Nomenclature:

Naming Chemicals

POPO443-3-

phosphate ionphosphate ion

CC22HH33OO22--

acetate ionacetate ion

HC2H3O2

Acetic Acid

Before naming….Some things you MUST know to be successful…. You really need to commit these things to memory

Ions

Atoms or groups of atoms with a charge.Cations- positive ions - get by losing

electron(s).Anions- negative ions - get by gaining

electron(s).Ionic bonding- held together by the opposite

charges. (usually a metal and a nonmetal)Ionic solids are called salts.Salts are electrolytes; they conduct

electricity when dissolved in water (aq.)

Conductors of heat and electricity

Make cations (lose e- to become + charged)

Malleable (made into sheets)

Ductile (made into wire)

Are a brittle solid or a gas Make anions (gain e- to become - charged)

Covalently bond to each other

•Characteristics of both metals and nonmetals

•More metallic as you go down PT

Alkali Metals

Alkaline Earth Metals

Transition metals

Inner Transition Metals

Halogens

Noble Gases

+1+2 -1-2-3+/-4+3

Variable, always +

Common Ions of Elements

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

+1 +2 -3 -2 -1 0

Cd+2

Polyatomic Ions

Groups of covalently bonded atoms that have a charge.* NO3

- :nitrate ion* NO2

- :nitrite ionYes, you have to

memorize them.Listed in your

resource handbook: memorize the required list!!!!

Patterns for Polyatomic Ions-ate ion

chlorate = ClO3-

-ate ion plus 1 O same charge, per- prefixperchlorate = ClO4

-

-ate ion minus 1 O same charge, -ite suffixchlorite = ClO2

-

-ate ion minus 2 O same charge, hypo- prefix, -ite suffixhypochlorite = ClO-

Polyatomic IonsPolyatomic IonsYou can make additional polyatomic ions by adding a H+

to the ion!CO3 -2 is carbonate

HCO3– is hydrogen carbonate

PO4 3- is phosphate

HPO4 is hydrogen phosphate

H2PO4 is dihydrogen phosphate

HSO4–2 is hydrogen sulfate

The 3 types of Chemical Bonds:Ionic, Covalent, & MetallicElectronegativity and Bond type

Bond type can be determined by the difference in electronegativity between the bonds involved.

Differences of:≥ 2 = ionic0.5 – 1.9 = polar covalent ≤ 0.4 = nonpolar covalent

Metals bonded to other metals are metallically bonded, regardless of the difference in electronegativity

..

Metallic bondsThe atoms of metals

are held together when the atom’s valence electrons float around the nuclei of the metals – the “sea of electrons”

Electrostatic forces keep everything together

The 3 types of Chemical Bonds:Ionic, Covalent, & Metallic

Ionic—complete transfer of 1 or more electron from one atom to another (or another group)one loses one or more e-, the other gains those

e-

Atoms involved are a metal and either a non-metal or a

polyatomic ionThe cation and anion are attracted to

each other by electrostatic attraction

..

Ionic compounds are neutralIonic compounds are neutral

That is, they have no overall chargeThis is because the number of electrons that are given up by the metal is the same number of electrons that are gained by the anion for the formula.

Formulas reflect this neutrality- the charges on the individual ions are not written in because they cancel out overall for the compound

CATIONCATION + + ANIONANION ---> --->

COMPOUNDCOMPOUND

CATIONCATION + + ANIONANION ---> --->

COMPOUNDCOMPOUND

A neutral compound A neutral compound requiresrequires

equal number of + equal number of + and - charges.and - charges.

A neutral compound A neutral compound requiresrequires

equal number of + equal number of + and - charges.and - charges.

COMPOUNDS COMPOUNDS FORMED FROM FORMED FROM IONSIONS

COMPOUNDS COMPOUNDS FORMED FROM FORMED FROM IONSIONS

Na+ + Cl- --> NaCl

Covalent Bonds2, 4, or 6 valence electrons that are shared

between atomsWe are going to name only simple covalent

compounds that have 2 elements involved

Most bonds are somewhere in between ionic and covalent

Because not all atoms share e- equallyThe conventions of naming assume absolute

difference in bond typesMetals bonded to nonmetals or polyatomic

ions are classified as having ionic bonds*Materials made out of all non-metals are

classified as having covalent bonds** semimetals are not a classification in

naming; you need to treat the elements that are on the right of the line as non-metals, and those on the left as metals.

More on this when we talk about bonding

Naming things:If there is only one element present,

name it. Atomic substances do not require “special” naming.

For anything with more than one element, remember that there is ONE MAIN THING to look for:

Is there a metal first?

So…Look to see if there is a metal first in

the formula Again, semimetals are not a classification in

naming; you need to treat the elements that are on the right of the line as non-metals, and those on the left as metals.

