Zn(No2)2 Chemical Name

The chemical name for the compound V2S3 is vanadium(III) sulfide.

The chemical formula for the compound zinc nitrite is Zn(NO2)2. This means that in one molecule of the compound, there is one atom of zinc (Zn) and two ions of nitrite (NO2-). The nitrite ion consists of one nitrogen atom (N) and two oxygen atoms (O), and carries a negative charge.

It is important to note that the subscript 2 in the formula indicates that there are two nitrite ions present in the compound. Therefore, the overall charge of the compound must be neutral, which means that the zinc ion has a charge of +2 to balance out the two -1 charges from the nitrite ions.

In terms of structure, zinc nitrite is a coordination compound, meaning that the zinc ion is surrounded by ligands (in this case, the nitrite ions). The geometry of the compound is octahedral, with the zinc ion at the center and the nitrite ions arranged around it in a symmetrical manner.

Overall, understanding the chemical formula and structure of zinc nitrite is crucial for accurately predicting its properties and behavior in various chemical reactions.

The compound C6H12O6 is a hexose sugar, specifically glucose.

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The molar mass of the compound Zn(NO2)2 is calculated as follows:

- The atomic weight of Zn (zinc) is 65.38 g/mol.

- The molecular weight of NO2 (nitrite ion) is calculated by adding the atomic weights of nitrogen and oxygen, which are 14.01 g/mol and 16 g/mol respectively. Thus, the molecular weight of NO2 is 14.01 + 2(16) = 46.01 g/mol.

- Since there are two NO2 groups in the compound, the total molecular weight is 65.38 + 2(46.01) = 157.4 g/mol.

Therefore, the molar mass of Zn(NO2)2 is 157.4 g/mol.

The oxidation state of Zn in Zn(NO2)2 is +2. The nitrite ion (NO2-) has an overall charge of -1, and since there are two NO2- ions present in the compound, the total charge contributed by them is -2. Since Zn(NO2)2 is a neutral compound, the sum of the oxidation states of all the atoms in it must be equal to zero. Therefore, the oxidation state of Zn must be +2 to balance out the -2 charge contributed by the NO2- ions.

Zinc nitrite, Zn(NO2)2, is not a stable compound and therefore does not have a well-defined melting point. However, if you meant to ask about zinc nitrate, Zn(NO3)2, the melting point is approximately 262 °C. It's important to clarify the compound in question as they are different compounds with different properties.

The solubility of Zn(NO2)2 in water depends on various factors such as temperature, pressure, and the presence of other dissolved species. At room temperature (25°C), the solubility of Zn(NO2)2 in water is approximately 4 g/L. However, this value may vary depending on the specific conditions under which it is measured. Additionally, the solubility of Zn(NO2)2 can be influenced by the pH of the solution, with higher pH levels resulting in higher solubility due to the formation of Zn(OH)2. Overall, the solubility of Zn(NO2)2 can be described as moderately soluble in water.

Zn(NO2)2 is a white crystalline powder that can pose potential hazards if mishandled. It is primarily hazardous if ingested, inhaled or comes into contact with the skin or eyes.

When inhaled, Zn(NO2)2 can cause irritation to the respiratory tract, leading to coughing, shortness of breath and chest pain. If ingested, it can cause abdominal pain, vomiting, diarrhoea and nausea.

In case of skin contact, Zn(NO2)2 can cause irritation, redness, and itching. Eye contact may result in eye irritation, tearing, and redness.

Additionally, Zn(NO2)2 can be harmful to aquatic life and the environment if not disposed of properly. It should be handled with care to prevent accidental spills or releases into the environment.

Proper personal protective equipment (PPE) such as gloves, goggles, and respirators should be worn when working with Zn(NO2)2 to minimize the risk of exposure. Waste material containing Zn(NO2)2 should be properly stored and disposed of according to local regulations.

Zn(NO2)2, also known as zinc nitrite, is a chemical compound that has various applications. Some of the common uses of Zn(NO2)2 are:

1. Corrosion inhibitor: Zn(NO2)2 is added to coatings and paints to prevent corrosion of metal surfaces.

2. Pyrotechnics: Zn(NO2)2 is used in pyrotechnic compositions to produce green flames.

3. Chemical synthesis: Zn(NO2)2 is used as a reagent in some chemical synthesis reactions.

4. UV stabilizer: Zn(NO2)2 is used in plastics and polymers as a UV stabilizer to prevent degradation by UV radiation.

5. Antimicrobial agent: Zn(NO2)2 has been shown to have antimicrobial properties and is being investigated as a potential agent for use in disinfectants and preservatives.

It is important to note that the specific application and use of Zn(NO2)2 may depend on its purity, concentration, and other factors, and should be carefully evaluated before use.

Zn(NO2)2 can be synthesized by the reaction of zinc oxide or zinc metal with nitric acid in the presence of a suitable reducing agent such as sulfur dioxide or hydrazine. The reaction typically proceeds at elevated temperatures and the resulting product is isolated by filtration, washing, and drying. Alternatively, Zn(NO2)2 can also be prepared by the reaction of zinc chloride with sodium nitrite in aqueous solution, followed by precipitation and purification steps. Care should be taken to ensure that all reactants are pure and properly proportioned, and that the reaction conditions are carefully controlled to achieve the desired product.

Zn(NO2)2 is a white crystalline solid with a powdery or granular appearance. It is odorless and has a molecular weight of 213.41 g/mol. The compound is slightly soluble in water and soluble in ethanol and acetone. When heated, Zn(NO2)2 decomposes to form nitrogen dioxide (NO2) gas and zinc oxide (ZnO).

The density of Zn(NO2)2 depends on its physical state (solid, liquid, or gas) and temperature. At room temperature and pressure, Zn(NO2)2 is a solid with a density of approximately 2.882 g/cm3. However, if the compound is in a different physical state or at a different temperature, its density may vary accordingly.