HomeSS 2ChemistryCHLORINE AND OTHER HALOGENS

CHLORINE AND OTHER HALOGENS

Subject :Chemistry

Term : Second Term

Week :Week 5

Topic :

CHLORINE AND OTHER HALOGENS

 

 

 

Objectives:

  • Students will be able to describe the physical and chemical properties of chlorine and hydrogen chloride.
  • Students will be able to explain the laboratory and industrial preparation of chlorine and hydrogen chloride.
  • Students will be able to identify the uses and hazards associated with chlorine and hydrogen chloride

 

Materials:

  • Whiteboard and markers
  • Handout with notes on the topic
  • Visual aids, such as pictures or diagrams, of chlorine and hydrogen chloride and their uses

 

Content

CHLORINE AND OTHER HALOGENS

TOPIC: CHLORINE AND OTHER HALOGENS

CONTENT

  • Electronic Configuration of Halogens
  • Physical and Chemical Properties of Halogens.
  • Laboratory and Industrial Preparation of Chlorine.
  • Preparation, Properties and Uses.
  • Compound of Chlorine: Hydrogen Chloride.
  • Test for Chlorides

Halogens are a group of elements in the periodic table that includes fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). They are located in Group 17 or Group VIIA of the periodic table.

Halogens are highly reactive nonmetals that have seven electrons in their outermost energy level (except for astatine, which has only six). This makes them very reactive and they readily form compounds with other elements.

Here are some examples of halogens and their uses:

  1. Chlorine: Chlorine is a greenish-yellow gas that is used to purify water in swimming pools and drinking water supplies. It is also used to make many household cleaning products.
  2. Fluorine: Fluorine is a pale yellow gas that is used in the production of many industrial chemicals, including refrigerants and plastics.
  3. Bromine: Bromine is a reddish-brown liquid that is used in flame retardants, pesticides, and pharmaceuticals.
  4. Iodine: Iodine is a bluish-black solid that is used in the production of disinfectants and pharmaceuticals. It is also an important nutrient for human health, as it is necessary for the production of thyroid hormones.
  5. Astatine: Astatine is a radioactive element that is not found in nature. It has few uses outside of scientific research.

 

Halogens are a group of highly reactive nonmetals that have seven electrons in their outermost energy level. They are used in a wide variety of industrial and scientific applications, from water purification to the production of pharmaceuticals

 

ELECTRONIC CONFIGURATION OF HALOGENS

 

Halogens are a group of elements in the periodic table that includes fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). They are located in Group 17 or Group VIIA of the periodic table.

The electronic configuration of halogens can be determined by knowing their atomic number. Each element has a unique number of protons, which determines the number of electrons in the atom. The electronic configuration of halogens is based on the distribution of electrons in the energy levels of their atoms.

Here are the electronic configurations of halogens:

  1. Fluorine (F): The atomic number of fluorine is 9, which means it has 9 electrons. The electronic configuration of fluorine is 1s2 2s2 2p5. This means that there are two electrons in the first energy level (1s), two electrons in the second energy level (2s), and five electrons in the third energy level (2p).
  2. Chlorine (Cl): The atomic number of chlorine is 17, which means it has 17 electrons. The electronic configuration of chlorine is 1s2 2s2 2p6 3s2 3p5. This means that there are two electrons in the first energy level (1s), two electrons in the second energy level (2s), six electrons in the third energy level (2p), two electrons in the fourth energy level (3s), and five electrons in the fifth energy level (3p).
  3. Bromine (Br): The atomic number of bromine is 35, which means it has 35 electrons. The electronic configuration of bromine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5. This means that there are two electrons in the first energy level (1s), two electrons in the second energy level (2s), six electrons in the third energy level (2p), two electrons in the fourth energy level (3s), six electrons in the fifth energy level (3p), ten electrons in the sixth energy level (3d), and five electrons in the seventh energy level (4p).
  4. Iodine (I): The atomic number of iodine is 53, which means it has 53 electrons. The electronic configuration of iodine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5. This means that there are two electrons in the first energy level (1s), two electrons in the second energy level (2s), six electrons in the third energy level (2p), two electrons in the fourth energy level (3s), six electrons in the fifth energy level (3p), ten electrons in the sixth energy level (3d), two electrons in the seventh energy level (4s), ten electrons in the eighth energy level (4d), and five electrons in the ninth energy level (5p).
  5. Astatine (At): The atomic number of astatine is 85, which means it has 85 electrons. The electronic configuration of astatine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p5

