Nomenclature!!!

Nomenclature!!!

What’s in a name?

REMEMBER!!!

1. When naming compounds ALWAYS, ALWAYS have a periodic table in front of you!

2. Ions – positively or negatively charged atom due to an decrease or increase of electrons– Cations – positively charged ( metals that loose

electrons) ex. Na+

– Anion – negatively charged (non-metal that gains electrons) ex. Cl-

Predicting Charges on Monatomic IonsPredicting Charges on Monatomic IonsKNOW THESE !!!!KNOW THESE !!!!

+1 +2 +3 -3 -2 -1 0

Cd+2

Quick Review

Write the correct formula for the compounds containing the following ions:1. Na+, S2-

a) NaS b) Na2S c) NaS2

2. Al3+, Cl-

a) AlCl3 b) AlCl c) Al3Cl

3. Mg2+, N3-

a) MgN b) Mg2N3 c) Mg3N2

Naming Binary Ionic Compounds

• Binary Ionic Compound– A compound that has 2 atoms– 1 cation and 1 anion– Cation is always first

• Two types– Type I– Type II


• Type I– The metal only forms 1 type

of cation– ex. Li Li+

• Type 2– The metal can form 2 or more

cations– ex. Cu Cu+ or Cu2+


• How can you tell if it is a Type I or Type II?– Type I: Group 1 and 2,

Al, Zn, Cd, and Ag,

– Transition metals are almost always Type II

Binary Ionic CompoundsType I

Rules for Naming Type I Ionic Compounds1.Cation (metal) is named before the anion (non-

metal).2.Cation (metal) is the name of the element.3.Anion (non-metal) is the “root” of the element +

ide4.Combine the Cation and Anion


Ex. NaCl1.Cation is named before the anion.

– we know that Na is first because it’s a cation

2.Cation is the name of the element.– Na is Sodium

3.Anion is the “root” of the element + ide– Cl is Chlorine, root is Chlor + ide = Chloride

4.Combine the Cation and Anion– Sodium Chloride is the name!!

Lets try one on our own: NaI

Ex. NaI1. Cation is named before the anion.

– we know that Na is first because it’s a cation2. Cation is the name of the element.

– Na is Sodium3. Anion is the “root” of the element + ide

– I is Iodine, root is Iod + ide = Iodide4. Combine the Cation and Anion

– Sodium Iodide is the name!!

Lets try another: CaO

Ex. CaO1. Cation is named before the anion.

– we know that Ca is first because it’s a cation2. Cation is the name of the element.

– Ca is Calcium 3. Anion is the “root” of the element + ide

– O is Oxygen, root is Ox + ide = Oxide4. Combine the Cation and Anion

– Calcium Oxide is the name!!


• Notice:• The formula doesn’t show the charges of the

individual ions.• Ex. NaCl means Na+ is present with Cl-

• Ex. CaS means Ca2+ is present with S2-

Let’s try some!!

• CsF

• AlCl3

• MgI2

Binary Ionic CompoundsType II

• Some metals can form more than one ion.• This is what makes them Type II• Ex. Lead(Pb) => Pb2+ or Pb4+

• Ex. Iron(Fe) => Fe2+ or Fe3+

• Transition metals are almost always Type II


• To name these we use the same naming method except we add a Roman numeral to the cation name.

• The anion stays the same as before.

It’s so easy….even a caveman could do it.

Binary Ionic CompoundsType II (the cation)

EXTEMELY IMPORTANT!!!• The Roman numeral tells the charge, not the #

of ions present. • Ex. Fe3+ => iron(III) and Fe2+ => iron(II)• Ex. Pb2+ => lead(II) and Pb4+ => lead(IV)

You would be wise to remember this.

