Answer
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Hint: Lewis dot structure is satisfied by their charges. So to determine if the given lewis dot structure is correct or not, one should look for the formal charge on that atom in a molecule. Formal charges are the charge on an atom of a molecule, assuming that all electrons are equally shared in a bond.
Complete answer:
To solve this question, we have to understand about the lewis dot structure and its formal charge.
So, lewis dot structure or formulas are the diagrams that represent the bonding between the atoms of a molecule, it also depicts about the number of lone pairs and the shared electrons.
So, in case of \[B{F_3}\] we have two lewis dot structures, this fact can be attributed because of overlapping phenomena in case of fluorine bonding with boron.
This is because fluorine lone pairs are of the appropriate size and exact symmetry to overlap with the empty \[p\] orbitals of boron.
Generally in lewis dot structure, we can see that the structure of a molecule is satisfied by each atom sharing or having complete 8 valence electrons in the valence shell. But we can say Boron is an exception, it can be satisfied by 6 electrons in its valence shell.
Note:
Also for the molecule \[^ + F = B = {F_2}\]
We can calculate the formal charge as , the fluorine with double bond has \[6\] electrons around it , which is one less than required so , its formal charge is \[1\] and fluorine with single bond has formal charge \[0\] has they have 7 electrons around them , as required . But when we talk about Boron it has \[4\] electrons, which is \[1\] more than required, so charge is + \[1\], so this is a quite contrary structure
Complete answer:
To solve this question, we have to understand about the lewis dot structure and its formal charge.
So, lewis dot structure or formulas are the diagrams that represent the bonding between the atoms of a molecule, it also depicts about the number of lone pairs and the shared electrons.
So, in case of \[B{F_3}\] we have two lewis dot structures, this fact can be attributed because of overlapping phenomena in case of fluorine bonding with boron.
This is because fluorine lone pairs are of the appropriate size and exact symmetry to overlap with the empty \[p\] orbitals of boron.
Generally in lewis dot structure, we can see that the structure of a molecule is satisfied by each atom sharing or having complete 8 valence electrons in the valence shell. But we can say Boron is an exception, it can be satisfied by 6 electrons in its valence shell.
Note:
Also for the molecule \[^ + F = B = {F_2}\]
We can calculate the formal charge as , the fluorine with double bond has \[6\] electrons around it , which is one less than required so , its formal charge is \[1\] and fluorine with single bond has formal charge \[0\] has they have 7 electrons around them , as required . But when we talk about Boron it has \[4\] electrons, which is \[1\] more than required, so charge is + \[1\], so this is a quite contrary structure