Multiple Choice
Given the following bonds: (i) H–F, (ii) H–Cl, (iii) H–Br, rank them from most polar to least polar.
2
views
13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Is the molecule SO_2 polar or nonpolar?
A
SO_2 is nonpolar because it contains only nonpolar bonds.
B
SO_2 is polar because it has a bent molecular geometry and an uneven distribution of electron density.
C
SO_2 is polar because it has a tetrahedral geometry.
D
SO_2 is nonpolar because its molecular geometry is linear and the dipoles cancel out.
Verified step by step guidance1
Step 1: Determine the Lewis structure of SO\_2. Sulfur (S) is the central atom bonded to two oxygen (O) atoms. Count the total valence electrons: sulfur has 6, each oxygen has 6, so total valence electrons = 6 + 2\times6 = 18.
Step 2: Draw the Lewis structure with sulfur in the center bonded to two oxygens. Assign lone pairs to complete the octets on oxygen atoms and place remaining electrons on sulfur. This results in a structure with one double bond and one single bond, and a lone pair on sulfur.
Step 3: Determine the electron geometry and molecular shape using VSEPR theory. With two bonding regions and one lone pair on sulfur, the electron geometry is trigonal planar, but the molecular shape is bent (angular).
Step 4: Analyze the polarity of the bonds and the molecule. The S–O bonds are polar due to the difference in electronegativity between sulfur and oxygen. Because the molecule is bent, the dipole moments do not cancel out.
Step 5: Conclude that SO\_2 is polar because it has a bent molecular geometry and an uneven distribution of electron density, resulting in a net dipole moment.
Related Videos
Related Practice
Molecular Polarity practice set
Problem sets built by lead tutorsExpert video explanations