The electronic configuration of the Bromine atom is given by 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 5. There is also a lone pair attached to the Bromine atom. It can be observed from the BrF 5 Lewis structure that there are five Fluorine atoms surrounding the central Bromine atom. To determine the hybridization, we take a look at the Lewis structure of the BrF 5 molecule. BrF 5 Hybridizationīromine Pentafluoride comprises 5 Fluorine atoms, all pulled together by the central Bromine atom. The formal charges being 0 for all of the atoms in the BrF 5 molecule tells us that the structure shown above is stable. Two valence electrons are used in the formation of a Bromine- Fluorine bond.įC = Valence Electrons – Non-bonding electrons – (Bonding electrons ÷ 2) Bromine forms covalent bonds with the surrounding Fluorine atoms. We can now use these to form bonds and fill octets.īromine acts as the central atom here and will facilitate bond formation. There are 42 valence electrons available to us. The first step to determining the Lewis structure is to calculate the number of valence electrons available.

Lewis structures also help predict polarity and reactivity. The outermost electrons are also shown attached to their constituent atoms as well. It tells us about the nature of the bonds present while also giving insight into the molecular geometry and bond angles of the compound. The Lewis structure of a compound represents a schematic arrangement of all the atoms present in the compound. Therefore, the total number of valence electrons in BrF5 is given by:ħ + 35 = 42 Valence Electrons BrF 5 Lewis Structure Therefore, the five Fluorine atoms present contribute: 7 x 5 = 35 Valence Electrons. Therefore, the Bromine atom contributes: 7 x 1 = 7 Valence Electronsįluorine is in group 17 of the periodic table with the electronic configuration 2s 2 2p 5. There are five Fluorine atoms and one Bromine atom.īromine is in group 17 of the periodic table and has an electronic configuration of 4s☣d¹⁰4p⁵. Each element in the compound contributes a certain number of valence electrons from its outermost shell.īrF 5 is an interhalogen compound that comprises Bromine and Fluorine. To draw the Lewis structure for a compound, we must first calculate the number of valence electrons available to us. These electrons are called valence electrons. This is because the force of attraction from the nucleus is weakest in the outermost shells. The electrons present in the outermost shell of the atom are the ones that are available for bond formation and exchange.

Brf5 molecular geometry