Binary Ionic CompoundsType II (the anion)

• The anion will be named the same way as with Type I (using ide for the ending)

• Anion is the “root” of the element + ide• Ex. O is Oxygen, root is Ox + ide = Oxide• Ex. Cl is Chlorine, root is Chlor + ide = Chloride


• All together:• FeCl2 => iron(II) chloride

• PbO2 => lead(IV) oxide

• How do we know it’s iron(II) and not iron(III)• How do we know it’s lead(IV) and not lead(II)• Lets take a closer look.

FeCl2

• We are given FeCl2

• We know the overall charge has to be natural.• We know:

– Cl is going to have a 1- charge. – there are 2 Cl– Cl2 has an overall charge of 2-

– There is only one Fe atom– Therefore the one Fe has to have a charge of 2+

• Draw out on board iron(II) chloride

PbO2

• We are given PbO2

• We know the overall charge has to be natural.• We know:

– O is going to have a 2- charge. – there are 2 O– O2 has an overall charge of 4-

– There is only one Pb atom– Therefore the one Pb has to have a charge of 4+

• Draw out on board lead(IV) oxide

Remember!!!

• The Roman numeral in a name indicates the charge of the ion, not the subscript in the formula.

• Ex. Iron(II) oxide => FeO• Ex. iron(II) chloride => FeCl2

Let’s try some!!!

• CuCl

• HgO

• Fe2O3

Naming Molecular Compounds

CH4 methaneBCl3 boron trichloride

CO2 Carbon dioxide

All are formed from two or more nonmetals.

Ionic compounds generally involve a metal and nonmetal (NaCl)

Binary Covalent Compound

Rules for naming: Prefix System 1.The first atom is the element name.2.The second atom is named like an anion.3.Add prefixes to indicate # of atoms. Omit

mono- prefix on the FIRST element. Ex. PCl3 => phosphorus trichloride

Binary Covalent Compound

• These are the prefixes that are used to indicate the number of atoms in a compound.

• Mono is never used for the first atom.

Binary Covalent Compound:I207

1. The first atom is the element name.– I becomes iodine

2. The second atom is named like an anion.– O is Oxygen, root is ox + ide = oxide

3. Prefixes are given to each atom to tell the number of atoms present.

– di = 2, hepta = 7– so… di + iodine = diiodine– and… hepta + oxide = heptoxide– Answer: diiodine heptoxide

Binary Covalent Compound:CF4

1. The first atom is the element name.– C becomes carbon

2. The second atom is named like an anion.– F is fluorine, root is fluor + ide = fluoride

3. Prefixes are given to each atom to tell the number of atoms present.

– mono = 1, tetra = 4– so… mono + carbon = monocarbon– and… tera + fluoride = tetrafluoride– Answer: carbon tetrafluoride– REMEMBER!!! Mono is never used for the first atom.

Let’s try some!!!

• BF3

• NO

• N2O5

Naming Binary Compounds Review

Review Practice1. AsF3

2. Al2S3

3. SnBr4

4. CS2

5. CdS

6. silver chloride7. dinitrogen pentaoxide8. iron(III) chloride9. phosphorus pentaoxide10.manganeses(IV) oxide

More Complex Compounds!!

Polyatomic Ions

• Polyatomic Ions– Charged entities composed of several atoms

bound together– Assigned special names– No system, must be memorized– (don’t worry you don’t have to, just know how to

use it)

• Ex. CN-, NH4+, NO3

-

Polyatomic Ions (pg 109)

Polyatomic IonsOxyanions

• Some of these polyatomic ions are called Oxyanions

• They contain an atom and different #’s of oxygen atoms.

• Ex. NO3-, ClO2

-, PO43-


• Some of these oxyanions, form in a series.• The smaller # O, ends with ite• The larger # O, ends with ate• Ex. NO2

- => nitrite

• Ex. NO3- => nitrate


• If there are more than 2 then…• The smallest # O, begins with hypo

– meaning less than

• The largest # O, begins with per– meaning more than

• Ex. ClO- => hypochlorite• Ex. ClO4

- => perchlorate


• All combined• smallest = hypo => ClO- = hypochlorite• Small = ite => ClO2

- = chlorite

• Large = ate => ClO3- = chlorate

• largest = per => ClO4- = perchlorate

• Now back to the naming complex compounds• Need to do one thing.

