Set of Chemistry CEE-4
Posted by Set of Chemistry CEE-4
1. The chemical formula for sodium bicarbonate is:
a) NaCl
b) Na2CO3
c) NaHCO3
d) NaOH
2. Which of the following compounds is an example of a Lewis base?
a) H2O
b) BF3
c) NH3
d) CO2
3. Which of the following elements is most likely to form a cation with a +2 charge?
a) Sodium
b) Calcium
c) Chlorine
d) Oxygen
4. What is the molecular geometry of carbon dioxide (CO2)?
a) Trigonal planar
b) Linear
c) Bent
d) Tetrahedral
5. Which of the following is the strongest acid?
a) Hydrochloric acid (HCl)
b) Nitric acid (HNO3)
c) Sulfuric acid (H2SO4)
d) Acetic acid (CH3COOH)
6. The unit of the rate constant in a second-order reaction is:
a) s⁻¹
b) M⁻¹s⁻¹
c) M²s⁻¹
d) M⁻²s⁻¹
7. Which of the following compounds is a non-electrolyte in water?
a) NaCl
b) KNO3
c) HCl
d) Glucose (C6H12O6)
8. What is the molarity of a solution made by dissolving 2 moles of NaCl in 1 liter of water?
a) 0.5 M
b) 1 M
c) 2 M
d) 3 M
9. The process in which a solid changes directly into a gas is called:
a) Sublimation
b) Deposition
c) Evaporation
d) Condensation
10. Which of the following is a correct statement about an ideal gas?
a) The gas molecules do not exert any force on each other.
b) The volume of the gas molecules is significant.
c) The gas molecules are in constant motion, but they interact with each other.
d) The gas molecules do not occupy any space.
11. What is the electron configuration of oxygen (O)?
a) 1s² 2s² 2p⁶
b) 1s² 2s² 2p⁴
c) 1s² 2s² 2p³
d) 1s² 2s² 2p²
12. The boiling point of water is higher than that of hydrogen sulfide (H2S) because:
a) Water has stronger hydrogen bonds than hydrogen sulfide.
b) Water is a non-polar molecule, while H2S is polar.
c) H2S is heavier than water.
d) Water has more electrons than H2S.
13. Which of the following is the weakest acid?
a) HCl
b) H2SO4
c) CH3COOH
d) HNO3
14. Which of the following molecules is non-polar?
a) H2O
b) NH3
c) CO2
d) CH3Cl
15. Which of the following ions is responsible for the reddish-brown color in a flame test?
a) Sodium (Na⁺)
b) Potassium (K⁺)
c) Calcium (Ca²⁺)
d) Copper (Cu²⁺)
16. What is the pH of a solution with a hydrogen ion concentration of 1 × 10⁻⁶ M?
a) 4
b) 5
c) 6
d) 7
17. Which of the following is an example of a molecular solid?
a) Sodium chloride (NaCl)
b) Carbon dioxide (CO2)
c) Calcium carbonate (CaCO3)
d) Magnesium oxide (MgO)
18. The substance that is oxidized in a reaction:
a) Loses electrons
b) Gains electrons
c) Is a reducing agent
d) Both a and c
19. Which of the following is a property of acids?
a) They turn blue litmus paper red.
b) They are slippery to touch.
c) They have a bitter taste.
d) They react with metals to form hydroxides.
20. The hybridization of the central atom in CO2 is:
a) sp
b) sp²
c) sp³
d) sp³d²
21. Which of the following compounds is an ionic compound?
a) NaCl
b) CO2
c) CH4
d) H2O
22. The atomic mass of an element is calculated by the average mass of:
a) The protons and neutrons only
b) The protons and electrons
c) The protons, neutrons, and electrons
d) The naturally occurring isotopes weighted by their relative abundance
23. What is the main gas responsible for the greenhouse effect?
a) Oxygen
b) Nitrogen
c) Carbon dioxide
d) Methane
24. The reaction of an acid with a base produces:
a) Salt and hydrogen
b) Salt and water
c) Salt and oxygen
d) Water and carbon dioxide
25. What is the oxidation number of chlorine in NaClO3?
a) -1
b) +1
c) +3
d) +5
26. The reaction between hydrogen and oxygen to form water is an example of:
a) Combustion reaction
b) Decomposition reaction
c) Displacement reaction
d) Synthesis reaction
27. Which of the following compounds is used as a disinfectant in water purification?
a) Chlorine (Cl2)
b) Hydrogen peroxide (H2O2)
c) Sodium hydroxide (NaOH)
d) Ammonium nitrate (NH4NO3)
