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Zinc Chloride is a chemical compound, composed of zinc and chlorine. It is a colourless liquid and it exhibits hygroscopic qualities, i.e., it attracts and captures the water molecule present in the environment. It is mildly corrosive towards metals. It is an ionic salt that is essential for the synthesis of protein, fats, and cholesterol. It may cause burns to the eyes, skin, and mucous membranes.
There are nine different crystalline forms of zinc chloride which are currently known. These hydrates of Zinc chloride are highly soluble in water.
Zinc Chloride Structure
A molecule of zinc chloride has an ionic bond between the zinc cation (Zn2+) and the chloride anions (Cl-).
Zinc chloride which is a colourless liquid is responsible for causing burns to the mucous membrane, eyes or skin, and also corrosive to metals. The molecular formula for zinc chloride is ZNCL2 or CL2ZN.
Zinc chloride is also known as zinc dichloride, butter of zinc, zinc(II)chloride. The molecular weight of the zinc is 136.3.
Zinc chloride is mildly corrosive to metals and causes burns to the eyes, mucous membrane and skin.
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Zinc chloride is a compound that can be prepared by a direct reaction, or by evaporating the aqueous solution formed in various reactions. Zinc chloride has nine different crystalline forms that are currently known. These hydrates of zinc chloride are mainly colourless or white in colour and all of them have a high solubility rate in water. Zinc chloride attracts the water molecules in its environment and therefore it can be said that it has hygroscopic qualities.
Physical Properties of Zinc Chloride
Zinc Chloride formula: ZnCl2.
Molecular Weight of Zinc Chloride: 136.315 gms/ mole
The boiling point of Zinc Chloride is - 732 °C
The Melting point of Zinc Chloride is - 290 °C
Its density is 2.907.
It forms white, odourless, very deliquescent granules.
Molten zinc chloride is viscous in nature and has a relatively low electrical conductivity.
Chemical Properties of Zinc Chloride
When ZnCl2 is dissolved in water, the solution becomes acidic. The pH of this aqueous solution of zinc chloride having a concentration equals 6M is approx 1.
After heating, the hydrated form of zinc chloride loses water and small quantities of ZnCl(OH) are obtained.
Zinc Chloride is soluble in water, glycerol, ether, and alcohol.
Zinc chloride is deliquescent in nature, so it should be protected from sources of moisture (water vapour).
Preparation of Zinc Chloride
The reaction between Zinc and hydrogen chloride gives an anhydrous form of zinc chloride. The chemical equation is given below:
Zn + 2HCl → ZnCl2 + H2
Hydrochloric acid reacts with zinc sulphide to form zinc chloride and hydrogen sulphide. The chemical equation is given by:
ZnS + 2HCl → ZnCl2 + H2S
There are some impurities present in zinc chloride samples due to the process of hydrolysis. The purification of chloride is simple due to its oxidation state Zn as +2. Purification can be done by recrystallization from hot dioxane. The purification of anhydrous zinc chloride can be done through sublimation with HCl gas, followed by the subsequent heating of the sublimate to around 400 °C with dry nitrogen gas. It can also be purified by treating it with thionyl chloride.
Uses of Zinc Chloride
Zinc Chloride finds its application in different industries including pharmaceuticals, health care, paper manufacturing industry. Chemical products are also made from zinc chloride.
Organic Product Synthesis - Organic products are synthesized in the laboratory for the preparation of Lewis acid reaction and various other organic reactions. It can be used as a catalyst in organic processes.
Metallurgical Industry - It is used as a flux in the soldering process and cleaning agent. It is also used in the manufacturing of magnesia cement.
Chemical Industry - Zinc chloride finds its application in the manufacture of various dyes, intermediate chemicals, and solvents like ethyl acetate. It is found in antiseptic mouthwash products.
Printing and Textile Industry - About 64% of zinc chloride in water can be used to dissolve silk, cellulose, and starch.
Petroleum - Zinc chloride is used as an emulsion breaker, which can separate oil from water.
Zinc chloride is used in dry cells as an electrolyte.
Other Uses - It is used as a condensing agent, disinfecting purposes, dehydrating agent, wood preservative, deodorant, and disinfectant.
A mixture of zinc oxide and hexachloroethane can be used in smoke grenades. While igniting, these compounds react with each other to form a smoke of zinc chloride, which serves as a smokescreen.
The Lucas reagent used is a solution of anhydrous zinc chloride and concentrated hydrochloric acid. This reagent is useful in preparing alkyl chlorides.
Zinc chloride is used as an alternative medicine for the cause of dead tissue, to cure skin cancers.
Zinc and Its Doses
Infants and Children: When taken by mouth properly in the prescribed quantities, zinc is likely Healthy. When used in high concentrations, zinc is Dangerous.
Pregnancy and Breast-Feeding: Zinc is likely safe when used in the prescribed daily quantities for most pregnant and breast-feeding women (RDA). Zinc, however, is potentially unsafe when used by breast-feeding women at high doses and likely unsafe when used by pregnant women at high doses. Not more than 40 mg of zinc should be taken per day by pregnant women over the age of 18, no more than 34 mg per day should be taken by pregnant women aged 14 to 18 years. No more than 40 mg of zinc per day should be taken by breastfeeding women over the age of 18, no more than 34 mg per day should be taken by breastfeeding women aged 14 to 18.
