Answer:
To determine if a molecule of general formula ABn (where n > 2) is polar, you need to consider the molecular geometry and the polarity of the individual bonds within the molecule.
1. Determine the molecular geometry: First, determine the arrangement of atoms in the molecule by considering the number of bonded atoms and lone pairs around the central atom (A). This will help you determine the molecular geometry.
2. Determine the polarity of individual bonds: Next, determine the polarity of each bond between the central atom (A) and the surrounding atoms (B). If there is a significant electronegativity difference between A and B, the bond is polar. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond.
3. Consider the molecular symmetry: If the molecule has an overall symmetrical distribution of polar bonds, the polarities of the bonds may cancel each other out, resulting in a nonpolar molecule. This occurs when the molecule has a symmetrical shape or is linear.
4. Consider the molecular dipole moment: If the molecule is asymmetrical and has polar bonds that do not cancel each other out, the molecule will have a net dipole moment and be polar.
It is important to note that this is a general guideline, and there may be exceptions and more complex cases. Additionally, the presence of lone pairs of electrons on the central atom can also affect molecular polarity.
Explanation:
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