Aluminum Bromide Formula

Aluminum Bromide Formula

Aluminium, a component of aluminium bromide, makes up more than 8.1 percent of the Earth’s crust, making it one of the most abundant minerals on the planet. Despite the fact that aluminium is found in a vast variety of compounds on Earth, it is rarely observed in its free metal form. Instead, it’s commonly found in minerals like bauxite and cryolite. Bromine, the other component of aluminium bromide, is a toxic, oily, scarlet liquid. Bromine, in addition to being used to make colours, insecticides, and fertilisers, is occasionally found in trace levels in living animals, although having no recognised biological function in humans.

Aluminum Bromide Formula is a colourless liquid that melts from a white crystalline compound. Furthermore, aluminium bromide is a hygroscopic substance. The dimeric compound form is mostly found in solid form. Experts use this compound as a catalyst in the Friedel-Crafts alkylation reaction.

What is Aluminium Bromide?

Aluminium bromide is a pale yellow chemical solution also known as tribromoalumane or aluminium tribromide (the most common kind). It’s a colourless, hygroscopic solid that may be sublimated. The molecular or chemical formula is AlBr3.

It has a lumpy solid odour when it is anhydrous and takes the form of a white to yellowish-red compound. In its watery state, it appears to be a liquid. The skin, mucous membranes, and eyes are all severely harmed by its exposure. It is frequently used in the synthesis of numerous compounds. It can be dissolved in various organic solvents, such as nitrobenzene, benzene, toluene, simple hydrocarbons, and xylene.

Aluminum Bromide Formula Structure

Aluminum Bromide Formula comprises one aluminium cation (Al3+) and one bromide anion (Br). As a result, the molecular formula for Aluminium Bromide is composed of one aluminium cation (Al3+) and one bromide anion (Br). As a result, the molecular or chemical formula for barium sulphate is AlBr3. Its chemical formula indicates that it is made up of one aluminium atom and three bromine atoms. Its molecular mass is 266.694 g/mol as an anhydrous compound and 374.785 g/mol as a hexahydrate. It has a monoclinic crystalline structure and a positive dipole moment.

Physical Properties of Aluminium Bromide

The physical properties of the Aluminum Bromide Formula are:

  • Aluminium Bromide is a white to light yellow powder with a strong odour.
  • It is a colourless, sublimable hygroscopic solid that is most commonly seen as aluminium tribromide.
  • Aluminium Bromide has a density of 3.2 g/cm3 as anhydrous and 2.54 g/cm3 as hexahydrate.
  • Aluminium Bromide has a melting temperature of 97.5 °C as an anhydrous and 93 °C as a hexahydrate.
  • Aluminium Bromide has a boiling point of 255 °C as an anhydrous and 252 °C as a hexahydrate.
  • Aluminium Bromide has a heat capacity of 100.6 J/mol K.
  • Aluminium Bromide has a standard molar entropy of 180.2 J/mol K.
  • The standard enthalpy of production for Aluminium Bromide is -572.5 kJ/mol.
  • Its aqueous solution is neutral in nature and has a pH of 6 at 14 °C.
  • It is slightly soluble in methanol, diethyl ether, acetone but entirely soluble in water.

Chemical Properties of Aluminium Bromide

Al2Br6 is the form of Aluminum Bromide Formula that is most frequently found. Strong Lewis acid, AlBr3, can be produced when Al2Br6 dissociates. Furthermore, Al2Br6 has a dimerisation tendency. In terms of this particular tendency, heavier main-group halides are more likely to exist as large aggregates. The empirical formulae need to reflect the size of these aggregates accurately. This tendency is also absent in lighter main group halides, such as boron tribromide, due to the smaller size of the central atom.

Derivation of Aluminium Bromide Formula

  • At 100 °C, aluminium tribromide combines with carbon tetrachloride to produce carbon tetrabromide.

4 AlBr3 + 3 CCl4 → 4 AlCl3 + 3 CBr4

  • It reacts with phosgene gas to produce carbonyl bromide and aluminium chlorobromide.

AlBr3 + COCl2 → COBr2 + AlCl2Br

  • Water hydrolyzes Al2Br6 in line with the properties of Lewis acid. Furthermore, water hydrolysis occurs during the development of HBr and the production of the Al-OH-Br species. It also reacts fast with alcohol and carboxylic acids.

Solved Question For Aluminium Bromide Formula

What is the process for the preparation of Aluminium Bromide?

Solution: Aluminium bromide is prepared by the reaction of Hydrogen bromide (HBr) with aluminium metal (Al).

2 Al + 6 HBr → Al2Br6 + 3 H2

The second method to obtain Aluminium Bromide is through bromination.

2 Al + 3 Br2 → Al2Br6

Chemistry Related Formulas
Urea Formula Pyrophosphoric Acid Formula
Ammonia Formula Silicon Dioxide Formula
Bleaching Powder Formula Sodium Cyanide Formula
Molarity Formula Sodium Fluoride Formula
Oxalic Acid Formula Barium Phosphate Formula
Methane Formula Barium Oxide Formula
Sulphuric Acid Formula Calcium Bromide Formula
Aluminium Chloride Formula Dilution Formula
Chloroform Formula Folic Acid Formula
Empirical Formula Fumaric Acid Formula

FAQs (Frequently Asked Questions)

1. How can one determine if he or she has been exposed to aluminium bromide?

The exposure to dangerous compounds such as aluminium bromide should be monitored on a regular basis. This may require taking personal and regional air samples. A worker’s employer can supply him with copies of the sample results.

2. What are the side effects of aluminium bromide?

Aluminum Bromide can harm you if inhaled. It is a highly corrosive chemical and direct contact can severely irritate and burn the skin and eyes, perhaps causing eye damage. It may irritate the nose, throat, and lungs, resulting in coughing, wheezing, and/or shortness of breath. Aluminum bromide is a reactive chemical that might cause an explosion.

3. How does aluminium bromide exist in nature?

In the solid state, solutions in noncoordinating solvents (e.g., CS2), the melt, and the gas phase, the dimeric form of aluminium tribromide (Al2Br6) predominates. These dimers only break down into monomers at high temperatures.

Al2Br6 → 2 AlBr3 (ΔH°diss = 59 kJ/mol)