the symbol of:
(a) Nitrogen
(b) Neon
(c) Nickel
(d) Sodium ✓

65. The valency depends upon the number of:
(a) protons in the nucleus
(b) neutrons in the nucleus
(c) electrons in the outermost shell ✓
(d) None of these

66. Valency of oxygen is:
(a) 0
(b) -1
(c) +2
(d) -2 ✓

67. Chemical formula of sugar is:
(a) CaO
(b) C₁₂H₂₂O₁₁ ✓
(c) CaCO₃
(d) Na₂CO₃.10H₂O

68. Chemical formula of sodium carbonate (washing soda) is:
(a) CaO
(b) C₁₂H₂₂O₁₁
(c) CaCO₃
(d) Na₂CO₃.10H₂O ✓

69. When two or more than two elements or compounds physically combined without any fixed ratio is known as:
(a) mixture ✓
(b) compound
(c) element
(d) mole

70. Salt water, air and blood are some examples of:
(a) heterogeneous mixture
(b) homogeneous mixture ✓
(c) compound
(d) mole

71. 1 a.m.u. = :
(a) 1.66 x 10^-14 gram
(b) 1.66 x 10^-20 gram
(c) 1.66 10^-24 gram ✓
(d) 1.66 x 10^-27 gram

72. The formula showing minimum relative numbers of each type of atoms in a molecule is called:
(a) Molecular formula
(b) Chemical formula ✓
(c) Empirical formula

(d) Formula mass

73. Empirical formula of glucose (C₆H₁₂O₆) is:
(a) CHO
(b) CH₂O
(c) C₂HO₂ ✓
(d) C₂H₃O₂

74. Molecular Formula = :
(a) Empirical Formula
(b) n(Empirical Formula)
(c) (Empirical Formula)ⁿ
(d) (Empirical Formula)_n ✓

75. The atomic mass is the sum of the number of:
(a) protons and neutrons ✓
(b) protons and electrons
(c) electrons and neutrons
(d) protons, neutrons and electrons

76. The number of atoms, molecules, or ions presents in one mole is: OR
Avogadro's number is:
(a) 6.02 10²³ ✓
(b) 6.02 x 10²⁷
(c) 6.02 10^-23
(d) 6.02 x 10^-27

77. Greek Scientist proposed idea of a substance as a combination of matter and form.
(a) Aristotle ✓
(b) Plato
(c) Democritus
(d) Cavendish

78. Greek Scientist describes theory of the Four Elements, fire, water, earth, air.
(a) Aristotle ✓
(b) Plato
(c) Democritus
(d) Cavendish

79. Greek Scientist proposed term ‘elements’ as composition of organic and inorganic bodies with particular shape:
(a) Aristotle
(b) Plato ✓
(c) Democritus
(d) Cavendish

80. Greek Scientist proposed the idea of atom, an indivisible particle of matter:
(a) Aristotle
(b) Plato
(c) Democritus ✓
(d) Cavendish

81. German scientist Scheele discovered:
(a) oxygen
(b) hydrogen
(c) chlorine ✓
(d) carbon

82. Cavendish discovered:
(a) oxygen
(b) hydrogen ✓
(c) chlorine
(d) carbon

83. Several chemical and physical properties of air and other gases was discovered by:
(a) Robert Boyle
(b) John Dalton
(c) Gay-Lussac ✓
(d) Rutherford

84. Jacques Charles described the:
(a) Gaseous law ✓
(b) Avogadro’s law
(c) Atomic theory of matter
(d) Quantum theory

85. Periodic arrangement of elements was discovered by:
(a) John Dalton
(b) Rutherford
(c) Mendeleev ✓
(d) J.J.Thomson

86. ________ use to kill the pathogenic organism to obtain pure water.
(a) Chlorine ✓
(b) Hydrogen
(c) Oxygen
(d) Bromine

87. The symbols of ___ elements in English derived from Latin, Greek and german
(a) 20
(b) 30 ✓
(c) 40
(d) 50

Fill In The blanks

1. Word science comes from latin word “Scientia” which means “ knowledge".
2. Chemistry purely deals with the matter which have mass and occupy space.
3. Robert Boyle (1627-1691 A.D) an English scientist put forward idea of chemistry as systematic investigation of nature.
4. J. Black (1728 1799 A.D), a Scottish scientist made study of carbon dioxide.
5. J.Priestley Discovered oxygen, sulphur dioxide and hydrogen chloride.
6. Avogadro Proposed Avogadro’s law that equal volumes of gases under constant temperature and pressure contain equal number of molecules.
7. French scientist Petit determined the classical expression for the molar specific [heat capacity] of certain chemical elements.
8. J.J.Berzelius Introduced symbols, formula and chemical equation to make study more systematic.
9. A piece of matter in pure form is termed as a substance.
10. Every substance has a fixed composition and specific properties.
11. Every substance has physical and chemical properties.
12. An Element is a substance made up of same type of atoms having same atomic number.
13. Element cannot be decomposes into simple substances by ordinary chemical reaction.
14. Elements occur in nature in free or combined form in solid, Liquid and gases states.
15. Now 118 elements have been discovered.
16. Symbol formula is an abbreviation to represent the name of element.
17. A symbol is taken from the name of that element in English, Latin and Greek.
18. When two or more than two elements or compounds physically combined without any fixed ratio is known as Mixture.
19. In mixture, the component substances retain their chemical properties.
20. Mixtures can be separated again by physical methods, as Filtration, Evaporation, Distillation and crystallization.
21. The Atomic Number is number of protons present in the nucleus of atom of any Element. It represented by symbol Z .
22. All atoms of an element have same atomic number due to the presence of same number of proton.
23. The Atomic Mass is sum of number of protons and neutrons present in the nucleus of atom of any element. It represented by symbol A
24. Atomic mass is calculated by A = Z + n where n is number of neutrons.
25. The atomic mass of an element expressed in gram is called gram atomic mass.
26. The molecular mass of an element or a compound expressed in gram is called gram molecular mass.
27. The formula mass of an ionic compound expressed in grams is called gram formula mass.
28. The atomic mass, molecular mass and formula mass of a substance expressed in grams is known as mole.
29. Avogadro an Italian scientist, calculated the number of atoms, molecules or ions present in one mole.
30. The value of Avogadro's number is found to be 6.02 x 10²³. This value is represented by N_A.
31. Calcium sulphate (CaSO₄) is commonly known as Plaster of Paris.
32. Sucrose is commonly known as pure sugar.
33. Sodium chloride (NaCl) is commonly known as table salt.