If there are only metals, name both metals (metallic bonding; nothing else need be done)

If ONLY the first element is a metal, then the compound is an ionic compound

Nonmetals only signify a covalent compound

There is a flow chart in your handbook to help!

Naming ionic compounds:Remember that those are compounds

that have a metal first in the formula*, and then a nonmetal or a polyatomic ion.

*Two exceptions to this rule: Compounds that start with either ammoniums (NH4

+) or hydronium (H3O+)We can handle these as simple binary (2

element) and ternary (more than two element) compounds

General information for naming ionic compoundsIf the cation is monatomic- Name the

metal (cation). Use Roman Numerals for transition

metals (ONLY) after the metal If the cation is polyatomic- name it.If the anion is monatomic- name it

but change the ending to –ide. If the anion is poly atomic- just name

itPractice.

Name the cation first, then the anion root with an –ide suffix

For CaCl2, the monatomic cation is Ca2+ , calcium, and the monatomic anion is Cl , named chloride.

We use chloride because the root for chlorine is chlor, and we use = root + -ide for the second element in binary compounds

CaCl2 = calcium chloride

Example: CaCl2, or calcium chloride

Practice Naming Binary Ionic Compounds

Examples:

NaCl

ZnI2

Al2O3

Learning Check Complete the names of the following binary compounds:Na3N

KBr

Al2O3

MgS

If the Metal is a Transition Metal…Transition metals are Type II Cations, and

are elements that can have more than one

possible charge. They MUST have a

Roman Numeral to indicate the charge on

the individual ion.

1+ or 2+ 2+ or 3+

Cu+, Cu2+ Fe2+, Fe3+

copper(I) ion iron(II) ion copper (II) ion iron(III) ion

Type II CationsThese elements REQUIRE Roman Numerals because they can have more than one possible charge:anything except Group 1A, 2A, Ag, Zn, Cd, and Al

(You should already know the charges on these!)

Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.

FeCl3 (Fe3+) iron (III) chlorideCuCl (Cu+ ) copper (I) chlorideSnF4 (Sn4+) tin (IV) fluoridePbCl2 (Pb2+) lead (II) chloride

Fe2S3 (Fe3+) iron (III) sulfide

You will appreciate this more when we go from names to formulas!

Type II CationsSome Type II cations have a name

using the “old” system as well as the “new system”.

The old system, still widely used, adds to the root or stem of the Latin name of the metal the suffixes –ous and –ic. These represent the lower and higher charges respectively.

Learning Check Complete the names of the following binary compounds with variable metal ions:

FeBr2

CuCl

SnBr4

Fe2O3

Hg2S

Writing Formulas for Ionic Compounds from NamesFormulas of ionic compounds are determined

from the charges on the ions

Na + F Na+ + F- NaF

Sodium atom + fluorine atom sodium fluoride

Charge balance: 1+ + 1- = 0

Remember that all ionic compounds have no net charge, and that the charges are not written in! Ever. Nope.

Neutral, you say?Formulas are written to make the

compound have a neutral charge overall.

You do NOT write the charges in the formula because they MUST cross out to accurately represent the compound.

Ex: NaF2 is INCORRECT for sodium chloride because Na has an oxidation state of +1, and F of -1. There is a one to one ratio of Na+ to F- to make a neutral ionic compound.

Writing the formula…Write the formula for the barium chloride, the compound that will form between Ba2+ and Cl-.

Solution:1. Write the cation, and then the anion2. Balance charge with the number of +

and – ions

3. Write the number of ions needed as

subscripts:

BaBa++++ Cl- Cl- Think: Think: Cl-Cl- Why is ClWhy is Cl written twice? written twice?

BaClBaCl22

So what if the oxidation numbers aren’t even?If the oxidation numbers or charges do

not balance, you can write the number of ions of each until you get the same number of each charge in total.

Yes. The “Criss Cross” method. You take the charge number from the cation, and you make it the number of anions, and take the charge on the anion, and you make that many cations.

Is there an easier way?Is there an easier way?

Criss-Crossing in action:Example: Lead (II) nitrate

Pb2+ N3- *the charges do not balance

Pb2+ N3- Pb3N2

The 2 and the 3 are brought down to the opposite element, so that there are now 3 Pb2+ ions and 2 N3- ions

This means there were 6e- transferred from the lead atoms to the nitrogen atoms; the compound is neutral

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

a) NaS b) Na2S c) NaS2

2. Al3+ and Cl-

a) AlCl3 b) AlCl c) Al3Cl

3. Mg2+ and N3-

a) MgN b) Mg2N3 c) Mg3N2

Ternary Ionic Compounds:Contain at least 3 elementsThere MUST be at least one polyatomic ion

(it helps to circle the ions)Examples:NaNO3 Sodium nitrate

K2SO4 Potassium sulfate

Al(HCO3)3 Aluminum bicarbonate(Aluminum hydrogen

carbonate)

Name the cation first, then polyatomic ion

For NaNO3, the monatomic cation is Na+ , sodium, and the polyatomic anion is NO3

, named nitrate.

