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Mobile App Chapter 12: Problem 37
Distinguish between polarizability and polarity. How does each influence intermolecular forces?
Short Answer
Expert verified
Polarizability affects London dispersion forces and is about electron cloud distortion, while polarity affects dipole-dipole interactions based on charge distribution.
Step by step solution
01
- Define Polarizability
Polarizability is the measure of how easily the electron cloud of a molecule can be distorted by an electric field. Larger and more easily distorted electron clouds lead to higher polarizability.
02
- Define Polarity
Polarity refers to the distribution of electrical charge over the atoms in a molecule. A molecule is polar if it has a net dipole moment resulting from the uneven distribution of electrons between bonded atoms.
03
- Influence on Intermolecular Forces
Polarizability influences intermolecular forces by enhancing London dispersion forces. Molecules with higher polarizability exhibit stronger dispersion forces. On the other hand, polarity influences intermolecular forces by creating dipole-dipole interactions, which occur between molecules with net dipole moments.
04
- Comparison and Contrast
While both polarizability and polarity affect intermolecular forces, polarizability primarily affects London dispersion forces, and polarity affects dipole-dipole interactions. Thus, nonpolar molecules with high polarizability can have strong intermolecular forces due to dispersion, while polar molecules have additional dipole-dipole interactions.
05
- Summarize
In summary, polarizability is about the ease of electron cloud distortion and affects London dispersion forces, whereas polarity deals with the distribution of electrical charge affecting dipole-dipole interactions.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Intermolecular Forces
Intermolecular forces are the forces that hold molecules together. These forces occur between molecules and influence many physical properties of substances, such as boiling points, melting points, and solubility.
There are several types of intermolecular forces, including:
There are several types of intermolecular forces, including:
- London dispersion forces
- Dipole-dipole interactions
- Hydrogen bonding (a special case of dipole-dipole interactions)
London Dispersion Forces
London dispersion forces, also known as van der Waals forces, are the weakest type of intermolecular forces. They arise due to temporary fluctuations in electron density within molecules, which create transient dipoles.
These transient dipoles induce similar dipoles in neighboring molecules, leading to an attraction between them.
Several factors affect the strength of London dispersion forces:
These transient dipoles induce similar dipoles in neighboring molecules, leading to an attraction between them.
Several factors affect the strength of London dispersion forces:
- Polarizability: Larger molecules with more electrons have higher polarizability, leading to stronger dispersion forces.
- Molecular Shape: Long, slender molecules have greater surface area for interactions, resulting in stronger dispersion forces.
Dipole-Dipole Interactions
Dipole-dipole interactions occur between molecules that have permanent dipole moments. A dipole moment arises when there is an uneven distribution of electrons between atoms in a molecule, leading to a partial positive charge on one end and a partial negative charge on the other.
For these interactions to occur effectively, molecules must be aligned so that the positive end of one dipole is near the negative end of another.
Factors influencing dipole-dipole interactions include:
For these interactions to occur effectively, molecules must be aligned so that the positive end of one dipole is near the negative end of another.
Factors influencing dipole-dipole interactions include:
- Polarity: Molecules with greater polarity (larger dipole moments) have stronger dipole-dipole interactions.
- Distance and Orientation: The strength of interactions increases when molecules are closer and properly aligned.
Electron Cloud Distortion
Electron cloud distortion refers to the ability of an electron cloud to be deformed by an electric field. This deformation leads to the temporary formation of dipoles, which are critical for generating London dispersion forces.
Factors that influence electron cloud distortion include:
Factors that influence electron cloud distortion include:
- Size of the Molecule: Larger electron clouds are more easily distorted.
- Type of Atoms: Atoms with more electrons can lead to higher polarizability.
- Temperature: Higher temperatures can increase the movement of electrons, aiding distortion.
Net Dipole Moment
A net dipole moment measures the overall polarity of a molecule and results from the vector sum of all individual bond dipoles within the molecule.
Factors leading to a net dipole moment include:
Factors leading to a net dipole moment include:
- Differences in Electronegativity: When atoms with different electronegativities are bonded, electrons are shared unevenly.
- Molecular Geometry: The shape of the molecule determines how individual dipoles sum up. For instance, in a linear molecule with two identical polar bonds in opposite directions, the net dipole moment can be zero.
