acid/bases

Define the following:

BRONSTED ACID
BRONSTED BASE
BRONSTED REACTION

label them according to the bronsted definition

label them according to the bronsted definition

Lewis Base vs Lewis Acid

✅ Quick Memory Trick:

“Base = Brings Electrons”
Lewis Base = Brings or Gives electron pair

DIA

label it

stronger KA means what?

stronger acid

smaller pka means what?

stronger acid

1 pka unit= …. change in acidity

10x change in acidity

lower pkb means what?

stronger base

higher strength of an acid means what in terms of pka and PKB?

lower strength of an acid means what in terms of pka and PKB?

which side of the equation is preferred?

"Equilibrium favors the more stable side of the equation" means what

This means:

• In a reaction, the system will shift toward the side with more stable molecules.

• Stable = lower energy = favored.

Strong acids/bases are blank stable + why

Weak acids/bases are more stable + why

HA + B⁻ ⇌ A⁻ + HB

• Left side: strong acid (HA) + strong base (B⁻) → less stable

• Right side: weak acid (HB) + weak base (A⁻) → more stable 

• WHERE WILL IT MOVE

✅ So equilibrium shifts toward the weaker acid/base side (right).

1. What makes an acid stronger?

Answer:
→ If its conjugate base is more stable.
Why?
Because a stable conjugate base is okay holding the negative charge, so the acid is happy to give away H⁺.

2. How does conjugate base stability affect pKa?

Answer:
→ More stable base = lower pKa = stronger acid.
Why?
Stable base = acid gives H⁺ easily = stronger acid.

3. What makes a conjugate base stable? Name 2 things.

Answer:
→ Resonance and electronegative atoms (like oxygen).
Why?
They spread or hold the negative charge better.

6. What does a low pKa mean?

Answer:
→ Strong acid.
Why?
Low pKa = acid gives up H⁺ easily.

7. What does a high pKa mean?

Answer:
→ Weak acid.
Why?
High pKa = acid wants to keep H⁺ = conjugate base is unstable.

label them acids and anions (stronger + weaker)

ARIO?

atom

In the same row → more electronegative atom = is better at what holding blank charge? more/less base? weaker/stronger acid?

In the same row → more electronegative atom = better at holding negative charge = more stable base = stronger acid.

groups vs periods on periodic table

Bigger atom = better at holding negative charge = more stable conjugate base = stronger acid. but why?

🧠 Why does size matter?

• A big atom spreads the negative charge out more (this is called polarizability).

• A small atom holds the negative charge tightly in one spot → more unstable.

D

More stable anion → weaker base but why?

💡 Think about what a base does:

• A base wants to grab a proton (H⁺).

• If the conjugate base (anion) is very stable, it is happy just staying as it is.

• So it doesn’t want to react or grab H⁺ → meaning it is a weak base.

less stable anion --> stronger base why?

Because…

• A less stable anion (negatively charged ion) is uncomfortable holding that negative charge.

• To feel more stable, it wants to get rid of that negative charge.

• The easiest way to do that is to grab a proton (H⁺).

• A molecule that really wants to grab a proton is called a strong base.

The inductive effect is
affected by

electronegativity,
2. # of electronegative
atoms
3. distance