Chemical Nomenclature 1 Binary Ionic Compounds Type I

Chemical Nomenclature 1. Binary Ionic Compounds - Type I 2. Binary Ionic Compounds - Type II 3. Ionic Compounds & Polyatomic (Complex) Ions 4. Oxy-Acids 5. Hydrated Ionic Compounds 6. Binary Acids 7. Binary Covalent Compounds

Type I Binary Ionic Compounds n The metal cations in these compounds have only ONE possible charge. Na+ sodium Zn 2+ zinc Al 3+ aluminum Ca 2+ calcium The charges are memorized or predicted using a periodic table! n The cations are bonded to nonmetal anions: O 2 oxide N 3 nitride Ffluoride Br bromide Notice that simple anions are always named with the suffix “ide”

n n In an ionic compound, the charges of the cations and anions must always cancel out. Subscripts are used if more than one atom is needed to cancel the charges: sodium chloride: Na+ and Cl- ® lithium oxide: Li+ and O 2 - ® aluminum bromide: Al 3+ and Br - ® Al. Br 3 zinc nitride: Zn 2+ and N 3 - ® Zn 3 N 2 potassium iodide: K+ and I- ® silver phosphide: Ag+ and P 3 - ® Ag 3 P Na. Cl Li 2 O KI

Examples: Type I Binary Ionic Compounds Write the formulas: Write the names: • potassium oxide • K 3 N • zinc chloride • Ag. I • silver sulfide • Zn. Br 2 • aluminum nitride • Al 2 O 3 • gallium oxide • Ba 3 P 2 • calcium iodide • Li. H

Type II Binary Ionic Compounds n These are ionic compounds where the metal cation can form TWO different charges. Fe 2+ iron (II) Fe 3+ iron (III) Ni 2+ nickel (II) Ni 3+ nickel (III) Co 2+ cobalt (II) Co 3+ cobalt (III) Cu+ copper (I) Cu 2+ copper (II) Au+ gold (I) Au 3+ gold (III) Sn 2+ tin (II) Sn 4+ tin (IV) An older system uses suffixes and Latin names, -ous for the lower charge, -ic for the higher charge: Ferrous & Ferric, Cuprous & Cupric, Stannous & Stannic

Examples: Type II Binary Ionic Compounds Write the formulas: Write the names: • iron (II) oxide • Fe 2 O 3 • copper (II) chloride • Sn. S • tin (IV) sulfide • Ni. Br 2 • cupric nitride • Cu. S • nickel (III) oxide • Pb 3 P 2 • ferrous iodide • Cu. Br • cobalt (III) selenide • Fe. Cl 3

Examples: Type II Binary Ionic Compounds Write the formulas: • iron (II) oxide Fe. O • copper (II) chloride Cu. Cl 2 • tin (IV) sulfide Sn. S 2 • cupric nitride Cu 3 N 2 • nickel (III) oxide Ni 2 O 3 • ferrous iodide Fe. I 2 • cobalt (III) selenide Co 2 Se 3

n n n n Write the names: Fe 2 O 3 Iron (III) oxide Ferric oxide Sn. S Tin(II)sulphide stannous sulfide Ni. Br 2 Nickle (II) bromide Cu. S Copper (II) Sulfide Cupric sulphide Pb 3 P 2 L Cu. Br Fe. Cl

Polyatomic (Complex) Ions n n n All of the cations and anions so far have been simple ions - single atoms that have lost or gained electrons. A molecule is a particle that forms when two or more atoms bond together. A complex ion is a charged molecule. Complex ions may be cations or anions. examples: nitrate: NO 3 - sulfate: SO 42 - hydroxide: OH-

Writing formulas with Complex Ions a) Ammonium chloride b) Silver sulfate c) Aluminum hydroxide d) Calcium phosphate e) Iron (III) nitrate f) Copper(II) permanganate g) Ammonium dichromate h) Zinc acetate

Writing formulas with Complex Ions a) Ammonium chloride NH 4 Cl b) Silver sulfate Ag 2 SO 4 c) Aluminum hydroxide Al(OH)3 d) Calcium phosphate Ca 3(PO 4)2 e) Iron (III) nitrate Fe(NO 3)3 f) Copper(II) permanganate Cu(Mn. O 4)2 g) Ammonium dichromate (NH 4)2 Cr 2 O 7 h) Zinc acetate Zn(CH 3 COO)2

Things to Notice n n Most complex ions are anions. Ammonium, NH 4+, is the most common complex cation. Several complex ions form a short series of ions. The ions differ only in the number of oxygen atoms: perchlorate Cl. O 4 - sulfate SO 42 - chlorate Cl. O 3 - sulfite SO 32 - chlorite Cl. O 2 - hypochlorite Cl. O- nitrate NO 3 - nitrite NO 2 -

More Formulas with Complex Ions a) Sodium carbonate b) Nickel (II) sulfite c) Aluminum chlorate d) Barium phosphite e) Iron (III) sulfite f) Cupric sulfate g) Zinc periodate

