Chemistry HL
6
Chapters
243
Notes
Chapter 1 - Models Of The Particulate Nature Of Matter
Chapter 2 - Models Of Bonding & Structure
Chapter 3 - Classification Of Matter
Chapter 4 - What Drives Chemical Reactions?
Chapter 5 - How Much, How Fast & How Far?
Chapter 6 - What Are The Mechanisms Of Chemical Change?
Chemistry HL
Chapter 6 - What Are The Mechanisms Of Chemical Change?
Unraveling Lewis Acid-Base Reactions: Dive Into Reactivity 3.4.7!
543 words
3 mins read
Last edited on 5th Nov 2024
Table of content
The 'Electron-y' World of Lewis Bases and Acids
-
🧲 Nucleophiles: They are the electron-rich guys. Think of them as the generous ones, always ready to donate their extra electrons.
- Have at least one pair of electrons chilling out by themselves (lone pair)
- Can be a negatively charged species (think of them as those with a little negative ⚡cloud around them) or just a neutral molecule.
- Real-World Analogy: Think of nucleophiles as someone with extra cash 💵 willing to lend it out!
-
Lewis Base: Just another fancy name for a nucleophile.
- So a Lewis base = an electron donor. (They're the Santa Claus 🎅 of electrons!)
-
🧲 Electrophiles: Opposite of nucleophiles. They're electron-poor and want those electrons real bad.
- Ready to accept a pair of electrons.
- Can be positively charged (think of them as those eager to get some extra ⚡ juice) or neutral.
- Real-World Analogy: Electrophiles are like someone short on cash 💸 hoping for a generous friend!
-
Lewis Acid: Yep, you guessed it. Another fancy name for an electrophile.
- So a Lewis acid = an electron acceptor. (They're the customers 🛍️ at Santa's store!)
The Lovely Dance of Lewis Acid-Base Reaction
- When a Lewis base (electron donor) and a Lewis acid (electron acceptor) meet, they form a coordination bond.
- Think of it as two people shaking hands 🤝. One offers a hand (electron donor) and the other accepts it (electron acceptor).
The Drama of Boron Trifluoride & Ammonia
- 🎭 Scene: Boron trifluoride, chilling with three sp2 hybrid orbitals and a vacant seat (the 2pz orbital).
- 🎭 Enter Ammonia, with a pair of electrons on the nitrogen.
- What happens? Ammonia donates its electrons to boron trifluoride's vacant seat, and voila, a bond is formed!
- Here, ammonia is like the friendly neighbor with a cup of sugar (nucleophile & Lewis base) and boron trifluoride is the one in need of sugar for the cake (electrophile & Lewis acid).
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Chemistry HL
Chapter 6 - What Are The Mechanisms Of Chemical Change?
Unraveling Lewis Acid-Base Reactions: Dive Into Reactivity 3.4.7!
543 words
3 mins read
Last edited on 5th Nov 2024
Table of content
The 'Electron-y' World of Lewis Bases and Acids
-
🧲 Nucleophiles: They are the electron-rich guys. Think of them as the generous ones, always ready to donate their extra electrons.
- Have at least one pair of electrons chilling out by themselves (lone pair)
- Can be a negatively charged species (think of them as those with a little negative ⚡cloud around them) or just a neutral molecule.
- Real-World Analogy: Think of nucleophiles as someone with extra cash 💵 willing to lend it out!
-
Lewis Base: Just another fancy name for a nucleophile.
- So a Lewis base = an electron donor. (They're the Santa Claus 🎅 of electrons!)
-
🧲 Electrophiles: Opposite of nucleophiles. They're electron-poor and want those electrons real bad.
- Ready to accept a pair of electrons.
- Can be positively charged (think of them as those eager to get some extra ⚡ juice) or neutral.
- Real-World Analogy: Electrophiles are like someone short on cash 💸 hoping for a generous friend!
-
Lewis Acid: Yep, you guessed it. Another fancy name for an electrophile.
- So a Lewis acid = an electron acceptor. (They're the customers 🛍️ at Santa's store!)
The Lovely Dance of Lewis Acid-Base Reaction
- When a Lewis base (electron donor) and a Lewis acid (electron acceptor) meet, they form a coordination bond.
- Think of it as two people shaking hands 🤝. One offers a hand (electron donor) and the other accepts it (electron acceptor).
The Drama of Boron Trifluoride & Ammonia
- 🎭 Scene: Boron trifluoride, chilling with three sp2 hybrid orbitals and a vacant seat (the 2pz orbital).
- 🎭 Enter Ammonia, with a pair of electrons on the nitrogen.
- What happens? Ammonia donates its electrons to boron trifluoride's vacant seat, and voila, a bond is formed!
- Here, ammonia is like the friendly neighbor with a cup of sugar (nucleophile & Lewis base) and boron trifluoride is the one in need of sugar for the cake (electrophile & Lewis acid).
Unlock the Full Content!
Dive deeper and gain exclusive access to premium files of Chemistry HL. Subscribe now and get closer to that 45 🌟
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