Question

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part a
determine whether each molecule is polar or nonpolar.
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if₃ so₂ brf₅ sef₄
polar
nonpolar

Explanation:

Step1: Analyze \( \text{IF}_3 \)

• Step1a: Determine molecular geometry

\( \text{IF}_3 \) has a central \( \text{I} \) atom with 7 valence electrons. It forms 3 single bonds with \( \text{F} \) and has 2 lone pairs. The electron - pair geometry is trigonal bipyramidal, and the molecular geometry is T - shaped.

• Step1b: Check polarity

The \( \text{I - F} \) bonds are polar. Due to the T - shaped geometry, the bond dipoles do not cancel out. So \( \text{IF}_3 \) is polar.

Step2: Analyze \( \text{SO}_2 \)

• Step2a: Determine molecular geometry

The central \( \text{S} \) atom in \( \text{SO}_2 \) has 6 valence electrons. It forms 2 double bonds with \( \text{O} \) and has 1 lone pair. The electron - pair geometry is trigonal planar, and the molecular geometry is bent.

• Step2b: Check polarity

The \( \text{S - O} \) bonds are polar. The bent geometry means the bond dipoles do not cancel. So \( \text{SO}_2 \) is polar.

Step3: Analyze \( \text{BrF}_5 \)

• Step3a: Determine molecular geometry

The central \( \text{Br} \) atom in \( \text{BrF}_5 \) has 7 valence electrons. It forms 5 single bonds with \( \text{F} \) and has 1 lone pair. The electron - pair geometry is octahedral, and the molecular geometry is square pyramidal.

• Step3b: Check polarity

The \( \text{Br - F} \) bonds are polar. The square pyramidal geometry results in a net dipole moment (the lone pair and bond dipoles do not cancel). So \( \text{BrF}_5 \) is polar.

Step4: Analyze \( \text{SeF}_4 \)

• Step4a: Determine molecular geometry

The central \( \text{Se} \) atom in \( \text{SeF}_4 \) has 6 valence electrons. It forms 4 single bonds with \( \text{F} \) and has 1 lone pair. The electron - pair geometry is trigonal bipyramidal, and the molecular geometry is see - saw.

• Step4b: Check polarity

The \( \text{Se - F} \) bonds are polar. The see - saw geometry means the bond dipoles do not cancel. So \( \text{SeF}_4 \) is polar.

Answer:

Polar: \( \text{IF}_3 \), \( \text{SO}_2 \), \( \text{BrF}_5 \), \( \text{SeF}_4 \)
Nonpolar: (No molecules in the given set are nonpolar)