 

 

HALOGENS and ELECTRONIC CONFIGURATION OF HALOGENS

  1. Which of the following elements is not a halogen? A) Fluorine B) Chlorine C) Nitrogen D) Bromine E) Iodine
  2. Halogens are located in which group of the periodic table? A) Group 1 B) Group 2 C) Group 7 D) Group 8 E) Group 18
  3. How many electrons are in the outermost energy level of a halogen? A) 1 B) 2 C) 6 D) 7 E) 8
  4. What is the electronic configuration of fluorine? A) 1s2 2s2 2p6 3s2 3p5 B) 1s2 2s2 2p6 C) 1s2 2s2 2p5 D) 1s2 2s2 2p6 3s2 3p6 E) 1s2 2s2 2p6 3s2 3p3
  5. What is the electronic configuration of chlorine? A) 1s2 2s2 2p6 3s2 3p5 B) 1s2 2s2 2p6 C) 1s2 2s2 2p5 D) 1s2 2s2 2p6 3s2 3p6 E) 1s2 2s2 2p6 3s2 3p3
  6. What is the electronic configuration of bromine? A) 1s2 2s2 2p6 3s2 3p5 B) 1s2 2s2 2p6 C) 1s2 2s2 2p5 D) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 E) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2
  7. Which halogen is a bluish-black solid that is used in the production of disinfectants and pharmaceuticals? A) Fluorine B) Chlorine C) Bromine D) Iodine E) Astatine
  8. What is the atomic number of astatine? A) 53 B) 17 C) 9 D) 85 E) 35
  9. How many electrons are in the third energy level of a halogen? A) 2 B) 6 C) 8 D) 10 E) 12
  10. What is the maximum number of electrons that can be in the fourth energy level of a halogen? A) 2 B) 6 C) 8 D) 10 E) 14

PHYSICAL PROPERTIES OF THE HALOGENS

  1. State at room temperature: All halogens are nonmetals and exist in different states at room temperature. Fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.
  2. Color: Halogens have distinct colors. Fluorine is pale yellow, chlorine is greenish-yellow, bromine is reddish-brown, and iodine is bluish-black.
  3. Odor: Halogens have strong odors. Fluorine has a pungent smell, chlorine smells like bleach, bromine has a strong, irritating odor, and iodine has a distinct odor.
  4. Solubility: Halogens have different solubilities in water. Fluorine and chlorine are highly soluble in water, while bromine and iodine are only slightly soluble.
  5. Density: The density of halogens increases as you move down the group. For example, the density of fluorine is 1.7 g/L, while the density of iodine is 4.9 g/L.
  6. Melting and boiling points: The melting and boiling points of halogens also increase as you move down the group. For example, the melting point of fluorine is -219°C, while the melting point of iodine is 113°C.
  7. Reactivity: Halogens are highly reactive and readily form compounds with other elements. Their reactivity decreases as you move down the group.
  8. Toxicity: Halogens are toxic in their pure form, especially in the case of fluorine and chlorine gases. They should be handled with care and proper safety precautions.
  9. Electronegativity: Halogens are highly electronegative, which means they have a strong attraction for electrons. Fluorine is the most electronegative element on the periodic table.
  10. Ionization energy: The ionization energy of halogens increases as you move up the group, which means it becomes harder to remove an electron from the atom. This is due to the increased nuclear charge of the atom as you move up the group

CHEMICAL PROPERTIES OF THE HALOGENS

  1. Reactivity: The halogens are highly reactive and readily form compounds with other elements. They react with most metals to form salts, and with nonmetals to form covalent compounds.
  2. Electronegativity: Halogens are highly electronegative and have a strong attraction for electrons. This makes them highly reactive and able to form bonds with other elements.
  3. Oxidation states: Halogens can have a variety of oxidation states, ranging from -1 to +7. In most of their compounds, halogens have a negative oxidation state.
  4. Halides: Halogens can form salts with metals, known as halides. Halides are generally soluble in water, and their solubility decreases as the size of the halogen increases.
  5. Reaction with hydrogen: Halogens react with hydrogen to form hydrogen halides, such as hydrochloric acid (HCl) and hydrofluoric acid (HF).
  6. Reaction with oxygen: Halogens react with oxygen to form oxides, such as chlorine dioxide (ClO2) and iodine pentoxide (I2O5).
  7. Reaction with water: Halogens react with water to form acids, such as hydrochloric acid (HCl) and hypochlorous acid (HOCl).
  8. Halogen displacement: Halogens can displace less reactive halogens from their compounds. For example, chlorine can displace iodine from potassium iodide to form potassium chloride and free iodine.
  9. Bleaching action: Halogens have a bleaching action and are used as disinfectants and bleaches in many industrial and household products.
  10. Reaction with metals: Halogens react with many metals to form metal halides, which can be used in a variety of applications such as catalysis and electrolysis

