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Chemical Nomenclature (Naming and Formulas) Binary Ionic Compounds Naming Metal cation named first (full name) Non-metal anion second (-ide suffix) Eg. Al2O3 → aluminum oxide eg. calcium fluoride Formula 1. Write the symbol of each element with valence numbers. 2. Criss-cross the valences so they become subscripts of the opposite element. 3. Divide subscripts by the highest common factor, omit subscripts of 1. 1. Ca2+ F1- 2. Ca1 F2 3. CaF2 Transition Metals Transition metals and some representative metals are multivalent (more than one valence). Naming eg. Name of the metal ion includes the valence charge in roman numerals and brackets. CuCl → copper (I) chloride CuCl2 → copper (II) chloride * Sometimes the classical naming system is used with the Latin name for the element with the suffix –ous for the metal ion with the smaller charge. The Latin name with suffix –ic is used for the metal ion with the larger charge. Compounds with Polyatomic Ions Na3PO4(aq) is an example of a tertiary compound. PO43- is a polyatomic ion. It is also an oxyanion (contains oxygen). Naming Metal or Polyatomic cation is the first part of the name. Non-Metal or Polyatomic anion makes up second part of name. eg. calcium chlorate → Ca(ClO3)2 For naming a polyatomic compound, you may need to determine the type of oxyanion: Determines stem of the ion name Ion charge ClO3Determines suffix and prefix of the ion name ClOClO2ClO3ClO4- hypochlorite ion chlorite ion chlorate ion perchlorate ion Hydrates The formula for a hydrate includes both the formula of the compound and the formula of for the water of hydration. eg. CuSO4·5 H2O The IUPAC names of ionic hydrates indicate the number of water molecules by a Greek prefix (Table 5, page 78). The above is an example of copper (II) sulfate pentahydrate. Molecular Compounds: Naming In naming compounds formed from two non-metals, a Greek prefix is attached to the name of each element in the binary compound indicating the number of atoms of that element in the molecule. If there is only one of the first type of atom, we leave out the prefix “mono”. eg. N2O → dinitrogen monoxide CCl4 → carbon tetrachloride The prefix system is also not used for hydrogen. H2S → hydrogen sulfide Most of the compounds we encounter everyday do not contain ions. Rather, they contain neutral groups of atoms called molecules. Number 1 2 3 4 5 6 Prefix MonoDiTriTetraPentaHexa- Example CO (carbon monoxide) SO2 (sulfur dioxide) SO3 (sulfur trioxide) CCl4 (carbon tetrachloride) PCl5 (phosphorus pentachloride) SF6 (sulfur hexafluoride) SCH 3U1 BINARY IONIC COMPOUNDS: Names and Formulas 1. Write the name of the binary ionic compounds that corresponds to the formulas given below. (Remember your ROMAN NUMERALS in brackets after the name of the metal IF it has more than one valence or charge!) Formula NaCl Name Formula Na2 O Name Formula CaO KF KI K2 O NiO NiCl3 FeO AgCl MgS Al2 O3 Ca3 P2 AuCl AuCl3 RbCl Sr3 P2 BaI 2 AlBr3 Na2 S MgO LiF Li2 S HgBr Hg2 Br CuO Cu2 O Name 2. Write the formula that corresponds to the following binary ionic compound. Name Calcium iodide Formula Name Sodium fluoride Formula Name Calcium oxide Iron(II) oxide Nickel(I) oxide Copper(II) oxide Potassium sulfide Iron(II) chloride Magnesium iodide Tin(IV) oxide Potassium oxide Calcium hydride Zinc fluoride Silver oxide Barium oxide Cesium nitride Strontium oxide Potassium chloride Strontium fluoride Aluminum oxide Gold(III) chloride Calcium chloride Gold(I) chloride Silver phosphide Lead(IV) oxide Lead(II) oxide Lead(IV) nitride Formula SCH 3U1 POLYATOMIC IONIC COMPOUNDS: Names and Formulas 1. Polyatomic ions are