Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine the molecular geometry
\text{Molecular geometry: T-shaped}
- BrF₃ has a central bromine (Br) atom with three fluorine (F) atoms - Using VSEPR theory, this creates a T-shaped molecular geometry
Step 3:: Analyze the electronegativity
\Delta\text{Electronegativity} = |3.98 - 2.96| = 1.02
- Bromine electronegativity: 2.96 - Fluorine electronegativity: 3.98 - There is a significant electronegativity difference between Br and F
Step 4:: Examine bond polarities
\text{Br}^{\delta+} - \text{F}^{\delta-}
- The Br-F bonds are polar due to the electronegativity difference - Fluorine is more electronegative, creating partial negative charge
Step 5:: Assess molecular symmetry
- The T-shaped geometry means the bond dipoles do not cancel - Unequal distribution of charge creates a net dipole moment
Final Answer
BrF₃ is a polar molecule due to its asymmetric T-shaped geometry and polar Br-F bonds.
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