Introductory Chemistry: A Foundation FOURTH EDITION by Steven

Introductory Chemistry:

A Foundation

FIFTH EDITION by Steven S. Zumdahl

University of Illinois

Copyright©2004 by Houghton

Mifflin Company. All rights reserved.

1

Nomenclature

Chapter 5



2

Mineral towers in Mono Lake,

California

Source:



3

An Apothecary Shop



4

Naming of Compounds

•

Naming of compounds has long been necessary to identify something

• Names originally based upon “common names”

– Common name

–

Epsom salts

–

Gypsum

– Blue vitriol

–

Calomel

–

Saltpeter

– Quicklime

–

Caustic soda

Stock system name

Magnesium chloride

Calcium sulfate

Copper (II) sulfate

Mercury (I) chloride

Potassium nitrate calcium oxide sodium hydroxide



5

An ancient painting showing

Romans drinking wine.

Sugar of Lead

•

Boiling of wine produced a thick, sweet liquid which was used as a sweetener.

•

Actually contained lead acetate

– Pb(C

2

H

3

O

2

)

2

–

Thought to have lead to the downfall of the

Roman empire due to lead poisoning (in addition to lead water pipes)

–

Lead poisoning causes lethargy and mental illness



7

Problems

•

These common names were impractical

–

Worldwide communication problems

–

4 million compounds

– We needed a system to “systematically” name all of these compounds, you wouldn’t have to memorize each name to know what it was.

–

If you learn the system, you will be able to name a compound from its formula and vice versa



8

Common Names - Exceptions

• Common names still in use today……..

•

H

2

O = water, steam, ice

•

NH

3

•

CH

4

= ammonia

= methane

•

NaCl = table salt

•

C

12

H

22

O

11

= table sugar

•

CaSO

4

•2H

2

O=plaster of paris



9

An artist using plaster of Paris, a gypsum plaster.

Source:



10

Naming Starts with Classifying Compounds

1.

Binary Compounds = only 2 elements

2.

Compounds containing polyatomic ions

(sometimes called “ternary” compounds)

3.

Acids = formula generally starts with H



11

5.2 Naming Compounds

Binary Type I and II



12

Classifying Binary Compounds

•

Compounds containing a metal and a nonmetal are binary ionic

–

Type I and II

•

Compounds containing two nonmetals are

Covalent

–

Type III

• Compounds containing H and a nonmetal = Acids



13

Binary Ionic

•

Made of metal cation and nonmetal anion

•

Name by naming the ions



14

Metal Cations

•

Type I

–

Metals that can only have one possible charge

–

Determine charge by position on the

Periodic Table

•

Type II

–

Metals that can have more than one possible charge

– Determine metal cation’s charge from the charge on anion



15



16

Type I Binary Ionic Compounds

•

Contain Metal Cation + Nonmetal Anion

•

Metal listed first in formula & name

¶

Name metal cation first, name nonmetal anion second

¶

Simple metal cation name is the metal name

– simple metals are Groups 1A, 2A and Al, Ga & In

¶

Nonmetal anion named by changing the ending on the nonmetal name to ide



17

•

KCl

•

MgBr

2

•

SrO

•

Al

2

O

3

•

Rb

3

N

•

KI

Examples

potassium chloride magnesium bromide strontium oxide aluminum oxide rubidium nitride potassium iodide



18

Type II Binary Ionic Compounds

•

Contain Metal Cation + Nonmetal Anion

• Metal listed first in formula & name

¶

Name metal cation first, name nonmetal anion second

¶

Metal cation name is the metal name followed by a

Roman Numeral in parentheses to indicate its charge

–

Determine charge from anion charge

–

Common Type II cations in Table 5.2

¶

Nonmetal anion named by changing the ending on the nonmetal name to ide



19



20

Determining the Charge on a Cation – Au

2

S

3



Determine the charge on the anion

Au

2

S

3

- the anion is S, since it is in Group 6A, its charge is -2



Determine the total negative charge since there are 3 S in the formula, the total negative charge is -6



Determine the total positive charge since the total negative charge is -6, the total positive charge is +6



Divide by the number of cations since there are 2 Au in the formula & the total positive charge is +6, each Au has a +3 charge



21

•

FeS

•

Fe

2

S

3

•

Cu

2

O

•

CuO

•

PbCl

2

•

PbCl

4

•

Hg

2

Se

Examples

iron (II) sulfide iron (III) sulfide copper (I) oxide copper (II) oxide lead (II) chloride lead (IV) chloride mercury (II) selenide



22


Binary Type III



23

Type III - Binary Compounds of 2 Nonmetals

•

Name first element in formula first, use the full name of the element

•

Name the second element in the formula as if it were an anion

– However, remember these compounds do not contain ions, they are covalent compounds!!!!!!