ions that are made up of 2 or more atoms that behave as a single unit. Each polyatomic ion has its own charge. Polyatomic Ion Formula Chlorate NO31 Carbonate Sulfate PO43 NH41 Hydroxide 2. Name the following ionic compounds that contain polyatomic ions. Formula AlPO4 Name Formula CaSO4 K2 SO4 Sr (ClO3 ) 2 ( NH4 ) 2 CO3 Al ( NO3 ) 2 NH4 Cl KOH Fe(OH ) 2 Fe(OH ) 3 Ca3 ( PO4 ) 2 NaClO3 Al2 (CO3 ) 3 NH4 NO3 Name 3. Write the formulas that correspond to the following polyatomic ionic compounds names. Name Ammonium chloride Formula Calcium phosphate Name Potassium carbonate Magnesium sulfate Sodium chlorate Calcium carbonate Iron(II) sulfate Iron(III) sulfate Sodium hydroxide Cesium nitrate Aluminum sulfate Zinc carbonate Strontium nitrate Lithium carbonate Formula SCH 3U1 MOLECULAR COMPOUNDS: Names and Formulas 1. Write the name of the covalent compounds that corresponds to the formulas given below. (Remember your prefixes!) Formula SO2 Name Formula Cl2 O CO2 P4 O10 Cl2 O7 N 2 O4 XeF6 IF5 SiO2 H2 O N2O P2 O5 SO3 N 2 H4 SF6 NO CCl4 NCl3 P2 S5 N 2 O5 Name 2. Write the formula that corresponds to the following names. Name Dinitrogen tetroxide Formula Name Boron triflouride Dihydrogen monsulfide Carbon disulfide Diiodine pentoxide Xenon triiodide Carbon tetrabromide Tetraphosphorus decoxide Iodine tetrachloride Nitrogen trihydride Nitrogen monoxide Dichlorine monoxide Diphosphorus pentasulfide Diphosphorus pentoxide Dichlorine heptoxide Carbon monoxide Carbon dioxide Sulfur trioxide Formula NAMING HYDRATES - Practice A number of ionic compounds called hydrates produce water when they decompose upon heating. When the formula of a hydrated compound is written, the number of water molecules is also included. For example, the formula for copper (II) sulfate pentahydrate is written as CuSO45H2O. The name for CuSO45H2O is copper (II) sulfate pentahydrate indicating that five molecules of water are bonded within the ionic crystal for every one formula unit of CuSO4. The prefixes to be used are the same as those given for molecular formulas. The prefix indicates the number of water molecules in a hydrated compound. All hydrates are ionic compounds, therefore they are solid at room temperature unless otherwise indicated. Make sure you include the state of matter with each chemical formula. Table 1 - Naming Hydrated Compounds Name of Hydrate E.g. copper (II) sulfate pentahydrate 1. 2. sodium carbonate decahydrate 3. 4. barium chloride dihydrate 5. 6. 7. zinc sulfate heptahydrate 8. lithium chloride tetrahydrate 9. 10. cobalt (II) chloride hexahydrate 11. 12. 13. barium hydroxide octahydrate 14. nickel (II) chloride hexahydrate 15. Common Name, Use or Description blue vitriol, bluestone, copper plating, blue solid Epsom salts, white solid explosives, matches washing soda, soda ash, water softener, white solid white solid, fireproofing wood, disinfectants, parchment paper white solid, pigments, dyeing fabrics, tanning leather white solid, photographic emulsions white solid, embalming material, fireproofing lumber, vulcanizing white solid, clarifying glue, preserving wood, and skins white solid, soldering aluminum, in fireworks photographic hypo, antichlor, white solid pink solid, humidity and water indicator, foam stabilizer in beer white solid, antiperspirant Formula de-icer used on icy highways, added to cement mixtures to prevent freezing during winter, white solid white solid, manufacture of glass, water softener green solid, absorbent for ammonia in gas masks Glauber's salt (a medicine), white solid, drying agent CaCl22H2O(s) CuSO45H2O(s) MgSO47H2O(s) MgCl26H2O(s) Cd(NO3)24H2O(s) ZnCl26H2O(s) Na2S2O35H2O(s) AlCl36H2O(s) Na2SO4 10H2O(s)