Name Of Elements in English, Derived Names From (Latin, Greek and German) And Symbols

S.NO.	English Names	Derived Names	Symbols
1.	Hydrogen	Greek (root genes)	H
2.	Helium	Greek (Helios)	He
3.	Lithium	Greek (Lithos)	Li
4.	Beryllium	Greek (Beryllos)	Be
5.	Boron	Latin (Borium)  Arabic (Buroq)	B
6.	Carbon	Latin (Carbone)	C
7.	Nitrogen	Greek (Nitrumgenes)	N
8.	Oxygen	Greek (Oxygeinomes)	O
9.	Florine	Latin (Flour)	F
10.	Neon	Greek (Neos)	Ne
11.	Sodium	Latin (Natrium)	Na
12.	Magnesium	Greek (Magnesium)	Mg
13.	Aluminium	Latin (Alumen)	Al
14.	Silicon	Latin (Silen)	Si
15.	Phosphorus	Greek (Phoros)	P
16.	Sulphur	Latin (Sulphur)	S
17.	Chlorine	Greek (Chloros)	Cl
18.	Argon	Greek (Argon)	Ar
19.	Potassium	Latin (Potash)	K
20.	Calcium	Greek (Calix)	Ca
21.	Scandium	Latin (Scandia)	Sc
22.	Titanium	Greek (Titan)	Ti
23.	Vanadium	Greek (Vanadis)	V
24.	Chromium	Greek (Chroma)	Cr
25.	Manganese	Greek (Magnesia)	Mn
26.	Iron	Latin (Ferrum)	Fe
27.	Cobalt	German (Kobold)	Co
28.	Nickle	German (Kupanickel)	Ni
29.	Copper	Latin (Cuprum)	Cu
30.	Zinc	German (Zink)	Zn

Name Of Elements with their Symbols, Atomic Numbers and valency

S.NO.	Elements with symbols	Atomic Numbers	Valency
1.	Hydrogen (H)	1	-1 +1
2.	Helium (He)	2	0
3.	Lithium (Li)	3	+1
4.	Beryllium (Be)	4	+2
5.	Boron (B)	5	+3
6.	Carbon (C)	6	+4 +2
7.	Nitrogen (N)	7	+3
8.	Oxygen (O)	8	-2
9.	Florine (F)	9	-1
10.	Neon (Ne)	10	0
11.	Sodium (Na)	11	+1
12.	Magnesium (Mg)	12	+2
13.	Aluminium (Al)	13	+3
14.	Silicon (Si)	14	+4
15.	Phosphorus (P)	15	+3
16.	Sulphur (S)	16	+2
17.	Chlorine (Cl)	17	+1
18.	Argon (Ar)	18	0
19.	Potassium (K)	19	+1
20.	Calcium (Ca)	20	+2
21.	Scandium (Sc)	21	+3
22.	Titanium (Ti)	22	+2 +3
23.	Vanadium (V)	23	+2 +3 +4
24.	Chromium (Cr)	24	+3
25.	Manganese (Mn)	25	+2 +3 +6
26.	Iron (Fe)	26	+2 +3
27.	Cobalt (Co)	27	+2 +3 +4
28.	Nickel (Ni)	28	+1 +2
29.	Copper (Cu)	29	+1 +2 +3
30.	Zinc (Zn)	30	+2
31.	Lead (Pb)	82	+2 +4

Compounds with their Formulas

S.No.	Compound	Molecular Formula / Chemical Formula
-	Acetic Acid	CH3COOH
.	Ammonia	NH3
-	Benzene	C6H6
.	Calcium carbonate (limestone)	CaCO3
.	Calcium oxide	CaO
.	Carbon dioxide	CO2
.	Ethyl alcohol	C2H5OH
.	Glucose	C6H12O6
.	Hydrochloric acid /  Hydrogen chloride	HCl
.	Hydrogen peroxide	H2O2
.	Nitric acid	HNO3
.	Silicon dioxide (sand)	SiO2
.	Sodium carbonate (washing soda)	Na2CO3.10H2O
.	Sodium chloride (common salt)	NaCl
.	Sodium hydroxide (caustic soda)	NaOH
.	Sugar	C12H22O11
.	Sulphuric acid	H2SO4
.	Sulphur dioxide	SO2
.	Water	H2O

Chemistry For Class IX (New Book ) - Chapter No. 2- Atomic Structure - Multiple Choice Questions And Fill In The Blanks

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Chapter No.2 - Atomic Structure
MCQs And Fill In The Blanks
Text Book Exercise

SECTION- A: MULTIPLE CHOICE QUESTIONS
Tick Mark (✓) the correct answer

1. In an atom number of protons and neutrons are added to obtain:
(a) number of electrons
(b) number of nucleons ✓
(c) atomic number of element
(d) number of isotopes

2. If proton number is 19, electron configuration will be:
(a) 2, 8, 9
(b) 2, 8, 8, 1 ✓
(c) 2, 8, 1
(d) 2, 8, 3

3. If nucleon number of potassium is 39, number of neutrons will be:
(a) 39
(b) 19
(c) 20 ✓
(d) 29

4. The isotope C-12 is present in abundance of:
(a) 96.9%
(b) 97.6%
(c) 98.8% ✓
(d) 99.7%

5. Electronic configuration is distribution of:
(a) proton
(b) neutron
(c) electron ✓
(d) positron

6. Which one of the following is most penetrating?
(a) electron
(b) Proton
(c) alpha particle
(d) neutron ✓

7. How many sub-shells in a L shell:
(a) one
(b) two ✓
(c) three
(d) four

8. De Brog extend the wave particle duality to electron in:
(a) 1920
(b) 1922
(c) 1923 ✓
(d) 1925

9. Name the material of screen which used in Rutherford atomic model:
(a) Aluminum foil
(b) Zinc sulphide ✓
(c) Sodium sulphide
(d) Aluminum sulphide

10. Which rays are used for sterilization of medical instruments:
(a) α-rays
(b) β-rays
(c) γ-rays ✓
(d) x-rays

11. The word atom is derived from a Greek word ATOMOS means:
(a) unbreakable ✓
(b) indivisible
(c) inconsequential
(d) insignificant

12. The word atom is derived from a word ATOMOS, which was first described by Greek philosopher:
(a) Socrates
(b) Aristotle
(c) Plato
(d) Democritus ✓

13. Democritus belief that all matter consists of very small indivisible particles which are known as:
(a) atoms ✓
(b) molecules
(c) ions
(d) electrons

14. This English chemist suggested the fundamental atomic theory.
(a) J.J. Thomson
(b) John Dalton ✓
(c) William Crooks
(d) M. Faraday

15. The first subatomic particle, electron, was discovered by:
(a) M. Faraday & Chadwick
(b). J. J. Thomson & Rutherford
(c) M. Faraday, J.J. Thomson & Chadwick
(d) M. Faraday, William Crooks & J.J. Thomson ✓

16. Goldstein and Ernest Rutherford identified the subatomic particle:
(a) electron
(b) proton ✓
(c) neutron
(d) nucleus

17. The third subatomic particle, neutron, was revealed by:
(a) J.J. Thomson
(b) William Crooks
(c) Chadwick ✓
(d) Rutherford

18. Which particle is the lightest in the following?
(a) Electron ✓
(b) Proton
(c) Neutron
(d) 𝛼-particles

19. It was discovered in discharge tube experiment.
(a) 𝛼-particles
(b) Neutron
(c) Proton
(d) Electron ✓

20. Cathode rays consist of fast moving:
(a) atoms
(b) electrons ✓
(c) protons
(d) neutrons

21. In discharge tube, cathode rays travel in straight line from:
(a) cathode towards anode ✓
(b) anode towards cathode
(c) cathode to all directions
(d) anode to all directions

22. Which one of the following has a negative charge?
(a) Neutrons
(b) Protons
(c) Electrons ✓
(d) Nucleus

23. The charge and mass ratio (e/m) of cathode particles (or electrons) is:
(a) 1.7588 x 10⁸ coulomb per gram ✓
(b) 6.63 x 10^-34 JS
(c) 9.11 x 10^-26 coulomb per gram
(d) 1.67 x 10^-25 JS

24. Cathode rays (or electrons) can produce mechanical pressure indicating they possess:
(a) mass
(b) charge
(c) potential energy
(d) kinetic energy ✓

