Multiple bonds are pretty fancy and packed with electrons! They can make things a bit tricky when we’re figuring out the geometry of molecules. But no worries, we'll break it down with some real-world examples!

• Domains: Think of a domain like a neighborhood where electrons live.
  • Double & Triple Bonds? They're just ONE domain. 🏠
  • But...a double bond has 2 electron pairs, and a triple bond has 3! They're like apartment complexes with multiple residents in the same space.
• Repulsion: Ever been in a crowded bus? That's how electrons feel.
  • More electron pairs = more repulsion. 🚌💥🚌
  • Multiple bonds have more electron pairs, so they push harder against other bonds.
• Bond Angles: This is where the real twist (literally!) comes in.
  • More repulsion from multiple bonds can cause bond angles to be different from what we'd expect.

• Picture ethene as two friends (carbon atoms) holding hands (double bond), with each friend holding a balloon (hydrogen atom) in their other hands.
• Normally, if the two friends and their balloons stand in a circle, the angle between the balloons would be 120° (like a perfect slice of pizza 🍕).
• BUT! The double bond acts like one of those super strong magnet toys, pulling the balloons slightly in.
  • The result? H–C–H bond angle is 117° (just a smidge less pizza for us 🙁) and the H–C=C bond angle is 121.5° (a bit more pizza here! 🥳).