• Bonding: The attraction that holds atoms and ions together.
• Intermolecular Forces: The forces between molecules. Think of it like how you’re attracted to your favorite snack; you just want to be near it! 😜

They're the forces that keep molecules close to each other, like the BFF glue that holds your friendship squad together!

Note: The strength and type of these forces depend on the size and polarity (how charged) of the molecules.

• London (dispersion) forces: Weak forces caused by momentary changes in electron distribution. Imagine a crowd doing "the wave" at a sports game. Sometimes, you join in even if you didn't plan to!
• Dipole-induced dipole forces: When a polar molecule (with a positive and negative end) makes a neighboring non-polar molecule polar for a while. Like when a popular kid makes an underrated song popular by singing it!
• Dipole-dipole forces: The attractive forces between the positive end of one polar molecule and the negative end of another. Think of it like magnets – opposites attract!
• Hydrogen bonding: A super special type of dipole-dipole force involving a hydrogen atom. The bond in your favorite soap, making your bath bubbles last longer!
• 🎈 Fun Fact: London, dipole-induced dipole, and dipole-dipole forces are collectively called van der Waals forces.

• Water is H₂O – two hydrogen atoms bonded to an oxygen atom.
• Question: Why do water molecules stick together in a glass or in ice?
  Answer: Intermolecular forces! Just like how fans cluster together at a concert.