SULPHUR :GENERAL PROPERTIES OF SULPHUR GROUP

Subject :Chemistry

Term : Second Term

Week :Week 8

Topic :

SULPHUR

OBJECTIVES

Objective: By the end of this lesson, students should be able to understand the physical and chemical properties of sulfur, the extraction and production processes, and the various industrial and commercial applications of sulfur.

Materials Needed:

• Whiteboard or blackboard
• Markers or chalk
• Projector (optional)
• Handouts (optional)

WEEK EIGHT

DATE: _________

TOPIC: SULPHUR

CONTENT

• General Properties of Sulphur Group.
• Electronic Structure of Sulphur Group.
• Extraction of Sulphur.
• Allotropes of Sulphur.
• Uses of Sulphur

SULPHUR

Sulphur is a chemical element with the symbol S and atomic number 16. It is a non-metal and can be found in nature in various forms, such as minerals like pyrite, gypsum, and epsom salt. Sulphur is also present in many organic compounds like amino acids and proteins.

Here are some examples of how sulphur is used in our daily lives:

1. Fertilizer production: Sulphur is used in the production of fertilizers like ammonium sulphate and sulphuric acid, which are essential for agriculture.
2. Rubber industry: Sulphur is used in the vulcanization process of rubber to make it more durable and heat resistant.
3. Matches: Sulphur is used in the production of matchsticks. When struck against a rough surface, the sulphur reacts with oxygen in the air, producing a flame.
4. Preservative: Sulphur dioxide is used as a preservative in food and drinks to prevent bacterial growth and oxidation.
5. Pharmaceuticals: Sulphur is used in the production of various drugs, such as antibiotics and anti-inflammatory medications.
6. Beauty products: Sulphur is used in some beauty products like acne creams, shampoos, and skin cleansers due to its antibacterial properties.

These are just a few examples of how sulphur is used in our daily lives. It’s a very important element with a wide range of applications

GENERAL PROPERTIES OF THE SULPHUR GROUP (GROUP VI ELEMENTS)

The group VI elements include: Oxygen, Sulphur, Selenium, Tellurium and Polonium.

1. Metallic property increases down the group. Oxygen and sulphur are non-metal; selenium and tellurium are metalloid; while polonium is a metal.
2. All the elements are solid except oxygen which is a gas at room temperature. 
3. Oxygen and sulphur exhibit allotropy.
4. They have six electrons in their outermost shell. Hence their oxidation number is -2; though sulphur can exhibit -4 and -6 states in some compounds.
5. Electronegativity decreases down the group. Thus, oxygen is a good oxidizing agent.

The Sulphur Group refers to a group of chemical elements that share similar properties to sulfur (S), including selenium (Se), tellurium (Te), and polonium (Po). Here are some general properties of the Sulphur Group:

1. Non-metals: All the elements in the Sulphur Group are non-metals. They do not conduct electricity well, are not malleable or ductile, and tend to be brittle.
2. Similar chemical properties: The elements in the Sulphur Group have similar chemical properties. They all react with oxygen to form oxides, and with halogens to form halides.
3. Allotropes: Sulphur, selenium, and tellurium have multiple allotropes, meaning they can exist in different forms with different physical properties. For example, sulfur can exist in the form of rhombic and monoclinic crystals, as well as as amorphous powder.
4. Toxicity: Polonium is highly radioactive and toxic, and can be lethal in small doses.
5. Uses: The elements in the Sulphur Group have a variety of uses. For example, selenium is used in the production of photovoltaic cells, while tellurium is used in the manufacture of solar panels. Polonium has been used in atomic batteries, while sulfur is used in the production of fertilizers, rubber, and various chemicals.

These are just some of the general properties of the Sulphur Group. Each element in the group has its own unique characteristics and applications.

