Acids & Bases

Water and acid combine in an exothermic reaction - releasing large amounts of heat.

Water and acid combine in an exothermic reaction - releasing large amounts of heat.

Acid - Base Theories Lavoisier Arrhenius Bronsted-Lowry Lewis Lavoisier Arrhenius Bronsted-Lowry Lewis

Antoine Lavoisier

Acidity is caused by the presence of oxygen in the compound. Lavoisier

He even created the word oxygen - from the Greek oxys, "sour" and genes, "born" Lavoisier

Oxygen means "acid maker". Lavoisier

Lavoisier's idea about acids turned out to be wrong... Lavoisier

but it is historically important since it is the first scientific attempt to chemically characterize acids and bases. Lavoisier

Arrhenius Bronsted-Lowry Lewis

Svante August Arrhenius

Arrhenius Acid Any substance that produces hydrogen ions, H +, in water solution.

Any substance that produces hydroxide ions, OH -, in water solution. Arrhenius Base

In a formula, such as HCl, the positive part of a Arrhenius acid will ALWAYS be hydrogen.

In a formula, such as NaOH, the negative part of a Arrhenius base will ALWAYS be hydroxide.

Arrhenius acids and bases, and soluble salts, are called electrolytes.

When each dissolves, ions are released that conduct electricity.

If a solution has NO ions, it cannot conduct electricity.

Johannes Nicolaus Bronsted Bronsted-Lowry Theory

Thomas Martin Lowry Bronsted-Lowry Theory

Any substance that acts as a proton donor. Bronsted-Lowry Acid

A B-L acid MUST have hydrogen somewhere in its formula. Bronsted-Lowry Acid

When an electron is removed from a hydrogen atom Bronsted-Lowry Acid

a hydrogen ion is produced - a proton. + Bronsted-Lowry Acid

Bronsted-Lowry Base Any substance that acts as a proton acceptor.

Bronsted-Lowry Base Most negative ions can acts as B-L bases.

The acid/base definitions are broadened because no specific ion must be formed, although hydrogen is the only source of protons. Bronsted-Lowry Theory

What is the formula for the hydronium ion?

H3O+H3O+

The hydronium ion is formed by combining a hydrogen ion and a water molecule. H 2 O + H + H 3 O + Bronsted-Lowry Theory

conjugate base Bronsted-Lowry Theory

A conjugate base is the particle that remains AFTER an acid gives up a proton. Bronsted-Lowry Theory

conjugate acid Bronsted-Lowry Theory

A conjugate acid is the particle formed when a base accepts a proton. Bronsted-Lowry Theory

HCl + H 2 O Cl - + H 3 O + Identify the B-L acid in this equation. What gives up a proton from the left side to the right?

HCl + H 2 O Cl - + H 3 O + HCl donates a proton, it is the B-L acid.

Identify the B-L base in this equation. What gains a proton from the left side to the right? HCl + H 2 O Cl - + H 3 O +

H 2 O accepts a proton, it is the B-L base.

HCl + H 2 O Cl - + H 3 O + Identify the conjugate base in this equation. What is left when the acid gives up a proton?

HCl + H 2 O Cl - + H 3 O + Cl - is left when HCl gives up a proton, it is the conjugate base.

HCl + H 2 O Cl - + H 3 O + Identify the conjugate acid in this equation. What is formed when the base accepts a proton?

HCl + H 2 O Cl - + H 3 O + H 3 O + is formed when water accepts a proton, it is the conjugate acid.

HCl + H 2 O Cl - + H 3 O + acids have conjugate bases

HCl + H 2 O Cl - + H 3 O + bases have conjugate acids

Remove a proton from an acid to get its conjugate base. H 2 SO 4 HI H 2 O

Remove a proton from an acid to get its conjugate base. HSO 4 - H 2 SO 4 HI H 2 O

Remove a proton from an acid to get its conjugate base. HSO 4 - I - H 2 SO 4 HI H 2 O

Remove a proton from an acid to get its conjugate base. HSO 4 - I - OH - H 2 SO 4 HI H 2 O

Add a proton to a base to get its conjugate acid. Cl - H 2 O NO 3 -

Add a proton to a base to get its conjugate acid. HClCl - H 2 O NO 3 -

Add a proton to a base to get its conjugate acid. HCl H 3 O + Cl - H 2 O NO 3 -

Add a proton to a base to get its conjugate acid. HCl H 3 O + HNO 3 Cl - H 2 O NO 3 -

Gilbert Newton Lewis The Lewis Theory

Lewis Acid Any substance that acts as an electron-pair acceptor.

Lewis Base Any substance that acts as an electron-pair donor.

The Lewis Theory This theory is the broadest of all.

The Lewis Theory Any reaction that involves the exchange of electrons WILL have a Lewis acid and Lewis base.

The Lewis Theory In an equation, the Lewis acid gets MORE NEGATIVE from the left side to the right side - it gains e -.

