Bronsted-Lowry & Lewis Acids & Bases

Supposedly An Acid Has To Contain An H^+ & A Base Had To Contain An OH^- When Dissociation...

BUT, many compounds behave as bases that do release OH^- in solution do not have OH in their formula (NH3 / Amines / Weak acid salts)

Bronsted-Lowry Acid...

Any species that DONATES a H^+ (A proton donor) (MUST HAVE H+ In FORMULA) (All Arrhenius Acids are also Bronsted-Lowry acids)

Bronsted-Lowry Bases...

Any species that ACCEPTS an H^+ (A proton acceptor) (BASE MUST CONTAIN LONE PAIR OF ELECTRONS TO ACCEPT PROTON) (Bronsted-Lowry bases are not Arrhenius bases but all Arrhenius Bases are Bronsted-Lowry bases)

Conjugate Acid...

Has one more H^+ and one fewer -1 charge

Conjugate Base...

Has one less H+ and one more -1 charge

When A Reaction Is Reversed, The Ka & Kb Are...

Inversed

Ka =...

[H3O^+][A^-] / [HA]

Net Reaction Direction...

Reaction proceeds to side with weaker acid and base

Strong Acids Have...

Weaker Conjugate Bases

Strong Bases Have...

Weaker Conjugate Acids

Lewis Acid...

Any substance ACCEPTING an electron pair (Look for atoms not filling octet rule)

Lewis Base...

Any substance DONATING an electron pair (Look for atoms with lone pair) (Family 5)

Lewis Acids do Not Need...

To Have H in formula (No protons protons are transferred)

Lewis Acids Include...

Electron-deficient molecules (Group 3) / Metal cations (Al^3+ / Zn^2+ / Cu^2+ ) / Molecules with double bond

Lewis Acids & Bases Always Form...

An adduct because the product contains a new covalent bond

Arrhenius Definition Recap...

Acid: Donates H^+ in water / Base: Donates OH^- in water

Bronsted-Lowry Definition Recap...

Acid: Donates H^+ in water / Base: Received H^+ in water

Lewis Definition Recap...

Acid: Receives electron pair /Base: Donates electron pair

Lewis Acid (elec or nuc)

electrophile

Lewis Base (elec or nuc)

nucleophile