Lesson Notes By Weeks and Term - Senior Secondary 3

Iron

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TERM׃ IST TERM

WEEK FIVE

Class: Senior Secondary School 3

Age: 17 years

Duration: 40 minutes of 5 periods each

Date:

Subject: Chemistry

Topic: IRON

SPECIFIC OBJECTIVES: At the end of the lesson, pupils should be able to

  1. Describe the extraction process of Iron
  2. Identify the uses of iron.
  3. Define rusting of Iron
  4. discuss the methods of preventing rusting of Iron.

INSTRUCTIONAL TECHNIQUES: Identification, explanation, questions and answers,

demonstration, videos from source

INSTRUCTIONAL MATERIALS: Videos, loud speaker, textbook, iron, water, paint or oil, grease, Rusted nails, keys, spoons, etc

INSTRUCTIONAL PROCEDURES

PERIOD 1-2

PRESENTATION

TEACHER’S ACTIVITY

STUDENT’S

ACTIVITY

STEP 1

INTRODUCTION

The teacher describe  the extraction process of Iron to the students

 

Students pay

attention

STEP 2

EXPLANATION

Teacher discusses the uses of iron and then explains how iron rusting takes place

Students pay

attention and

participate

STEP 3

DEMONSTRATIO

N

Teacher discusses the methods of preventing Iron rusting.

Students pay

attention and

participate

STEP 4

NOTE TAKING

The teacher writes a summarized

note on the board

 

The students

copy the note in

their books

 

NOTE

IRON

The extraction of iron involves a series of chemical reactions in a blast furnace. The following are the steps of iron extraction from its ore, hematite (Fe2O3):

  1. Reduction of Iron Ore:

   Fe2O3 + 3CO  2Fe + 3CO2

   This equation represents the reduction of iron ore (hematite) by carbon monoxide (produced from coke). The iron ore is reduced to elemental iron, and carbon dioxide is produced as a byproduct.

  1. Formation of Slag:

   CaCO3  CaO + CO2

   This equation represents the decomposition of limestone (CaCO3) into calcium oxide (CaO) and carbon dioxide. Calcium oxide reacts with impurities in the iron ore to form slag.

  SiO2 + CaO  CaSiO3

   This equation represents the combination of silicon dioxide (SiO2) from impurities with calcium oxide to form calcium silicate, the primary component of the slag.

  1. Overall Reaction:

   The overall reaction for the extraction of iron from hematite can be represented as a combination of the reduction of iron ore and the formation of slag:

   Fe2O3 + 3CO + CaCO3  2Fe + 3CO2 + CaSiO2

Uses of IRON

Iron is a crucial metal with a wide range of applications due to its strength, durability, and versatility. Here are some common uses of iron:

  1. Iron, especially in the form of structural steel, is a primary material for building construction, bridges, and infrastructure projects.
  2. Iron and steel are used extensively in the manufacturing of vehicles, including cars, trucks, trains, and ships.
  3. Iron-based alloys, such as carbon steel, are commonly used in the production of tools and implements due to their strength and hardness.
  4. Iron and steel are used in the manufacturing of household items, including appliances, cookware, and furniture.
  5. Tinplate, a steel sheet coated with a thin layer of tin (an alloy of iron), is used in the production of food and beverage cans.
  6. Iron is an essential element for human health, and iron-based compounds are used in supplements and medical treatments.
  7. Iron is employed in water treatment processes to remove impurities and contaminants from water.

Rusting of IRON

The rusting of iron is a chemical reaction where iron reacts with oxygen and water to form iron oxide, commonly known as rust. This process is accelerated in the presence of moisture and can be slowed down through methods like coating or galvanizing.

The rusting of iron involves the following chemical reactions:

  1. Formation of Iron(II) ions:

 Fe(s)   Fe}2+(aq) + 2e-

  1. Reaction of Iron(II) ions with Oxygen:

   4Fe2+(aq) + O2(g)  +  4H2O(l)   4Fe3+(aq) + 4OH-(aq)

  1. Formation of Rust (Iron(III) oxide):

    4Fe3+(aq) + 3O2(g)  2Fe2O3(s)

Methods of preventing Iron from rusting

Several methods can be employed to prevent or minimize the rusting of iron

  1. Applying a protective layer of paint or varnish creates a barrier, preventing direct contact between iron and moisture or oxygen.
  2. Coating iron with a layer of zinc through galvanization provides a sacrificial layer that corrodes preferentially, protecting the underlying iron.
  3. Oil or Grease Coating: Applying a layer of oil or grease helps to inhibit contact between iron and moisture, reducing the likelihood of rust formation.
  4. Use of Stainless Steel: Stainless steel contains chromium, which forms a passive oxide layer, protecting the iron from corrosion.
  5. Cathodic Protection: Connecting iron to a more reactive metal, such as zinc, and allowing the zinc to corrode instead can protect the iron through cathodic protection.
  6. Electroplating: Coating iron with a thin layer of a more corrosion-resistant metal, such as chromium or nickel, through electroplating provides protection against rust.

EVALUATION:   1. Describe the extraction process of Iron

  1. Identify 4 uses of iron
  2. Mention 4 methods of preventing Iron from rusting

CLASSWORK: As in evaluation

CONCLUSION: The teacher commends the students positively