chapter 5 nomenclature of inorganic...

Chapter 5

Nomenclature of Inorganic Compounds

What type of compound is it ?

Ionic Compound Covalent (Nonionic) Compound Acid

Cation with fixed charge

Cation with variable charge

Binary Contains polyatomic ion Binary Contains

polyatomic ion

Binary Acid

Oxy Acid

Aluminum, AlChlorine, Cl2 Aluminum chloride, AlCl3Iron (II) chloride, FeCl2Sodium Phosphate, Na3PO4Tin (IV) Chloride SnCl4 Carbon monoxide, COCarbon dioxide, CO2Hydrochloric Acid, HClPerchloric Acid, HClO4

atomic element

ionic compoundmolecular element

molecular compound

ionic compoundionic compound

ionic compound

molecular compoundbinary acidoxy acid

What type of compound is it ?Practice:

Ionic Compounds

Compounds of metals with nonmetals are made of ions. Metal atoms form cations, nonmetal atoms form

anions.

No individual molecule units. A 3-dimensional array of cations and anions made of formula units.

Many contain polyatomic ions-several atoms attached together by covalent bonds into one ion.

Compound must have no total charge, therefore we must balance the numbers of cations and anions in a

compound to get o charge.

Naming Metal Cations

Some metals have one possible charge

Groups 1A1+ & 2A2+, Al3+, Ag1+, Zn2+, Sc3+

cation name = metal name

Naming Metal Cations

Metals with Variable Charges metals whose ions can have

more than one possible charge

Determine charge by charge on anion and cation

cation name = metal name (charge)

IVA VA VIA VIIA

H -

hydride

C4-

carbideN3-

nitrideO2-

oxideF -

fluoride

Si4-

silicideP3-

phosphideS2-

sulfideCl -

chloride

As3-

arsenideSe2-

SelenideBr -

bromide

Te2-

TellurideI -

iodide

Naming Monatomic Nonmetal AnionsDetermine the charge from position on the Periodic Table.

To name anion, change ending on the element name to –ide.

Naming Binary Ionic Compounds for Metals with Invariant Charge

1. Name the metal cation first, name nonmetal anion second

2. Cation name is the metal name

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

name of cation(metal)

base name of anion (nonmetal) “ide”+ +

1. KCl

2. MgBr2

3. Al2S3

potassium chloride

magnesium bromide

aluminum sulfide


base name of anion (nonmetal) “ide”+ +

Name the following compounds

Naming Binary Ionic Compounds for Metals with Invariant Charge

Naming Binary Ionic Compounds for Metals with Variable Charge

1. Name metal cation first, name nonmetal anion second

2. The metal cation name is the metal name followed by a Roman numeral in parentheses to indicate its charge which is determined by charge on the anion.

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


base name of anion (nonmetal) “ide”+( )+ +charge of cation (metal)

in roman numerals

Determine a charge from the formula of a specific compound.

The sum of all the charges must be zero.

Example: The charge on iron (Fe) in FeCl3 must be 3+ in order for the compound to be charge neutral with

the three Cl- anions.


base name of anion (nonmetal) “ide”+( )+ +charge of cation (metal)

in roman numerals

Name the following compounds

1 CuF2 2. TiCl4 3. PbBr2

4. CrO3

5. Fe3N2

6. Fe2S3

Charge on Cation?Cu= 2+

Ti = 4+

Pb = 2+

Cr = 6+Fe = 2+Fe= 3+

copper (II) fluoride

titanium (IV) chloride

lead (II) bromide

chromium (VI) oxideiron (II) nitrideiron (III) sulfide

Na +Na

Cl - NaCl

ClFeCl2

Fe

Fe 2+

Cl

Cl - Cl -

Cl

Fe 3+FeCl3

Using dot structures can illustrate the formation of binary ionic compounds.

sodium chloride

iron (II) chloride

iron (III) chloride

ClFe

Cl

Cl

Cl -

Cl -Cl -

O

FeOFe

Fe 2+

Na

Na

O 2-Na +Na +

Na2O

Using dot structures can illustrate the formation of binary ionic compounds.

sodium oxide

iron (II) oxide

iron (III) oxide

O O 2-

Fe Fe

O O O

Fe 3+

Fe 3+

O 2-

O 2-O 2- Fe2O3

Compounds Containing Polyatomic Ions

Polyatomic ions are ions that contain more than one atom.

Often identified by parentheses around ion in formula

Name and charge of polyatomic ion do not change

An ionic compound is always named by naming the cation first and then the anion.