• NaNO3 is sodium nitrate

For Co(NO3)2, the monatomic cation is Co+2, cobalt (II) and the polyatomic anion is NO3

, named nitrate.

• Co(NO3)2 is cobalt (II) nitrate

Examples: Examples: NaNO3, and Co(NO3)2

Learning Check Match each set with the correct name:1. Na2CO3 a) magnesium sulfite

MgSO3 b) magnesium sulfate

MgSO4 c) sodium carbonate

2 . Ca(HCO3)2 a) calcium carbonate

CaCO3 b) calcium phosphate

Ca3(PO4)2 c) calcium bicarbonate

Writing Formulas for Ternary Ionic CompoundsWrite the cation first, then the anion. Overall charge must equal Overall charge must equal zerozero..

If charges cancelIf charges cancel, just write symbols.If not, use subscripts to balance charges.

Use parentheses to show more than one of a particular polyatomic ion.

Use Roman numerals indicate the ion’s charge when needed (transition metals)

Remember that the final formula should not have charges written in.

Writing Formulas with Polyatomic IonsExample:

Cr2+ PO43- *the charges do not balance

Cr2+ PO43- Cr3(PO4)2

The polyatomic ions is in parentheses whenever a subscript is added

This is so that we know to count a number of those groups!

Learning Check 1. aluminum nitrate a) AlNO3 b) Al(NO)3 c) Al(NO3)3

2. copper(II) nitrate a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3)

3. Iron (III) hydroxide

a) FeOH b) Fe3OH c) Fe(OH)3

4. Tin(IV) hydroxide

a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)

Ternary Ionic Nomenclature:You Criss-cross these, too.

Sodium Sulfate

Iron (III) hydroxide

Ammonium carbonate

Ternary Ionic Nomenclature:You Criss-cross these, too.

Sodium SulfateNa+ and SO4 -2

Na2SO4

Iron (III) hydroxideFe+3 and OH-

Fe(OH)3

Ammonium carbonateNH4

+ and CO3 –2

(NH4)2CO3

Write the Formula:

Copper (II) chlorate Calcium nitrideAluminum carbonatePotassium bromideBarium fluorideCesium hydroxide

General naming rules for covalent compoundsNames are two words, with prefixes.Prefixes tell you how many.First element whole name with the

appropriate prefix, except mono.Second element, -ide ending with

appropriate prefix.Practice

neverYou NEVER criss-cross charges with covalent compounds.

Since you are sharing electrons, rather than giving them away/ picking them up, the charges are not relevant.

Covalent Naming Prefixes:

PREFIXmono-di-tri-tetra-penta-hexa-hepta-octa-nona-deca-

NUMBER123456789

10

Name the first element, using a prefix if there is more than one atom of the element present

Name the second element, using the appropriate prefix in all cases

CO2 is carbon dioxide because there is one carbon (no prefix when there is only one atom of the element,) and two oxygens (di- prefix)

Example: Example: CO2 is carbon dioxide

Learning Check 1. P2O5 a) phosphorus oxide

b) phosphorus pentoxidec) diphosphorus pentoxide

2. Cl2O7 a) dichlorine heptoxide

b) dichlorine oxidec) chlorine heptoxide

3. Cl2 a) chlorineb) dichlorinec) dichloride

Learning Check Give the names of following covalent

compounds:

CO

CO2

PCl3

CCl4

N2O

CCl4

N2O5

SF6

Covalent Naming Examples

arsenic trichloride

dinitrogen pentoxide

tetraphosphorus decoxide

More Molecular Examples

Hydrates: Ionic Compounds·WaterSome salts trap water crystals when

they form crystals. Ex: CuSO4·5H2OThese are hydrates.Both the name and the formula

needs to indicate how many water molecules are trapped.

In the name we add the word hydrate with a prefix that tells us how many water molecules.

CuSO4·5H2O is copper (II) sulfate pentahydrate

HydratesIn the formula you put a dot and

then write the number of molecules.

Calcium chloride dihydrate = CaCl22

Chromium (III) nitrate hexahydrate = Cr(NO3)3 6H2O

Acid NomenclatureAcids

Compounds that form H+ in water.

Formulas usually begin with ‘H ’.

