AIC SS1 Chemistry Revision Test 2nd Term
  • 1. The diagram above represents the arrangement of valence electrons in the molecule AB2. Which of the following pairs of electrons could be A and B respectively?
A) Oxygen and hydrogen
B) Nitrogen and oxygen
C) Carbon and oxygen
D) Sulphur and oxygen
  • 2. What is the empirical formular of a hydrocarbon containing 0.08 moles of carbon and 0.32 moles of hydrogen?[H=1, C=12, O= 16]
A) C2H4
B) CH2
C) CH4
D) CH3
  • 3. An organic compound contains 0.188g carbon, 0.062g hydrogen and 0.25g oxygen. What is the empirical formula of the compound?.[H=1, C=12, O= 16]
  • 4. If an element X with atomic number 13 combines with an element Y whose atomic number is 8, the most likely formula of the compound formed between X and Y is .....
A) X2Y
B) XY2
C) X3Y2
D) X2Y3
  • 5. 13. In the equation above, the value p and x respectively are .......
A) 6 and 2
B) 2 and 3
C) 1 and 3
D) 8 and 2
  • 6. The IUPAC system uses -------- in naming compounds.
A) Atomic mass
B) No of moles
C) Molar mass
D) Oxidation numbers
  • 7. What is the oxidation number of manganese in KMNO4?
A) -7
B) +8
C) +7
D) -5
  • 8. When a solid substance changes directly to a gas on heating without passing through the liquid state, the substance is said to have undergone:
A) Crystallisation
B) Melting
C) Evaporation
D) Sublimation
  • 9. What is the mass number of an element if its atom contains 10 protons, 10 electrons, and 12 neutrons?
A) 22
B) 10
C) 20
D) 32
  • 10. What is the percentage by mass of sulphur in aluminium tetraoxosulphate (VI), Al2(SO4)_3. ( Al = 27, S = 32, O = 16)
A) 21.33%
B) 42.66%
C) 28.07%
D) 14.71%
  • 11. What is the molecular mass of calcium trioxonitrate (V) 2Ca (NO3)_2 (Ca = 40, N = 14, O = 16)
A) 164
B) 328
C) 346
D) 160
  • 12. The electronic configuration of an atom is: 2, 8, 8,1. What element is it?
A) Argon
B) Sulphur
C) Potassium
D) Chlorine
  • 13. Coordinate bonding involves the sharing of:
A) Neutrons between two atoms
B) Protons between two atoms
C) Electrons between two atoms
D) Electrons from one atom to another
  • 14. Which of the following compounds exhibits coordinate bonding?
A) H2O
B) NaCl
C) NH3
D) CO2
  • 15. Metallic bonding is characterized by the:
    a) b) c)
A) Formation of covalent bonds between atoms
B) Sharing of electrons between atoms
C) Transfer of electrons between atoms
D) Presence of positive ions in a sea of delocalized electrons
  • 16. Which of the following is an example of a metallic compound?
A) Carbon dioxide
B) Iron
C) Sodium chloride
D) Water
  • 17. Covalent bond formation is influenced by:
A) Atomic radius of atoms
B) Electron affinity of atoms
C) Electronegativity difference between atoms
D) All of the above
  • 18. Hydrogen bonds are formed between hydrogen and:
A) Carbon
B) Helium
C) Nitrogen
D) Oxygen
  • 19. Which of the following compounds exhibits hydrogen bonding?
A) Ammonia (NH3)
B) Methane (CH4)
C) Carbon dioxide (CO2)
D) Ethanol (C2H5OH)
  • 20. Vander Waal's forces are:
A) Strong electrostatic attractions between ions
B) Weak intermolecular forces between molecules
C) Strong covalent bonds between atoms
D) Weak intramolecular forces within molecules
  • 21. Which of the following substances is primarily held together by Vander Waal's forces?
A) Sodium chloride (NaCl)
B) Hydrogen peroxide (H2O2)
C) Methane (CH4)
D) Ethanol (C2H5OH)
  • 22. According to the kinetic model of matter, particles in a gas:
A) Have strong intermolecular forces of attraction
B) Have fixed positions in a lattice structure
C) Are closely packed together
D) Have negligible volume compared to the space they occupy
  • 23. The kinetic theory of gases explains the behavior of gases based on:
A) The arrangement of particles within a gas
B) The motion of particles within a gas
C) The density of particles within a gas
D) The chemical reactions occurring within a gas
  • 24. According to the kinetic model, solids:
A) Have particles that are highly compressed and free to move
B) Have particles that are highly compressed and far apart
C) Have particles that are closely packed together and vibrate in fixed positions
D) Have particles that are far apart and moving randomly
  • 25. Which of the following is an example of a physical change?
A) Digestion of food
B) Melting of ice
C) Rusting of iron
D) Burning of wood
  • 26. Boyle's law describes the relationship between:
A) Volume and number of moles of a gas
B) Temperature and volume of a gas
C) Pressure and volume of a gas
D) Pressure and temperature of a gas
  • 27. Charles's law describes the relationship between:
A) Pressure and temperature of a gas
B) Volume and number of moles of a gas
C) Temperature and volume of a gas
D) Pressure and volume of a gas
  • 28. The general gas equation combines which of the following laws?