Evaluation

1. What is the atomic number of sulphur? a) 16 b) 17 c) 18 d) 19
2. Which of the following is a mineral that contains sulphur? a) Quartz b) Pyrite c) Halite d) Calcite
3. Sulphur is a: a) Metal b) Non-metal c) Metalloid d) Noble gas
4. Which of the following is NOT an allotrope of sulphur? a) Rhombic b) Monoclinic c) Amorphous d) Tetrahedral
5. Which of the following is NOT a use of sulphur? a) Production of fertilizers b) Production of rubber c) Production of batteries d) Production of chemicals
6. Which of the following elements is NOT part of the Sulphur Group? a) Selenium b) Tellurium c) Polonium d) Xenon
7. What is the primary use of selenium? a) Production of fertilizers b) Production of solar panels c) Production of matches d) Production of pharmaceuticals
8. What is the most common form of sulphur found in nature? a) Rhombic crystals b) Monoclinic crystals c) Amorphous powder d) Tetrahedral molecules
9. Which of the following is NOT a general property of the Sulphur Group? a) Allotropes b) Toxicity c) Metallicity d) Similar chemical properties
10. Which of the following is NOT a use of tellurium? a) Production of solar panels b) Production of glass c) Production of ceramics d) Production of alloys

ELECTRONIC STRUCTURE OF SULPHUR GROUP

The electronic structure of the Sulphur Group elements, sulfur (S), selenium (Se), tellurium (Te), and polonium (Po), can be determined by their atomic numbers and their positions in the periodic table.

Sulfur has an atomic number of 16, which means it has 16 protons and 16 electrons in its neutral state. Its electron configuration can be written as 1s² 2s² 2p⁶ 3s² 3p⁴. This means that sulfur has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbitals, two in its 3s orbital, and four in its 3p orbitals.

Selenium has an atomic number of 34, which means it has 34 protons and 34 electrons in its neutral state. Its electron configuration can be written as 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁴. This means that selenium has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbitals, two in its 3s orbital, six in its 3p orbitals, two in its 4s orbital, ten in its 3d orbitals, and four in its 4p orbitals.

Tellurium has an atomic number of 52, which means it has 52 protons and 52 electrons in its neutral state. Its electron configuration can be written as 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁴. This means that tellurium has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbitals, two in its 3s orbital, six in its 3p orbitals, two in its 4s orbital, ten in its 3d orbitals, six in its 4p orbitals, two in its 5s orbital, ten in its 4d orbitals, and four in its 5p orbitals.

Polonium has an atomic number of 84, which means it has 84 protons and 84 electrons in its neutral state. Its electron configuration can be written as 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁴. This means that polonium has two electrons in its 1s orbital, two in its 2s orbital, six in its 2p orbitals, two in its 3s orbital, six in its 3p orbitals, two in its 4s orbital, ten in its 3d orbitals, six in its 4p orbitals, two in its 5s orbital, ten in its 4d orbitals, six in its 5p orbitals, two in its 6s orbital, fourteen in its 4f orbitals, ten in its 5d orbitals, and four in its 6p orbitals

Members of the sulphur family include: Oxygen, Sulphur, Selenium, Tellurium and Polonium. Their electronic configurations are shown below:  

Oxygen = 8: 1s2 2s2 2p4

Sulphur = 16: 1s2 2s2 2p6 3s2 3p4

Selenium= 34: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p4

Tellurium = 52: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p4

Polonium = 84: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 5d10 5f14 6s2 6p4

 

SULPHUR 

Sulphur is an element. It occurs freely as deposits and in combined state as sulphide and as tetraoxosulphate (IV).

 

EXTRACTION OF SULPHUR 

Sulphur is extracted from underground by Frasch process. A three concentric sulphur pump is driven down a hole dug to the sulphur bed. The solid sulphur is melted at 115oC by super – heated water at 170oC and 10atms. The molten sulphur is forced out by hot compressed air at 15atm. The molten sulphur is then continuously pumped out and allowed to solidify in a large tank. The sulphur obtained is 99.5% pure. 

