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Add lone pairs to these Lewis structures of interhalogen compounds. BrF3 and
BrF5.
Add lone pairs to these Lewis structures of interhalogen compounds. BrF3 and BrF5..
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Add lone pairs to these Lewis structures of interhalogen compounds. BrF3 and
BrF5.
Lone pair electrons are electrons that don’t participate in bonding. These lone-pair electrons are also known as valance electrons and can be found in the outermost shells of atoms. The structure indicates the lone pair electrons to help you find the non-bonded pair.
Here’s an example of a single pair electron:
The molecule ammonia contains three hydrogens and nitrogen. The electronic configuration for nitrogen is [katex]{\rm{1}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{3}}}[/katex]
[katex]\begin{array}{l}\\{\rm{Br}}\,\,{\rm{ = }}\,\,{\rm{[Ar]}}\,{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{5}}}\\\\{\rm{Br}}\,\,{\rm{ = }}\,\,7\\\end{array}[/katex]
[katex]\begin{array}{l}\\{\rm{F}}\,\,{\rm{ = }}\,\,\left[ {{\rm{He}}} \right]{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{5}}}\\\\{\rm{3F = }}\,\,{\rm{3}}\,{\rm{ \times }}\,{\rm{7}}\,\,\\\\{\rm{3F = }}\,{\rm{21}}\\\end{array}[/katex]
[katex]\begin{array}{l}\\{\rm{Br}}{{\rm{F}}_{\rm{3}}}{\rm{ = }}\,\,{\rm{21 + 7}}\\\\{\rm{Br}}{{\rm{F}}_{\rm{3}}}{\rm{ = }}\,{\rm{28}}\\\end{array}[/katex]
Structure of $equaTag4
[katex]\begin{array}{l}\\{\rm{Br}}\,\,{\rm{ = }}\,\,{\rm{[Ar]}}\,{\rm{3}}{{\rm{d}}^{{\rm{10}}}}{\rm{4}}{{\rm{s}}^{\rm{2}}}{\rm{4}}{{\rm{p}}^{\rm{5}}}\\\\{\rm{Br}}\,\,{\rm{ = }}\,\,7\\\end{array}[/katex]
[katex]\begin{array}{l}\\{\rm{F}}\,\,{\rm{ = }}\,\,\left[ {{\rm{He}}} \right]{\rm{2}}{{\rm{s}}^{\rm{2}}}{\rm{2}}{{\rm{p}}^{\rm{5}}}\\\\{\rm{5F = }}\,\,5\,{\rm{ \times }}\,{\rm{7}}\,\,\\\\{\rm{5F = }}\,\,35\\\end{array}[/katex]
[katex]\begin{array}{l}\\{\rm{Br}}{{\rm{F}}_5}{\rm{ = }}\,\,35{\rm{ + 7}}\\\\{\rm{Br}}{{\rm{F}}_5}{\rm{ = }}\,\,42\\\end{array}[/katex]
Structure of $equaTag8
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Structure of $equaTag4