Nomenclature Naming Compounds

Binary Compounds

Compounds with only two elements in any ratio

KClNO 2 CaCl 2 P 2 O 5 Al 2 O 3 H 2 S Na 2 Oetc

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

KCl CaCl 2 Al 2 O 3 Na 2 O

Name Each: CaCl 2 CaS K 2 OLiF

Name Each: FeCl 2 FeCl 3

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

CuClFe 2 O 3 MnO 2 CrO 3 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 Prefixes 1-mono5-penta 2-di6-hexa 3-tri7-hepta 4-tetraetc

COS 2 O 3 N 2 H 4 SO 3 Name Each:

Nomenclature HW Work problems: on page 51

CaOP 2 O 5 Al 2 S 3 SO 2 Drill: Name Each:

Deriving Formulas 1)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 PO 4 -3 SO 4 -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 PO 4 -3 = phosphate Some are unusual

CN -1 OH -1 C 2 H 3 O 2 -1 C 2 O 4 -2

H 2 O H 3 O +1 NH 3 NH 4 +1

Polyatomic Ion Endings Maximum O = -ate 1 less than max O = -ite SO 4 -2 = sulfate SO 3 -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

CaCO 3 K 2 SO 4 Name Each:

Pb(NO 3 ) 2 MgSO 3 Name Each:

Write Formulas For: Lead (II) nitrate Aluminum sulfate Potassium chlorate Ammonium phosphite

Name the Following: BaSO 4 CuNO 3 SO 2 (NH 4 ) 3 PO 4

Naming Acids

Binary acids become: Hydro _____ ic acids HCl - Hydrochloric acid

Ternary acids become: _____ ic acids or _____ ous acids H 2 SO 4 - Sulfuric acid H 2 SO 3 - 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 %

MgCl 2 Mg = 24.3 g/mole 2 Cl = 2 x 35.5 = 71.0 g/mole MgCl 2 = total = 95.3 g/mole % Mg =24.3/95.3 x 100% % Cl = 71.0/95.3 x 100 %

Determine % Comp for Each: Fe 2 O 3 C 3 H 6 O 3 CuSO 4 *5H 2 O

Empirical Formula

Lowest whole number ratio of elements in a compound C 6 H 12 O 6 : EF = CH 2 O

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 = 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 Fe 2 O 3

Find empirical for a compound with: 70.0 % Fe 30.0 % O

Find empirical for a compound with: 40 % Ca 12 % C 48 % O

Find empirical for a compound with: 40.0 % C 6.7 % H 53.3 % O

Molecular Formula

The actual whole number for each element in the compound

Molecular Formula C 6 H 12 O 6 Empirical Formula CH 2 O

Solving MF from EF 1) Solve empirical mass 2) Divide EM into MM 3) Multiply EF by quotient

Name each of the following: KBrMgS BaF 2 K 3 P K 2 OLiH Al 2 O 3 H 2 S

Name each of the following: FeO Fe 2 O 3

Name each of the following: CuOMnS PbO 2 Cu 2 O CrCl 2 MnF 2 CrCl 3 SnCl 4

Name each of the following: SeOCS 2 NO 2 Cl 2 O N 2 O 4 PCl 3

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: SO 4 -2 SO 3 -2 PO 4 -3 NO 3 -1 ClO 4 -1 ClO 3 -1 ClO 2 -1 ClO -1

Derive formulas for each: Chromate Arsenate Arsenite Bromite

Name each of the following: BaCO 3 KNO 2 CuClO 3 Al 2 (SO 4 ) 3

Derive formulas for each: Potassium sulfate Lead(II)chromate Aluminum hydroxide Ammonium cyanide

Name each of the following: Cl 2 OSO 2 N 2 O 3 P 2 O 5 CO 2 CO SO 3 N 2 H 4

Derive formulas for each: Silicon dioxide phosphorus trichloride Sulfur hexafluoride Iodine trifluoride

Name each of the following: NH 4 ClBaSO 4 KC 2 H 3 O 2 K 2 HPO 3 KNO 3 CuBrO Li 2 CO 3 MgC 2 O 4

Name each of the following: HClH 2 SO 4 H 2 S H 3 PO 3 HNO 3 HBrO H 2 CO 3 HBrO 4

Derive formulas for each: Chromic acid Hydroiodic acid Sulfurous acid Bromic acid

Name each of the following: KClMnSO 4 SO 2 HI (aq) NaNO 3 HClO H 2 CO 3(aq) NH 4 BrO 4

Name each of the following: NaCl MnSO 4 S 2 O 3 HBr (aq) Na 2 CO 3 HClO HNO 3(aq) NH 4 IO 4

Chapter 3 General Define all the Key Terms on page 74

Nomenclature Work problems 43 – 56 On Pages 51 & 52