9th Class Chemistry Chapter 7 Electrochemistry Important Short Questions 2024

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Class 9 Chemistry Chapter 7 Notes

Post TopicShort Questions
Book CodeChemistry
Class9th Class
Chapter/FullChapter 7
BoardPunjab Board

9th Class Chemistry Chapter 7 Electrochemistry Short Questions Notes

  • Oxidation is the addition of oxygen removal of hydrogen or loss of electrons by an element and as a result oxidation number increases.
  • Reduction is the addition of hydrogen removal of oxygen or gain of electrons by an element and as a result oxidation number decreases.
  • The oxidation number is the apparent charge on an atom. It may be positive or negative.
  • Oxidizing agents are the species that oxidize the other elements and reduce themselves. Non-metals are oxidizing agents.
  • Reducing agents are species that reduce the other elements and oxidize themselves. Metals are reducing agents.
  • Chemical reactions in which the oxidation state of species changes are termed redox reactions. A redox reaction involves oxidation and reduction processes taking place simultaneously.
  • Redox reactions either take place spontaneously and produce energy or
  • electricity is used to drive the reaction.
  • The process in which electricity is used for the decomposition of a chemical compound is called electrolysis. It takes place in electrolytic cells such as Downs cell and Nelson’s cell.
  • Galvanic cells are those in which spontaneous reactions take place and generate electric current. They are also called voltaic cells.
  • Sodium metal is manufactured from fused sodium chloride in the Downs cell.
  • NaOH is manufactured from brine in Nelson’s cell.
  • Corrosion is slow and continuous eating away of a metal by the surrounding medium. The most common example of corrosion is rusting of iron.
  • The rusting principle is an electrochemical redox reaction, in which iron behaves as an anode. Iron is oxidized to form rust Fe O . nH O. 2 3 2
  • Corrosion can be prevented by many methods. The most important is electroplating.
  • Electroplating is the depositing of one metal over the other by means of electrolysis.
  • Iron can be electroplated by tin, zinc, silver, or chromium.
  • Define oxidation in terms of electrons. Give an example.
  • Define reduction in terms of loss or gain of oxygen or hydrogen. Give an example.
  • What is the difference between valency and oxidation state?
  • Differentiate between oxidizing and reducing agents
  • Differentiate between strong and weak electrolytes.
  • How electroplating of tin on steel is carried out?
  • Why steel is plated with nickel before the electroplating of chromium?
  • How can you explain, that the following reaction is oxidation in terms of the increase of oxidation number?
  • How can you prove with an example that the conversion of an ion to an atom is an oxidation process?
  • Why does the anode carry a negative charge in the galvanic cell but a positive charge in an electrolytic cell? Justify with comments.
  • Where do the electrons flow from the Zn electrode in Daniel’s cell?
  • Why do electrodes get their names ‘anode’ and cathode in galvanic cells?
  • What happens at the cathode in a galvanic cell?
  • Which solution is used as an electrolyte in Nelson’s cell?
  • Name the by-products produced in Nelson’s cell.
  • Why is galvanizing done?
  • Why an iron grill is painted frequently?
  • Why is O necessary for rusting? 2
  • In the electroplating of chromium, which salt is used as an electrolyte?
  • Write the redox reaction taking place during the electroplating of chromium.
  • In the electroplating of silver, from where do Ag ions come, and where do they deposit?
  • What is the nature of the electrode used in the electrolyting of chromium?

Chemistry Chapter 7 Short Questions PDF Download

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Chemistry Chapter 7 Short Questions


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