Evaluation

  1. Which of the following is not a halogen? A) Chlorine B) Fluorine C) Carbon D) Iodine E) Bromine
  2. Which halogen is a gas at room temperature? A) Chlorine B) Fluorine C) Bromine D) Iodine E) Astatine
  3. Which of the following halogens is the most electronegative element on the periodic table? A) Chlorine B) Fluorine C) Bromine D) Iodine E) Astatine
  4. Which halogen is a reddish-brown liquid at room temperature? A) Chlorine B) Fluorine C) Bromine D) Iodine E) Astatine
  5. What is the general trend in the boiling points of the halogens as you move down the group? A) Boiling points increase B) Boiling points decrease C) Boiling points remain the same D) Boiling points increase, then decrease E) Boiling points decrease, then increase
  6. Which of the following is a common use of halogens? A) As a fertilizer B) As a sweetener C) As a lubricant D) As a disinfectant E) As a fuel
  7. What is the general trend in the reactivity of the halogens as you move down the group? A) Reactivity increases B) Reactivity decreases C) Reactivity remains the same D) Reactivity increases, then decreases E) Reactivity decreases, then increases
  8. What is the general trend in the ionization energy of the halogens as you move down the group? A) Ionization energy decreases B) Ionization energy increases C) Ionization energy remains the same D) Ionization energy increases, then decreases E) Ionization energy decreases, then increases
  9. Which halogen is commonly used as a disinfectant and bleach? A) Chlorine B) Fluorine C) Bromine D) Iodine E) Astatine
  10. What is the general trend in the solubility of halides as you move down the group? A) Solubility increases B) Solubility decreases C) Solubility remains the same D) Solubility increases, then decreases E) Solubility decreases, then increases

EVALUATION

  1. Write the electronic configuration of the following atoms/ions: Cl, F-, Br.
  2. Give three physical properties of the halogens

 

Answers:

 

Electronic configuration of the following atoms/ions:

Chlorine (Cl): 1s2 2s2 2p6 3s2 3p5

Fluoride ion (F-): 1s2 2s2 2p6

Bromine (Br): 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

Three physical properties of the halogens:

State at room temperature: Halogens exist in different states at room temperature. Fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.

Color: Halogens have distinct colors. Fluorine is pale yellow, chlorine is greenish-yellow, bromine is reddish-brown, and iodine is bluish-black.

Solubility: Halogens have different solubilities in water. Fluorine and chlorine are highly soluble in water, while bromine and iodine are only slightly soluble

 

CHLORINE

Chlorine is a chemical element with the symbol Cl and atomic number 17. It is one of the halogens and is found in the periodic table in group 17. Chlorine is a highly reactive, greenish-yellow gas with a pungent odor. It is the second-lightest halogen after fluorine and forms a diatomic molecule with itself.

Chlorine has a wide range of applications, such as in the production of PVC plastic, pesticides, and water purification. It is also used as a disinfectant in swimming pools and in the production of paper products. Chlorine is highly toxic in its pure form and can cause severe burns and respiratory problems.

In terms of its chemical properties, chlorine is highly electronegative and reactive, making it able to form compounds with many other elements. It reacts with metals to form chlorides, and with nonmetals to form covalent compounds. Chlorine also reacts with hydrogen to form hydrochloric acid (HCl) and with oxygen to form chlorine dioxide (ClO2).

Chlorine was first discovered in 1774 by Swedish chemist Carl Wilhelm Scheele. It was later used as a weapon in World War I, causing severe injuries and fatalities. Today, it is mainly used for industrial purposes and water treatment

 

LABORATORY PREPARATION OF CHLORINE

Chlorine can be prepared in the laboratory by the reaction of hydrochloric acid (HCl) with an oxidizing agent. One common method of preparation involves the reaction of hydrochloric acid with manganese dioxide (MnO2):

  1. Mix hydrochloric acid (HCl) and manganese dioxide (MnO2) in a round-bottomed flask.
  2. Heat the mixture gently under reflux (with a condenser on top of the flask) to initiate the reaction.

