nomenclature naming compounds. binary compounds compounds with only two elements in any ratio

NomenclatureNaming

Compounds

Binary Compounds

•Compounds with only two elements

in any ratio

KCl NO2

CaCl2 P2O5

Al2O3 H2S

Na2O etc

•Binary compounds can be either ionic

or covalent

Naming Binary

Compounds

Naming Ionic

Compounds

•Name positive element first with its normal name

•Name negative element last & change its ending to -ide

KClCaCl2

Al2O3

Na2O

Name Each:

CaCl2 CaS

K2O LiF

Name Each:

FeCl2

FeCl3

If the Positive element is not from columns I or II

•its ox # must be determined and written in roman numerals

Determining the Charge

1) Add up the oxidation numbers of all the negative elements

2) The positive portion must balance out the negative portion

3) Divide the positive portion by the metal subscript

CuCl Fe2O3

MnO2 CrO3

Name Each:

Molecule

•A covalent compound that can exist as a separate unit

•Non-metals bond to form molecules

Naming Molecules or

Covalent Compounds

•Same rules as ionic compounds except:

•use geometric prefixes to determine the # of each atom

Geometric Prefixes1-mono 5-penta2-di 6-hexa3-tri 7-hepta4-tetra etc

CO S2O3

N2H4 SO3

Name Each:

Nomenclature HW

•Work problems:

49 - 54

on page 51

CaO P2O5

Al2S3 SO2

Drill: Name Each:

Deriving Formulas1) Write the symbol for each

element

2) Determine ox #s for each

3) Determine lowest common multiple to balance the charge

4) Apply subscripts

Write formulas for:•Sodium sulfide

•Lead (II) iodide

•Diphosphorus

pentoxide

Write formulas for:

•Chromium(III) oxide

•Aluminum carbide

Polyatomic Ion

•A group of atoms chemically

combined that together have a

charge

•Most are oxoanions

•PO4-3 SO4

-2

•A root element bound to oxygen

Naming Polyatomic

Ions

•Learn the polyatomic table on page 42 & 43

•Learn how to use the periodic table to determine polyatomic ions

•Name the root element

•Change the ending

to -ate

•PO4-3 = phosphate

•Some are unusual

CN-1 OH-1

C2H3O2-1

C2O4-2

H2O H3O+1

NH3 NH4+1

Polyatomic Ion Endings

•Maximum O = -ate

•1 less than max O = -ite

•SO4-2 = sulfate

•SO3-2 = sulfite

Naming Ternary

Compounds

Ternary Compounds

•Compounds containing more than two different elements

•Most contain polyatomic ions

•Follow ionic rules for naming the compound

•Name the polyatomic ion as the positive or negative portion

CaCO3

K2SO4

Name Each:

Pb(NO3)2

MgSO3

Name Each:

Write Formulas For:•Lead (II) nitrate

•Aluminum sulfate

•Potassium chlorate

•Ammonium phosphite

Name the Following:

BaSO4 CuNO3

SO2 (NH4)3PO4

Naming Acids

•Binary acids become:

•Hydro _____ ic acids

•HCl - Hydrochloric acid

•Ternary acids become:

•_____ ic acids or

•_____ ous acids

•H2SO4 - Sulfuric acid

•H2SO3 - Sulfurous acid

•____ ic acids form from polyatomic ions ending with ___ ate

•____ ous acids form from polyatomic ions ending with ___ ite

•___ ide ions become:

•hydro ___ ic acids

•___ ate ions become:

•___ ic acids

•___ ite ions become:

•___ ous acids

Percent Composition

by Mass

• Determine the atomic mass of each element in the compound

• Determine the molecular mass of the compound by adding

• Divide each elemental mass by molecular mass

• Multiply by 100 %

MgCl2

• Mg = 24.3 g/mole• 2 Cl = 2 x 35.5 = 71.0 g/mole

• MgCl2 = total = 95.3 g/mole

• % Mg =24.3/95.3 x 100%

• % Cl = 71.0/95.3 x 100 %

Determine % Comp for Each:

Fe2O3

C3H6O3

CuSO4*5H2O

EmpiricalFormula

•Lowest whole number ratio of elements in a compound

•C6H12O6: EF = CH2O

Determining Empirical

formulas from percent

composition

• Assume 100 g• Change % directly to grams• Use molar conversions to

convert grams to moles• Divide each molar amount

by the smallest molar amount

• Substance = 30 % O & 70 & Fe

• 30 % O --> 30 g O &

• 70 % Fe --> 70 g Fe

• 30/16 = 1.875 moles O

• 70 / 56 = 1.25 moles Fe

• 1.25/1.25 = 1 & 1.875/1.25 = 1.5

• Ratio = 1.5 : 1 x 2 = 3 : 2

• Empirical Formula Fe2O3

Find empirical for a compound with:

70.0 % Fe30.0 % O

Find empirical for a compound with:

40 % Ca12 % C48 % O

Find empirical for a compound with:

40.0 % C6.7 % H

53.3 % O

MolecularFormula

•The actual whole number for each element in the

compound

Molecular FormulaC6H12O6

Empirical FormulaCH2O

Solving MF from EF1) Solve empirical mass

2) Divide EM into MM

3) Multiply EF by quotient

Name each of the following:

•KBr MgS

•BaF2 K3P

•K2O LiH

•Al2O3 H2S

Name each of the following:

FeO

Fe2O3

Name each of the following:

•CuO MnS

•PbO2 Cu2O

•CrCl2 MnF2

•CrCl3 SnCl4

Name each of the following:

•SeO CS2

•NO2 Cl2O

•N2O4 PCl3

Derive formulas for each:

•Cesium oxide

•Barium chloride

•Calcium phosphide

•Aluminum sulfide

Derive formulas for each:

•Lead(IV)oxide

•Copper(II)sulfide

•Manganese(VII)oxide

•Nickel(II)fluoride

Name each of the following:

•SO4-2 SO3

-2

•PO4-3

NO3-1

•ClO4-1

ClO3-1

•ClO2-1

ClO-1

Derive formulas for each:

•Chromate

•Arsenate

•Arsenite

•Bromite

Name each of the following:

•BaCO3

•KNO2

•CuClO3

•Al2(SO4)3

Derive formulas for each:

•Potassium sulfate

•Lead(II)chromate

•Aluminum hydroxide

•Ammonium cyanide

Name each of the following:

•Cl2O SO2

•N2O3 P2O5

•CO2 CO

•SO3 N2H4

Derive formulas for each:

•Silicon dioxide

•phosphorus trichloride

•Sulfur hexafluoride

• Iodine trifluoride

Name each of the following:

NH4Cl BaSO4

KC2H3O2 K2HPO3

KNO3 CuBrO

Li2CO3 MgC2O4

Name each of the following:

HCl H2SO4

H2S H3PO3

HNO3 HBrO

H2CO3 HBrO4

Derive formulas for each:

•Chromic acid

•Hydroiodic acid

•Sulfurous acid

•Bromic acid

Name each of the following:

KCl MnSO4

SO2 HI(aq)

NaNO3 HClO

H2CO3(aq) NH4BrO4

Name each of the following:

NaCl MnSO4

S2O3 HBr(aq)

Na2CO3 HClO

HNO3(aq) NH4IO4

Chapter 3 General

•Define all the Key Terms on page 74

Nomenclature•Work problems 43 – 56

•On Pages 51 & 52