– Recognize common polyatomic ions

• Now when you see NH4C2H3O2 you can break it down.

• NH4- => ammonium

• C2H3O2 => acetate

• It’s name is ammonium acetate

• NH4- => ammonium

• C2H3O2+ => acetate

• NH4C2H3O2

• Notice that it’s separate parts have a charge but together they are neutral

• Just like binary compounds.

• Also like Type II, Binary Compounds, you may need Roman numerals

• Ex. FeSO4 => iron(II) sulfate

• Ex. Mn(OH)2 => manganese(II) hydroxide

FeSO4

• What are the two parts?• We know the overall charge has to be natural.• We know:

– SO4 is going to have a 2- charge.

– There is only one Fe atom– Therefore the one Fe has to have a charge of 2+– So the name is iron(II) sulfate

• Draw out on board

Mn(OH)2

• What are the two parts?• We know the overall charge has to be natural.• We know:

– OH is going to have a 1- charge. – There are 2 OH– (OH)2 has an overall charge of 2-

– There is only one Mn atom– Therefore the one Mn has to have a charge of 2+– So the name is manganese(II) hydroxide

Lets practice some!!

• Na2(SO)4

• KH2PO4

• Fe(NO3)3

Naming Acids!!

Acids

• Is a molecule with one or more H+ ions attached to an anion.

• Translation:– A molecule with H+ and non-metals

• Ex. HCl, HCN, H2S

Naming Acids

• Two types:1.Ones that contain oxygen2.Ones without oxygen

Those with oxygen

1. Start with the root of the anion.2. Add the prefix hydro3. Add the suffix icEx. hydrochloric acidEx. hydrofluoric acid

HCl

1. Start with the root of the anion.Cl is chlorine, root => chlor

2. Add the prefix hydrohydro + chlore = hydrochlore

3. Add the suffix ichydrochlore + ic = hydrochloreic

Answer: hydrochloreic acid

HF

1. Start with the root of the anion.F is fluorine, root => fluor

2. Add the prefix hydrohydro + fluor = hydrofluor

3. Add the suffix ichydrofluor + ic = hydrofluoric

Answer: hydrofluoric acid

A few exceptions

• HCN => hydrocyanic acid• H2S => hydrosulfuric acid

• Why are they exceptions?

Lets try a few

• HBr

• HI

Those with out oxygen

1. Start with the root of the anion.2. If the anion ends with an ate

– Drop the ate and add ic– Ex. Acetic acid

3. If the anion ends with ite– Drop the ite and add ous– Ex. Nitrous acid

HC2H3O2

1. Start with the root of the anion.C2H3O2 is Acetate = > root is acet

2. If the anion ends with an ate– Drop the ate and add icAcet + ic => aceticAnswer: acetic acid

3. If the anion ends with ite– Drop the ite and add ous– Ex. Nitrous acid

HNO2

1. Start with the root of the anion.NO2 is nitrite = > root is nitr

2. If the anion ends with an ate– Drop the ate and add ic

3. If the anion ends with ite– Drop the ite and add ous– Ex. Nitrous acidNitr + ous => nitrousAnswer: nitrous acid

A few exceptions

• Sulfur– H2SO4 => sulfuric acid

• H3PO4 => phosphoric acid

• How are they exceptions?

Lets try a few

• HClO4

• HNO3

Perchloric acid

Nitric acid

Naming acids flow chart

Lets try a few

• Pg 111 practice problems (yellow box)– #’s a-g

• Pg 112 practice problems (yellow box)– #’s a-g

• Pg 115 practice problems (yellow box)– #’s a-e

Nomenclature!!!

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