A) Boyle's law, Charles's law, and Avogadro's law
B) Boyle's law and Charles's law
C) Charles's law and Avogadro's law
D) Boyle's law and Avogadro's law
  • 29. The ideal gas equation is given by:
A) PV = nT
B) P = V/nRT
C) PV = nRT
D) PV = RT
  • 30. Graham's law of diffusion states that the rate of diffusion of a gas is inversely proportional to its:
A) Pressure
B) Square root of its molar mass
C) Temperature
D) Volume
  • 31. Gay-Lussac's law relates the pressure and temperature of a gas at constant:
A) Number of moles
B) Atomic mass
C) Volume
D) Density
  • 32. Avogadro's number represents the number of:
A) Moles in one liter of a gas
B) Electrons in one atom of a substance
C) Particles in one gram of a substance
D) Atoms in one mole of a substance
  • 33. Lewis structures show which molecule exhibits coordinate covalent bonding?
B) H2O
C) NH3
D) CO2
  • 34. Which factor favors the formation of an electrovalent bond between two elements?
A) Large difference in electronegativity
B) Similar electron affinity values
C) Both elements are non-metals
D) High similarity in electronegativity
  • 35. Which element is most likely to form a metallic bond?
A) Helium
B) Oxygen
C) Sodium
D) Chlorine
  • 36. Which statement is NOT true about covalent bonds?
A) They are responsible for the high melting and boiling points of many molecules.
B) They form between atoms with similar electronegativity.
C) They can be polar or non-polar
D) They involve sharing electrons.
  • 37. Which intermolecular force is responsible for the high boiling point of water?
A) Dipole-dipole interactions
B) Covalent bonding
C) Hydrogen bonding
D) London dispersion forces
  • 38. According to the kinetic theory, which statement is true about gas particles?
A) They have specific shapes.
B) They occupy a significant volume.
C) They are constantly in motion.
D) They attract each other strongly
  • 39. The kinetic model can explain why...
A) liquids flow easily and have indefinite shapes.
B) gases expand to fill their container.
C) solids are rigid and have definite shapes
D) all three statements are true.
  • 40. Charles's Law states that at constant pressure, the volume of a gas is...
A) constant
B) dependent on the container size.
C) inversely proportional to its temperature
D) directly proportional to its temperature
  • 41. The general gas equation combines Boyle's Law, Charles's Law, and Avogadro's Law into a single equation. What is the symbol for the constant in this equation?
A) P
B) R
C) V
D) K
  • 42. When wood burns, it reacts with oxygen to form carbon dioxide and water vapor. According to the law of conservation of mass, the total mass of the:
A) wood and oxygen is less than the mass of the products.
B) wood and oxygen is greater than the mass of the products.
C) wood decreases, while the mass of the products remains constant.
D) wood and oxygen is equal to the mass of the carbon dioxide and water vapor.
  • 43. When solving a mass-to-mass stoichiometry problem, the molar masses of the:
A) are not needed, only the coefficients are important.
B) reactants and products are used to convert between grams and moles.
C) compounds are ignored.
D) elements are used directly.
  • 44. To solve a stoichiometry problem, you need to:
A) perform complex mathematical calculations.
B) know the physical properties of all the reactants and products.
C) memorize the names of all elements and compounds.
D) balance the chemical equation first.
  • 45. Which of the following statements does NOT support the law of definite proportions?
A) The color of a compound can vary depending on its source.
B) Water (H₂O) always contains hydrogen and oxygen in a 2:1 ratio by mass.
C) Carbon dioxide (CO₂) has a constant ratio of carbon to oxygen, regardless of its origin.
D) All samples of table salt (NaCl) have the same ratio of sodium to chlorine.
  • 46. If element X combines with element Y to form two different compounds, XY₂ and XY₃, the ratio of the masses of Y in these compounds will be:
A) 2:3
B) Cannot be determined without additional information.
C) 1:2
D) 1:3/2
  • 47. The equation 2H₂ + O₂ -> 2H₂O tells us that:
A) Two molecules of hydrogen react with one molecule of oxygen to form two molecules of water.
B) Water can decompose into hydrogen and oxygen under specific conditions.
C) 2 grams of hydrogen react with 1 gram of oxygen to produce water.
D) Hydrogen and oxygen react explosively to form water.
  • 48. The law of multiple proportions applies to:
A) only elements, not compounds.
B) all chemical reactions.
C) compounds that can react with each other.
D) elements that can form more than one compound with another element.
  • 49. In a balanced chemical equation, the coefficients represent:
A) the relative amounts of each molecule or atom involved in the reaction.
B) the names of the reactants and products
C) the states of matter of the reactants and products.
D) the order in which the reactants combine.
  • 50. If 5 moles of methane (CH₄) react completely, how many moles of carbon dioxide (CO₂) are produced according to the balanced equation: CH₄ + 2O₂ -> CO₂ + 2H₂O?
A) 5 moles
B) Cannot be determined without additional information.
C) 2.5 moles
D) 10 moles
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