10th Science - Important Book Inside

Scoring a perfect mark on objective assessments requires a deep reading of your text, which is why mastering Class 10 Science Book Inside One Mark Questions is so critical. Board exams frequently feature tricky, micro-conceptual queries pulled directly from the paragraphs, diagrams, and side-notes of your textbook rather than just the end-of-chapter exercises. This dedicated compilation highlights vital single-mark questions across physics, chemistry, and biology chapters—covering critical chemical reactions, fundamental formulas, and complex anatomical terms. Reviewing these high-yield internal questions ensures you bridge any minor gaps in your conceptual knowledge, helps you build rapid recall speed, and secures those crucial foundational points on your final test paper.

Grade X • Science (Physics & Chemistry)

STD: X • BOOK INSIDE IMPORTANT ONE MARK QUESTIONS

Comprehensive Revision Reference Notes (English Medium)

PHYSICS UNITS

1. Uses of force (1.4.2)

2. Define torque? Formula and unit: τ = F × d (SI unit: N m) (Page 5)

3. Write short notes on 'Gears' (Page 6)

4. Impulse (1.6): J = F × t, formula and unit (Page 7)

5. Acceleration due to gravity: g = GM / R²

6. Mass of the Earth: M = gR² / G = 5.972 × 10²⁴ kg

7. Value of 'g' depends on the geometric radius of the Earth

8. Value of 'g' at the centre of the Earth is zero (g = 0)

9. Gravity: Polar region – maximum; Equator – minimum; higher altitude – decreases; below Earth surface – decreases

10. Gravitational force: g = acceleration due to gravity at sea level = 9.8 m s^-2

11. Acceleration due to gravity on the Moon = 1.625 m s^-2

12. Weight: W = mg; on the Moon for 60 kg: W = 60 × 1.625 N

13. Define the term weightlessness (Page 12)

14. State First Law of Refraction (Page 17)

15. Tyndall scattering, Raman scattering (Page 19)

16. Applications of concave and convex lens (Page 21)

17. Lens maker's formula: 1 / f = (μ − 1)(1 / R₁ − 1 / R₂)

18. Power of a lens definition & formula: P = 1 / f (Page 23)

19. The minimum distance required for distinct vision = 25 cm

20. Persistence of vision: If time interval between two consecutive light pulses < 0.1 s (or 1/16 s)

21. Presbyopia is otherwise called old age hypermetropia

22. Astigmatism definition

23. Advantages and disadvantages of Telescopes; uses of simple microscope (Page 26)

24. Define kilocalorie (Page 34), Avogadro's law (Page 37)

25. What is temperature? SI unit: Kelvin (Page 38)

26. Current flowing through a conductor: I = Q / t

27. Nichrome has high resistivity = 1.5 × 10^-6 Ω m

28. Series connection: R_S = R₁ + R₂ + R₃; Parallel connection: 1 / R_P = 1 / R₁ + 1 / R₂ + 1 / R₃

29. Difference between series and parallel connections (Page 49, Table 4.3)

30. Electric heating device and fuse wire (Page 50)

31. 1 horse power = 746 watt

32. 1 kWh = 1000 × (60 × 60) J = 3.6 × 10⁶ J

33. Do you know: Domestic voltage ratings in India, USA & UK (Page 52)

34. LED – Light Emitting Diode

35. LCD – Liquid Crystal Display

36. Acoustics definition (Page 59)

37. Difference between sound waves and light waves (Page 60)

38. Laws of reflection of sound (Page 62)

39. Rarer medium and denser medium (Page 63)

40. Applications of echo (5.3.2) (Page 64)

41. Various possibilities / cases of Doppler effect (Page 65)

42. Definition of Doppler effect

43. Applications of Doppler effect (Page 67)

44. Discovery of Radium by Marie Curie and Pierre Curie

45. Rutherford, Becquerel definition (Page 76)

46. Uranium discovered after the planet Uranus by Martin Klaproth

47. Nuclear fission and nuclear fusion with equations (Page 78, 80)

48. Do you know: Nuclear bomb that was dropped on Japan (Page 79, 81)

49. Table 6.3: Uses of radioisotopes in medicine, agriculture, and industries

50. Americium and Californium uses (Page 83)

51. 6.5.3: Permissible radiation limits; Lead apron usage

52. The first nuclear reactor was built in 1942 at Chicago, USA

53. Uses of nuclear reactor

54. Dr. Homi Jehangir Bhabha was the first Chairman of Indian Atomic Energy Commission

55. BARC – Bhabha Atomic Research Centre (Page 84)

56. Nuclear power in India: India is the fifth largest source of electricity from nuclear power

57. India's first nuclear power station: Tarapur Atomic Power Station

58. Atomic power in Tamil Nadu: Kalpakkam and Kudankulam

59. Safe limit of receiving radiation exposure is about 100 mR per week

CHEMISTRY UNITS

60. First scientific Atomic Theory proposed by John Dalton

61. Atomic number (Z) = Number of protons or Number of electrons

62. Mass number (A) = Number of protons + Number of neutrons

63. If a molecule is made of similar kind of atoms, it is called a homoatomic molecule

64. If a molecule contains more than three atoms, it is called a polyatomic molecule

65. RMM (Relative Molecular Mass) calculations (Page 95)

66. Table 7.5: Difference between atom and molecule (Page 96)

67. Molar volume at NTP / STP = 22.4 litres (or 22,400 ml)

68. Formulas for Number of moles:
• Number of moles = Mass / Atomic mass
• Number of moles = Mass / Molecular mass
• Number of moles = Number of Atoms / (6.023 × 10²³)
• Number of moles = Number of Molecules / (6.023 × 10²³)

