Chlorine and Hydrogen Chloride — Explained

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1. I. Chlorine ($Cl_2$): The Greenish-Yellow Oxidizer
2. A. Conceptual Foundation:
3. B. Preparation of Chlorine:
4. C. Physical Properties:
5. D. Chemical Properties:
6. E. Uses of Chlorine:
7. F. Common Misconceptions about Chlorine:
8. II. Hydrogen Chloride (HCl): The Corrosive Gas and Acid
9. A. Conceptual Foundation:
10. B. Preparation of Hydrogen Chloride:
11. C. Physical Properties:
12. D. Chemical Properties:
13. E. Uses of Hydrogen Chloride/Hydrochloric Acid:
14. F. Common Misconceptions about Hydrogen Chloride:
15. G. NEET-Specific Angle:

Detailed Explanation

The study of Chlorine and Hydrogen Chloride is central to understanding the chemistry of Group 17 elements, the halogens. These two substances, an element and a compound respectively, showcase distinct yet interconnected chemical behaviors that are frequently tested in NEET UG.

I. Chlorine ($Cl_2$): The Greenish-Yellow Oxidizer

A. Conceptual Foundation:

Chlorine is the second element in Group 17, following fluorine. Its atomic number is 17, and its electronic configuration is $[Ne]3s^23p^5$. This configuration signifies that chlorine has seven valence electrons, making it highly eager to gain one electron to achieve a stable octet, resembling the noble gas argon.

This strong electron affinity is the driving force behind its high reactivity and its role as a potent oxidizing agent. Under standard conditions, chlorine exists as a diatomic molecule, $Cl_2$, held together by a strong covalent bond.

B. Preparation of Chlorine:

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Laboratory Preparation:

* **From $MnO_2$ and HCl:** The most common lab method involves heating manganese dioxide with concentrated hydrochloric acid.

$$MnO_2(s) + 4HCl(aq) \xrightarrow{\Delta} MnCl_2(aq) + Cl_2(g) + 2H_2O(l)$$

Here, $MnO_2$ acts as an oxidizing agent, oxidizing $HCl$ to $Cl_2$.

Other oxidizing agents like potassium permanganate ($KMnO_4$) or potassium dichromate ($K_2Cr_2O_7$) can also be used with $HCl$. * From Bleaching Powder: Chlorine can also be liberated by reacting bleaching powder with dilute acids.

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Industrial Preparation:

* Deacon's Process: This process involves the catalytic oxidation of hydrogen chloride gas by atmospheric oxygen in the presence of cuprous chloride ($CuCl_2$) as a catalyst at 723 K.

$$4HCl(g) + O_2(g) \xrightarrow{CuCl_2, 723 K} 2Cl_2(g) + 2H_2O(g)$$

This is an environmentally friendly method as it utilizes HCl, often a byproduct of other industrial processes.

* Electrolytic Process (Castner-Kellner Cell): This is the most significant industrial method, involving the electrolysis of concentrated aqueous sodium chloride solution (brine). This process is also known as the chlor-alkali process because it produces chlorine, sodium hydroxide (an alkali), and hydrogen gas.

* At anode (oxidation): $2Cl^-(aq) \rightarrow Cl_2(g) + 2e^-$ * At cathode (reduction): $2H_2O(l) + 2e^- \rightarrow H_2(g) + 2OH^-(aq)$ * Overall reaction: $2NaCl(aq) + 2H_2O(l) \xrightarrow{\text{electrolysis}} 2NaOH(aq) + Cl_2(g) + H_2(g)$ A mercury cathode is often used to prevent the reaction of $Cl_2$ with $NaOH$.

C. Physical Properties:

Chlorine is a greenish-yellow gas with a pungent and suffocating odor. It is about 2.5 times heavier than air. It can be easily liquefied into a greenish-yellow liquid at room temperature under pressure or by cooling. It is sparingly soluble in water, forming chlorine water, which is a mixture of $HCl$ and $HOCl$ (hypochlorous acid).

