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Formula, Name writing, and Balancing Review Formula writing steps: Only subscripts, no coefficients 1. Identify the symbols - Are any a polyatomic ion? Nonmetal and nonmetal? 2. If a metal or polyatomic ion is the first symbol, identify the valence or charge of each symbol and write it just above the symbol; if transition metal use the roman number to determine the charge (positive) 3. If it’s a nonmetal and nonmetal – use prefixes (mono-, di-, tri-, etc.) to determine subscripts; should it be diatomic? 4. Balance the total positive and negative charges – crisscross charges to subscripts or use least common multiple 5. Once you have determined the number of units needed for each element those become the subscripts that are placed right after the respective symbol SHORTER SUMMARY FOR IONIC BONDS (Metal) 1. Identify the symbols of the cation and anion 2. Identify the charge for each and place above the symbol 3. Balance the positive and negative charges 4. Write the formula placing the subscripts right after the symbol they go with. Example 1: Example 2: Example 3: Example 4: Example 5: Lead (II) Acetate Calcium phosphate Nitrogen Aluminum bromide Dinitrogen hexachloride Pb(C2H3O2)2 Ca(PO4)2 N2 AlBr3 N2C6 Name writing steps: Metals (groups 1 and 2) and Non-metals Metal _________ + Non-Metal _________ide Transition Metals (groups 3 - 12) and Non-metals Metal ______ + Roman Numeral (__) + Non-Metal ________ide Subscripts criss-cross back the other way to give the oxidation number (charge) Nonmetals and Non-metals Prefix _______ Non-metal _________ + Prefix _______ Non-Metal ________ide Metals (groups 1 and 2) and Polyatomics Metal _________ + Polyatomic name ______ Transition Metals (groups 3 - 12) and Polyatomics Metal ______ + Roman Numeral (__) + Polyatomic name ______ Subscripts criss-cross back the other way to give the oxidation number (charge) Acids (with H in front) Binary acids (without oxygen in formula) Hydro _________ ic Acid Oxy acids (with oxygen in formula) -ate goes to –ic and –ite goes to –ous Example 1: Example 2: Example 3: Example 4: Example 5: Al(OH)3 CCl4 I2 FeCl3 H2SO4 Aluminum hydroxide Carbon tetrachloride Iodine Iron (III) Chloride Sulfuric Acid Balancing equations: only coefficients, no subscripts 1. 2. 3. 4. Write equation Count atoms Use coefficients to balance – same number and type of each atom on each side Check by recounting atoms HINTS: Start with odd numbers Types or reactions: Synthesis: simple + simple complex Decomposition: Complex simple + simple Single replacement: kick one out Double replacement: swap partners Example 1: Example 2: Example 3: Example 4: Example 5: KI K + I2 NaI + Br2 NaBr + I2 FeCl3 + NaOH Fe(OH)3 + NaCl H2 + N2 NH3 Ca(OH)2 + HNO3 Ca(NO3)2 + H2O 2KI 2K + I2 Decomposition 2NaI + Br2 2NaBr + I2 Single replacement FeCl3 + 3NaOH Fe(OH)3 + 3NaCl Double 3H2 + N2 2NH3 Synthesis Ca(OH)2 + 2HNO3 Ca(NO3)2 + 2H2O Double