Sulfur is extracted from its natural sources, such as pyrite, gypsum, and epsom salt, through a process called Frasch process. Here are the steps involved in the Frasch process:

1. Drilling: The first step in the Frasch process is drilling a hole into the ground to reach the sulfur deposit. The hole is typically several thousand feet deep.
2. Injection of hot water: Once the hole is drilled, hot water is injected into the deposit to melt the sulfur. The water is heated to a temperature of around 170°C and is under high pressure to prevent it from boiling.
3. Injection of compressed air: Compressed air is then injected into the deposit, which forces the melted sulfur to the surface through the hole. The sulfur is then collected in tanks and transported to a processing facility.
4. Purification: The collected sulfur may contain impurities, such as rocks and dirt. To purify the sulfur, it is melted and then filtered to remove any impurities. The purified sulfur is then solidified into blocks or pellets.
5. Storage and transportation: The final step is to store the sulfur in a dry, cool place until it is transported to its intended destination. Sulfur is often transported by truck, train, or ship to be used in various industries.

Here are some examples of how sulfur is used once it has been extracted:

1. Production of fertilizers: Sulfur is an essential component in the production of fertilizers like ammonium sulfate and superphosphate.
2. Production of chemicals: Sulfur is used in the production of various chemicals, such as sulfuric acid, which is used in the production of batteries and detergents.
3. Production of rubber: Sulfur is used in the vulcanization process of rubber to make it more durable and heat resistant.
4. Production of gunpowder: Sulfur is a key component in gunpowder, which is used in firearms and explosives.

These are just a few examples of how sulfur is used once it has been extracted. The Frasch process is a crucial method of obtaining this important element

Evaluation

1. What is the name of the process used to extract sulfur? a) Haber process b) Frasch process c) Solvay process d) Bayer process
2. At what temperature is the water injected in the Frasch process heated to? a) 50°C b) 100°C c) 170°C d) 200°C
3. What is injected into the sulfur deposit after the water in the Frasch process? a) Compressed air b) Nitrogen gas c) Carbon dioxide d) Helium gas
4. What is the purpose of injecting compressed air into the sulfur deposit during the Frasch process? a) To cool down the sulfur b) To prevent the sulfur from boiling c) To dissolve the sulfur d) To filter out impurities from the sulfur
5. What is the first step in the Frasch process? a) Cooling the sulfur deposit b) Filtering the sulfur c) Drilling a hole into the ground d) Purifying the sulfur
6. Which of the following is NOT a natural source of sulfur? a) Pyrite b) Gypsum c) Epsom salt d) Diamond
7. What is the final step in the extraction of sulfur? a) Cooling the sulfur b) Filtering the sulfur c) Purifying the sulfur d) Storing and transporting the sulfur
8. What is the most common form of sulfur used in fertilizers? a) Ammonium sulfate b) Sulfuric acid c) Sodium sulfide d) Calcium sulfide
9. Which of the following industries uses sulfur as a key component? a) Textile industry b) Automobile industry c) Chemical industry d) Food industry
10. What is sulfur used for in the production of rubber? a) To make it more brittle b) To make it more malleable c) To make it more durable and heat resistant d) To make it more elastic

ALLOTROPES OF SULPHUR 

Sulfur is a unique element that exhibits allotropy, which means that it can exist in different forms with different physical and chemical properties. Here are the three most common allotropes of sulfur:

1. Rhombic sulfur: This is the most stable and common allotrope of sulfur. It is yellow in color and forms needle-like crystals with a melting point of 112°C. Rhombic sulfur is insoluble in water, but soluble in organic solvents like carbon disulfide. It is also less reactive than the other allotropes of sulfur.
2. Monoclinic sulfur: This allotrope is less stable than rhombic sulfur and is formed by heating rhombic sulfur to a temperature between 96°C and 119°C. Monoclinic sulfur is reddish-brown in color and forms long, needle-like crystals. It has a melting point of 119°C and is more reactive than rhombic sulfur.
3. Amorphous sulfur: This is the least stable and least common allotrope of sulfur. It is formed by quickly cooling molten sulfur or by precipitating sulfur from a solution. Amorphous sulfur is yellow to brown in color and has a rubbery texture. It is soluble in carbon disulfide and other solvents and is highly reactive.

