1/28/13. Naming and Writing Formulas > for Ionic Compounds

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1 chemistry 1 of 29 Naming and Writing Formulas A recipe is a formula for the sauce a complete list of ingredients and their proportions. Chemistry also uses formulas. Once you know the rules, you can write the formula for any chemical compound. 2 of 29 Introduction A binary compound is composed of two elements and can be either ionic or molecular. 3 of 29 1

2 Introduction The rules for naming and writing formulas for compounds are possible only because compounds form from the elements in predictable ways. One of those ways is the law of definite proportions. 4 of 29 Introduction The Law of Definite Proportions The law of definite proportions states that in samples of any chemical compound, the masses of the elements are always in the same proportions 5 of 29 Introduction Water obeys the law of definite proportions. In every sample of water, the mass ratio of oxygen to hydrogen is always 8:1. 6 of 29 2

3 o Metal forms a cation. o Anion is a non-metal. Formula Type I Binary Ionic o Metal element symbol written first and non-metal element symbol written second, subscripts are used to indicate amount of each. o Net charge must equal zero. 7 of 29 Naming Type I Binary Ionic o The cation or metal is always named first and the anion or non-metal is named second. o The name of the cation is the name of the element. o The name of the anion has an ide ending. 8 of 29 Examples: Li + + I - à LiI Ca Cl - à CaCl 2 NaCl sodium chloride MgF 2 magnesium fluoride Type I Binary Ionic 9 of 29 3

4 Type II Binary Ionic o Metal can form a cation with different charges. o Anion is a non-metal. Formula o Metal element symbol written first and nonmetal element symbol written second, subscripts indicate amount of each. o Net charge must equal zero. 10 of 29 Naming Type II Binary Ionic o The cation is always named first and the anion is named second. o The name of the cation is the name of the element. o A roman numeral is written in parentheses after the cation to indicate the charge on the cation. o The name of the anion has ide added to the end. 11 of 29 Examples: CuCl 2 copper (II) chloride Cu 2+ Cl - Fe 2 S 3 iron (III) sulfide Fe 3+ S 2- Type II Binary Ionic 12 of 29 4

5 Ionic Containing Polyatomic Ions o A polyatomic ion is a group of atoms that are bound together with a net charge for the group. o Cation is ammonium (NH 4+ ) or a type I or type II metal. o Anion is a polyatomic ion or a non-metal. o Net charge must equal zero. 13 of 29 Formula Ionic Containing Polyatomic Ions o The cation is written first and the anion is written second. o If more than one polyatomic ion is necessary for the net charge to be zero, parenthesis must be used around the ion with the subscript following. 14 of 29 Naming Cation Ionic Containing Polyatomic Ions o If the cation is ammonium (NH 4+ ), that is the name used. o If the cation is a type I metal, use the element name. o If the cation is a type II metal, use the element name followed by a roman numeral to indicate the charge. 15 of 29 5

6 Ionic Containing Polyatomic Ions Anion o If the anion is a polyatomic ion, use the name of the ion. o If the anion is a non-metal, use the element name with the ide ending. 16 of 29 Examples: NH 4 Cl ammonium chloride NH 4 NO 3 ammonium nitrate K 2 SO 4 potassium sulfate Ca(NO 3 ) 2 calcium nitrate PbSO 4 lead (II) sulfate Ionic Containing Polyatomic Ions 17 of 29 An acid is a compound that contains one or more hydrogen atoms and produces hydrogen ions (H + ) when dissolved in water. have various uses. Three rules can help you name an acid with the general formula H n X. The rules for writing the names of acids can be reversed to write the formulas for acids, and vice versa. 18 of 29 6

7 o Hydrogen is always the cation. o A non-metal or polyatomic ion is the anion. Formula o Hydrogen is written first with a subscript, if necessary. o Non-metal or polyatomic ion is written second (the anion will never have a subscript). o Net charge must equal zero. 19 of 29 Naming o Anion is a non-metal or polyatomic ion without oxygen. o Add the prefix hydro- and the suffix ic to the root name of the non-metal. o The word acid is always added to the end of the name. 20 of 29 Example: HCl hydrochloric acid HCN hydrocyanic acid H 2 S hydrosulfuric acid 21 of 29 7

8 If the anion is a polyatomic ion containing oxygen: o No hydro- is used in the name. o If the anion name ends in ate, use the root name of the anion with the suffix ic. o If the anion name ends in ite, use the root name of the anion with the suffix ous. 22 of 29 Examples: PO 3-4 = phosphate ion H 3 PO 4 phosphoric acid SO 2-3 = sulfite ion H 2 SO 4 sulfurous acid CO 2-3 = carbonate ion H 2 CO 3 carbonic acid 23 of 29 Exceptions to the naming rule: o Phosphorus root is phosphor instead of phosph ie phosphoric instead of phosphic o Sulfur root is sulfur not sulf ie sulfuric instead of sulfic 24 of 29 8

9 Bases Just as acids are H + donors in a reaction, bases are H + acceptors. Bases are named in the same way as other ionic compounds the name of the cation is followed by the name of the anion. For example, aluminum hydroxide consists of the aluminum cation (Al 3+ ) and the hydroxide anion (OH ). The formula for aluminum hydroxide is Al (OH) of 29 Naming and Writing Formulas > for Molecular Ionic Type III Binary o Made up of two non-metals. o Numeric prefixes are used. Formula o Numeric prefixes indicate how many of each element are in the compound. o The only time an element will not have a prefix is if there is only one of the first element (mono- is never used with the first element). 26 of 29 Naming and Writing Formulas > for Molecular Ionic Type III Binary Naming o Name the elements in the order listed in the formula. o The first element is named first using the element name and a numeric prefix if there is more than one in the compound. o The second element is named second. The root of the element name has a numeric prefix indicating the number of atoms in the compound and the ide ending. o The vowel (a or o) of the prefix is dropped when the second element is oxygen to make pronouncing easier. 27 of 29 9

10 Naming and Writing Formulas > for Molecular Ionic Type III Binary Prefixes mono = 1 di = 2 tri = 3 tetra = 4 penta = 5 hexa = 6 hepta = 7 octa = 8 nona = 9 28 of 29 Naming and Writing Formulas > for Molecular Ionic Type III Binary Examples: CO 2 carbon dioxide CO carbon monoxide IF 5 iodine pentafluoride N 2 O 5 dinitrogen pentoxide 29 of 29 10

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