25. Which one of the following particles has positive charge?
(a) Neutrons
(b) Protons ✓
(c) Electrons
(d) Nucleus 

26. Goldstein justify that atoms are electrically:
(a) positive
(b) negative
(c) neutral ✓
(d) None of these

27. In discharge tube, canal rays (or protons) travel in straight line from:
(a) cathode towards anode
(b) anode towards cathode ✓
(c) cathode to all directions
(d) anode to all directions

28. The charge and mass ratio (e/m) of protons is:
(a) is much smaller than an electron bob ✓
(b) is much greater than electron
(c) is equal to the e/m ratio of electron
(d) None of these

29. The mass of a proton is 1836 times more than the mass of:
(a) atom
(b) neutron
(c) 𝛼-particle
(d) electron ✓

30. In 1932, he become successful to discover Neutron.
(a) Goldstein
(b) J.J. Thomson
(c) Rutherford
(d) Chadwick ✓

31. The neutrons have:
(a) negative charge
(b) positive charge
(c) no charge ✓
(d) None of them

32. The mass of a neutron is almost equal to that of:
(a) protrons ✓
(b) electron
(c) nucleus
(d) All of them

33. These particles are most penetrating in matter.
(a) proton
(b) neutrons ✓
(c) electrons
(d) atoms

34. All atoms can be identified by their:
(a) number of protons they contain ✓
(b) number of neutrons they contain
(c) number of electrons they contain
(d) atomic shells

35. The number of protons in the nucleus of an atom is called:
(a) atomic mass
(b) atomic weight
(c) atomic charge
(d) atomic number ✓

36. Atomic number represented by:
(a) N
(b) NA
(c) Z ✓
(d) None of these

37. The elements are identify by their:
(a) atomic weight
(b) atomic number ✓
(c) atomic mass
(d) valency

38. Different elements have different atomic numbers because of different number of:
(a) protons ✓
(b) electrons
(c) neutrons
(d) shells

39. Atomic number of Carbon (C) is 6. Each carbon atom has:
(a) 3 protons & 3 neutrons
(b) 3 protons & 3 electrons
(c) 6 protons & 6 neutrons
(d) 6 protons & 6 electrons ✓

40. The total sum of proton and neutrons in the nucleus of an atom is called:
(a) atomic weight
(b) atomic number
(c) mass number ✓
(d) valency

41. Mass number represented by:
(a) N
(b) NA
(c) Z
(d) A ✓

42. The sodium (Na) atom has Z = 11 and mass number A= 23. It has:
(a) 11 protons and 12 neutrons ✓
(b) 11 protons and 23 neutrons
(c) 23 protons and 11 neutrons
(d) 12 protons and 11 neutrons

43. Uranium, Radium and Polonium are:
(a) metals
(b) non-metals
(c) radioactive elements ✓
(d) gases

44. An atom consist of a positively charged, dense and very small nucleus containing protons and neutron. The entire mass is concentrated in the nucleus of an atom. It is a postulate of:
(a) Rutherford Atomic Model ✓
(b) Bohr's Atomic Model
(c) Modern Atomic Model
(d) None of them

45. The electrons are revolving around the nucleus in circular paths. These circular paths are known as:
(a) orbits
(b) shells
(c) Both 'a' & 'b' ✓
(d) None of them

46. The energy levels are represented by an integer (n = 1, 2, 3....) known as:
(a) Avogadro's number
(b) atomic number
(c) mass number
(d) quantum number ✓

47. The emission or absorption is discontinuous in the form of an energy packet called:
(a) quantum
(b) photon
(c) Both 'a' & 'b' ✓
(d) None of these

48. In 1900, quantum theory was presented by:
(a) Neil Bohr
(b) Max Planck ✓
(c) Louis De Broglie
(d) Schrodinger

49. He proposed a relationship between mass and energy to explain the photoelectric effect by wave-particle duality as E = mc².
(a) Louis De Broglie
(b) Albert Einstein ✓
(c) Schrodinger
(d) Max Planck

50. He proposed a hypothesis that all matter has particle as well as wave nature at the submicroscopic level.
(a) Louis De Broglie ✓
(b) Albert Einstein
(c) Schrodinger
(d) Max Planck

51. M shell has:
(a) 1 subshell
(b) 2 subshells
(c) 3 subshells ✓
(d) 4 subshells

52. The maximum number of electrons that can be accommodated in a shell is represented by the formula:
(a) 2n
(b) 2n² ✓
(c) 2n³
(d) 2n⁴

53. The electronic configuration of oxygen is:
(a) 1s² 2s² 2p¹
(b) 1s² 2s² 2p²
(c) 1s² 2s² 2p³
(d) 1s² 2s² 2p⁴ ✓

54. Electronic configuration of sodium is:
(a) 1s² 2s² 2p⁶ 3s² 3p²
(b) 1s² 2s² 2p⁶ 3s² 3p¹  ✓
(c) 1s² 2s² 2p² 3s²
(d) 1s² 2s² 2p⁶ 3s¹

55. Isotopes are atoms of the same element having the:
(a) same atomic number but the different mass number ✓
(b) same atomic number and mass number
(c) same mass number but different atomic number
(d) Both 'a' & 'b'

56. Isotopes have the:
(a) same number of neutrons but different number of electrons
(b) same number of neutrons but different number of protons
(c) same number of protons but the different number of neutrons ✓
(d) Both 'a' & 'b"

57. Isotopes have the:
(a) same physical properties but different chemical properties
(b) same chemical properties but different physical properties ✓
(c) same chemical and physical properties
(d) None of them

58. Hydrogen has:
(a) two isotopes
(b) three isotopes ✓
(c) four isotopes
(d) No isotopes

59. Carbon 13 possess:
(a) 6 protons and 7 neutrons ✓
(b) 6 protons and 6 neutrons
(c) 7 protons and 7 neutrons
(d) 7 protons and 7 electrons

60. Chlorine has:
(a) two isotopes ✓
(b) three isotopes
(c) four isotopes
(d) No isotopes

61. Number of protons + Number of neutrons of an element is:
(a) atomic number
(b) formula number
(c) mass number ✓
(d) isotopes


62. A-Z indicates the number of:
(a) electrons
(b) protons
(c) neutrons ✓
(d) 𝛼-particles

Fill In The Blanks:

1. The Electron is lightest particle carrying a negative charge in an Atom discovered by J.J.Thomson and William Crooks.
2. The Proton is positively charge particle discovered by Goldstein in 1886.
3. J.J.Thomson investigate properties of proton in 1897.
4. In 1932 Chadwick become successful to discover Neutron.
5. Lord Rutherford in 1911, carried out series of experiments and proposed a new model for the atom
6. Lord Rutherford in 1911, discovered that an atom contains nucleus at the center and electrons revolve around this nucleus.
7. In 1913 Neil Bohr proposed another atomic model to remove or replaced the Rutherford atomic model.
8. In 1913 Neil Bohr explained the line spectrum of Hydrogen atom based on quantum theory of Max Planck.
9. In 1923 Lois De Broglie extend the wave particle duality to electron.
10. In 1923 Lois De Broglie proposed a hypothesis that all matter has particle as well as wave nature at the sub microscopic level.
11. The Energy levels or Shell or Orbital are all possible paths on which electrons are revolving around nucleus.
12. The Energy levels or Shell or Orbital are shows by 'n'.
13. The Energy levels or Shell or Orbital are named as K, L, M, N, O, P.
14. Main energy level are divided in to sub energy levels and known as sub shells.
15. The distribution of electrons among the different orbits/shells and sub shells is known as the electronic configuration of an atom.
16. Atoms of the same elements having same atomic number but different atomic masses are called isotopes.
17. Isotopes have same number of electron and same number of protons, but different number of neutrons.
18. The Isotopes are used in research laboratories, medical centers, industrial facilities, food irradiation plants and many consumer products.

