This quiz works best with JavaScript enabled. Home > Class 11 > Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions – Quiz 9 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 9 (25 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. Why does the chlorine gas are able to displace the bromide ion from its salt solution? A) Because chlorine atoms are more electronegative than the bromide ions. B) Because bromide atoms are more electronegative than the chloride ions. C) Because chlorine atoms are more electropositive than the bromide atoms. D) Because the chlorine atoms transfer electrons from itself to the bromide atoms. Show Answer Correct Answer: A) Because chlorine atoms are more electronegative than the bromide ions. 2. The chemical equation for the reaction between sodium hydride and water is $NaH+H_2O\longrightarrow NaOH+H_2$ A) An oxidising agent. B) A reducing agent. C) Both an oxidising agent and a reducing agent. D) Neither an oxidisding agent nor a reducing agent. Show Answer Correct Answer: A) An oxidising agent. 3. What is the oxidation state of manganese in KMnO4? A) +6. B) +7. C) +4. D) +2. Show Answer Correct Answer: B) +7. 4. What happens to magnesium when it reacts with a dilute acid? A) It gains electrons and is reduced. B) It loses electrons and is oxidized. C) It gains protons and is oxidized. D) It loses protons and is reduced. Show Answer Correct Answer: B) It loses electrons and is oxidized. 5. How do you convert a redox reaction into a balanced ionic equation? A) A balanced ionic equation is obtained by combining the balanced oxidation and reduction half-reactions, ensuring mass and charge are conserved. B) Use coefficients that do not conserve mass or charge. C) Only write the oxidation half-reaction and ignore the reduction half-reaction. D) Combine the oxidation and reduction reactions without balancing them. Show Answer Correct Answer: A) A balanced ionic equation is obtained by combining the balanced oxidation and reduction half-reactions, ensuring mass and charge are conserved. 6. Consider the following reaction.NO$_{3}$$^{-}$ (aq) + Cu (s) $\rightarrow$ NO (g) + Cu$^{2+}$ (aq)Which statement is correct? A) Cu (s) is the reducing agent because it loses electrons. B) Cu (s) is the reducing agent because it gains electrons. C) Cu (s) is the oxidizing agent because it loses electrons. D) Cu (s) is the oxidizing agent because it gains electrons. Show Answer Correct Answer: A) Cu (s) is the reducing agent because it loses electrons. 7. What is the oxidation number of each atom in H$_{3}$PO$_{4}$? A) H =-1; P = +5; O =-2. B) H = 0; P = +3; O =-2. C) H = +1; P = +7; O =-2. D) H = +1; P = +1; O =-1. E) H = +1; P = +5; O =-2. Show Answer Correct Answer: E) H = +1; P = +5; O =-2. 8. Combustion and single-replacement reactions are ..... redox reactions. A) Always. B) Never. C) Sometimes. D) Mostly. Show Answer Correct Answer: A) Always. 9. How do you determine the endpoint in a titration using KMnO4? A) The endpoint is indicated by a persistent faint pink color in the solution. B) The endpoint is marked by a sudden color change to dark purple. C) The endpoint is indicated when the solution becomes completely clear. D) The endpoint is determined by the temperature of the solution. Show Answer Correct Answer: A) The endpoint is indicated by a persistent faint pink color in the solution. 10. In the redox reaction AgNO$_{3}$ + Na $\rightarrow$ NaNO$_{3}$ + Ag, which element has been reduced? A) Sodium (Na). B) Oxygen (O). C) Nitrogen (N). D) Silver (Ag). Show Answer Correct Answer: D) Silver (Ag). 11. Which of the following statements is true about net ionic equations? A) They include all ions present in the reaction. B) They only include the ions that participate in the reaction. C) They include only the spectator ions. D) They are the same as molecular equations. Show Answer Correct Answer: B) They only include the ions that participate in the reaction. 