The properties of these allotropes of sulfur are due to the different arrangements of sulfur atoms in their crystal structures. The rhombic and monoclinic forms have a crystalline structure, while the amorphous form lacks a defined crystal structure.

Sulfur is also known to form other allotropes like cyclic S8 rings, catenated chains, and crown sulfur. These forms are less common and have unique properties, but they are not as extensively studied as the three primary allotropes mentioned above

The two main crystalline allotropes of sulphur are: 

1. Rhombic sulphur: A bright yellow octahedral crystalline solid. Each crystal is made up of S8 molecules. Rhombic sulphur is stable below 96oC. 
2. Monoclinic Sulphur: This is amber coloured solid sulphur consisting of needle shaped S8 crystal. Stable above 96oC. It easily reverts to Rhombic below 96oC. The transition temperature between Rhombic and Monoclinic is 96oC. 

 

Comparison of the Physical Properties of Rhombic and Monoclinic Sulphur

1. Rhombic Sulphur melts at 113oC;while monoclinic sulphur melts at 119oC.
2. Rhombic sulphur has bright yellow colour; while monoclinic sulphur has amber colour.
3. Rhombic sulphur has octahedral shape; while monoclinic sulphur is needle-like in shape.
4. Rhombic sulphur is translucent; while monoclinic is transparent.

 

Sulphur also exists as non – crystalline solid. These are 

1. Amorphous sulphur 
2. Plastic sulphur

Rhombic sulfur and monoclinic sulfur are two allotropes of sulfur that have distinct physical properties. Here is a comparison of their physical properties:

1. Color: Rhombic sulfur is yellow in color, while monoclinic sulfur is reddish-brown.
2. Crystal structure: Rhombic sulfur has a crystal structure that is characterized by needle-like crystals with a rhombic shape, while monoclinic sulfur has a crystal structure that is characterized by needle-like crystals with a monoclinic shape.
3. Density: Rhombic sulfur has a density of 2.07 g/cm³, while monoclinic sulfur has a density of 1.96 g/cm³.
4. Melting point: Rhombic sulfur has a melting point of 112.8°C, while monoclinic sulfur has a higher melting point of 119°C.
5. Stability: Rhombic sulfur is the most stable allotrope of sulfur and is less reactive than monoclinic sulfur. Monoclinic sulfur is less stable than rhombic sulfur and is more reactive.
6. Solubility: Rhombic sulfur is insoluble in water, but soluble in organic solvents like carbon disulfide. Monoclinic sulfur is also insoluble in water, but is more soluble in organic solvents than rhombic sulfur.
7. Optical properties: Rhombic sulfur is optically active and exhibits birefringence, while monoclinic sulfur is optically inactive

EVALUATION 

1. Briefly explain the Frasch process.
2. Name the two allotropes of sulphur and state their transition temperature.
3. What is the color of rhombic sulfur? a) Reddish-brown b) Yellow c) Green d) Blue
4. What is the color of monoclinic sulfur? a) Reddish-brown b) Yellow c) Green d) Blue
5. Which allotrope of sulfur is more stable? a) Rhombic sulfur b) Monoclinic sulfur c) They are equally stable d) Sulfur does not exhibit allotropy
6. Which allotrope of sulfur has a higher melting point? a) Rhombic sulfur b) Monoclinic sulfur c) They have the same melting point d) Sulfur does not melt
7. Which allotrope of sulfur is more soluble in organic solvents? a) Rhombic sulfur b) Monoclinic sulfur c) They are equally soluble d) Sulfur is not soluble in organic solvents
8. Which allotrope of sulfur has a higher density? a) Rhombic sulfur b) Monoclinic sulfur c) They have the same density d) Sulfur is not dense
9. Which allotrope of sulfur is more optically active? a) Rhombic sulfur b) Monoclinic sulfur c) They are equally optically active d) Sulfur is not optically active
10. Which allotrope of sulfur is more reactive? a) Rhombic sulfur b) Monoclinic sulfur c) They are equally reactive d) Sulfur is not reactive
11. Which allotrope of sulfur is characterized by needle-like crystals with a monoclinic shape? a) Rhombic sulfur b) Monoclinic sulfur c) They both have the same shape d) Sulfur does not form crystals
12. Which allotrope of sulfur is optically inactive? a) Rhombic sulfur b) Monoclinic sulfur c) They are both optically active d) Sulfur is not optically active

