Multiple Choice
Which of the following best describes the polarity of a molecule of F_2?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Is the molecule OCl_2 (dichlorine monoxide) polar or nonpolar?
A
Nonpolar
B
Polar
Verified step by step guidance1
Step 1: Draw the Lewis structure of OCl_2. Oxygen (O) is the central atom bonded to two chlorine (Cl) atoms. Oxygen has 6 valence electrons, and each chlorine has 7 valence electrons, so count all valence electrons to distribute them properly.
Step 2: Determine the molecular geometry using the VSEPR theory. Oxygen has two bonding pairs (with Cl atoms) and two lone pairs of electrons. This arrangement corresponds to a bent or angular shape around the oxygen atom.
Step 3: Analyze the bond dipoles. The O–Cl bonds are polar because of the difference in electronegativity between oxygen and chlorine atoms, with oxygen being more electronegative.
Step 4: Consider the molecular shape and symmetry. Since the molecule is bent (not linear or symmetrical), the bond dipoles do not cancel out.
Step 5: Conclude that because the bond dipoles do not cancel and the molecule has a bent shape, OCl_2 is polar.
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