Multiple Choice
Is the molecule OCl_2 (dichlorine monoxide) polar or nonpolar?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Is the molecule OBr_2 polar or nonpolar?
A
Polar
B
Nonpolar
Verified step by step guidance1
Step 1: Draw the Lewis structure of OBr_2. Oxygen (O) is the central atom bonded to two bromine (Br) atoms. Count the total valence electrons: Oxygen has 6, each Bromine has 7, so total electrons = 6 + 2*7 = 20 electrons.
Step 2: Arrange the electrons to satisfy the octet rule for each atom. Place single bonds between O and each Br, then distribute the remaining electrons as lone pairs to complete octets, especially on the oxygen atom.
Step 3: Determine the molecular geometry using VSEPR theory. Oxygen with two bonded atoms and two lone pairs corresponds to a bent or angular shape, similar to water (H_2O).
Step 4: Analyze the bond dipoles. Oxygen is more electronegative than bromine, so each O–Br bond has a dipole moment pointing toward oxygen. Because of the bent shape, these dipoles do not cancel out.
Step 5: Conclude that due to the bent molecular geometry and the difference in electronegativity, the dipole moments add up to give a net dipole moment, making OBr_2 a polar molecule.
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