Chemistry For Class IX (New Book ) - Chapter No. 3 - Periodic Table And Periodicity Of Properties - Multiple Choice Questions And Fill In The Blanks

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Chapter No.3 - Periodic Table And Periodicity Of Properties
MCQs And Fill In The Blanks
Text Book Exercise

SECTION- A: MULTIPLE CHOICE QUESTIONS
Tick Mark (✓) the correct answer

1. In 1869 Mendeleev put forward his periodic law about:
(a) Atomic Number
(b) Chemical properties
(c) Physical properties
(d) Atomic Mass  ✓

2. The periodic table divided into S, P, d, and f block based on.
(a) Atomic Radius
(b). Electronic Configuration ✓
(c) Ionization Energy
(d). Electron Affinity

3. 4^th and 5^th period in periodic table are known as:
(a) Short period
(b) Long period ✓
(c) Normal period
(d) Very long period

4. Which one of the following decreases along the period?
(a) Ionization Energy
(b) Atomic Radius ✓
(c) Electronegativity
(d) Electron Affinity

5. The elements of VIIA group are known as:
(a) Lanthanides
(b) Actinides
(c) Halogens ✓
(d) Noble Gases

6. According to Moseley the chemical properties of elements are the periodic function of their:
(a) Atomic Size
(b) Atomic Mass
(c) Atomic Radius
(d) Atomic Number ✓

7. The shielding effect across the period:
(a) Increases
(b) Decrease
(c) Moderate
(d) Same ✓

8. The ability to attract shared pair of electron is called:
(a) Electron Affinity
(b) Electronegativity ✓
(c) Ionization Energy
(d) Shielding Effect

9. In group electron affinity values decreases from top to bottom because:
(a) Atomic size normal
(b) Atomic size increases ✓
(c) Atomic size decreases
(d) Atomic size same

10. All Transition Elements are:
(a) Gases
(b) Metals ✓
(c) Nonmetals
(d) Metalloids

11. He proposed the classification of Triads in which several groups of three elements classified based on atomic masses.
(a) Dobereiner ✓
(b) Newland
(c) Mendeleev
(d) Moseley

12. In the classification of Triads central element had an atomic mass average of the other:
(a) five elements
(b) four elements
(c) three elements
(d) two elements ✓

13. In 1864 British chemist Newland put forward the:
(a) classification of Triads
(b) Law of Octaves ✓
(c) 8 columns and rows arrangement
(d) 9 columns and groups arrangement

14. It is order of increasing atomic masses.
(a) classification of Triads
(b) Law of Octaves ✓
(c) 8 columns and rows arrangement
(d) 9 columns and groups arrangement

15. According to him the eighth element has similar properties as the first element in a group of eight elements.
(a) Dobereiner
(b) Moseley
(c) Newland ✓
(d) Mendeleev

16. In 1869, he published eight vertical columns (groups) and horizontal rows (periods) on the basis of physical and chemical properties of elements.
(a) Dobereiner
(b) Newland
(c) Mendeleev ✓
(d) Moseley

17. In 1869, this German scientist published a periodic table in which 56 elements were arranged in 9 vertical columns or groups based on atomic masses.
(a) Lother Meyer ✓
(b) Mendeleev
(c) Newland
(d) Moseley

18. His periodic table was the first attempt to arrange the elements.
(a) Dobereiner
(b) Moseley
(c) Newland
(d) Mendeleev ✓

19. Based on periodic Law a periodic table developed in which vertical columns are called:
(a) periods
(b) groups ✓
(c) triads
(d) classes

20. In periodic table, horizontal lines are called:
(a) periods ✓
(b) groups
(c) triads
(d) classes

21. In 1869, he proposed a periodic law based on physical and chemical properties empirically.
(a) Dobereiner
(b) Newland
(c) Mendeleev ✓
(d) Moseley

22. Mendeleev's Periodic law states that "The properties of the elements are a periodic function of their:
(a) atomic number
(b) atomic radius
(c) atomic charge
(d) atomic weight ✓

23. It is a fundamental property because it increases regularly from element to element and is fixed for every element.
(a) atomic number ✓
(b) atomic radius
(c) atomic charge
(d) atomic weight

24. In the periodic table, the atomic number increases from:
(a) right to left
(b) left to right ✓
(c) top to bottom
(d) bottom to top

25. In 1913, he discovered that Atomic number is the basic property of an atom.
(a) Dobereiner
(b) Moseley ✓
(c) Newland
(d) Mendeleev

26. He proposed a modern periodic law.
(a) Dobereiner
(b) Newland
(c) Mendeleev
(d) Moseley ✓

27. The long form of periodic table composed with:
(a) 9 rows & 8 columns
(b) 8 rows & 9 columns
(c) 7 rows and 8 columns ✓
(d) 8 rows and 7 columns

28. There are seven horizontal lines in periodic table known as:
(a) periods ✓
(b) groups
(c) triads
(d) classes

29. The first period is the shortest period which contains only:
(a) one elements
(b) two elements ✓
(c) three elements
(d) four elements

30. The second and the third periods contain:
(a) 2 elements
(b) 8 elements ✓
(c) 14 elements
(d) 32 elements

31. These periods contain 18 elements.
(a) The 6^th & 7^th
(b) The 5^th & 6^th
(c) The 4^th and 5^th ✓
(d) The 2^nd & 3^rd

32. The 6th period contains:
(a) 2 elements
(b) 8 elements
(c) 14 elements
(d) 32 elements ✓

33. The 14 elements in the bottom of the 6th period are named as:
(a) Lanthanides ✓
(b) Actinides
(c) Alkali metals
(d) Transition elements

34. It is the longest period of the periodic table.
(a) 4^th
(b) 5^th
(c) 6^th ✓
(d) 7^th

35. This period is consider as an incomplete.
(a) 4^th
(b) 5^th
(c) 6^th
(d) 7^th ✓

36. The 7^th period contains a group of 14 elements known as:
(a) Lanthanides
(b) Actinides ✓
(c) Alkali metals
(d) Transition elements

37. All the periods except the first period start with a / an:
(a) alkali metal ✓
(b) transition element
(c) noble gas
(d) Actinide

38. All the periods except the first-period end at a / an:
(a) alkali metal
(b) transition element
(c) noble gas ✓
(d) Actinide

39. There are eight vertical columns in periodic table known as:
(a) periods
(b) groups ✓
(c) triads
(d) classes

40. In periodic table, the sub groups are divided on the basis of their:
(a) atomic masses
(b) atomic numbers
(c) similar properties ✓
(d) None of these

41. The elements of subgroup B are called:
(a) Lanthanides
(b) Actinides
(c) Alkali metals
(d) Transition elements ✓

42. The group number indicates total number of electrons in:
(a) an atom of the element
(b) valence shell of the element ✓
(c) a nucleus of the element
(d) the first shell of the element

43. The elements of group I A are called:
(a) alkali metals ✓
(b) alkaline earth metals
(c) noble gases
(d) transition elements

44. Their valence shell contains one electron.
(a) Group I A ✓
(b) Group II A
(c) Group III A
(d) Group IV A

45. The elements of group II A are called:
(a) alkali metals
(b) alkaline earth metals ✓
(c) noble gases
(d) transition elements

