What is Ammonium NH4+?
The ammonium ion (NH4+) is a positively charged polyatomic ion consisting of one nitrogen atom and four hydrogen atoms. It is commonly found in fertilizers and organic compounds.
| IUPAC Name | Azanium |
| Molecular Formula | NH4+ |
| CAS Number | 14798-03-9 |
| Synonyms | Ammonium cation, Tetrahydridonitrogen(1+), Aminonium, Azanium, Nitrogen hydride cation, Hydronitrogen, Nitrogen ion |
| InChI | InChI=1S/H3N/h1H3/p+1 |
Note: The InChI is for the ammonium ion in its simplest form, with only one hydrogen ionized. The actual InChI may vary depending on the chemical environment of the ammonium ion.
Ammonium formula
The formula for the ammonium ion is NH4+. It is a polyatomic cation that consists of one nitrogen atom and four hydrogen atoms. The ammonium ion is formed by the protonation of ammonia (NH3) with a hydrogen ion (H+). The ammonium ion is a common cation in inorganic and organic compounds, including fertilizers, pharmaceuticals, and explosives.
Ammonium Cation
Ammonium cation, also known as NH4+, is a positively charged polyatomic ion composed of one nitrogen atom and four hydrogen atoms. It is formed when ammonia (NH3) accepts a proton (H+) from an acid, resulting in the formation of ammonium salt.
Ammonium Ion molar mass
The molar mass of the ammonium ion (NH4+) is 18.04 g/mol. This value is calculated by adding the atomic masses of one nitrogen atom (14.01 g/mol) and four hydrogen atoms (1.01 g/mol each). The molar mass is an important property of the ammonium ion as it allows for the conversion of its mass to moles and vice versa. This is useful in many chemical calculations, such as determining the amount of reactants needed in a chemical reaction.
Ammonium Ion boiling point
Since the ammonium ion is typically found as part of a salt, such as ammonium chloride (NH4Cl), it does not have a boiling point of its own. Instead, the boiling point of ammonium chloride, which is 520 °C, is influenced by various factors such as the strength of the ionic bond between the ammonium ion and the chloride ion, as well as the size and shape of the ammonium ion.
Ammonium Ion melting point
Similar to the boiling point, the ammonium ion does not have a melting point because it is not a substance that exists in a pure form. However, salts containing the ammonium ion, such as ammonium nitrate (NH4NO3), have a melting point of 169.6 °C. The melting point of ammonium nitrate is influenced by the strength of the ionic bond between the ammonium ion and the nitrate ion, as well as the crystal structure of the compound.
Ammonium Ion density g/ml
The density of the ammonium ion (NH4+) is not applicable as it is a polyatomic ion and does not exist as a separate entity. However, salts containing the ammonium ion, such as ammonium sulfate (NH4)2SO4, have a density of 1.77 g/cm³ at room temperature. The density of salts containing the ammonium ion is influenced by various factors, including the size and shape of the ions, the strength of the ionic bond, and the crystal structure of the compound.
Ammonium Ion molecular weight
The molecular weight of the ammonium ion (NH4+) is 18.04 g/mol, which is calculated by adding the atomic masses of one nitrogen atom and four hydrogen atoms. The molecular weight is an important property of the ammonium ion as it allows for the conversion of its mass to moles and vice versa. This is useful in many chemical calculations, such as determining the amount of reactants needed in a chemical reaction.
Ammonium Ion Structure
The ammonium ion (NH4+) has a tetrahedral molecular geometry with a nitrogen atom at the center and four hydrogen atoms at the corners of the tetrahedron. The nitrogen atom has a formal positive charge of +1, while each hydrogen atom has a formal charge of -1. The ammonium ion is a polyatomic cation that is formed by the protonation of ammonia (NH3) with a hydrogen ion (H+). The ammonium ion is a common cation in inorganic and organic compounds, including fertilizers, pharmaceuticals, and explosives.
