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Magnesium Iodide formula, also referred to as Diiodomagnesium formula, is the name for the chemical compounds with the formula Mgl2 and its various hydrates Mgl2x. This chemical compound has various hydrates which are typical ionic halides, and which do not dissolve in water. The chemical compound is generally used in internal medicine, apart from this, it also has some utilization in the preparation of compounds for organic synthesis. Moreover, diiodomagnesium is a crystalline solid white in colour and has no smell. It can be synthesized by using magnesium oxide, magnesium carbonate, and magnesium hydroxide and treating them with hydroiodic acid.
Key Takeaways: Magnesium iodide, diiodomagnesium formula, preparation of Magnesium iodide, properties of Magnesium iodide.
Read More: Number of Moles Formula
About Magnesium Iodide
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Magnesium iodide formula is also referred to as diiodomagnesium formula. It is an inorganic salt that can be easily found in seawater. This compound has various hydrates which are typical ionic halides and is generally insoluble in water.
Diiodomagnesium is a crystalline solid compound that is white in color and is odorless. It can be synthesized or made by using magnesium oxide, magnesium carbonate, and magnesium hydroxide and treating them with hydroiodic acid.
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Magnesium Iodide Formula and Structure
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The chemical and molecular formula of Magnesium Iodide is MgI2.
Additionally, it exists in various forms like MgI2 (anhydrous), MgI2. 6H2O (hexahydrate), MgI2..8 H2O (octahydrate).
The molar mass of the given form is:
Anhydrous Magnesium iodide = 278.1139 g/mol
Hexahydrate Magnesium iodide = 386.2005 g/mol
Octahydrate Magnesium iodide = 422.236 g/mol.
Structurally, the Magnesium cation i.e., Mg2+ reacts with the Iodine anion i.e., I2+. It exists in hexagonal crystal structure for anhydrous form, monoclinic structure for hexahydrate form, and an orthorhombic structure for octahydrate form.
Occurrence of Magnesium Iodide
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As earlier mentioned, in nature, it occurs in sea salt and is a common inorganic salt. Generally, it is immediately available in most volumes, sub-micron, nano-powder, and high purity. Scientists prepare them in the labs.
Preparation of Magnesium Iodide
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Magnesium iodide can be prepared from Magnesium oxide and magnesium carbonate with the treatment by hydroiodic acid. The reaction can be represented as,
MgO + HI → MgI2 + H2O
MgCO3 + 2HI → MgI2 + CO2 +H2O
Reactions of Magnesium Iodide
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It is stable under the high heat under the hydrogen atmosphere. But at the normal temperature or we can say at room temperature, it decomposes in the air by turning brown from the release of elemental iodine. Moreover, if we heat magnesium iodide in the air, it completely decomposes off.
An alternative method of preparation of Magnesium iodide (MgI2) is by mixing of the powdered elemental iodine with the magnesium metal to obtain anhydrous Magnesium Iodide but the condition from the reaction is that it should be conducted in the anhydrous atmosphere for which diethyl ether is a solvent can be used.
Read More: Dalton’s atomic theory
Properties of Magnesium Iodide (MgI2)
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It generally appears as a white crystalline solid and does not contain any odor. The densities are different for its different forms as an anhydrous solid its density is 4.43 g/cm3, the density of the hexahydrate solid is 2.353 g/cm3, and lastly, the density of the octahydrate solid is 2.098 g/cm3.
Additionally, it is soluble in alcohol, ammonia, and ether. The solubility of Magnesium iodide in water is very high. MgI2 has a heat capacity of 74 J/mol K. Although MgI2 is very stable but it can react in the presence of moisture and air. Magnesium iodide has a melting point of 637°C and if the temperature is above this it starts to decompose.
Uses of Magnesium Iodide
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It is generally used in internal medicines. Also, it finds some commercial uses as we can use it to prepare compounds for organic synthesis.
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Health and Safety Hazards Associated with Magnesium Iodide
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When coming in contact with the eyes and skin it results in irritation. Also, it can also lead to irritation if it is ingested or inhaled. The substance is toxic to the thyroid as it has iodine in it. Repeated and prolonged exposure to the MgI2 can cause serious damage to the organs. In some people, its ingestion can cause vomiting as well as breathing problem. Moreover, its long exposure to the eyes can even cause blindness.
Things to Remember
- The formula for Magnesium Iodide is MgI2.
- Magnesium iodide remains stable under high heat.
- At room temperature, it decomposes in the air by turning brown due to the release of elemental iodine.