46. Their valence shell contains two electrons.
(a) Group IA
(b) Group II A ✓
(c) Group III A
(d) Group IV A

47. This is also called the carbon family.
(a) Group I A
(b) Group II A
(c) Group III A
(d) Group IV A ✓

48. In their valence shell, the oxygen family has:
(a) 6 electrons ✓
(b) 5 electrons
(c) 4 electrons
(d) 3 electrons

49. All of the elements of this group exist in allotropic forms.
(a) IVA
(b) VA
(c) VIA ✓
(d) VII A

50. The group or inert or noble gases are:
(a) VIII B
(b) VIII A ✓
(c) VII A
(d) VII B

51. These are the groups of transition metals.
(a) IB to VIII B ✓
(b) IA to VIII A
(c) III B to VII B
(d) III A to VII A

52. The periodic table has been divided into:
(a) six blocks
(b) five blocks
(c) four blocks ✓
(d) three blocks

53. They are colorless, unreactive and diamagnetic gases.
(a) Transition elements
(b) Noble gases ✓
(c) Lanthanides
(d) Actinides

54. They are placed in zero group.
(a) alkali metals
(b) alkaline earth metals
(c) transition elements
(d) noble gases ✓

55. The elements of group IA and IIA are:
(a) s block elements ✓
(b) p block elements
(c) d block elements
(d) f block elements

56. Elements of this group / these groups are p block elements.
(a) IIIA to VII
(b) zero group
(c) Both 'a' & 'b' ✓
(d) None of these

57. d-block elements are also called:
(a) transition elements
(b) outer transition elements ✓
(c) inner transition elements
(d) noble gases

58. d-block elements consist of:
(a) six series
(b) five series
(c) four series
(d) three series ✓

59. f-block elements are also called:
(a) transition elements
(b) outer transition elements
(c) inner transition elements ✓
(d) noble gases

60. They exhibit electronic configuration ns² (n²)d1¹, (n-¹)f^1-14.
(a) f-block elements ✓
(b) d-block elements
(c) p-block elements
(d) s-block elements

61. f-block elements consist of:
(a) five series
(b) four series
(c) three series
(d) two series ✓

62. Half of this distance is considered to be the radius of the atom. It is measured in:
(a) centimeters (cm)
(b) Angstrom unit (A) ✓
(c) decimeters (dcm)
(d) None of these

63. 1A =:
(a) 10^-3 cm
(b) 10^-2 cm
(c) 10^-8 cm ✓
(d) 10^-11 cm

64. In the periodic table, that atomic radius increases from:
(a) left to right
(b) right to left
(c) top to bottom ✓
(d) bottom to top

65. As the atomic number increases from left to right, the atomic radius:
(a) decreases ✓
(b) increases
(c) remains the same
(d) does not follow any rule

66. The ionization energy is the amount of energy required to:
(a) add an electron in the outermost shell of a gaseous atom
(b) remove an electron from a gaseous state ✓
(c) to reduce the shielding effect
(d) All of these

67. The ionization energy is measured in:
(a) joule/kg
(b) joule/gram
(c) mole/kg
(d) joule/mole ✓

68. The ionization energy depends upon:
(a) atomic size
(b) nuclear charge
(c) Both 'a' & 'b' ✓
(d) None of these

69. The higher ionization energy means:
(a) removal of an electron is more difficult ✓
(b) removal of an electron is easier
(c) adding of an electron is more difficult
(d) adding of an electron is easier

70. If we move from left to right in periods the value of ionization energy:
(a) decreases
(b) increases ✓
(c) remains the same
(d) does not follow any rule

71. As we move down the group ionization energy decreases from:
(a) left to right
(b) right to left
(c) top to bottom ✓
(d) bottom to top

72. The electron affinity is the amount of energy released when:
(a) an electron is removed from the outermost shell of a gaseous atom
(b) an electron is added to the outermost shell of a gaseous atom ✓
(c) shielding effect is reduced
(d) shielding effect is increased

73. Electron affinity means tendency to accept electron to form:
(a) molecule
(b) radical
(c) cation
(d) anion ✓

74. In a period electron affinity increases from:
(a) left to right ✓
(b) right to left
(c) top to bottom
(d) bottom to top

75. In a group electron affinity values decrease from:
(a) left to right
(b) right to left
(c) top to bottom ✓
(d) bottom to top

76. As the size of iodine is bigger than bromine its electron affinity is:
(a) more than bromine
(b) less than bromine ✓
(c) equal to bromine
(d) zero

77. The ability of an atom to attract the shared pair of electrons towards itself in a molecule is called:
(a) ionization potential
(b) electron affinity
(c) shielding effect
(d) electronegativity ✓

78. In period, electronegativity increases from:
(a) left to right ✓
(b) right to left
(c) top to bottom
(d) bottom to top

79. Lanthanides and Actinides are the elements of block:
(a) s
(b) p
(c) d
(d) f ✓

80. The repetition of properties after regular intervals is called:
(a) grouping
(b) perioding
(c) periodicity ✓
(d) None of them

81. The elements of sub group A are called:
(a) transition elements
(b) representative elements ✓
(c) lanthanides
(d) actinides

82. In periodic table, the shielding effect increases:
(a) down the group ✓
(b) down the period
(c) left to the group
(d) down to the group

Chemistry For Class IX (New Book ) - Chapter No. 4 - Chemical Bonding - Multiple Choice Questions And Fill In The Blanks

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Chapter No.4 - Chemical Bonding
MCQs And Fill In The Blanks
Text Book Exercise

SECTION- A: MULTIPLE CHOICE QUESTIONS
Tick Mark (✓) the correct answer

1. An example of ionic compound is:
(a)H₂
(b)CH₄
(c) N₂
(d)NaCl ✓

2. Interaction between highly electron deficient hydrogen and highly electronegative atom is called:
(a) covalent bond
(b) ionic bond
(c) hydrogen bond ✓
(d) metallic bond

3. Two fluorine atoms share one electron each in their outermost shell to achieve electronic configuration of:
(a) Xe
(b) Ar
(c) Kr
(d) Ne ✓

4. Number of electrons lost by atoms of group IIIA equals:
(a) 1
(b) 2
(c) 3 ✓
(d) 4

5. Atom which loses two electrons from its outer shell to form ion is called:
(a) oxygen
(b) potassium
(c) magnesium ✓
(d) carbon

6. In NaCl crystal lattice each Na⁺ ion is surrounded by:
(a) 6 Cl^- ions ✓
(b) 6 Na⁺ ions
(c) 8 Cl^- ions
(d) 12 Cl^- ions

7. At room temperature most of ionic compounds are:
(a) amorphous solids
(b) crystalline solids ✓
(c) liquids
(d) gases

8. Tendency of atoms to acquire eight electrons in their valence shell is:
(a) octet rule ✓
(b) duplet rule
(c) triplet rule
(d) none of above

9. When one atom forms cation by losing electron and other forms anion by accepting that electron then bond form between them is:
(a) Covalent bond
(b) Ionic bond ✓
(c) coordinate covalent bond
(d) hydrogen bond

10. Noble gases are stable because they contain:
(a) 4 electrons in valence shell
(b) 6 electrons in valence shell
(c) 8 electrons in valence shell ✓
(d) 10 electrons in valence shell

11. Bond which involve 3 shared electron pairs is a:
(a) double covalent bond
(b) single covalent bond
(b) triple covalent bond ✓
(d) none of above

12. A non-metal atom form anion by:
(a) loses of electrons
(b) gain of electrons ✓
(c) loses of protons
(d) gain of protons

