Multiple Choice
Which one of the following molecules is polar?
13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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How many of the following molecules are polar: BrF_3, CS_2, SiF_4, SO_3?
A
4
B
3
C
2
D
1
Verified step by step guidance1
Step 1: Determine the molecular geometry of each molecule using the VSEPR theory. This involves counting the number of bonding pairs and lone pairs around the central atom.
Step 2: For BrF_3, identify the central atom (Br) and note that it has 3 bonded atoms (F) and 2 lone pairs, leading to a T-shaped molecular geometry.
Step 3: For CS_2, recognize that the molecule is linear because the central atom (C) is bonded to two S atoms with no lone pairs, resulting in a symmetrical shape.
Step 4: For SiF_4, note that the central atom (Si) is bonded to four F atoms with no lone pairs, giving a tetrahedral and symmetrical geometry.
Step 5: For SO_3, observe that the central atom (S) is bonded to three O atoms with no lone pairs, resulting in a trigonal planar and symmetrical shape. Then, determine polarity by checking if the molecular geometry is symmetrical and if bond dipoles cancel out.
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