 

 

PHYSICAL PROPERTIES 

1. Sulphur is a yellow solid.
2. It is insoluble in water but soluble in toluene and carbon (IV) sulphide.
3. It is a poor – conductor of heat and electricity.
4. It melts at 119oC and boils at 444oC.
5. Appearance: Sulfur is a yellow solid. It can also exist in other colors, such as reddish-brown in the monoclinic form and brown in the amorphous form.
6. Solubility: Sulfur is insoluble in water, but it is soluble in organic solvents like toluene and carbon disulfide. This makes it useful in various industries, such as the production of rubber and fertilizers.
7. Electrical conductivity: Sulfur is a poor conductor of both heat and electricity. This property is important in applications where electrical conductivity is not desired, such as in insulating materials.
8. Melting and boiling points: Sulfur has a relatively low melting point of 119°C and a boiling point of 444°C. This makes it easy to melt and work with in various industrial processes, such as in the production of sulfuric acid and fertilizers

 

 

CHEMICAL PROPERTIES 

1. It reacts directly with metals to form sulphide (S2-)

Fe(s) + S(s) → FeS(s)

1. It reacts with excess oxygen to form sulphur (IV) oxide 

         O2(g)  +  S(s)   →  SO2(g)

1. It reacts with hydrogen to form hydrogen sulphide; 

                      H2(g)   +   S(s) → H2S(g)

1. It reacts with coke (carbon) to form carbon (IV) sulphide.

            C(s)  +    2S(s) → CS2(l)

1. Combustibility: Sulfur is combustible and burns with a blue flame to form sulfur dioxide gas.
2. Reactivity: Sulfur reacts with many elements, such as oxygen, halogens, and metals, to form various compounds.
3. Acidic properties: When sulfur reacts with oxygen, it forms sulfur dioxide, which dissolves in water to form sulfurous acid. Sulfur can also react with water to form sulfuric acid.
4. Oxidation state: Sulfur has six valence electrons and can have a range of oxidation states from -2 to +6 in its compounds.
5. Polymerization: Sulfur can undergo polymerization, which means it can combine with itself to form long chains or rings of sulfur atoms. These polymers of sulfur have unique properties and are used in various industrial applications

USES 

1. Used in manufacturing tetraoxosulphate (IV) acid 
2. Used in vulcanization of rubber 
3. Used as germicides 
4. Used in manufacturing bleaching agent 
5. Fertilizers: Sulfur is a key ingredient in the production of fertilizers, such as ammonium sulfate and superphosphate. These fertilizers help improve soil fertility and increase crop yields.
6. Chemical industry: Sulfur is used in the production of various chemicals, such as sulfuric acid, which is used in the production of batteries, detergents, and other industrial products.
7. Rubber industry: Sulfur is used in the vulcanization process of rubber to make it more durable and heat resistant. This process involves heating rubber with sulfur to create cross-links between the rubber molecules.
8. Food industry: Sulfur dioxide is used as a preservative in the food industry to prevent the growth of bacteria and fungi. It is commonly used in dried fruits, wine, and other processed foods.
9. Pharmaceuticals: Sulfur is used in the production of various pharmaceuticals, such as antibiotics and anti-inflammatory drugs. It also has medicinal properties and is used in traditional medicine to treat various ailments

 

 