13. When two identical atoms share electron pairs and exert force on each other than bond form is:
(a) non-polar covalent bond ✓
(b) polar covalent bond
(c) double covalent bond
(d) coordinate covalent bond

14. Synthetic resins are used on places where:
(a) electric resistance is required
(b) water resistance is required ✓
(c) adhesion is required
(d) friction is required

15. Oxygen belongs to group VIA so number of electrons in its valence shell are:
(a) 3
(b) 4
(c) 5
(d) 6 ✓

16. Electron pairs which are not shared by atoms are called:
(a) electron pairs
(b) lone pairs ✓
(c) bond pairs
(d) shared pairs

17. Strength of intermolecular forces from ionic to covalent bond is:
(a) Weaker ✓
(b) stronger
(c) equal
(d) none of above

18. Ionic crystals have:
(a) high melting points✓
(b) moderate melting points
(c) low melting points
(d) none of above

19. Bond formed by mutual sharing of electron is:
(a) ionic bond
(b) coordinate covalent bond
(c) covalent bond ✓
(d) metallic bond

20. Which of the following diagram shows atoms are bonded with same electronegativity?
(a) A -----:----- B ✓
(b) A ----------: B
(c) A :---------- B
(d) A --:-------- B

21. The attractive force which binds atoms together is called:
(a) a chemical bond
(b) chemical forces
(c) Both 'a' & 'b' ✓
(d) None of above

22. Helium, neon, argon, xenon and krypton present in the atmosphere consist of:
(a) un-bounded atoms ✓
(b) bounded atoms
(c) ionic bonds
(d) covalent bonds

23. Electronic configuration of noble gases is:
(a) ns² np⁴
(b) ns² np⁵
(c) ns² np⁶ ✓
(d) ns² np⁸

24. Which one is not a noble gas?
(a) Helium
(b) Argon
(c) Radon
(d) Oxygen ✓

25. Noble gases are sometimes called the:
(a) slow gases
(b) inactive gases
(c) inert gases ✓
(d) idle gases

26. The outermost shell of the noble gases is:
(a) completely filled ✓
(b) half-filled
(c) partially filled
(d) None of these

27. All noble gases contain 8 electrons in the valence shell except:
(a) neon
(b) krypton
(c) xenon
(d) helium ✓

28. Because of these electronic configurations of noble gases are:
(a) stable and active
(b) stable and not active ✓
(c) unstable and active
(d) unstable and not active

29. Atoms to acquire two electrons in the valence shell is called:
(a) duplet rule ✓
(b) triplet rule
(c) octet rule
(d) divalent rule

30. In 1916 this chemist proposed the octet rule.
(a) John Dalton
(b) Chadwick
(c) G.N. Lewis ✓
(d) Goldstein

31. It plays an important role in determining the chemical properties of the atom, including its ability to form chemical bonds.
(a) number of protons
(b) number of neutrons
(c) electrons present in the innermost shell
(d) electrons present in the outermost shell ✓

32. These electrons in the outermost shell of an atom are called:
(a) valence electrons
(b) outer electrons
(c) Both 'a' & 'b' ✓
(d) None of them

33. Electronic configuration of an element is 1s², 2s² 2p¹, therefore the valence electrons this element has are:
(a) one
(b) two
(c) three ✓
(d) five

34. The valence electrons which are involved in chemical bonding are termed as:
(a) valence electrons
(b) bonding electrons ✓
(c) reactive electrons
(d) ionic electrons

35. The group number in the periodic table indicates the:
(a) number of valence electrons in an atom ✓
(b) total number of electrons in an atom
(c) number of protons in the nucleus
(d) number of neutrons in the nucleus

36. Sodium contains one electron in its valence shell so it belongs to:
(a) group I ✓
(b) group II
(c) group III
(d) zero group

37. Phosphorus belongs to group VA, so in the valence shell, it contains:
(a) one electron
(b) two electrons
(c) three electrons
(d) five electrons ✓

38. Chemical bonding is the combining of atoms to form:
(a) new elements
(b) new atoms
(c) new substances ✓
(d) All of these

39. An interaction that holds two atoms together is called a:
(a) chemical bond ✓
(b) ionic bond
(c) covalent bond
(d) coordinate bond

40. In the formation of an ionic bond, an atom loses electrons and changes into:
(a) negative ion
(b) positive ion ✓
(c) neutral atom
(d) None of these

41. The atom which gains electron changes into:
(a) negative ion ✓
(b) positive ion
(c) neutral atom
(d) None of these

42. The electrostatic force of attraction that holds the oppositely charged ions together is called:
(a) chemical bond
(b) ionic bond ✓
(c) covalent bond
(d) coordinate bond

43. Electrovalent bond is also known as:
(a) chemical bond
(b) ionic bond ✓
(c) covalent bond
(d) coordinate bond

44. Generally, an ionic bond is formed between the atoms of:
(a) two same metals
(b) two different metals
(c) two same groups
(d) two different groups ✓

45. Sodium chloride, potassium chloride, magnesium fluoride are:
(a) coordinate compounds
(b) covalent compounds
(c) ionic compounds ✓
(d) None of these

46. The electron arrangement of sodium atom is:
(a) 2, 8, 0
(b) 2, 8, 1 ✓
(c) 2, 8, 2
(d) 2, 8, 3

47. The electron arrangement of chlorine atom is:
(a) 2, 8, 1
(b) 2, 8, 3
(c) 2, 8, 5
(d) 2, 8, 7 ✓

48. The formula of magnesium oxide is:
(a) MgO ✓
(b) MgO₂
(c) MgO₃
(d) Mg₂O

49. The ionic bond between magnesium and oxygen is stronger than the ionic bond between sodium and chlorine because of the:
(a) larger size of the atoms
(b) larger size of cation
(c) greater charge density on the ions ✓
(d) None of these

50. A covalent bond between two atoms, is formed by the:
(a) electrostatic force between two ions
(b) mutual sharing of electrons ✓
(c) only one of the atoms contributes both electrons constituting the bond
(d) None of these

51. The bond in MgO is:
(a) electrovalent bond ✓
(b) covalent bond
(c) co-ordinate bond
(d) chemical bond

52. The electrons of atoms that pair up to form a chemical bond are called:
(a) pair electrons
(b) ionic pair electrons
(c) covalent pair electrons
(d) bond pair electrons ✓

53. The formations of H₂, HCl, CH₄ are few examples of this type of bonding.
(a) Electrovalent bond
(b) Single covalent bond ✓
(c) Double covalent bond
(d) Triple covalent bond

54. Oxygen (O₂) and ethene (C₂H₄) are examples of this type of bonding.
(a) Electrovalent bond
(b) Single covalent bond
(c) Double covalent bond ✓
(d) Triple covalent bond

55. It has 6 valence electrons in its outer shell.
(a) carbon
(b) chlorine
(c) sodium
(d) oxygen ✓

56. Nitrogen (N₂) and ethyne (C₂H₂) are examples of this type of bonding.
(a) Electrovalent bond
(b) Single covalent bond
(c) Double covalent bond
(d) Triple covalent bond ✓

57. In its outer shells, each nitrogen atom has:
(a) one electrons
(b) two electrons
(c) three electrons
(d) five electrons ✓

58. The covalent bond formed between identical atoms is called:
(a) non-polar covalent bond ✓
(b) polar covalent bond
(c) coordinate covalent bond
(d) dative covalent bond

59. The bond in a hydrogen molecule is:
(a) non-polar covalent bond ✓
(b) polar covalent bond
(c) coordinate covalent bond
(d) dative covalent bond