2HCl + MnO2 → MnCl2 + Cl2 + H2O

  1. Collect the chlorine gas by upward displacement of air in a gas jar. Since chlorine is denser than air, it will displace the air in the jar and collect at the bottom.
  2. Chlorine gas is yellow-green in color and has a pungent odor. It is highly toxic and should be handled with care in a well-ventilated laboratory with proper safety equipment.

Other oxidizing agents that can be used to prepare chlorine in the laboratory include potassium permanganate (KMnO4) and sodium hypochlorite (NaClO). The reaction conditions and procedures may vary depending on the oxidizing agent used.

It should be noted that the preparation of chlorine in the laboratory is not recommended for inexperienced chemists and should only be carried out under the supervision of a qualified teacher or laboratory professional

 

 

INDUSTRIAL PREPARATION OF CHLORINE

Chlorine is an important industrial chemical that is widely used in many industries, such as the production of PVC plastic, bleach, and water treatment. There are several methods for the industrial preparation of chlorine, including:

  1. Chlor-alkali process: The chlor-alkali process involves the electrolysis of a brine solution (sodium chloride in water) using a diaphragm cell or membrane cell. Chlorine gas is produced at the anode while hydrogen gas and caustic soda (sodium hydroxide) are produced at the cathode.
  2. Deacon process: The Deacon process involves the oxidation of hydrogen chloride (HCl) using a catalyst, usually copper chloride (CuCl2). The reaction takes place at high temperatures and produces chlorine gas and water.

4HCl + O2 → 2Cl2 + 2H2O

  1. Weldon process: The Weldon process involves the reaction of manganese dioxide (MnO2) with hydrochloric acid (HCl) to produce chlorine gas and manganese chloride (MnCl2). The manganese chloride is then reacted with lime (Ca(OH)2) to regenerate the manganese dioxide.

4HCl + MnO2 → MnCl2 + Cl2 + 2H2O MnCl2 + Ca(OH)2 → MnO2 + CaCl2 + 2H2O

  1. Dow process: The Dow process involves the electrolysis of a brine solution using a mercury cathode. Chlorine gas is produced at the anode and reacts with the mercury to form mercury(II) chloride, which is then oxidized to regenerate the mercury.

2NaCl + 2H2O → Cl2 + H2 + 2NaOH

These industrial methods for the preparation of chlorine are widely used due to their efficiency and large-scale production capabilities. However, they must be carried out with care and proper safety precautions due to the toxicity and hazardous nature of chlorine gas

 

 

Evaluation

  1. What is the chemical formula of hydrochloric acid? A) HCl B) Cl2 C) NaCl D) H2SO4 E) HNO3
  2. What is the oxidizing agent commonly used to prepare chlorine in the laboratory? A) Potassium permanganate B) Manganese sulfate C) Sodium chloride D) Calcium carbonate E) Sodium hypochlorite
  3. Which of the following is not a method for the industrial preparation of chlorine? A) Haber process B) Chlor-alkali process C) Deacon process D) Weldon process E) Dow process
  4. What is the source of chlorine in the chlor-alkali process? A) Sodium hydroxide B) Hydrogen chloride C) Potassium permanganate D) Calcium carbonate E) Sodium chloride
  5. Which of the following is not a product of the chlor-alkali process? A) Chlorine gas B) Hydrogen gas C) Sodium hydroxide D) Calcium chloride E) All of the above are products of the chlor-alkali process
  6. What is the function of the catalyst in the Deacon process? A) To produce chlorine gas B) To produce hydrogen gas C) To oxidize hydrogen chloride D) To reduce oxygen E) To produce caustic soda
  7. Which of the following is not a step in the Weldon process? A) Reaction of manganese dioxide with hydrochloric acid B) Reaction of manganese chloride with lime C) Electrolysis of brine solution D) Collection of chlorine gas E) All of the above are steps in the Weldon process
  8. What is the product of the reaction between manganese dioxide and hydrochloric acid? A) Chlorine gas B) Hydrogen gas C) Manganese chloride D) Water E) Sodium hydroxide
  9. What is the product of the reaction between manganese chloride and lime? A) Chlorine gas B) Hydrogen gas C) Manganese dioxide D) Calcium chloride E) Sodium hydroxide
  10. Which of the following is a hazard associated with the preparation of chlorine in the laboratory or industry? A) Fire hazard B) Toxicity C) Explosion hazard D) All of the above E) None of the above

 

Review Questions

  1. What is the common method for the laboratory preparation of chlorine?
  2. What is the common oxidizing agent used in the laboratory preparation of chlorine?
  3. What is the source of chlorine in the chlor-alkali process?
  4. What are the products of the chlor-alkali process?
  5. What is the function of the catalyst in the Deacon process?
  6. What is the function of manganese dioxide in the Weldon process?
  7. What is the product of the reaction between manganese chloride and lime in the Weldon process?
  8. What is the main hazard associated with the preparation of chlorine in the laboratory or industry?
  9. How is chlorine commonly used in industry?
  10. What are some safety precautions that must be taken when working with chlorine gas?