- Method for preparation of Magnesium iodide (MgI2) is by mixing of the powdered elemental iodine with the magnesium metal to obtain anhydrous Magnesium Iodide.
- In nature, it occurs in sea salt and is a common inorganic salt.
- It is very hazardous if it comes in contact with eyes and skin so be careful while handling MgI2 in the laboratory.
Read More: Gay-Lussac’s Law
Sample Questions
Ques. Explain the method for the preparation of Magnesium Iodide? (3 Marks)
Ans. Magnesium Iodide (MgI2) can be prepared by the reactions of magnesium hydroxide with the hydroiodic acid:
Mg(OH)2 + 2HI → MgI2 + 2H2O
When Magnesium hydroxide reacts with the hydroiodic acid it will result in the formation of Magnesium iodide and water.
Ques. Give the properties of Magnesium iodide. (4 Marks)
Ans.
| Chemical formula | MgI2 (anhydrous) |
| Molecular weight | Anhydrous Magnesium iodide = 278.1139 g/mol Hexahydrate Magnesium iodide = 386.2005 g/mol Octahydrate Magnesium iodide = 422.236 g/mol. |
| Density | 4.43 g/cm3 (anhydrous) 2.353 g/cm3 (hexahydrate) 2.098 g/cm3 (octahydrate) |
| Appears as | Crystalline solid and white in colour |
| 637°C |
Ques. Give the health hazard associated with the Magnesium Iodide. (3 Marks)
Ans.
- When coming in contact with the eyes and skin it results in irritation. Also, it can also lead to irritation if it is ingested or inhaled.
- The substance is toxic to the thyroid as it has iodine in it.
- Repeated and prolonged exposure to the MgI2 can cause serious damage to the organs.
- Its ingestion can cause vomiting as well as breathing problem. Moreover, it long exposure to the eyes can even cause blindness.
Ques. Write about the occurrence of Magnesium Iodide. (2 Marks)
Ans. Magnesium iodide is colorless or white crystalline in nature and is generally odorless. In nature, it occurs in sea salt and is a common inorganic salt. Generally, it is immediately available in most volumes, sub-micron, nano-powder, and high purity. Scientists prepare them in the labs.
Ques. write about the solubility of Magnesium iodide. (3 Marks)
Ans. Its solubility in various solvent are given below:
| Alcohol | soluble |
| Ammonia | soluble |
| Ether | soluble |
| Water | Highly soluble |
Ques. Write the reaction of Magnesium oxide and Magnesium carbonate when treated with hydroiodic acid? (3 Marks)
Ans. The reaction between Magnesium oxide and magnesium carbonate with the treatment by hydroiodic acid can yield Magnesium Iodide. The reaction can be represented as:
MgO + HI → MgI2 + H2O
MgCO3 + 2HI → MgI2 + CO2 +H2O
Here, MgO = Magnesium oxide
MgCO3 = Magnesium carbonate
HI = Hydroiodic acid
CO2= carbon dioxide
H2O = water.
Ques. What is the formula of Magnesium Iodide? Explain the concept behind having such a formula. (3 Marks)
Ans. As evident from the name, the given compound comprises metal magnesium and normal iodine. And it is known that any compound containing a metal and non-metal is an ionic compound so we have to take into account the charges of each of the elements present in the compound.
Magnesium is a metal and belong to group 1 with symbol Mg thus possesses +2 cationic charge while iodine which is a non metal having symbol I possesses -1 charge.
Now, according to the rule by exchanging the charges we will get MgI2 as magnesium iodide formula.
Ques. Write a balanced chemical reaction for the given compound and identify the type of reaction in this case. (3 Marks)
(a) Magnesium + Iodine → Magnesium iodide
Ans. firstly we have to write the formula of given compound so that we can easily write the reaction of the given compound.
Magnesium= Mg2+
Iodine = I-1
Now, reaction can be represented as follows:
2Mg + I2 → 2MgI2
To balance the above reaction we have to add 2 on the both side.
It is the type of combination reaction.
Ques. Write about the uses of Magnesium iodide? (2 marks)
Ans. It is generally used in internal medicines.
It finds some commercial uses as we can use it to prepare compounds for organic synthesis. It is also used as a reagent and intermediates in pharmaceuticals.
Ques. Is Magnesium iodide stable? (2 marks)
Ans. It is stable under the high heat under the hydrogen atmosphere. But at the normal temperature or at room temperature, it decomposes in the air by turning brown from the release of elemental iodine. Further, if we heat magnesium iodide in the air, it completely decomposes off.
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