Download Formula writing steps: Only subscripts, no coefficients

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