| Appearance | White crystalline solid or colorless gas |
| Specific Gravity | Not applicable (polyatomic ion) |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 18.04 g/mol |
| Density | Not applicable (polyatomic ion), density of salts varies (e.g. 1.77 g/cm³ for ammonium sulfate) |
| Melting Point | Not applicable (polyatomic ion), melting point of salts varies (e.g. 169.6 °C for ammonium nitrate) |
| Boiling Point | Not applicable (polyatomic ion), boiling point of salts varies (e.g. 520 °C for ammonium chloride) |
| Flash Point | Not applicable (polyatomic ion) |
| Water Solubility | Highly soluble (completely miscible) in water |
| Solubility | Soluble in alcohols and liquid ammonia |
| Vapor Pressure | Not applicable (polyatomic ion) |
| Vapor Density | Not applicable (polyatomic ion) |
| pKa | 9.25 (conjugate acid, ammonium cation) |
| pH | 7 (neutral) in aqueous solution |
Note: The values presented in the table may vary depending on the specific chemical form and conditions of the ammonium ion.
Ammonium Ion Safety and Hazards
Ammonium ion, in its pure form, is generally considered safe and non-toxic. However, like many chemical compounds, ammonium ion can pose some hazards and risks, especially when handled or used improperly. Ammonium ion can release toxic ammonia gas when it reacts with strong bases or strong acids. It can also be a fire and explosion hazard when exposed to heat or flame. In addition, exposure to high concentrations of ammonium ion or its derivatives can cause irritation to the eyes, skin, and respiratory system. It is important to follow proper safety protocols and handle ammonium ion and its derivatives with care to avoid potential hazards.
| Hazard Symbols | None assigned for pure ammonium ion |
| Safety Description | Harmful if swallowed, inhaled or absorbed through the skin. Causes skin, eye, and respiratory irritation. May release toxic ammonia gas. Can be a fire and explosion hazard. |
| UN ID | 3077 (for ammonium compounds, including ammonium salts) |
| HS Code | 2827.10.00 (for ammonium chloride, ammonium carbonate, and other ammonium salts) |
| Hazard Class | 9 (Miscellaneous dangerous substances and articles) for ammonium compounds, Class 8 (Corrosive substances) for ammonium hydroxide solution |
| Packing Group | III (for ammonium compounds) |
| Toxicity | Generally considered non-toxic in pure form, but can release toxic ammonia gas. Ammonium compounds and derivatives may be toxic or harmful to human health and the environment depending on their specific properties and usage. |
Ammonium Ion Synthesis Methods
Ammonium ion can be synthesized using a variety of methods, including chemical reactions and biological processes.
One common method for synthesizing ammonium ion is by reacting ammonia gas with an acid, such as hydrochloric acid or sulfuric acid, to produce ammonium salt. The reaction involves the displacement of hydrogen ions (H+) in the acid by ammonia molecules, resulting in the formation of ammonium cation (NH4+) and the corresponding anion of the acid (e.g. chloride, sulfate). The resulting ammonium salt can be purified and crystallized to obtain ammonium ion.
Biological processes, such as the breakdown of organic matter by microbes, can also result in the formation of ammonium ion. In this process, nitrogen-containing compounds are decomposed by bacteria and other microorganisms, producing ammonia and eventually ammonium ion. This process is known as ammonification and is an important step in the nitrogen cycle.
Another method for synthesizing ammonium ion is through the Haber-Bosch process, which involves the reaction of nitrogen gas and hydrogen gas in the presence of a catalyst at high pressure and temperature. The resulting ammonia gas can then be reacted with an acid to produce ammonium ion.
Ammonium Ion Uses
Ammonium ion has a variety of uses in industrial, agricultural, and laboratory settings.
It serves a wide range of industrial, agricultural, and laboratory settings, as it acts primarily as a fertilizer in agriculture, providing readily available nitrogen to plants while reducing soil pH.
The chemical industry employs ammonium ion as a key ingredient in producing various compounds, such as fertilizers, explosives, and pharmaceuticals, as well as utilizing it in the synthesis of antibiotics and other pharmaceuticals. Ammonium ion also functions as an explosive in the form of ammonium nitrate.
In laboratories, researchers use ammonium ion as a reagent in numerous chemical reactions, such as precipitation reactions and organic synthesis, and as a buffering agent to stabilize solution pH.
Moreover, ammonium ion finds use in household cleaning products as an antimicrobial agent due to its ability to kill bacteria and fungi.
The multiple uses of ammonium ion, and its versatility, make it an essential compound in various industries and applications.