Nomenclatu re Naming Compounds
Jan 04, 2016
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