D. Chemical Properties:

Chlorine is highly reactive due to its strong tendency to gain an electron. Its common oxidation states are -1, +1, +3, +5, and +7, though -1 is most stable.

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Reaction with Metals: — Reacts with almost all metals to form metal chlorides.

$$2Na(s) + Cl_2(g) \rightarrow 2NaCl(s)$$

$$2Fe(s) + 3Cl_2(g) \rightarrow 2FeCl_3(s) \text{ (ferric chloride, not ferrous)}$$

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Reaction with Non-metals: — Reacts with non-metals like hydrogen, phosphorus, and sulfur.

$$H_2(g) + Cl_2(g) \xrightarrow{\text{diffused sunlight}} 2HCl(g)$$

$$P_4(s) + 6Cl_2(g) \rightarrow 4PCl_3(l) \text{ (limited chlorine)}$$

$$P_4(s) + 10Cl_2(g) \rightarrow 4PCl_5(s) \text{ (excess chlorine)}$$

$$S_8(s) + 4Cl_2(g) \rightarrow 4S_2Cl_2(l)$$

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Reaction with Hydrogen: — Forms hydrogen chloride.

$$H_2(g) + Cl_2(g) \rightarrow 2HCl(g)$$

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Reaction with Water (Chlorine Water): — Forms hydrochloric acid and hypochlorous acid. Hypochlorous acid is unstable and decomposes to release nascent oxygen, which is responsible for its oxidizing and bleaching properties.

$$Cl_2(g) + H_2O(l) \rightleftharpoons HCl(aq) + HOCl(aq)$$

$$HOCl(aq) \rightarrow HCl(aq) + [O]$$

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Reaction with Alkalis: — The products depend on the temperature and concentration of the alkali.

* Cold, dilute NaOH:

$$Cl_2(g) + 2NaOH(aq) \rightarrow NaCl(aq) + NaOCl(aq) + H_2O(l)$$

(Sodium hypochlorite, used in household bleach) * Hot, concentrated NaOH:

$$3Cl_2(g) + 6NaOH(aq) \rightarrow 5NaCl(aq) + NaClO_3(aq) + 3H_2O(l)$$

(Sodium chlorate)

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Oxidizing and Bleaching Properties: — Chlorine is a strong oxidizing agent. Its bleaching action is due to the formation of nascent oxygen from hypochlorous acid, which oxidizes colored substances to colorless ones. This bleaching is permanent.

$$Cl_2 + H_2O \rightarrow HCl + HOCl$$

$$HOCl \rightarrow HCl + [O]$$

$$Colored,matter + [O] \rightarrow Colorless,matter$$

* NEET Angle: Remember that chlorine's bleaching action requires moisture. Dry chlorine does not bleach.

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Reaction with Ammonia:

* Excess Ammonia: Forms nitrogen and ammonium chloride.

$$8NH_3(g) + 3Cl_2(g) \rightarrow N_2(g) + 6NH_4Cl(s)$$

* Excess Chlorine: Forms nitrogen trichloride (an explosive substance) and HCl.

$$NH_3(g) + 3Cl_2(g) \rightarrow NCl_3(l) + 3HCl(g)$$

E. Uses of Chlorine:

Disinfectant for water purification (drinking water, swimming pools).
Bleaching agent for textiles (cotton, linen) and paper pulp.
Manufacture of various organic compounds (PVC, chloroform, carbon tetrachloride, DDT, refrigerants).
Production of inorganic compounds (bleaching powder, hydrochloric acid).
Extraction of metals like gold and platinum.

F. Common Misconceptions about Chlorine:

Dry chlorine bleaches: — Incorrect. Moisture is essential for the formation of HOCl, which is the actual bleaching agent.
Chlorine is a reducing agent: — Incorrect. It is a strong oxidizing agent, gaining electrons.
Reaction with iron always forms $FeCl_2$: — Incorrect. With chlorine, iron forms $FeCl_3$ because chlorine is a strong enough oxidizing agent to oxidize $Fe^{2+}$ to $Fe^{3+}$.