Roman numeral indicating charge

(if needed)

name of cationic species

name of anionic species

+ +

Compounds Containing Polyatomic Ions

metal or polyatomic

cation

nonmetal or polyatomic

anion

Name the Following Compounds

1. Na2SO4

2. Fe(NO3)3

3. NH4Cl

4. Ca(C2H3O2)2

5. Cu(NO3)2

sodium sulfate

iron (III) nitrate

ammonium chloridecalcium acetate

copper(II) nitrate

SO42-, sulfate; NO3 -, nitrate;

NH4 +, ammonium; (C2H3O2) -, acetate

Writing formula for ionic compounds containing polyatomic ions

Aluminum sulfate

Iron (III) phosphate

Chromium (II) hydrogen carbonate

Al2(SO4)3

FePO4

Cr(HCO3)2

SO42-, sulfate; PO4 3-, phosphate;

(HCO3) -, hydrogen carbonate

Hydrates

Hydrates are ionic compounds containing a specific number of waters

for each formula unit.

In formula, attached waters indicated

CoCl2·6H2O or CoCl2(H2O)6

In name attached waters indicated by prefix+hydrate

after name of ionic compound:

CoCl2·6H2O cobalt(II) chloride hexahydrate

CaSO4·½H2O calcium sulfate hemihydrate

Writing Names of Binary Molecular Compounds of Two Nonmetals

1. Write name of first element in formula a) element furthest left and down on the Periodic Table b) use the full name of the element

2. Writes name the second element in the formula with an -ide suffix, as if it were an anion, however, remember these compounds do not contain ions!

3. Use a prefix in front of each name to indicate the number of atoms (Never use the prefix mono- on the first element)

Subscript <–> Prefixes

1 = mono- 2 = di- 3 = tri- 4 = tetra- 5 = penta-

6 = hexa- 7 = hepta- 8 = octa- 9 = nona-10 = deca-

prefix prefix “ide”name of first element

name of second element+ + + +

BF3

NO2

PCl5

I2F7

Formulas --------------> Names

boron trifluoride

nitrogen dioxide

phosphorous pentafluoride

diiodine heptafluoride



Name -------------> Formula

dinitrogen pentoxide

dinitrogen tetroxide

sulfur hexafluoride

diarsenic trisulfide

N2O5

N2O4

SF6

As2S3



Acids

Acids are molecular compounds that form H+ when dissolved in water.

(aq) is often written after the formula

Sour taste

Dissolve many metals such as Zn, Fe, Mg; but not Au, Ag, Pt

Formula generally starts with H e.g., HCl, H2SO4

The oxygen is generally associated with a polyatomic anion.

Acids

Binary Acidscontain only two elements

Oxyacidscontain oxygen

Naming Binary Acids

HCl HF HI

hydrochloric acid

base name of nonmetal“hydro” “ic” acid+ + +

hydrofluoric acidhydroiodic acid

Naming OxyacidsName the polyatomic anion !!!!!

If polyatomic ion name ends in –ate,

base name of oxyanion

“ic” acid

If polyatomic ion name ends in –ite,


“ous” acid

+ +

+ +

Oxyanion formula

Oxyanion name Acid Formula

Acid Name NO2 ⊖ nitrite H+ HNO2 nitrous

NO3 ⊖ nitrate H+ HNO3 nitric

SO3 2⊖ sulfite 2H+ H2SO3 sulfurous

SO4 2⊖ sulfate 2H+ H2SO4 sulfuric

ClO2 ⊖ chlorite H+ HClO2 chlorous

ClO2 ⊖ chlorate H+ HClO3 chlorate

C2H3O2 ⊖ acetate H+ HC2H3O2 acetic

CO3 2⊖ carbonate 2H+ H2CO3 carbonic

Names of Common Oxyacids and Their Oxyanions

Naming Oxyacids

“-ate” = “-ic” ; “-ite” = “-ous”

H2SO4 sulfuric acidH2SO3 sulfurous acid

HClO hypochlorous acidHClO2 chlorous acidHClO3 chloric acidHClO4 perchloric acid

“-ate” = “-ic” ; “-ite” = “-ous”

Naming Oxyacids

Naming OxyacidsName the polyatomic anion !!!!!

If polyatomic ion name ends in –ate,


“ic” acid

If polyatomic ion name ends in –ite,


“ous” acid

+ +

+ +

Formula ----------> Namea. HCl(aq)

b. HBr(aq) c. H2S(aq)

d. H2SO4 e. H2SO3

f. HClO3

g. HNO2

hydrochloric acid

hydrobromic acid

hydrosulfuric acid

sulfuric acid

sulfurous acid

chloric acid

nitrous acid

SO4 2-, sulfate

SO3 2-, sulfite

ClO3-, chlorate

NO2-, nitrite

a. chlorous acid

b. phosphoric acid

c. hydroiodic acid

Name ----------> Formula

HClO2

H3PO4

HI (aq)

chapter 5 nomenclature of inorganic...

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