60. Non-polar covalent bonds are formed when the electronegativities of the two atoms are:
(a) unequal
(b) equal ✓
(c) zero
(d) larger

61. Bonds in HCl, H₂O, NH₃ are:
(a) non-polar covalent bond
(b) polar covalent bond ✓
(c) coordinate covalent bond
(d) dative covalent bond

62. When the difference between electronegative values of two bonded atoms is more than 1.7, the bond will be purely:
(a) polar covalent
(b) non-polar covalent
(c) ionic or electrovalent ✓
(d) covalent

63. When the difference between electronegative values of two bonded atoms is less than 1.7, the bond will be:
(a) polar covalent
(b) non-polar covalent
(c) ionic or electrovalent
(d) covalent ✓

64. The bond will be pure covalent or nonpolar if the electronegativity difference of bonded atoms is:
(a) zero ✓
(b) 1.7
(c) less than 1.7
(d) more than 1.7

65. The type of bond in which bond pair of electrons is contributed by one atom only, is called a:
(a) coordinate covalent 
(b) dative covalent bond
(c) Both 'a' & 'b' ✓
(d) None of these

66. The reaction between ammonia and hydrogen chloride involves the formation of a / an:
(a) ionic bond
(b) covalent bond
(c) polar covalent bond
(d) dative bond ✓

67. Most ionic compounds form:
(a) liquids
(b) crystals ✓
(c) gases
(d) metals

68. The melting and boiling points of ionic compounds are:
(a) high ✓
(b) low
(c) moderate
(d) None of these

69. Aqueous solutions of ionic compounds are:
(a) non-conductor of electricity
(b) conductor of electricity ✓
(c) sometimes conduct electricity
(d) partial conductor of electricity

70. Ionic compounds usually dissolve in:
(a) covalent solvent
(b) ionic solvent
(c) polar solvent ✓
(d) non-polar solvent

71. Ionic compounds are insoluble in:
(a) covalent solvent
(b) ionic solvent
(c) polar solvent
(d) non-polar solvent ✓

72. Which one of these is polar solvent?
(a) oil
(b) water ✓
(c) petrol
(d) kerosene oil

73. As compared to ionic bond, covalent bonds are generally:
(a) weak ✓
(b) strong
(c) stable
(d) unstable

74. Sugar crystals and diamond are the examples of:
(a) ionic compounds
(b) covalent compounds ✓
(c) polar compounds
(d) non-polar compounds

75. Non-polar covalent compounds are generally:
(a) soluble in water
(b) insoluble in water ✓
(c) sometimes insoluble in water
(d) sometimes soluble in water

76. Polar covalent compounds are soluble in:
(a) oil
(b) water ✓
(c) petrol
(d) kerosene oil

77. They do not conduct electricity in the solid, molten or aqueous solution.
(a) Ionic compounds
(b) polar compounds
(c) non-polar compounds ✓
(d) All of these

78. They are bad conductors of electricity.
(a) covalent compounds ✓
(b) ionic compounds
(c) polar compounds
(d) None of these

79. Which one is a polar covalent compound?
(a) CO₂
(b) CH₄
(c) C₂H₆
(d) HCl ✓

80. Which one is non-polar covalent compound?
(a) H₂SO₄
(b) CO₂ ✓
(c) H₂O
(d) HF

81. It is a common white glue.
(a) Polyurethane
(b) Resin glue
(c) Polyvinyl acetate ✓
(d) Epoxy resins

82. It is used in the construction of vehicles, trucks, boats and aircraft.
(a) Polyurethane
(b) Resin glue
(c) Polyvinyl acetate
(d) Epoxy resins ✓

Chemistry For Class IX (New Book ) - Chapter No. 5 - Physical States of Matter - Multiple Choice Questions And Fill In The Blanks

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Chapter No.5 - Physical States of Matter
MCQs And Fill In The Blanks
Text Book Exercise

SECTION- A: MULTIPLE CHOICE QUESTIONS
Tick Mark (✓) the correct answer

1. Which of the following gas diffuses fastest?
(a) Hydrogen ✓
(b) Chlorine
(c) Fluorine
(d) Helium

2. The vapour pressure of a liquid increases with the:
(a) increase of pressure
(b) increase of temperature ✓
(c) increase of intermolecular forces
(d) increase the polarity of molecules

3. The freezing point depends upon:
(a) Nature of liquid
(b) Pressure
(c) Temperature ✓
(d) Volume

4. One atmospheric pressure is equal to:
(a) 10325 Pascal
(b) 106075 Pascal
(c) 10523 Pascal
(d) 101325 Pascal ✓

5. Which of the following does not affect the boiling point:
(a) Intermolecular forces
(b) External pressure
(c) Initial temperature of liquid ✓
(d) Nature of liquid

6. The mobility of liquids is lesser than:
(a) Solids
(b) Gases ✓
(c) Plasma
(d) Bose Einstein Condensate

7. Which of the following have sharp melting point in solids:
(a) Plastic
(b) Rubber
(c) Glass
(d) Diamond ✓

8. Which of the following are lightest form of matter:
(a) Solid
(b) Liquid
(c) Gases
(d) Plasma ✓

9. The liquid molecules leave the surface of liquid in evaporation process because:
(a) Energy is low
(b) Energy is moderate
(c) Energy is high ✓
(d) None of these

10.The density of gases increases when its:
(a) Pressure increased ✓
(b) Temperature increased
(c) Volume increased
(d) None of these

11. Anything which has mass and occupies space is the definition of:
(a) matter ✓
(b) atom
(c) space
(d) mass

12. A gas has no fixed:
(a) mass
(b) weight
(c) volume ✓
(d) density

13. It can easily be compressed and expanded.
(a) Liquid
(b) Gas ✓
(c) Solid
(d) Plasma

14. Liquid has no fixed:
(a) mass
(b) weight
(c) volume
(d) shape ✓

15. The different physical states of matter are due to:
(a) arrangement of molecules
(b) intermolecular forces
(c) Both 'a' & 'b' ✓
(d) None of them

16. The gaseous state molecules are lying away from one another, this assumption was proposed by:
(a) Boltzmann
(b) Maxwell
(c) Kelvin
(d) All of them ✓

17. Spontaneous mixing of molecules by random motion and collision to form a homogeneous mixture is called:
(a) Diffusion ✓
(b) Effusion
(c) Mobility
(d) Compressibility

18. Gases are rapidly diffusible and depend upon the:
(a) the atomic mass of the gases
(b) molecular mass of the gases ✓
(c) the density of the gases
(d) temperature of the gases

19. It is the movement of particles from an area of high concentration to one of low concentration.
(a) Diffusion ✓
(b) Effusion
(c) Mobility
(d) Compressibility

20. The rate of diffusion does not depend upon:
(a) temperature
(b) viscosity of the medium
(c) volume ✓
(d) the size & mass of the particles

21. This is NOT an example of diffusion.
(a) You can smell perfume
(b) Garbage stinks
(c) Smoke in the air
(d) Leakage of air through a tyre pinhole ✓

22. It is escaping of gas molecules through a tiny hole into space with lesser pressure.
(a) Diffusion
(b) Effusion ✓
(c) Mobility
(d) Compressibility

23. Effusion depends upon:
(a) molecular masses of gases ✓
(b) viscosity of the medium
(c) the size & mass of the particles
(d) temperature

24. Which of the following gas effuses rapidly?
(a) Hydrogen ✓
(b) Chlorine
(c) Fluorine
(d) Helium

25. It is an example of effusion.
(a) You can smell perfume
(b) Garbage stinks
(c) Leakage of helium through gas balloons ✓
(d) Smoke in the air