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II. Hydrogen Chloride (HCl): The Corrosive Gas and Acid

A. Conceptual Foundation:

Hydrogen chloride is a diatomic molecule formed by a covalent bond between hydrogen and chlorine atoms. Due to the significant electronegativity difference between H (2.20) and Cl (3.16), the bond is highly polar, with chlorine carrying a partial negative charge ($\delta^-$) and hydrogen a partial positive charge ($\delta^+$).

In its gaseous state, it is a molecular compound. When dissolved in water, it ionizes almost completely, donating a proton ($H^+$) to water to form hydronium ions ($H_3O^+$) and chloride ions ($Cl^-$), thus acting as a strong acid.

This aqueous solution is known as hydrochloric acid.

B. Preparation of Hydrogen Chloride:

1
Laboratory Preparation:

* **From NaCl and $H_2SO_4$:** This is the standard laboratory method. Sodium chloride is reacted with concentrated sulfuric acid. * At low temperature (below 200°C):

$$NaCl(s) + H_2SO_4(conc) \xrightarrow{<200^\circ C} NaHSO_4(s) + HCl(g)$$

* At high temperature (above 200°C):

$$NaHSO_4(s) + NaCl(s) \xrightarrow{>200^\circ C} Na_2SO_4(s) + HCl(g)$$

The overall reaction at higher temperatures is:

$$2NaCl(s) + H_2SO_4(conc) \xrightarrow{\Delta} Na_2SO_4(s) + 2HCl(g)$$

The $HCl$ gas produced is dried by passing it through concentrated $H_2SO_4$.

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Industrial Preparation:

* Direct Synthesis: By directly combining hydrogen and chlorine gases, often byproducts of the chlor-alkali process.

$$H_2(g) + Cl_2(g) \xrightarrow{\text{combustion}} 2HCl(g)$$

* As a Byproduct: HCl is also produced as a byproduct in many organic chlorination reactions, for example, in the production of vinyl chloride.

C. Physical Properties:

Hydrogen chloride is a colorless gas with a pungent odor. It is extremely soluble in water, forming hydrochloric acid. One volume of water can dissolve about 450 volumes of HCl gas at room temperature. This high solubility can be demonstrated by the 'fountain experiment.' It fumes in moist air due to the formation of tiny droplets of hydrochloric acid. It boils at -85°C and freezes at -114°C.

D. Chemical Properties:

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Acidic Nature: — HCl is a strong monoprotic acid. In aqueous solution, it completely ionizes.

$$HCl(aq) + H_2O(l) \rightarrow H_3O^+(aq) + Cl^-(aq)$$

* Reaction with Metals: Reacts with metals above hydrogen in the reactivity series to produce hydrogen gas and metal chlorides.

$$Zn(s) + 2HCl(aq) \rightarrow ZnCl_2(aq) + H_2(g)$$

* Reaction with Metal Oxides/Hydroxides (Bases): Forms salt and water (neutralization reaction).

$$CuO(s) + 2HCl(aq) \rightarrow CuCl_2(aq) + H_2O(l)$$

$$NaOH(aq) + HCl(aq) \rightarrow NaCl(aq) + H_2O(l)$$

* Reaction with Carbonates and Bicarbonates: Produces carbon dioxide gas, salt, and water.

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Reaction with Ammonia: — Forms dense white fumes of ammonium chloride.

$$NH_3(g) + HCl(g) \rightarrow NH_4Cl(s)$$

This reaction is often used as a test for HCl gas.