Alcoholism: Excessive, long-term consumption of alcohol is related to low absorption of zinc in the body.
Kidney Disease: The risk of having kidney disease rises with low zinc in the diet. People with hemodialysis kidney disease are also at risk for zinc deficiency and may need zinc supplements.
Vegetarianism: Vegetarian diets are often associated with lower absorption of zinc. This form of diet is also seen as a risk factor for the depletion of zinc. But in the long term, the body adapts. Zinc absorption and zinc loss elimination are getting stronger.
Conclusion:
You can learn more about the affair between Zinc and Chlorine through this wonderfully crafted article. You can use them from an exam point of you or to enrich your knowledge.
FAQs on What Happened when Zinc Met Chlorine?
1. What happens when zinc reacts with chlorine?
When zinc metal (Zn) reacts with chlorine gas (Cl₂), they undergo a synthesis reaction to form zinc chloride (ZnCl₂). This reaction is typically exothermic, releasing heat, and results in the formation of a white, crystalline solid. The balanced chemical equation for this reaction is: Zn(s) + Cl₂(g) → ZnCl₂(s).
2. What is the chemical formula for the product formed when zinc reacts with chlorine?
The product formed is zinc chloride, and its chemical formula is ZnCl₂. This formula is derived from the ionic charges of the elements. Zinc typically forms a cation with a 2+ charge (Zn²⁺), while chlorine forms an anion with a 1- charge (Cl⁻). To create a neutral compound, two chloride ions are needed to balance the charge of one zinc ion.
3. What type of chemical bond is formed between zinc and chlorine, and why?
An ionic bond is formed between zinc and chlorine. This occurs because zinc is a metal that readily loses its two valence electrons to achieve a stable electron configuration, forming a positively charged ion (Zn²⁺). Chlorine, a non-metal, readily gains one electron to achieve stability, forming a negatively charged ion (Cl⁻). The strong electrostatic force of attraction between the oppositely charged Zn²⁺ and Cl⁻ ions constitutes the ionic bond.
4. Describe the key chemical properties of zinc chloride.
Zinc chloride exhibits several key chemical properties:
- Appearance: It is a white, odourless, crystalline solid.
- Hygroscopic Nature: It is deliquescent, meaning it has a strong tendency to absorb moisture from the surrounding air.
- Solubility: It is highly soluble in water. It is also soluble in other polar solvents like alcohol, ether, and glycerol.
- Acidity in Solution: When dissolved in water, zinc chloride forms an acidic solution due to the hydrolysis of the Zn²⁺ ion.
5. What is the appearance of zinc chloride and what colour is its aqueous solution?
In its pure, solid form, zinc chloride is a white crystalline powder. When it is dissolved in water to form an aqueous solution, the resulting solution is colourless. The zinc ion (Zn²⁺) does not have partially filled d-orbitals, which are typically required for a transition metal compound to exhibit colour.
6. Why is zinc chloride considered a Lewis acid?
Zinc chloride is classified as a Lewis acid because the central zinc atom in the ZnCl₂ molecule is electron-deficient and has vacant orbitals. This allows it to act as an electron pair acceptor. It can readily accept a lone pair of electrons from a Lewis base (an electron pair donor), such as ammonia (NH₃) or water (H₂O), to form a stable coordination complex.
7. What are some important real-world applications of zinc chloride?
Zinc chloride has several important industrial and commercial uses, including:
- Soldering Flux: It is used to clean metal surfaces by dissolving the layer of oxides, ensuring a stronger solder joint.
- Wood Preservation: It acts as a fungicide, protecting wood from rot and decay.
- Textile Industry: It is used as a mordant to help dyes adhere to fabrics and as a fire-proofing agent.
- Chemical Synthesis: It serves as a powerful dehydrating agent and a catalyst in many organic reactions.
- Disinfectants: Due to its antiseptic properties, it is an ingredient in some types of mouthwash.
8. How does the structure of solid zinc chloride differ from its gaseous state?
The structure of zinc chloride changes significantly with its physical state. In the solid state, it typically has a polymeric structure where each zinc atom is tetrahedrally coordinated to four bridging chlorine atoms. In the gaseous state, at high temperatures, the polymer breaks down, and it exists as simple, discrete, and linear ZnCl₂ molecules with a more covalent character.
9. What safety precautions are necessary when handling zinc chloride?
Zinc chloride is a corrosive and hazardous substance that requires careful handling. Key safety precautions include:
- Wearing appropriate personal protective equipment (PPE), such as safety goggles, gloves, and a lab coat, to prevent skin and eye contact.
- Working in a well-ventilated area or under a chemical fume hood to avoid inhaling its dust.
- Storing it in a dry, cool, and tightly sealed container because it is highly hygroscopic and will absorb moisture from the air.
- Avoiding contact with water unless intended, as the dissolution process can be highly exothermic.
10. Explain why a solution of zinc chloride in water is acidic.
A solution of zinc chloride in water is acidic due to a process called salt hydrolysis. When ZnCl₂ dissolves, it dissociates into Zn²⁺ and Cl⁻ ions. The small, highly charged Zn²⁺ ion strongly attracts the oxygen atoms of water molecules, polarising the O-H bonds. This polarisation weakens the bonds enough for a water molecule coordinated to the zinc ion to release a proton (H⁺) into the solution. This increase in the concentration of H⁺ ions lowers the pH, making the solution acidic.