GENERAL EVALUATION/REVISION

1. State THREE physical and chemical properties of sulphur.
2. Outline THREE differences between monoclinic and rhombic sulphur.
3. Descried the Frasch process for the extraction of sulphur.
4. State TWO differences between a conductor and an electrolyte.
5. List the steps involve in the treatment of water for municipal supply.
6. What color is sulfur? a) Red b) Blue c) Yellow d) Green
7. What is the melting point of sulfur? a) 50°C b) 100°C c) 119°C d) 200°C
8. Which of the following solvents is sulfur soluble in? a) Water b) Ethanol c) Carbon disulfide d) All of the above
9. What is the density of sulfur? a) 0.9 g/cm³ b) 1.8 g/cm³ c) 2.1 g/cm³ d) 3.6 g/cm³
10. What is the most stable allotrope of sulfur? a) Monoclinic sulfur b) Amorphous sulfur c) Rhombic sulfur d) Cyclic S8 sulfur
11. What is the chemical formula for sulfuric acid? a) H2SO3 b) H2SO4 c) H2S d) SO2
12. What is the primary use of sulfur in agriculture? a) Fertilizers b) Pesticides c) Herbicides d) Animal feed additives
13. What is the process called when sulfur combines with itself to form long chains or rings of sulfur atoms? a) Polymerization b) Oxidation c) Reduction d) Combustion
14. Which of the following is a common use of sulfur dioxide? a) Food preservative b) Fertilizer c) Rubber vulcanization d) Antibiotics
15. What is the chemical symbol for sulfur? a) S b) Sr c) Su d) Sl

 

 

READING ASSIGNMENT

New School Chemistry for Senior Secondary Schools by O. Y. Ababio (6th edition), page 381-384

 

WEEKEND ASSIGNMENT

SECTION A: Write the correct option ONLY

1. Sulphur is extracted by (a) Haber process (b) Frasch process (c) Solvay process (d) Contact process
2. Which of the following is a crystalline allotropes of sulphur (a) Monoclinic (b) Plastic (c) Amorphous (d) Colloidal
3. The density of rhombic sulphur is (a) 1.2 (b) 1.5 (c) 2.08 (d) 1.98
4. The shape of monoclinic sulphur is (a) needle shape (b) hexagonal (c) octahedral (d) tetrahedral
5. Sulphur is used for (a) making of cellulose (b) cooking rice (c) vulcanizing rubber (d) manufacturing glass
6. What is the primary use of sulfur in the production of fertilizers? a) To improve soil fertility b) To prevent pest infestation c) To increase crop yields d) To reduce soil acidity
7. What is the process called when sulfur is heated with rubber to make it more durable? a) Vulcanization b) Polymerization c) Combustion d) Oxidation
8. What is the common use of sulfur dioxide in the food industry? a) To prevent bacterial growth b) To enhance flavor c) To add color d) To increase shelf life
9. What is the primary use of sulfuric acid? a) To produce batteries b) To produce detergents c) To produce fertilizers d) To produce pharmaceuticals
10. What is the traditional use of sulfur in medicine? a) To treat skin conditions b) To treat respiratory conditions c) To treat digestive disorders d) To treat cardiovascular diseases
11. What is the process called when sulfur reacts with oxygen to form sulfur dioxide? a) Combustion b) Oxidation c) Reduction d) Polymerization
12. What is the primary use of sulfur in the rubber industry? a) To improve elasticity b) To prevent cracking c) To enhance color d) To reduce cost
13. What is the common use of sulfur in the production of gunpowder? a) To increase explosive power b) To reduce explosive power c) To improve stability d) To add color
14. What is the primary use of sulfur in the petroleum industry? a) To remove impurities b) To enhance fuel efficiency c) To increase viscosity d) To prevent corrosion
15. What is the primary use of sulfur in the production of matches? a) To produce friction b) To add color c) To enhance burning time d) To reduce toxicity

 

 

Lesson plan presentation for the topic of Sulfur:

Title: Introduction to Sulfur

 

Lesson Outline: I. Introduction (5 minutes)

• Greet the students and introduce the topic of sulfur.
• Explain the objectives and goals of the lesson.

II. Physical Properties of Sulfur (15 minutes)

• Define the physical properties of sulfur, such as appearance, solubility, melting and boiling points, and density.
• Give examples of each property.
• Use visual aids to illustrate the properties, such as pictures or diagrams.

III. Chemical Properties of Sulfur (15 minutes)

• Define the chemical properties of sulfur, such as combustibility, reactivity, acidic properties, oxidation state, and polymerization.
• Give examples of each property.
• Use visual aids to illustrate the properties, such as chemical equations or molecular models.