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Formation of Aqua Regia: — A mixture of concentrated nitric acid and concentrated hydrochloric acid in a 1:3 molar ratio is called aqua regia (royal water). It is capable of dissolving noble metals like gold and platinum, which are otherwise unreactive to individual acids.

$$Au(s) + 4HCl(aq) + HNO_3(aq) \rightarrow H[AuCl_4](aq) + NO(g) + 2H_2O(l)$$

The nascent chlorine and nitrosyl chloride formed are responsible for its dissolving power.

$$HNO_3 + 3HCl \rightarrow NOCl + 2H_2O + 2[Cl]$$

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Reducing Properties: — While HCl itself is not a strong reducing agent, the chloride ion ($Cl^-$) can be oxidized by strong oxidizing agents to $Cl_2$. This is evident in the lab preparation of chlorine using $MnO_2$ and $HCl$.

E. Uses of Hydrogen Chloride/Hydrochloric Acid:

Pickling of steel (removing rust and scale before galvanizing or tinning).
Manufacture of glucose from starch.
Production of chlorides, e.g., $NH_4Cl$.
In the textile, leather, and dye industries.
As a laboratory reagent.
In the food industry for processing.

F. Common Misconceptions about Hydrogen Chloride:

HCl gas is an acid: — Incorrect. Anhydrous HCl gas is covalent and does not show acidic properties (e.g., does not turn blue litmus red). It is only acidic in the presence of water, where it ionizes to produce $H^+$ ions.
Aqua Regia is just a mixture of acids: — While true, its unique property of dissolving noble metals comes from the synergistic action of both acids, leading to the formation of nascent chlorine and complex ions, not just the individual acidic properties.

G. NEET-Specific Angle:

For NEET, focus on the balanced chemical equations for preparation methods (Deacon's, Electrolytic, Lab methods for both). Understand the conditions (temperature, catalyst) for these reactions. Pay close attention to the oxidizing and bleaching properties of chlorine, and the acidic reactions of HCl (with metals, carbonates, bases).

The concept of aqua regia and its specific ratio is also a frequent question. Distinguish between HCl gas and hydrochloric acid. Understand the different products formed when chlorine reacts with cold/dilute vs.

hot/concentrated alkalis. Oxidation states of chlorine in various compounds ($NaOCl$, $NaClO_3$) are also important.

Often confused with

Side-by-side differences the NEET paper likes to test.

Chlorine and Hydrogen Chloride vs Chlorine (Cl2) vs. Hydrogen Chloride (HCl)

Aspect	Chlorine and Hydrogen Chloride	Chlorine (Cl2) vs. Hydrogen Chloride (HCl)
Nature	Element (diatomic molecule)	Compound (covalent molecule)
Physical State (STP)	Greenish-yellow gas	Colorless gas
Odor	Pungent, suffocating	Pungent, irritating
Reactivity	Highly reactive, strong oxidizing agent	Gas is less reactive; aqueous solution (HCl acid) is highly reactive
Acidic/Basic Nature	Neither acidic nor basic (but forms acids in water)	Anhydrous gas is neutral; aqueous solution is a strong acid
Bleaching Property	Acts as a bleaching agent (in presence of moisture)	Does not exhibit bleaching properties
Role in Redox	Primarily an oxidizing agent (Cl oxidation state 0 to -1, +1, +3, +5, +7)	Chloride ion ($Cl^-$) can be oxidized to $Cl_2$ by strong oxidizers

Chlorine ($Cl_2$) is a reactive elemental gas, characterized by its greenish-yellow color and strong oxidizing power, crucial for bleaching and disinfection. Hydrogen chloride (HCl), on the other hand, is a colorless gaseous compound that, upon dissolving in water, forms hydrochloric acid – a potent strong acid.

While chlorine's reactivity stems from its desire to gain an electron, HCl's acidic nature arises from its ability to donate a proton in aqueous solution. Their distinct chemical roles, from elemental reactivity to compound acidity, are fundamental to inorganic chemistry.

Why it is tested: For NEET, understanding these differences is crucial for predicting reaction products, identifying correct chemical tests, and distinguishing between the properties of an element and its hydride. Questions often test the acidic nature of HCl (only in water), the bleaching action of $Cl_2$ (requires moisture), and their respective roles in redox reactions and industrial processes.

