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Questions and Answers
Which type of intermolecular force is present between ALL molecules?
Which type of intermolecular force is present between ALL molecules?
Permanent dipole-dipole forces are present between non-polar molecules.
Permanent dipole-dipole forces are present between non-polar molecules.
False (B)
What is the primary characteristic that facilitates the formation of hydrogen bonds?
What is the primary characteristic that facilitates the formation of hydrogen bonds?
Hydrogen bonded to F, N, or O
Instantaneous dipoles are caused by the movement of ___________ in atoms or molecules.
Instantaneous dipoles are caused by the movement of ___________ in atoms or molecules.
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Match the intermolecular force with the molecules that it commonly occurs between:
Match the intermolecular force with the molecules that it commonly occurs between:
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Which of the following best describes London forces?
Which of the following best describes London forces?
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Hydrogen bonds are stronger than both London forces and permanent dipole-dipole interactions.
Hydrogen bonds are stronger than both London forces and permanent dipole-dipole interactions.
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List two factors that increase the strength of London forces.
List two factors that increase the strength of London forces.
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In contrast to London forces, dipole-dipole interactions are formed between molecules with permanent ______.
In contrast to London forces, dipole-dipole interactions are formed between molecules with permanent ______.
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Match the following intermolecular forces with the types of molecules most likely to exhibit them:
Match the following intermolecular forces with the types of molecules most likely to exhibit them:
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Flashcards
London Forces
London Forces
Attraction forces between induced or instantaneous dipoles in all molecules, especially non-polar ones.
Dipole-Dipole Forces
Dipole-Dipole Forces
Attraction forces between permanent dipoles of polar molecules with uneven charge distribution.
Hydrogen Bonds
Hydrogen Bonds
Structured bonds formed between H atoms bonded to F, N, or O and lone pairs on these electronegative atoms.
Permanent Dipoles
Permanent Dipoles
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Instantaneous Dipoles
Instantaneous Dipoles
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Induced Dipoles
Induced Dipoles
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Strength of Intermolecular Forces
Strength of Intermolecular Forces
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Effect of Size on London Forces
Effect of Size on London Forces
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Study Notes
London Dispersion Forces
- Attraction forces between induced or instantaneous dipoles
- Act between all molecules, but most significant in nonpolar molecules or very large nonpolar segments
- Electrons in atoms/molecules are constantly moving, creating temporary uneven distributions
- This uneven distribution creates temporary partial charges (instantaneous dipoles)
- These temporary dipoles induce dipoles in neighboring molecules
- Strength increases with larger atoms and longer molecules due to increased polarizability
Permanent Dipole-Dipole Forces
- Attraction forces between permanent dipoles
- Present between polar molecules containing atoms with partial charges
- Dipoles are created by differences in electronegativity between atoms in a molecule
- Oppositely charged partial charges in neighbouring molecules attract each other
Hydrogen Bonds
- Structured bonds between permanent dipoles
- Involve a hydrogen atom bonded to a highly electronegative atom (Fluorine, Oxygen, or Nitrogen)
- Strongest intermolecular force; about 20 times weaker than a covalent or ionic bond
- The electronegative atom attracts electrons, causing a partial positive on the hydrogen
- The lone electron pairs on the electronegative atom attract the partially positive hydrogen atom of a neighbouring molecule, forming a hydrogen bond.
- Strength increases with increasing electronegativity of the atom bonded to the hydrogen atom.
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Description
Test your understanding of intermolecular forces, including London dispersion forces, permanent dipole-dipole forces, and hydrogen bonds. This quiz covers their characteristics, significance, and the conditions under which they occur. Enhance your knowledge of molecular interactions and their implications in chemistry.
