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