 

Four physical properties of chlorine are:

  1. Chlorine is a greenish-yellow gas with a pungent odor.
  2. Chlorine is highly reactive and can react explosively with certain substances.
  3. Chlorine is denser than air and can accumulate in low-lying areas.
  4. Chlorine gas is toxic and can cause severe respiratory irritation and damage.

Five chemical properties of chlorine, along with their balanced equations, are:

  1. Chlorine reacts with metals to form metal chlorides: 2Na + Cl2 → 2NaCl
  2. Chlorine reacts with nonmetals to form covalent compounds: H2 + Cl2 → 2HCl
  3. Chlorine reacts with hydrogen to form hydrochloric acid: H2 + Cl2 → 2HCl
  4. Chlorine reacts with water to form hypochlorous acid and hydrochloric acid: Cl2 + H2O → HOCl + HCl
  5. Chlorine reacts with organic compounds, such as hydrocarbons, to form chlorinated organic compounds: CH4 + Cl2 → CH3Cl + HCl

It should be noted that chlorine is a highly reactive and potentially hazardous chemical, and these reactions should only be performed by trained professionals with proper safety equipment and precautions

COMPOUNDS OF CHLORINE

HYDROGEN CHLORIDE

Compounds of Chlorine: Chlorine forms compounds with a wide range of elements, such as metals, nonmetals, and metalloids. Some examples of chlorine compounds include sodium chloride (NaCl), hydrogen chloride (HCl), chlorine dioxide (ClO2), and chloroform (CHCl3). Chlorine compounds are widely used in various industries, such as in the production of PVC plastic, bleach, and pesticides.

Hydrogen Chloride: Hydrogen chloride (HCl) is a covalent compound composed of hydrogen and chlorine. It is a colorless gas with a pungent odor and is highly soluble in water, forming hydrochloric acid. Hydrogen chloride is widely used in various industries, such as in the production of PVC plastic, pharmaceuticals, and electronics.

Hydrogen chloride can be prepared in the laboratory by the reaction of hydrochloric acid with a reducing agent, such as zinc or iron:

2HCl + Zn → ZnCl2 + H2

In the industrial production of hydrogen chloride, it is produced by the reaction of chlorine gas with hydrogen gas in the presence of a catalyst, such as activated carbon or platinum:

H2 + Cl2 → 2HCl

Hydrogen chloride is highly corrosive and can cause severe burns and respiratory irritation. It should be handled with care and proper safety precautions should be taken when working with it

 

Hydrogen chloride (marine-acid gas) exists as a gas at room temperature. It dissolves in water to form hydrochloric acid. It occurs in traces in the air as industrial by-product and is considered as air pollutant; but it can be easily washed down as acid rain since it is very

soluble in water.

 

It is true that hydrogen chloride exists as a gas at room temperature and is highly soluble in water, forming hydrochloric acid. Hydrogen chloride can be found in small amounts in the atmosphere as a result of industrial processes and can contribute to acid rain. However, the solubility of hydrogen chloride in water also means that it can be easily washed down and diluted in the environment, reducing its impact. It is important to properly regulate industrial processes to minimize the release of hydrogen chloride into the environment and prevent its harmful effects on human health and the environment

 

LABORATORY PREPARATION OF HYDROGEN CHLORIDE

Hydrogen chloride (HCl) can be prepared in the laboratory by the reaction of hydrochloric acid (HCl) with a reducing agent, such as zinc or iron:

  1. Place hydrochloric acid in a round-bottomed flask.
  2. Add a small amount of zinc or iron filings to the hydrochloric acid.
  3. Heat the mixture gently under reflux (with a condenser on top of the flask) to initiate the reaction.

