![]() Hence, B makes 3 single bonds (6 electrons) with atoms of F.Īssign the remaining 18 valence electrons around in a way that each F consists of 6 electrons surrounding it. ![]() To get the number of lone pairs, calculate the difference between the number of valence electrons and the number of bonding pairs electrons.īefore placing electrons around the atoms to complete the octets, select the central atom.Īs per arrangements of elements in the table, B is the least electronegative than F. ![]() Now, find the total number of bonding electrons that are used for bonding in the Lewis dot structure.Ĭompute the difference between required electrons and total valence electrons.Ħ number of bonding pairs of electrons is equal to 3 covalent bonds formed between F and B atoms. To compute the required number of electrons that must share by each atom, F needs 8 electrons in its outermost shell and B needs most 6 valence electrons in its last shell. After computation, the result says that 24 valence electrons need to be shared to make a bond between atoms. In the compound, there is 1 atom of boron and 3 atoms of fluorine. It needs 6 valence electrons in its outermost shell. Hence, you can calculate the number of valence electrons of both the atoms using electronic configuration.Īs per the octet rule, born is an exceptional case.
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