Bromine Lewis dot structure represents that bromine is a diatomic molecule with the formula Br2. This article explains the bromine Lewis dot structure with itself and other elements along with its visual representation
Bromine belongs to group 17 of the periodic table. So there is a total of 7 electrons in its valence shell. To achieve its nearest noble gas configuration, it only needs 1 electron. So bromine shares its 1 electron with 1 electron of another bromine atom, thereby forming a single covalent Br-Br bond. As there is a single bond between bromine atoms so each bromine will have 3 lone pairs of electrons around them.
Discussing the properties of bromine, then it is non-metal and belongs to the halogen family. It is a volatile red-brown liquid at room temperature and has a sharp and pungent smell. Its periodic properties are intermediate between chlorine and iodine. Bromine also has two stable isotopes 79Br and 81Br. Both of them are the only natural isotopes of bromine.
In terms of occurrence and production, then unlike its other halogen counterparts, its abundance is observed in oceans due to long term leaching. Commercially it is produced by halogen exchange reaction and is transported in big metallic drums to required areas. Laboratory production of bromine is not required as it is easily available commercially with easy storage and long shelf life.
Bromine though has many usages in organic synthesis and has a biological role is very toxic and should be used with care by the chemist in laboratory settings. It can cause chemical burns and its inhalation affects the respiratory tract. Chronic exposure can lead to bronchial infection and death as well.
To achieve octet stability bromine can react with other elements and can form various Lewis dot structures. Some of them are:
· Bromine Lewis dot structure (Bromide ion)
· Bromine Lewis dot structure with Hydrogen
· Bromine Lewis dot structure with Lithium
· Bromine Lewis dot structure with Carbon
· Bromine Lewis dot structure with Aluminium
· Bromine Lewis dot structure with Sulphur
· Bromine Lewis dot structure with Potassium
· Bromine Lewis dot structure with Calcium
Bromine Lewis dot structure (Bromide ion)
Bromine (Atomic number = 35 and electronic configuration = 2,8,18,7) belongs to group 17 of the periodic table. So it has 7 valence electrons that are involved in chemical bond formation. So to achieve its octet stability it needs to gain 1 electron. Now with 8 electrons in its valence shell, it is no longer a bromine atom but a bromide ion which is represented by the negative sign. The negative sign denotes the addition of 1 electron and the formation of an anion.
Bromine Lewis dot structure with Hydrogen
Bromine Lewis dot structure with hydrogen leads to the formation of hydrogen bromide (HBr). Hydrogen (Atomic number = 1 and electronic configuration = 1) belongs to the 1st group of the periodic table and consists of 1 electron. Likewise, bromine belongs to group 17 and comprises 7 electrons in its valence shell. Both of them need 1 electron to achieve the nearest noble gas configuration. So they will share their 1 electron to form a single covalent bond leading to the H-Br molecule. Also, there are 3 lone pairs of electrons on the bromine atom in the HBr molecule.
Bromine Lewis dot structure with Lithium
Lithium (Atomic number = 3 and electronic configuration = 2,1) belongs to 1st group of periodic table with 1 electron in its valence shell. Similarly, bromine belongs to the 17th group of the periodic table with 7 electrons in its valence shell. Lithium being an alkali metal will lose 1 electron to achieve its nearest noble gas configuration of helium. So it will become Li+ ion. On the flip side bromine being an electronegative element will gain that 1 electron to acquire its octet stability and results in Br_ ion. This will lead to the formation of the ionic compound Lithium bromide (LiBr). The bond between both lithium and bromine will be electrovalent.
Bromine Lewis dot structure with Carbon
Carbon (Atomic number = 6 and electronic configuration = 2,4) belong to group 14 of the periodic table and has 4 electrons in its valence shell. On the other hand, bromine belongs to group 17 and consists of 7 valence electrons. To fulfil the octet stability carbon will form a single covalent bond with 4 bromine atoms. Carbon being less electronegative will be the central atom surrounded by 4 bromine atoms. Here carbon will share its 4 electrons with 1 electron of each bromine atom thereby forming carbon tetrabromide (CBr4).
Bromine Lewis dot structure with Aluminium
Aluminium (Atomic number = 13 and electronic configuration = 2,8,3) belongs to group 13 of the periodic table and has 3 electrons in its valence shell. Bromine belongs to group 17 and has 7 electrons in its valence shell. Aluminium being the least electronegative will be the central atom surrounded by 3 bromine atoms.
So aluminium will share its 3 valence electrons with 1 electron of each bromine atom forming a single covalent bond between them. This will form a stable Lewis structure AlBr3. Another noteworthy point in this structure is that bromine can achieve octet stability but aluminium will not form any octet. It has 6 electrons in its valence shell and it is stable. So AlBr3 is an exception to octet rule stability criteria.
Bromine Lewis dot structure with Sulphur
Sulphur (Atomic number = 16 and electronic configuration = 2,8,6) belongs to group 16 of the periodic table and gas has 6 electrons in its valence shell. On the other hand, bromine belongs to group 17 and has 7 electrons in its valence shell. So to form the Lewis structure sulphur will be the central atom surrounded by 2 terminal bromine atoms. To achieve octet stability criteria sulphur will share its 2 valence electrons with 1 valence electron of each bromine atom. A single covalent bond will be formed between sulphur and bromine thereby forming a sulphur dibromide (SBr2) molecule.
Bromine Lewis dot structure with Potassium
Potassium (Atomic number = 19 and electronic configuration= 2,8,8,1) belongs to group 1 of the periodic table with 1 valence electron. Bromine as mentioned above several times belongs to group 17 with 7 electrons in its valence shell. Potassium being an alkali metal will donate its 1 valence electron which will be gained by a more electronegative bromine atom. This will fulfil the stability criteria and result in potassium cation and bromide anion. Also, it will lead to the formation of electrovalent or ionic compound potassium bromide (KBr).
Bromine Lewis dot structure with Calcium
Calcium (Atomic number = 20 and electronic configuration = 2,8,8,2) belong to group 2 of the periodic table and consist of 2 valence electrons. On similar lines, bromine belongs to group 17 and has 7 valence electrons. To achieve stability calcium being an alkaline earth metal will donate its 1 valence electron each to 2 bromine atoms. So calcium being metal will gain +2 charge and both the bromine atoms being electronegative and non-metals will gain -1 charge each. This will result in the formation of an electrovalent bond between calcium and bromine atoms and the formation of the ionic compound CaBr2.
Bromine Lewis dot Structure (Related FAQs)
Why certain compounds are an exception to the octet rule?
The molecules which have the odd number of electrons are the exceptions to the octet rule. Usually, it is compounds formed from boron and aluminium. They usually form compounds with six valence electrons. Other than the odd number of valence electrons there are many other criteria like when there are very few valence electrons and when there are too many valence electrons
What is the formal charge?
It can be defined as the charge on the particular atom in a molecule when all of its electrons are shared equally. It is crucial when determining the covalency and predicting the reactivity of the compound, It also keeps track of the electrons.
What is the role of electronegativity in deciding the central atom in a molecule?
Electronegativity means the tendency to attract electrons. During chemical bond formation the less electronegative atom is designated as the central atom because it will not pull electron density towards itself like the terminal atoms. This will reduce the repulsion tension between bonded electron pairs on the central atom.
How solubility of bromine is related to its polarity?
Bromine is itself a heavy liquid among halogens. Talking about its solubility then it is partially miscible in water or an aqueous medium. But it is readily soluble in various organic solvents. As bromine is a non-polar molecule and the organic solvent is also non-polar, the only intermolecular force between them is the Vander Waal dispersion forces
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