More Formulas with Complex Ions a) Sodium carbonate Na 2 CO 3 b) Nickel (II) sulfite Ni. SO 3 c) Aluminum chlorate Al(Cl. O 3)3 d) Barium phosphite Ba 3(PO 3)2 e) Iron (III) sulfite Fe 2(SO 3)3 f) Cupric sulfate Cu. SO 4 copper (II) Sulphate Cuprous sulphate Cu 2 SO 4 copper (I)Sulphate g) Zinc periodate Zn(IO 4)2

Hydrated Ionic Compounds n n A HYDRATE is an salt that has water molecules trapped within its crystals. Every hydrate has a certain number of water molecules associated with each formula unit of the ionic compound. The number of water molecules is indicated by using prefixes. Cu. SO 4 · 5 H 2 O mono di tri tetra penta hexa hepta octa nona deca copper (II) sulfate pentahydrate Mg. CO 3 · 10 H 2 O magnesium carbonate decahydrate

Examples of hydrates: n n Write the formulas: copper(II) fluoride tetrahydrate Cu. F 2 · 4 H 2 O calcium nitrate trihydrate Ca(NO 3)2 · 3 H 2 O Write the names: Mg. SO 4 · 7 H 2 O magnesium sulfate heptahydrate Fe. Cl 2 · H 2 O iron (II) chloride monohydrate

Examples of hydrates: n Write the formulas: copper(II) fluoride tetrahydrate calcium nitrate trihydrate n Write the names: Mg. SO 4 · 7 H 2 O Fe. Cl 2 · H 2 O

Oxy-Acids n An acid can also be made of a hydrogen ion bonded to a complex ion. Complex ions whose names end in “ate”: NO 3 - SO 42 - nitric acid: HNO 3 CO 32 - sulfuric acid: H 2 SO 4 carbonic acid: H 2 CO 3 phosphoric acid: H 3 PO 4 Chloric acid HCl. O 3 PO 43 - Can you propose a rule for naming oxy-acids with complex ions ending in “ate”?

More Oxy-Acids n Complex ions ending in “ite”: NO 2 - SO 32 - Cl. O- nitrous acid: HNO 2 sulfurous acid: H 2 SO 3 hypochlorous acid: ( from hypochlorite ion) chlorous acid HCl. O 2 - Can you propose a rule for naming oxy-acids with complex ions ending in “ite”?

Acids n n Nitric Acid Nitrous acid Hyposulphurous acid Perchloric acid

Acids Nitric Acid HNO 3 Nitrous acid HNO 2 n Hyposulphurous acid H 2 SO 2 n Perchloric acid HCl. O 4 n

n Acid Salts Acid Salt ions can be formed if an oxy ion carries a charge like “-2” or “ 3”, a series of related ions can be formed by adding hydrogen cations (H+) while still leaving a remainder net charge: examples: Sulfate: SO 42 - hydrogen sulfate: HSO 4(bisulfate) Carbonate: CO 32 - hydrogen carbonate: HCO 3 - (bicarbonate) Phosphate: PO 43 - hydrogen phosphate: HPO 42 - dihydrogen phosphate: H 2 PO 4 -

More Formulas with Complex Ions a) Sodium hydrogen carbonate b) Nickel (II) hydrogen sulfate c) Aluminum perchlorate d) Barium dihydrogen phosphate e) Iron (III) sulfite f) Cuprous Hydrogen hyposulphite g) Zinc periodate

More Formulas with Complex Ions a) Sodium bicarbonate Na. HCO 3 b) Nickel (II) hydrogen sulfate Ni(HSO 4)2 c) Aluminum perchlorate Al(Cl. O 4)3 d) Barium dihydrogen phosphate Ba(H 2 PO 4)2 e) Iron (III) sulfite f) Cuprous hydrogen hyposulphite g) Zinc periodate Fe 2(SO 3)3 Cu. HSO 2 Zn(IO 4)2

Binary Acids n n n A simple definition of an “acid” is a substance which produces H+ ions in water. Most acids have hydrogen ions in their formulas. A binary acid composed of a hydrogen cation bonded to one other element: HCl hydrochloric acid HBr hydrobromic acid H 2 S hydrosulfuric acid Binary acids are always named: hydro____ic acid

Binary Covalent Compounds n n n Covalent compounds are made of two NONMETAL elements sharing valence electrons. There are no ions involved!! Because there are no charges to help us write the formulas of covalent compounds, prefixes are used to indicate the number of each atom present in the formula. Brandon is awesome. CO 2 is named “carbon dioxide” CO is named “carbon monoxide” N 2 O is named “dinitrogen monoxide” SO 3 is named “sulfur trioxide” The prefix, “mono” is never used for the first element in the formula!

Examples of Covalent Naming n Write the names: SO 2 P 4 O 10 n Write the formulas: phosphorus pentachloride dinitrogen trioxide

Examples of Covalent Naming n n Write the names: SO 2 sulfur dioxide P 4 O 10 tetraphosphorus decoxide Write the formulas: phosphorus pentachloride PCl 5 dinitrogen trioxide N 2 O 3