12. The species that gain electron is ..... and usually the ..... agent A) Oxidized;oxidizing. B) Reduced;reducing. C) Reduced;oxidizing. D) Oxidized; reducing. Show Answer Correct Answer: C) Reduced;oxidizing. 13. ..... synthesis and decomposition reactions involve the transfer of electrons. A) All. B) Most. C) No. D) Some. Show Answer Correct Answer: B) Most. 14. The reaction H$_{2}$SO$_{4}$ + 2NaOH $\rightarrow$ Na$_{2}$SO$_{4}$ + 2H$_{2}$O A) Is a redox reaction. B) Is not a redox reaction. C) All the above. D) None of the above. Show Answer Correct Answer: B) Is not a redox reaction. 15. Balance the following redox equations for reactions that occur in neutral solution:Fe$^{3+}$ + I$^{-}$ $\rightarrow$ Fe$^{2+ }$+ I$_{2. }$: A) Fe$^{3+}$ + 2I$^{-}$ $\rightarrow$ Fe$^{2+}$ + 2I$_{2}$. B) Fe$^{3+}$ + I$^{-}$ $\rightarrow$ Fe$^{2+}$ + I$_{2}$. C) 2Fe$^{3+}$ + I$^{-}$ $\rightarrow$ 2Fe$^{2+}$ + I$_{2}$. D) 2Fe$^{3+}$ + 2I$^{-}$ $\rightarrow$ 2Fe$^{2+}$ + I$_{2}$. Show Answer Correct Answer: D) 2Fe$^{3+}$ + 2I$^{-}$ $\rightarrow$ 2Fe$^{2+}$ + I$_{2}$. 16. How many electrons are transferred in the reaction of MnO4-with I-? A) 5 electrons are transferred in the reaction. B) 8 electrons are transferred in the reaction. C) 10 electrons are transferred in the reaction. D) 12 electrons are transferred in the reaction. Show Answer Correct Answer: C) 10 electrons are transferred in the reaction. 17. What is the oxidation state of the hydroxide ion in the reaction with silver diamine? A) 0. B) -1. C) +1. D) +2. Show Answer Correct Answer: B) -1. 18. 2Na + 2H$_{2}$O $\rightarrow$ 2NaOH + H$_{2}$Which statement is correct? A) Hydrogen is oxidised from +1 to 0. Sodium is reduced from 0 to +1. B) Hydrogen is reduced from +1 to 0. Sodium is oxidised from 0 to +1. C) Hydrogen is reduced from +2 to 0. Sodium is oxidised from 0 to +2. D) Hydrogen is oxidised from +2 to 0. Sodium is reduced from 0 to +2. Show Answer Correct Answer: B) Hydrogen is reduced from +1 to 0. Sodium is oxidised from 0 to +1. 19. What is the name of this equation:Fe$^{2+}$ $_{(aq)}$ + 2e$^{-}$ $\rightarrow$ Fe$_{(s)}$ A) A full redox equation. B) A net chemical equation. C) A half redox equation. D) An overall chemical equation. Show Answer Correct Answer: C) A half redox equation. 20. What is the oxidation number of chromium in $K_2Cr_2O_7$ A) +3. B) +6. C) +7. D) +2. Show Answer Correct Answer: B) +6. 21. Describe the role of electrons in redox reactions. A) Electrons are only involved in ionic reactions. B) Electrons are produced during redox reactions but not transferred. C) Electrons are transferred between reactants, causing oxidation and reduction in redox reactions. D) Electrons do not play a significant role in chemical reactions. Show Answer Correct Answer: C) Electrons are transferred between reactants, causing oxidation and reduction in redox reactions. 22. During the formation of an ionic compound metal atoms act as ..... A) Oxidizing agents. B) Reducing agents. C) Oxidants. D) Spectator ions. Show Answer Correct Answer: B) Reducing agents. 23. Which of these metals tends to resist losing electrons to corrosion? A) Aluminium. B) Iron. C) Platinum. D) Zinc. Show Answer Correct Answer: C) Platinum. 24. What is used to indicate the oxidation number? A) Numbers. B) Integers. C) Roman numerals. D) None of the above. Show Answer Correct Answer: C) Roman numerals. 25. What is the oxidation state of hydrogen in most compounds? A) 0. B) -1. C) +1. D) +2. Show Answer Correct Answer: C) +1. ← PreviousNext →Related QuizzesClass 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 1Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 2Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 3Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 4Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 5Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 6Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 7Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 8Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 10Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 11 🏠 Back to Homepage 📘 Download PDF Books 📕 Premium PDF Books