How are Van der Waals forces and ionic bonds similar?
They're not that similar...
van der Waals forces are short-range intermolecular forces, specifically the interaction of loose, fluctuating PARTIAL charges, i.e. temporary dipoles... dynamic in time, influenced by instantaneously-changing charge density distributions.
Ionic bonds are interactions of FULL charges, i.e. due to complete transfer of valence electrons. They are permanent charges, and mostly static in time.
NOTE: Ionic bonding should not be confused with ion-pairing interactions:
Aspartate and arginine are clearly not bonding to each other, but their full charges are still interacting.
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Though the types of particles involved and the strength of the interactions are different, van der Waals forces and ionic bonds are similar in that they both involve electrostatic interactions between atoms or molecules; ionic bonds occur between ions of opposite charges, whereas temporary dipoles or induced dipoles cause van der Waals forces to occur between non-polar or polar molecules.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- What type of intermolecular force would water molecules have? London dispersion? Dipole dipole? Or hydrogen bonding?
- Why do nonpolar molecules usually have a much lower surface tension than polar ones?
- What are the strongest bonds in water?
- As liquid water freezes, the molecules arrange themselves in a way that takes up more space than llquid water. What would most likely occur if the arrangement of frozen water molecules required less space than that of liquid water molecules?
- Why does #HI# have a higher boiling point than #HBr#, and #HCl#?

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