•

Use a prefix in front of each name to indicate the number of atoms

•

Never use the prefix monoon the first element



24

Prefixes

Subscript

1

5

6

7

8

2

3

4

Prefix mono-

(not used on first nonmetal) ditritetrapentahexaheptaocta-

• Drop last “a” in the prefix if the name begins with vowel



25



26

•

CO

•

CO

2

•

BF

3

•

N

2

O

5

•

NO

•

CCl

4

•

NO

2

Examples

carbon monoxide carbon dioxide boron trifluoride dinitrogen pentoxide nitrogen monoxide carbon tetrachloride nitrogen dioxide



27

•

Na

2

O

•

Cs

3

N

•

H

2

O

•

Mg

3

P

2

•

CuF

•

CrCl

3

A mix of types

LiF

SnO

HgS

CoN

NCl

3

CS

2



28


Containing Polyatomic Ions



29

Compounds Containing

Polyatomic Ions

•

Polyatomic ions are charged entities that contain more than one atom

–

Must memorize name, formula and charge

– Look for Patterns!!

•

Polyatomic compounds contain one or more polyatomic ions

•

Name polyatomic compounds by naming cation and anion

– Non-polyatomic ions named like Type I and II

•

Polyatomic Acids contain H + and a polyatomic anion



30

Polyatomic Ions to be memorized!!!!!!

• Carbonate

•

Nitrate

• Phosphate

•

Chlorate

• Bromate

•

Sulfate

• Hydroxide

•

Ammonium

CO

3

2-

NO

3

1-

PO

4

3-

ClO

3

1-

BrO

3

1-

SO

4

2-

OH 1-

NH

4

1+



31



32

Copper (II) sulfate crystals.



33

Patterns for Polyatomic Ions



Elements in the same column on the Periodic

Table form similar polyatomic ions

– same number of O’s and same charge

ClO

3

= chlorate



BrO

3

= bromate



If the polyatomic ion starts with H, add hydrogen - before the ions name and add 1 to the charge

CO

3

2= carbonate



HCO

3

= hydrogen carbonate



34

Patterns for Polyatomic Ions

•

-ate ion

– chlorate = ClO

3

-

• -ate ion plus 1 O

 same charge, perprefix

– perchlorate = ClO

4

-

• -ate ion minus 1 O

 same charge, ite suffix

– chlorite = ClO

2

-

• -ate ion minus 2 O

 same charge, hypoprefix, ite suffix

– hypochlorite = ClO -



35

Oxyanions

•

Polyatomic ions that contain a given element and different numbers of oxygen atoms

– SO

2

2-

–

SO

3

2-

– SO

4

2-

–

SO

5

2hyposulfite ion sulfite ion sulfate ion persulfate ion



36

Some other Oxyanions

•

CO

3

2Carbonate, etc

•

NO

3

1Nitrate, etc

•

ClO

3

1Chlorate, etc

•

PO

4

3Phosphate, etc



37

•

NaNO

3

•

CuSO

4

•

Ca

3

(PO4)

2

•

Fe(OH)

2

•

NH

4

ClO

3

•

Mg(ClO

4

)

2

Name these…..



38

5.6 Naming Acids



39

Acids

•

Contain H + cation and anion

•

Binary acids have H + cation and a nonmetal anion

•

Oxyacids have H + cation and a polyatomic anion



40



41



42

Rules for Naming Acids

•

If anion does not contain oxygen, acid is named with hydro- added to the front of anion, and –ic is added to end of anion name, along with acid

–

HCl hydro chlor ic acid

– HF hydro fluor ic acid

–

H

2

S hydro sulfur ic acid



43

Rules for Naming Acids cont.

•

When anion contains oxygen (oxyanion) the root name of the anion is used, along with

– ic acid for oxyanions ending in –ate

– ous acid for oxyanions ending in –ite

– H

2

SO

4

–

HNO

3

– HNO

2 sulfate ion Sulfur ic acid nitrate ion Nitr ic acid nitrite ion Nitr ous acid



44

Other examples

HClO hypochlorite ion hypochlorous acid

HClO

HClO

3

2 chlorite ion chlorous acid chlorate ion chloric acid

HClO

4

•

HIO

4 perchlorate ion perchloric acid

?????!!!!!!



45

5.7 Writing Formulas from Names



46

Writing the Formulas from the Names

•

For Type III compounds, use the prefixes to determine the subscripts

•

For Type I, Type II, polyatomic

Compounds and Acids

– Determine the ions present

–

Determine the charges on the cation and anion

–

Balance the charges to get the subscripts



47

Figure 5.3: A flow chart for naming acids. The acid is considered as one or more H + ions attached to an anion.



48

Introductory Chemistry: A Foundation FOURTH EDITION by Steven

Introductory Chemistry:

A Foundation

Nomenclature

Mineral towers in Mono Lake,

California

An Apothecary Shop

Naming of Compounds

Sugar of Lead

Problems

Common Names - Exceptions

An artist using plaster of Paris, a gypsum plaster.

Classifying Binary Compounds

Binary Ionic

Metal Cations

Type I Binary Ionic Compounds

Examples

Type II Binary Ionic Compounds

Examples

Prefixes

Examples

A mix of types

Compounds Containing

Polyatomic Ions

Copper (II) sulfate crystals.

Patterns for Polyatomic Ions

Patterns for Polyatomic Ions

Oxyanions

Some other Oxyanions

Name these…..

5.6 Naming Acids

Acids

Rules for Naming Acids

Rules for Naming Acids cont.

Other examples

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Introductory Chemistry: A Foundation FOURTH EDITION by Steven