Lecture 2 Video 1

🧲 What Is Nucleophilicity?

Nucleophilicity describes how good an atom, ion, or molecule is at acting as a nucleophile—that is, how well it can donate electron density to form a bond with a positively charged or electron-poor nucleus.

💡 Intuition: A nucleophile is “electron-rich” and likes to attack “electron-poor” centers.

🔋 What Makes a Good Nucleophile?

At a first approximation, good nucleophiles:

• Have extra electrons to donate
• Often carry a negative charge
• Possess lone pairs

Typical Examples

• Halide anions: F⁻, Cl⁻, Br⁻, I⁻
• Hydroxide: OH⁻

These species are electron-rich and therefore well-suited to bond with positive or partially positive atoms.

🧪 Where Do These Extra Electrons Come From?

Halides

Halogens normally have 7 valence electrons. By gaining one extra electron, they become negatively charged halide ions, making them potential nucleophiles.

Hydroxide (OH⁻)

• Derived from water (H₂O)
• Oxygen is highly electronegative and can fully take an electron from hydrogen
• The result is OH⁻ and H⁺ (a bare proton)

⚠️ Important: When you see H⁺, it is literally just a proton—no electrons at all.

🌊 Solvent Effects: The Big Twist

Not all nucleophiles behave the same way in different solvents. The key distinction is between:

• Protic solvents
• Aprotic solvents

This distinction completely changes the nucleophilicity trend.

💧 Protic Solvents

Definition

A protic solvent has hydrogens that can be released as protons.

Examples:

• Water
• Alcohols

Why?

• Hydrogen is bonded to oxygen
• Oxygen can pull electron density away, leaving a free or reactive proton

What Happens to Nucleophiles?

• Nucleophiles form hydrogen bonds with the solvent
• This creates a solvation shell that blocks nucleophilic attack

Small, Highly Charged Ions (like F⁻)

• Very tightly solvated
• Strong hydrogen bonding
• Poor nucleophiles in protic solvents

Large, Diffuse Ions (like I⁻)

• Less tightly solvated
• Electron cloud is spread out
• More polarizable
• Better nucleophiles

✅ Nucleophilicity Order (Protic Solvent)

I⁻ > Br⁻ > Cl⁻ > F⁻

📌 Key ideas:

• Size matters
• Polarizability matters
• Hydrogen bonding hurts nucleophilicity

⚡ Aprotic Solvents

Definition

An aprotic solvent lacks acidic hydrogens.

Example:

• Diethyl ether

Why hydrogens don’t matter here:

• Hydrogens are bonded to carbon
• Carbon is not electronegative enough to release protons

What Happens Now?

• No strong hydrogen bonding to nucleophiles
• Nucleophilicity depends more on basicity

🔁 The Trend Reverses!

In aprotic solvents:

• Stronger bases = better nucleophiles
• Smaller, more electronegative ions win

✅ Nucleophilicity Order (Aprotic Solvent)

F⁻ > Cl⁻ > Br⁻ > I⁻

📌 Why?

• Fluoride is the strongest base
• Not stabilized by hydrogen bonding
• Highly reactive when unsolvated

🧠 Polarizability: A Crucial Concept

• Large ions (like I⁻) have valence electrons far from the nucleus
• Their electron cloud can distort easily
• This makes them especially reactive toward partial positive charges (e.g., carbon in C–Br bonds)

This is why iodide excels in polar protic solvents despite being a weak base.

🧠 Big Picture Summary

⚠️ Critical takeaway: Nucleophilicity ≠ Basicity, even though they are related. This distinction is emphasized as a setup for the next lecture.

🧩 Mental Shortcut (Exam Gold ⭐)

• Protic solvent → think “shielding” → bigger is better
• Aprotic solvent → think “basicity” → smaller is better