Questions students ask

6 answered on this topic.

Why does chlorine act as a bleaching agent, and what is the role of moisture?

Chlorine's bleaching action is primarily due to its ability to form hypochlorous acid (HOCl) in the presence of moisture. When chlorine dissolves in water, it undergoes hydrolysis to produce HCl and HOCl.

Hypochlorous acid is unstable and readily decomposes to yield nascent oxygen ($[O]$). This nascent oxygen is a powerful oxidizing agent that reacts with colored organic substances, oxidizing them into colorless compounds.

Therefore, moisture is absolutely essential for chlorine to exhibit its bleaching properties; dry chlorine gas does not bleach.

Explain the difference in products when chlorine reacts with cold, dilute NaOH versus hot, concentrated NaOH.

The reaction of chlorine with sodium hydroxide is a disproportionation reaction, where chlorine is simultaneously oxidized and reduced. With cold, dilute NaOH, chlorine forms sodium chloride (NaCl) and sodium hypochlorite (NaOCl).

Here, chlorine is in the -1 and +1 oxidation states, respectively. However, with hot, concentrated NaOH, chlorine disproportionates further, forming sodium chloride (NaCl) and sodium chlorate ($NaClO_3$).

In this case, chlorine is in the -1 and +5 oxidation states. This difference highlights the temperature and concentration dependence of redox reactions involving halogens.

What is aqua regia, and why is it capable of dissolving noble metals like gold?

Aqua regia, meaning 'royal water,' is a highly corrosive mixture of concentrated nitric acid ($HNO_3$) and concentrated hydrochloric acid ($HCl$) in a 1:3 molar ratio. Neither acid alone can dissolve noble metals like gold or platinum.

However, in aqua regia, nitric acid acts as a powerful oxidizing agent, oxidizing the metal, while hydrochloric acid provides chloride ions that react with the metal ions to form stable soluble complex anions (e.

g., tetrachloroaurate(III) ion, $[AuCl_4]^-$). This removal of metal ions from solution shifts the equilibrium, allowing more metal to dissolve. The nascent chlorine and nitrosyl chloride formed also contribute to its strong oxidizing power.

Is HCl gas acidic? How does it differ from hydrochloric acid?

Anhydrous HCl gas is not acidic in nature. It is a covalent molecule and does not dissociate to produce $H^+$ ions in the absence of water. For example, dry HCl gas does not turn blue litmus paper red.

However, when HCl gas dissolves in water, it ionizes completely to form hydronium ions ($H_3O^+$) and chloride ions ($Cl^-$), making the aqueous solution (hydrochloric acid) strongly acidic. The presence of water is crucial for HCl to exhibit its acidic properties, as water acts as a proton acceptor.

Describe the industrial preparation of chlorine using the Deacon's process.

The Deacon's process is an industrial method for producing chlorine by the catalytic oxidation of hydrogen chloride gas. In this process, a mixture of hydrogen chloride gas and atmospheric oxygen is passed over a catalyst, typically cuprous chloride ($CuCl_2$), at a high temperature of about 723 K.

The reaction is $4HCl(g) + O_2(g) \xrightarrow{CuCl_2, 723 K} 2Cl_2(g) + 2H_2O(g)$. This method is significant because it utilizes HCl, which is often a byproduct of other industrial processes, making it an economically and environmentally viable route for chlorine production.

Why is chlorine used for water purification?

Chlorine is widely used for water purification due to its potent disinfectant properties. When chlorine is added to water, it reacts to form hypochlorous acid (HOCl) and hydrochloric acid (HCl). Hypochlorous acid is a powerful oxidizing agent that can penetrate the cell walls of bacteria, viruses, and other microorganisms, disrupting their cellular processes and effectively killing them.

This action makes water safe for consumption by eliminating harmful pathogens. The residual chlorine also helps prevent recontamination in the distribution system.