IV. Extraction and Production of Sulfur (10 minutes)

• Explain the extraction process of sulfur, such as the Frasch process and the Claus process.
• Discuss the various methods of producing sulfur, such as the refining of crude oil and the burning of sulfur-containing fuels.
• Use visual aids to illustrate the extraction and production processes, such as flowcharts or animations.

V. Industrial and Commercial Applications of Sulfur (15 minutes)

• Discuss the various industrial and commercial applications of sulfur, such as in fertilizers, chemicals, rubber, food preservatives, and pharmaceuticals.
• Give examples of each application.
• Use visual aids to illustrate the applications, such as product labels or advertisements.

VI. Conclusion and Review (10 minutes)

• Summarize the main points of the lesson.
• Ask students to recall and review the physical and chemical properties of sulfur, the extraction and production processes, and the industrial and commercial applications of sulfur.
• Answer any remaining questions or concerns.

Assessment:

• Quiz or worksheet on the physical and chemical properties of sulfur, the extraction and production processes, and the industrial and commercial applications of sulfur.

Homework:

• Research and report on a specific industrial or commercial application of sulfur, such as in the production of fertilizers or the manufacturing of rubber

Weekly Assessment /Test 

1. Sulfur is a __________ solid with a yellow color.
2. Sulfur is __________ in water but soluble in organic solvents like toluene and carbon disulfide.
3. Sulfur is a poor __________ of heat and electricity.
4. The melting point of sulfur is __________°C.
5. Sulfur has a density of __________ g/cm³.
6. The most stable allotrope of sulfur is __________ sulfur.
7. Sulfuric acid has a chemical formula of __________.
8. Sulfur is a key ingredient in the production of __________, which helps improve soil fertility and increase crop yields.
9. Sulfur dioxide is commonly used as a __________ in the food industry to prevent the growth of bacteria and fungi.
10. Sulfur can undergo __________, which means it can combine with itself to form long chains or rings of sulfur atoms
11. What is the primary color of sulfur? a) Red b) Blue c) Yellow d) Green
12. Which of the following solvents is sulfur soluble in? a) Water b) Ethanol c) Carbon disulfide d) All of the above
13. What is the melting point of sulfur? a) 50°C b) 100°C c) 119°C d) 200°C
14. What is the most stable allotrope of sulfur? a) Monoclinic sulfur b) Amorphous sulfur c) Rhombic sulfur d) Cyclic S8 sulfur
15. What is the chemical formula for sulfuric acid? a) H2SO3 b) H2SO4 c) H2S d) SO2
16. What is the primary use of sulfur in agriculture? a) Fertilizers b) Pesticides c) Herbicides d) Animal feed additives
17. What is the common use of sulfur dioxide in the food industry? a) To prevent bacterial growth b) To enhance flavor c) To add color d) To increase shelf life
18. What is the process called when sulfur is heated with rubber to make it more durable? a) Vulcanization b) Polymerization c) Combustion d) Oxidation
19. Which of the following is a common use of sulfur in the production of chemicals? a) To produce batteries b) To produce detergents c) To produce fertilizers d) To produce pharmaceuticals
20. What is the process called when sulfur reacts with oxygen to form sulfur dioxide? a) Combustion b) Oxidation c) Reduction d) Polymerization

 

SECTION B

1. Give three differences between rhombic sulphur and monoclinic sulphur
2. Briefly describe the extraction of sulphur
3. What are the physical properties of sulfur?
4. How is sulfur extracted from the ground?
5. What is the most stable allotrope of sulfur?
6. What is the chemical formula for sulfuric acid?
7. What are the industrial and commercial applications of sulfur?
8. How does sulfur react with oxygen to form sulfur dioxide?
9. What is the process called when sulfur combines with rubber to make it more durable?
10. What is the common use of sulfur dioxide in the food industry?
11. What is the primary use of sulfur in agriculture?
12. What is the process called when sulfur combines with itself to form long chains or rings of sulfur atoms?