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Questions and Answers
What is a dipole moment?
What is a dipole moment?
- The total charge of a molecule
- A measure of the separation of positive and negative charges in a molecule (correct)
- The ability of a molecule to form hydrogen bonds
- The energy required to break a covalent bond
How is dipole moment represented?
How is dipole moment represented?
- By the strength of the van der Waals forces in the molecule
- By an arrow pointing from the negative to the positive charge (correct)
- By the bond angle between atoms in the molecule
- By the total number of electrons in the molecule
In which type of molecule is the dipole moment zero?
In which type of molecule is the dipole moment zero?
- Nonpolar molecules (correct)
- Ionic molecules
- Hydrogen-bonded molecules
- Metallic molecules
What is a dipole moment?
What is a dipole moment?
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What does a non-zero dipole moment indicate about a molecule?
What does a non-zero dipole moment indicate about a molecule?
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What factors affect the magnitude of a molecule's dipole moment?
What factors affect the magnitude of a molecule's dipole moment?
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Study Notes
Dipole Moment
- A dipole moment is a measure of the separation of positive and negative electric charge within a molecule.
- It is a vector quantity, represented by the symbol μ (mu), and is typically measured in Debye units (D).
Representation of Dipole Moment
- The dipole moment is represented by an arrow pointing from the positive charge to the negative charge.
- The length of the arrow is proportional to the magnitude of the dipole moment.
Dipole Moment in Different Molecules
- In a molecule with a centro-symmetric shape (e.g., CO2, CH4), the dipole moment is zero.
- In a molecule with a non-centro-symmetric shape (e.g., H2O, CO), the dipole moment is non-zero.
Implications of Non-Zero Dipole Moment
- A non-zero dipole moment indicates the presence of a permanent electric dipole in the molecule.
- This suggests that the molecule is polar, with a partial positive charge on one end and a partial negative charge on the other.
Factors Affecting Dipole Moment Magnitude
- The magnitude of a molecule's dipole moment is affected by the difference in electronegativity between atoms in the molecule.
- The bond length and angle also influence the dipole moment magnitude.
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