In order to be an acid instead of a gaseous covalent compound, it must be aqueous

Meaning dissolved in water; symbolized by (aq)

Ternary acids are ALL aqueous

Two types: Oxyacids Non-oxyacids

Naming acids

If the acid doesn’t have oxygenadd the prefix hydro-change the suffix -ide to -ic acid

HCl Hydrochloric acidH2S Hydrosulfic acid

HCN Hydrocyanic acid

Naming acidsIf the formula has oxygen in itwrite the name of the anion, but change

ate to -ic acidite to -ous acid

Watch out for sulfuric and sulfurous!

H2CrO4

HMnO4

HNO2

Chromic acid

Manganic acid

Nitrous acid

Acid Nomenclature Flowchart

Anion Ending Acid Name

-ide hydro-(stem)-ic acid

-ate (stem)-ic acid

-ite (stem)-ous acid

Acid Nomenclature

Binary Binary

Ternary Ternary

An easy way to remember which goes with which…An easy way to remember which goes with which…

““In the cafeteria, you In the cafeteria, you ATEATE something something ICICkyky””

HBr (aq)

H2CO3 (aq)

H2SO3 (aq)

Acid Nomenclature

HBr (aq)

H2CO3 (aq)

H2SO3 (aq)

2 elements, -ide

3 elements, -ate

3 elements, -ite

hydrobromic acid

carbonic acid

sulfurous acid

Acid Nomenclature

Acid Name

HNO3 Nitric acid

HNO2 Nitrous acid

H2SO4 Sulfuric acid

H2SO3 Sulfurous acid

H3PO4 Phosphoric acid

HC2H3O2 Acetic Acid

Name ‘Em!HI (aq)

H2C2O4

(aq)

H2S2O3

(aq)

HIO4 (aq)

Formulas for acidsBackwards from names.If it has hydro- in the name it has no oxygen

Anion ends in -ideNo hydro, anion ends in -ate or -iteWrite anion and add enough H to balance the charges.

hydrofluoric acid

phosphorus acid

nitrous acid

Acid Nomenclature

hydrofluoric acid

sulfuric acid

nitrous acid

2 elements

3 elements, -ic

3 elements, -ous

Acid Nomenclature

H+ F-

H+ SO42-

H+ NO2-

hydrofluoric acid

sulfuric acid

nitrous acid

2 elements

3 elements, -ic

3 elements, -ous

HF (aq)

H2SO4 (aq)

HNO2(aq)

Acid Nomenclature

H+ F-

H+ SO42-

H+ NO2-

Write the Formula!Hydrobromic acid

Boric acid

Carbonic acid

Phosphoric acid

Hydrotelluric acid

Write the Formula!Hydrobromic acid

Boric acid

Carbonic acid

Phosphoric acid

Hydrotelluric acid

HBr(aq)

H3BO3(aq)

H2CO3(aq)

H3PO4(aq)

H2Te(aq)

Common NamesA lot of chemicals have

common names as well as the proper IUPAC name.

Chemicals that should always be named by common name and never named by the IUPAC method are:H2O water, not dihydrogen

monoxideNH3 ammonia, not nitrogen

trihydride

Mixed Practice1. Dinitrogen monoxide2. Potassium sulfide3. Copper (II) nitrate4. Dichlorine heptoxide5. Chromium (III)

sulfate6. Iron (III) sulfite7. Calcium oxide8. Barium carbonate9. Iodine monochloride

Match each set with the correct name:

Na2CO3 a) sodium carbonate

MgSO3 b) magnesium sulfite

MgSO4 c) magnesium sulfate

Ca(HCO3)2 a) calcium bicarbonate

CaCO3 b) calcium carbonate

Ca3(PO4)2 c) calcium phosphate

Mixed Review Name the following compounds:1. CaO

a) calcium oxide b) calcium(I) oxide

c) calcium (II) oxide d) calcium monoxide

2. SnCl4

a) tin tetrachloride b) tin(II) chloride

c) tin(IV) chloride

3. N2O3

a) nitrogen oxide b) dinitrogen trioxidec) nitrogen trioxide

Mixed Practice1. BaI2

2. P4S3

3. Ca(OH)2

4. FeCO3

5. Na2Cr2O7

6. I2O5

7. Cu(ClO4)2

8. CS2

9. B2Cl4

DONE!Now it is time to study!

Rainbow Matrix GameLink on Chemistry Geek.com on

Chemistry I pagehttp://chemistrygeek.com/rainbow

Use [ ] to represent subscripts since you can’t enter subscripts into the computer

So H2O would be H[2]OAnd Al2(SO4)3 would be Al[2](SO[4])[3]

Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!)

Borate = BO3 -3 ; Silicate = SiO4 -4 ;Manganate = MnO4 -2 (permanganate is -1)