26. The force exerted by gaseous particles per unit area is called:
(a) viscosity
(b) density
(c) rigidity
(d) gas pressure ✓

27. Pressure = _____:
(a) Force x Area
(b) Force / Area ✓
(c) Area / Force
(d) Force x Area / 2

28. S.I. unit of pressure is:
(a) Nm²
(b) Nm^-2 ✓
(c) N^2m
(d) N^-2m

29. It is used to measure the atmospheric pressure.
(a) Barometer ✓
(b) Manometer
(c) Lactometer
(d) Ammeter

30. The capacity of something to be flattened or reduced in size by pressure is called:
(a) density
(b) mobility
(c) effusion
(d) compressibility ✓

31. The gases are highly compressible due to:
(a) the size & mass of the particles
(b) molecular masses of gases
(c) larger spaces between their molecules ✓
(d) density of gases

32. It is degree of compactness or closeness of a molecules.
(a) Mobility
(b) Density ✓
(c) Effusion
(d) Diffusion

33. Gases have:
(a) low density ✓
(b) moderate density
(c) high density
(d) zero density

34. Gas density is expressed in:
(a) Nm^-2
(b) kelvin
(c) pascal
(d) grams per dm³ ✓

35. At constant temperature, the volume of a given mass of a gas is inversely proportional to its:
(a) density
(b) weight
(c) pressure ✓
(d) viscosity

36. At constant temperature, according to Boyle's law the volume of a given mass of a gas:
(a) decreases with the increase of pressure ✓
(b) decreases with the decrease of pressure
(c) decreases with the increase of density
(d) decreases with the decrease of density

37. Mathematical representation of Boyle's Law is:
(a) P/V = K
(b) PV = K ✓
(c) V/T = K
(d) VT = K

38.The average distance that a gas particle travels between successive collisions with other gas particles is called:
(a) average path
(b) independent path
(c) free path
(d) mean free path ✓

39. 1 atm = ___:
(a) 760 mm of Hg ✓
(b) 780 torr
(c) 103325 pascal
(d) All of these

40. If the pressure is kept constant, the volume of a given mass of a gas is:
(a) directly proportional to atmospheric pressure
(b) inversely proportional to atmospheric pressure
(c) directly proportional to the absolute temperature ✓
(d) inversely proportional to the absolute temperature

41. Mathematical representation of Charles's Law is:
(a) P/V = K
(b) PV = K
(c) V/T = K ✓
(d) VT = K

42. Zero of absolute temperature scale or Kelvin scale is equal to:
(a) 273°C
(b) -273°C ✓
(c) 273°F
(d) -273°F

43. At absolute zero (-273°C), an ideal gas would have:
(a) zero volume ✓
(b) minimum volume
(c) maximum volume
(d) None of these

44. 273 kelvin is equal to:
(a)-273 Celsius
(b) 273 Celsius
(c) 100 Celsius
(d) zero Celsius ✓

45. Which one is correct?
(a) (T)°C (T) K+ 273
(b) (T)°C = (T) K - 273 ✓
(c) (T)°C = 273-(T) K
(d) None of them

46. The boiling point of liquids depends on the:
(a) temperature in Celsius
(b) temperature in kelvin
(c) external atmospheric pressure ✓
(d) volume of the liquid

47. Evaporation is directly proportional to the:
(a) volume of the liquid
(b) temperature ✓
(c) pressure
(d) density

48. The evaporation is considered as:
(a) cooling process ✓
(b) heating process
(c) reversible process
(d) convertible process

49. Neither definite shape nor volume is the property of:
(a) solid
(b) gas ✓
(c) liquid
(d) None of them

50. The process in which molecules escape from the surface of a liquid is called:
(a) effusion
(b) evaporation ✓
(c) boiling
(d) melting

51. A gas possesses neither definite shape nor definite:
(a) volume ✓
(b) power
(c) energy
(d) density

52. The intermediate state between solid and gas is:
(a) plasma
(b) liquid ✓
(c) Bose Einstein condensate
(d) All of them

53. If the surface area is greater than rate of evaporation is:
(a) zero
(b) moderate
(c) lower
(d) higher ✓

54. The rate of evaporation increases with:
(a) less intermolecular forces ✓
(b) strong intermolecular forces
(c) Both 'a' & 'b'
(d) None of these

55. Vapour pressure depends on:
(a) nature of liquid
(b) size of molecules
(c) temperature
(d) All of them ✓

56. The temperature at which vapour pressure of a liquid become equal to atmospheric pressure is called:
(a) evaporation of the liquid
(b) boiling point of the liquid ✓
(c) melting point of the liquid
(d) freezing point of the liquid

57. The boiling point is directly proportional to:
(a) temperature
(b) density
(c) atmospheric pressure ✓
(d) volume

58. The temperature at which the vapour pressure of a liquid state becomes equal to the vapour pressure of its solid state is known as:
(a) evaporation of the liquid
(b) boiling point of the liquid
(c) melting point of the liquid
(d) freezing point of the liquid ✓

59. At this temperature liquid and solid coexist in dynamic equilibrium.
(a) evaporation of the liquid
(b) boiling point of the liquid
(c) melting point of the liquid
(d) freezing point of the liquid ✓

60. The energy that molecules have is:
(a) potential energy
(b) kinetic energy ✓
(c) atomic energy
(d) molecular energy

61. The liquids diffuse less rapidly than:
(a) solids
(b) gases
(c) plasma ✓
(d) Bose Einstein condensate

62. Density can be expressed as D = ___:
(a) mass / volume ✓
(b) volume / mass
(c) mass / 2(volume)
(d) mass x volume

63. If we increase temperature, the density of a liquid will:
(a) become zero
(b) decrease ✓
(c) increase
(d) None of these

64. The solids in which molecules are arranged in definite three dimensional geometrical pattern are called:
(a) powder
(b) dense solids
(c) amorphous solids
(d) crystalline solids ✓

65. The solids in which molecules are not arranged in geometrical pattern are called:
(a) powder
(b) dense solids
(c) amorphous solids ✓
(d) crystalline solids

66. Which one of these is NOT an amorphous solid?
(a) Sodium Chloride ✓
(b) Glass
(c) Rubber
(d) Plastic

67. Which one of these is a crystalline solid?
(a) Glass
(b) Diamond ✓
(c) Rubber
(d) Plastic

68. The existence of an element in more than one crystalline forms is known as:
(a) cosmogenic
(b) radioactivity
(c) allotropy ✓
(d) isotope

69. Diamond and graphite are the allotropic form of:
(a) sodium
(b) gold
(c) Sulphur
(d) carbon ✓

70. In this form, the carbon atoms are bonded together in spheres, cylinders or egg-shaped formations.
(a) Diamond
(b) Graphite
(c) Graphane
(d) Fullerenes ✓

71. English scientist William Crookes identify the fourth states of matter known as:
(a) gas
(b) liquid
(c) plasma ✓
(d) Bose Einstein condensate

72. It is plasma naturally.
(a) Lightning ✓
(b) Lava formation
(c) Center of the earth
(d) All of these

73. It is super-hot and super excited atoms:
(a) Plasma ✓
(b) Bose Einstein condensate
(c) Both 'a' & 'b'
(d) None of these

74. Atoms are super unexcited and super cold in:
(a) Plasma
(b) Bose Einstein condensate ✓
(c) Both 'a' & 'b'
(d) None of these