Acids & Bases Water and acid combine in an exothermic reaction - releasing large amounts of heat

Acids & BasesAcids & Bases

Water and acid combine inan exothermic reaction - releasing large amountsof heat.

Water and acid combine inan exothermic reaction - releasing large amountsof heat.

Acid - Base Theories Acid - Base Theories

• Lavoisier

• Arrhenius

• Bronsted-Lowry

• Lewis

• Lavoisier

• Arrhenius

• Bronsted-Lowry

• Lewis

AntoineLavoisier

QuickTime™ and aTIFF (Uncompressed) decompressor

are needed to see this picture.

Acidity is caused by

the presence of

oxygen in the

compound.

Lavoisier - 1777Lavoisier - 1777



He even created the word

oxygen - from the

Greek oxys, "sour"

and genes, "born"




Oxygen means

"acid maker".




Lavoisier's idea about

acids turned out

to be wrong...




but it is historically important

since it is the first scientific

attempt to chemically

characterize acids

and bases.




Arrhenius

Bronsted-Lowry

Lewis

SvanteAugust

Arrhenius QuickTime™ and a

TIFF (Uncompressed) decompressorare needed to see this picture.



Arrhenius AcidArrhenius Acid

Any substance

that produces

hydrogen ions,

H+, in water

solution.

Any substance

that produces

hydroxide ions,

OH-, in water

solution.



Arrhenius BaseArrhenius Base

In a formula, such as HCl,

the positive part of a

Arrhenius acid

will ALWAYS

be hydrogen.QuickTime™ and a


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.

JohannesNicolausBronsted



Bronsted-Lowry TheoryBronsted-Lowry Theory

ThomasMartinLowry




Any substance that

acts as a proton donor.

Bronsted-Lowry AcidBronsted-Lowry Acid



A B-L acid MUST have

hydrogen somewhere

in its

formula.




When an electron is

removed from a

hydrogen atom...

+ -


a hydrogen ion is

produced - a proton.

+


Bronsted-Lowry BaseBronsted-Lowry Base

Any substance that

acts as a proton

acceptor.QuickTime™ and a


Bronsted-Lowry BaseBronsted-Lowry Base

Most negative ions can

acts as B-L bases.



The acid/base definitionsare broadened because nospecific ion must be formed,although hydrogen is the only source of protons.


What is the formula for the hydronium ion?

H3O+

The hydronium ion is formedby combining a hydrogen ion and a water molecule.

H2O + H+ H3O+


conjugate base


A conjugate base is the

particle that remains

AFTER an acid gives

up a proton.


conjugate acid


A conjugate acid is the

particle formed when a

base accepts a proton.


HCl + H2O Cl- + H3O+

Identify the B-L acid in this equation.

What gives up a proton fromthe left side to the right?


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?



H2O accepts a proton,it is the B-L base.


Identify the conjugate

base in this equation.

What is left when the

acid gives up a proton?


Cl- is left when HCl gives up a proton, itis the conjugate base.


Identify the conjugate

acid in this equation.

What is formed when the

base accepts a proton?


H3O+ is formed whenwater accepts a proton,it is the conjugate acid.


acids have conjugate bases


bases have conjugate acids

Remove a proton from an acid to get its conjugate base.

H2SO4

HI

H2O


HSO4-H2SO4

HI

H2O


HSO4-

I-

H2SO4

HI

H2O


HSO4-

I-

OH-

H2SO4

HI

H2O

Add a proton to a base to get its conjugate acid.

Cl-

H2O

NO3-


HClCl-

H2O

NO3-


HCl

H3O+

Cl-

H2O

NO3-


HCl

H3O+

HNO3

Cl-

H2O

NO3-

GilbertNewtonLewis



The Lewis TheoryThe Lewis Theory

Lewis AcidLewis Acid

QuickTime™ and aTIFF (Uncompressed) decompressorare needed to see this picture.

Any substance thatacts as anelectron-pairacceptor.

Lewis BaseLewis Base


Any substance thatacts as anelectron-pairdonor.



This theory is thebroadest of all.



Any reaction thatinvolves the exchangeof electrons WILL have a Lewis acidand Lewis base.


In an equation, the Lewisacid gets

MORE NEGATIVEfrom the left side to theright side - it gains e-.