28. What is the molecular formula of methane?
a) CH3
b) CH4
c) C2H6
d) C3H8
29. Which of the following gases has the highest density at STP?
a) Hydrogen
b) Oxygen
c) Nitrogen
d) Carbon dioxide
30. What is the name of the compound with the formula KNO3?
a) Potassium nitrate
b) Potassium nitrite
c) Potassium hydroxide
d) Potassium sulfide
31. Which of the following is a reducing agent?
a) Oxygen
b) Hydrogen
c) Chlorine
d) Nitrogen
32. Which of the following ions is present in an acidic solution?
a) OH⁻
b) H⁺
c) Na⁺
d) Cl⁻
33. The reaction 2Na + Cl2 → 2NaCl is an example of a:
a) Synthesis reaction
b) Decomposition reaction
c) Displacement reaction
d) Redox reaction
34. Which of the following is the primary component of natural gas?
a) Methane (CH4)
b) Ethane (C2H6)
c) Propane (C3H8)
d) Butane (C4H10)
35. What is the volume of 2 moles of an ideal gas at STP?
a) 11.2 L
b) 22.4 L
c) 44.8 L
d) 33.6 L
36. Which of the following elements is a halogen?
a) Oxygen
b) Nitrogen
c) Chlorine
d) Carbon
37. Which of the following is the electron configuration of the sulfur (S) atom?
a) 1s² 2s² 2p⁶ 3s² 3p⁶
b) 1s² 2s² 2p⁶ 3s² 3p⁴
c) 1s² 2s² 2p⁶ 3s² 3p³
d) 1s² 2s² 2p⁶ 3s² 3p²
38. The element with atomic number 17 is:
a) Oxygen
b) Chlorine
c) Phosphorus
d) Sulfur
39. Which of the following is the main use of sulfuric acid (H2SO4)?
a) As a
disinfectant
b) In fertilizers
c) In soap production
d) In food preservation
40. The gas produced when an alkali metal reacts with water is:
a) Oxygen
b) Hydrogen
c) Nitrogen
d) Carbon dioxide
41. Which of the following metals is extracted from its ore using electrolysis?
a) Copper
b) Iron
c) Aluminum
d) Zinc
42. Which of the following gases is produced during the reaction between an acid and a metal?
a) Oxygen
b) Nitrogen
c) Hydrogen
d) Carbon dioxide
43. Which of the following elements is most likely to form a covalent bond?
a) Sodium
b) Magnesium
c) Oxygen
d) Calcium
44. Which of the following is an example of a polyatomic ion?
a) Na⁺
b) OH⁻
c) Cl⁻
d) Fe³⁺
45. What is the chemical formula for aluminum oxide?
a) AlO
b) Al₂O₃
c) Al₂O₄
d) AlO₂
46. Which of the following gases is colorless, odorless, and tasteless at room temperature?
a) Oxygen
b) Nitrogen
c) Carbon dioxide
d) Methane
47. Which of the following represents the correct order of increasing electronegativity?
a) F < Cl < Br < I
b) I < Br < Cl < F
c) Cl < F < I < Br
d) F < I < Br < Cl
48. The process of freezing is an example of:
a) Endothermic change
b) Exothermic change
c) Chemical change
d) Physical change
49. Which of the following is a non-metal?
a) Calcium
b) Oxygen
c) Sodium
d) Potassium
50. Which of the following is a characteristic of a base?
a) Turns red litmus paper blue
b) Tastes sour
c) Reacts with metals to form hydrogen gas
d) Releases H⁺ ions in water
Answer Key:
- c) NaHCO3
- c) NH3
- b) Calcium
- b) Linear
- c) Sulfuric acid (H2SO4)
- b) M⁻¹s⁻¹
- d) Glucose (C6H12O6)
- b) 1 M
- a) Sublimation
- a) The gas molecules do not exert any force on each other.
- b) 1s² 2s² 2p⁴
- a) Water has stronger hydrogen bonds than hydrogen sulfide.
- c) CH3COOH
- c) CO2
- d) Copper (Cu²⁺)
- c) 6
- b) Carbon dioxide (CO2)
- d) Both a and c
- a) They turn blue litmus paper red.
- a) sp
- a) NaCl
- d) The naturally occurring isotopes weighted by their relative abundance
- c) Carbon dioxide
- b) Salt and water
- d) +5
- d) Synthesis reaction
- a) Chlorine (Cl2)
- b) CH4
- d) Carbon dioxide
- a) Potassium nitrate
- b) Hydrogen
- b) H⁺
- a) Synthesis reaction
- a) Methane (CH4)
- c) 44.8 L
- c) Chlorine
- b) 1s² 2s² 2p⁶ 3s² 3p⁴
- b) Chlorine
- b) In fertilizers
- b) Hydrogen
- c) Aluminum
- c) Hydrogen
- c) Oxygen
- b) OH⁻
- b) Al₂O₃
- b) Nitrogen
- b) I < Br < Cl < F
- b) Exothermic change
- b) Oxygen
- a) Turns red litmus paper blue
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