2HCl + Zn → ZnCl2 + H2

  1. Collect the hydrogen gas by upward displacement of air in a gas jar. Since hydrogen is lighter than air, it will rise and collect at the top of the jar.
  2. Bubble the hydrogen gas through water to dissolve the hydrogen chloride and form hydrochloric acid.

H2 + Cl2 → 2HCl

  1. Hydrogen chloride gas is highly corrosive and should be handled with care in a well-ventilated laboratory with proper safety equipment.

It should be noted that the preparation of hydrogen chloride gas in the laboratory should only be performed by experienced chemists and with proper safety precautions

The gas is prepared by the action of hot concentrated H2SO4 on any soluble chloride. Example 2NaCl(s) + H2SO4(aq) → Na2SO4(aq) + 2HCl(g) Note: NaHSO4 is first formed at a lower temperature and later at higher temperature HCl gas is formed. The gas is dried by passing it through concentrated H2SO4 in another flask and collected.

 

Hydrogen chloride gas can also be prepared by the reaction of hot concentrated sulfuric acid (H2SO4) with a soluble chloride, such as sodium chloride (NaCl). The reaction proceeds in two steps, with sodium bisulfate (NaHSO4) being formed first at a lower temperature, followed by the formation of hydrogen chloride gas at a higher temperature:

2NaCl(s) + H2SO4(aq) → Na2SO4(aq) + 2HCl(g)

To collect the hydrogen chloride gas, it can be dried by passing it through concentrated sulfuric acid in another flask and then collected. It is important to handle hydrogen chloride gas with care due to its highly corrosive and toxic nature, and proper safety precautions should be taken when working with it.

 

Lesson plan presentation for the topic

“Chlorine and Hydrogen Chloride”:

Topic: Chlorine and Hydrogen Chloride

Grade level: Senior Secondary School 2

Introduction (10 minutes):

  • Introduce the topic of chlorine and hydrogen chloride, and ask students what they already know about these substances.
  • Briefly discuss the importance of chlorine and hydrogen chloride in various industries, such as water treatment, plastics, and pharmaceuticals.

Body (50 minutes):

  • Present the physical and chemical properties of chlorine and hydrogen chloride, including their electronic configurations, melting and boiling points, reactivity, and toxicity.
  • Discuss the laboratory and industrial preparation of chlorine and hydrogen chloride, including the reaction equations and methods used.
  • Identify the uses of chlorine and hydrogen chloride in various industries, such as water treatment, plastics, and pharmaceuticals.
  • Highlight the hazards associated with chlorine and hydrogen chloride and the importance of proper handling and safety precautions.

Conclusion (10 minutes):

  • Recap the key points discussed in the lesson.
  • Ask students if they have any questions or would like to discuss any aspects of the topic further.
  • Distribute handouts with notes on the topic for students to review and study.

Assessment:

  • Administer a short quiz or worksheet to test students’ understanding of the properties, preparation, and uses of chlorine and hydrogen chloride.
  • Observe and evaluate students’ participation and engagement during the lesson

Weekly Assessment /Test 

  1. Chlorine is a highly reactive ___________ element with the atomic number 17.
  2. The electronic configuration of chlorine is ___________, indicating that it has seven valence electrons.
  3. Hydrogen chloride is a ___________ compound composed of hydrogen and chlorine.
  4. Hydrogen chloride gas dissolves readily in ___________ to form hydrochloric acid.
  5. Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with a reducing agent, such as ___________ or iron filings.
  6. In the industrial production of hydrogen chloride, it is produced by the reaction of chlorine gas with hydrogen gas in the presence of a ___________ catalyst.
  7. Chlorine gas is widely used in various industries, such as in the production of PVC plastic, ___________, and pesticides.
  8. Hydrogen chloride gas is highly ___________ and can cause severe burns and respiratory irritation.
  9. Chlorine gas is a ___________ irritant and can cause severe respiratory damage and even death.
  10. Hydrogen chloride gas can be prepared in the laboratory by the reaction of hot concentrated sulfuric acid with a soluble chloride, such as ___________
  11. What is the atomic number of chlorine?
  12. What is the electronic configuration of chlorine?
  13. What is hydrogen chloride and how is it formed?
  14. What is the product of dissolving hydrogen chloride gas in water?
  15. How can chlorine gas be prepared in the laboratory?
  16. How is hydrogen chloride produced in the industrial process?
  17. What are some common uses of chlorine gas?
  18. What are the hazards associated with hydrogen chloride gas?
  19. What are the hazards associated with chlorine gas?
  20. How can hydrogen chloride gas be prepared in the laboratory?

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