69. Avogadro Hypothesis and Applications of Avogadro's law (Page 98)

70. Define Isotopes, Isobars, and Isotones (Page 102)

71. State the Modern Periodic Law (Page 107)

72. Group Number – Family classification tabular column (Page 109)

73. Difference between anion and cation; Ionisation energy (Page 110)

74. Electronegativity values: F = 4.0, Cl = 3.0, Br = 2.8, I = 2.5, H = 2.1, Na = 0.9; Distance between two hydrogen nuclei = 0.74 Å

75. If electronegativity difference between two elements is 1.7, the bond has 50% ionic character and 50% covalent character

76. If ΔEN < 1.7 it is a covalent bond; if ΔEN > 1.7 it is an ionic bond

77. Periodic trends tabular column (Page 112)

78. Physical properties of metals (Page 114)

79. Define metallurgy, gangue or matrix, flux, slag (Page 112, 113)

80. Magnetic separation method

81. Hall-Héroult process, physical properties & uses of Aluminium (Page 115)

82. Aluminothermic process (Page 116)

83. Blister copper contains 2% impurities (Page 116)

84. Uses of copper (Page 117)

85. Chief ores of Iron: Haematite, Magnetite, Iron pyrites

86. Uses of Iron; Alloys, Amalgams, reasons for alloying; Corrosion (Page 119)

87. Pure copper is purified by electrolytic refining; Copper alloys, Aluminium alloys, Iron alloys (Page 120)

88. Methods of preventing corrosion

89. The process of uniform distribution of solute into solvent is called dissolution (Page 125)

90. Binary solution and Ternary solution (Page 125)

91. Types of binary solutions – Table 9.1; Saturated and Supersaturated solution (Page 126, 127)

92. Solubility formula = (Mass of the solute / Mass of the solvent) × 100

93. Henry's law (Page 129 – More to know)

94. Table 9.3: Hydrated Salts and Water of Crystallization

95. What happens during heating of green vitriol / blue vitriol; balanced chemical equation

96. Define chemical reaction, reactants, and products

97. Page 138 – Types of reactions; Page 146 & 147 (Do you know)

98. Types of combination reactions:
• Element + Element → Compound (e.g., 2Mg + O₂ → 2MgO)
• Compound + Element → Compound (e.g., 2CO + O₂ → 2CO₂ / PCl₃ + Cl₂ → PCl₅)
• Compound + Compound → Compound (e.g., CaO + SiO₂ → CaSiO₃)

99. Formula for chalk, marble, limestone: CaCO₃

100. Thermolysis, Exothermic, Endothermic, Photolysis, Metathesis (Double Displacement), Precipitation, and Neutralization reactions with examples

101. Difference between combination reaction and decomposition reaction (Page 142)

102. Activity series / Reactivity table of metals

103. Rate of a chemical reaction – More to know (Page 144, 145)

104. Physical equilibrium & Chemical equilibrium (Page 147)

105. Soda water contains Carbonic acid (H₂CO₃): H₂O + CO₂ ↔ H₂CO₃

106. pH scale tabular column; Ionic product of water: K_w = [H⁺][OH^-] = 1.0 × 10^-14 at 25°C (Page 148)

107. General Formulas for Hydrocarbons:
• Alkane formula: C_nH_2n+2
• Alkene formula: C_nH_2n
• Alkyne formula: C_nH_2n-2
• Alkyl radical formula: C_nH_2n+1

108. Characteristics of hydrocarbons: Saturated vs Unsaturated hydrocarbons; test to identify unsaturated hydrocarbons (Bromine water decolourisation)

109. Define functional group; Table 11.2 – Classes of organic compounds (Page 158)

110. Characteristics of homologous series (11.3.2, Page 159)

111. IUPAC – International Union of Pure and Applied Chemistry

112. Three components of IUPAC name: Root word + Prefix + Suffix

113. Table 11.4: Root words based on number of carbon atoms (Page 160)

114. Table 11.5: Prefixes for IUPAC name (Page 161)

115. Table 11.6: Primary and secondary suffixes for IUPAC nomenclature (Page 163)

116. Esterification, Dehydration, Dehydrogenation, uses of ethanol (Page 164 – More to know)

117. Glacial acetic acid, Decarboxylation (removal of CO₂), uses of ethanoic acid; Difference between hard soap and soft soap (Page 167 – Do you know)

118. Advantages of detergents over soaps; disadvantages of detergents; TFM (Total Fatty Matter in soaps) (Page 168)