The Lewis Theory In an equation, the Lewis base gets MORE POSITIVE from the left side to the right side - it loses e -.

Cl 2 + I - Cl - + I 2 Identify the Lewis acid in this equation. What gets more negative?

Cl 2 gets more negative from the left side to the right, it is the Lewis acid. Cl 2 + I - Cl - + I 2

Identify the Lewis base in this equation. What gets more positive? Cl 2 + I - Cl - + I 2

I - gets more positive from the left side to the right, it is the Lewis base. Cl 2 + I - Cl - + I 2

End Acid - Base Theories

Binary Acids Acids composed of two elements: hydrogen and a halogen

First: Determine the stem word. The stem word comes from the negative element. Naming Binary Acids

First: Determine the stem word. Example - HCl chlorine is the negative element - CHLOR is the stem. Naming Binary Acids

Second: Add the prefix hydro to the stem. Naming Binary Acids

Second: Add the prefix hydro to the stem. Example - hydro + chlor Naming Binary Acids

Third: Change the ending of the stem to ic. Naming Binary Acids

Third: Change the ending of the stem to ic. Example - hydro + chlor + ic Naming Binary Acids

Final name: hydrochloric acid Naming Binary Acids

HCl HF HBr HI Naming Binary Acids

HCl hydro chlor ic acid HF HBr HI Naming Binary Acids

HCl hydro chlor ic acid HF hydro fluor ic acid HBr HI Naming Binary Acids

HCl hydro chlor ic acid HF hydro fluor ic acid HBr hydro brom ic acid HI Naming Binary Acids

HCl hydro chlor ic acid HF hydro fluor ic acid HBr hydro brom ic acid HI hydro iod ic acid Naming Binary Acids

Ternary acids composed of three elements: hydrogen, oxygen, and a nonmetal Naming Ternary Acids

First: Determine the stem part of the name of the third element Naming Ternary Acids

First: Determine the stem Example - H 2 SO 4 sulfur is the third element, SULFUR is the stem. Naming Ternary Acids

Second: The most common form of the acid is given the suffix ic. Naming Ternary Acids

Second: The most common form of the acid is given the suffix ic. Example - sulfur + ic acid Naming Ternary Acids

Third: If the acid is NOT in its most common form, do the following: Naming Ternary Acids

Add the prefix per if the acid has one more oxygen than the most common form.

Add the prefix per if the acid has one more oxygen than the most common form. Example - H 2 SO 5 per + sulfuric acid Naming Ternary Acids

Add the suffix ous if the acid has one less oxygen than the most common form.

Add the suffix ous if the acid has one less oxygen than the most common form. Example - H 2 SO 3 sulfur + ous acid Naming Ternary Acids

Add the prefix hypo if the acid has two less oxygen atoms than the most common form.

Add the prefix hypo if the acid has two less oxygen atoms than the most common form. Example - H 2 SO 2 hypo + sulfur + ous acid Naming Ternary Acids

HClO 3 Chloric Acid Naming Ternary Acids

HClO 4 HClO 3 Chloric Acid Naming Ternary Acids

HClO 4 Perchloric Acid HClO 3 Chloric Acid Naming Ternary Acids

HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Naming Ternary Acids

HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Chlorous Acid Naming Ternary Acids

HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Chlorous Acid HClO Naming Ternary Acids

HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Chlorous Acid HClO Hypochlorous Acid Naming Ternary Acids

Strong or Weak

Strong acids and bases ionize completely in water solution.

Strong or Weak HCl, HBr, and HI are the only Strong binary acids.

Strong or Weak In Strong ternary acids, the number of oxygen atoms exceeds the number of...

Strong or Weak hydrogen atoms by two or more. H 2 SO 4 and HNO 3 are strong. H 3 PO 4 is weak.

Strong or Weak Hydroxides of groups 1 and 2, except Be, are Strong bases.

Amphoteric A substance that acts as either an acid or base, depending on what it reacts with.

Water is the most common amphoteric substance. HOH

Anhydrous - Without H 2 O

Acid Anhydride - an oxide that produces an acid in water.

SO 2 + H 2 O H 2 SO 3 Acid Anhydride - oxides of nonmetals

Basic Anhydride - an oxide that produces a base in water.

Na 2 O + H 2 O 2NaOH Basic Anhydride - oxides of metals

Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 2. H 2 C 2 O 4 3. H 3 PO 4 4. H 4 C 2 O 2

Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 SO 2 2. H 2 C 2 O 4 3. H 3 PO 4 4. H 4 C 2 O 2

Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 SO 2 2. H 2 C 2 O 4 C 2 O 3 3. H 3 PO 4 4. H 4 C 2 O 2

Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 SO 2 2. H 2 C 2 O 4 C 2 O 3 3. H 3 PO 4 HPO 3 4. H 4 C 2 O 2

Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 SO 2 2. H 2 C 2 O 4 C 2 O 3 3. H 3 PO 4 HPO 3 4. H 4 C 2 O 2 C 2