In an equation, the Lewisbase gets

MORE POSITIVEfrom the left side to theright side - it loses e-.

Cl2 + I- Cl- + I2

Identify the Lewis acid

in this equation.

What gets more negative?

Cl2 gets more negative

from the left side to the

right, it is the Lewis acid.

Cl2 + I- Cl- + I2

Identify the Lewis base

in this equation.

What gets more positive?

Cl2 + I- Cl- + I2

I- gets more positive

from the left side to the

right, it is the Lewis base.

Cl2 + I- Cl- + I2

End Acid - Base

Theories

End Acid - Base

Theories






Binary AcidsBinary 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 AcidsNaming Binary Acids

First:

Determine the stem word.

Example - HCl

chlorine is the negative

element - CHLOR is the stem.


Second:

Add the prefix hydro

to the stem.


Second:

Add the prefix hydro

to the stem.

Example - hydro + chlor


Third:

Change the ending

of the stem to ic.


Third:

Change the ending

of the stem to ic.

Example - hydro + chlor + ic


Final name:

hydrochloric acid


• HCl

• HF

• HBr

• HI


• HCl hydro chlor ic acid

• HF

• HBr

• HI



• HF hydro fluor ic acid

• HBr

• HI




• HBr hydro brom ic acid

• HI




• HBr hydro brom ic acid

• HI hydro iod ic acid


Ternary acids composed of

three elements:

hydrogen, oxygen,

and a nonmetal

Naming Ternary AcidsNaming Ternary Acids

First:

Determine the stempart of the name of

the third element


First:

Determine the stemExample - H2SO4

sulfur is the third element,

SULFUR is the stem.


Second:

The most common form of the acid is given the suffix ic.


Second:

The most common form of the acid is given the suffix ic.

Example - sulfur + ic acid


Third:

If the acid is NOT in its

most common form,

do the following:



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


Example - H2SO5

per + sulfuric acid


Naming Ternary AcidsNaming Ternary AcidsAdd the suffix ous if the acid

has one less oxygen than


Add the suffix ous if the acid

has one less oxygen than


Example - H2SO3

sulfur + ous acid



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 - H2SO2

hypo + sulfur + ous acid


HClO3 Chloric Acid


HClO4

HClO3 Chloric Acid


HClO4 Perchloric Acid

HClO3 Chloric Acid



HClO3 Chloric Acid

HClO2



HClO3 Chloric Acid

HClO2 Chlorous Acid



HClO3 Chloric Acid

HClO2 Chlorous Acid

HClO



HClO3 Chloric Acid

HClO2 Chlorous Acid

HClO Hypochlorous Acid


Strong or

Weak

Strong or

Weak

Strong or WeakStrong or Weak

Strong acids and bases

ionize completely in

water solution.


HCl, HBr, and HI are the

only Strong binary acids.


In Strong ternary acids,

the number of oxygen

atoms exceeds the

number of...


hydrogen atoms by

two or more.H2SO4 and HNO3 are strong.

H3PO4 is weak.


Hydroxides of

groups 1 and 2,

except Be, are

Strong bases.

AmphotericAmphoteric

A substance that acts

as either an acid or

base, depending on

what it reacts with.

Water is the most

common amphoteric

substance.

HOHHOH

Anhydrous -

Without H2O

Acid Anhydride -

an oxide that produces

an acid in water.

SO2 + H2O H2SO3

Acid Anhydride -

oxides of nonmetals

Basic Anhydride -

an oxide that produces

a base in water.

Na2O + H2O 2NaOH

Basic Anhydride -

oxides of metals

Anhydrous - Without H2OAnhydrous - Without H2O

Write the anhydrous form of:

1. H2SO3

2. H2C2O4

3. H3PO4

4. H4C2O2



1. H2SO3 SO2

2. H2C2O4

3. H3PO4

4. H4C2O2



1. H2SO3 SO2

2. H2C2O4 C2O3

3. H3PO4

4. H4C2O2



1. H2SO3 SO2

2. H2C2O4 C2O3

3. H3PO4 HPO3

4. H4C2O2



1. H2SO3 SO2

2. H2C2O4 C2O3

3. H3PO4 HPO3

4. H4C2O2 C2

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Acids & Bases Water and acid combine in an exothermic reaction - releasing large amounts of heat