What Defines a Polar Molecule?

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SUMMARY

A polar molecule is defined by an uneven distribution of electron density, which is the correct answer to the posed question. Option b, stating that a polar molecule has a linear polarity without charge, is misleading as it does not accurately describe the nature of polar molecules. The discussion clarifies that while temporary dipole moments can arise from uneven electron distribution, they do not exclusively indicate polarity. Therefore, the defining characteristic of polar molecules is their uneven electron density, distinguishing them from other molecular types.

PREREQUISITES
  • Understanding of molecular geometry and polarity
  • Knowledge of dipole moments and their significance
  • Familiarity with Van der Waals forces
  • Basic principles of electron distribution in molecules
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  • Study the concept of dipole moments in detail
  • Explore molecular geometry types and their implications on polarity
  • Learn about Van der Waals forces and their role in molecular interactions
  • Investigate examples of polar and non-polar molecules
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Chemistry students, educators, and anyone interested in molecular chemistry and the properties of polar molecules.

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Homework Statement


Which statement describe a polar molecule?
a. The molecule has an uneven distribution of electron density [ans]
b. The molecule has a linear polarity without charge
c. The molecule has a tetrahedral geometry
d. All of the above

The Attempt at a Solution



I would personally go for option b as any number of dipole moment may be resolved into a linear polarity by vector sum. Also for option a, it doesn't sound convincing as temporary dipole moment (van der waal forces) may also attributed to uneven distribution of electron density, and it is not exclusive to polar molecule per se.
 
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icystrike said:
linear polarity without charge
What does this particular sequence of words mean?
 
icystrike said:

Homework Statement


Which statement describe a polar molecule?
a. The molecule has an uneven distribution of electron density [ans]
b. The molecule has a linear polarity without charge
c. The molecule has a tetrahedral geometry
d. All of the above

The Attempt at a Solution



I would personally go for option b as any number of dipole moment may be resolved into a linear polarity by vector sum. Also for option a, it doesn't sound convincing as temporary dipole moment (van der waal forces) may also attributed to uneven distribution of electron density, and it is not exclusive to polar molecule per se.

It's saying that all polar molecules have an uneven distribution of electron density, not that all molecules with an uneven distribution are polar.
 

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