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57 Cards in this Set
- Front
- Back
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acetate
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(C2H3O2)-1
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bicarbonate
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(HCO3)-1
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bisulfate
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(HSO4)-1
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bisulfide
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(HS)-1
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cyanide
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(CN)-1
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cyanate
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(CNO)-1
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thiocyanate
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(SCN)-1
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hydroxide
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(OH)-1
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permanganate
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(MnO4)-1
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perchlorate
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(ClO4)-1
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chlorate
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(ClO3)-1
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chlorite
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(ClO2)-1
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hypochlorite
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(ClO)-1, for Br and I too
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nitrate
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(NO3)-1
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nitrite
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(NO2)-1
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carbonate
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(CO3)-2
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manganate
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(MnO4)-2
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oxalate
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(C2O4)-2
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peroxide
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(O2)-2
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silicate
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(SiO3)-2
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tetraborate
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(B4O7)-2
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sulfate
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(SO4)-2
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sulfite
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(SO3)-2
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thiosulfate
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(S2O3)-2 (thio means you take out an oxygen and put in a sulfur)
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chromate
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(CrO4)-2
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dichromate
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(Cr2O7)-2
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arsenate
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(AsO4)-3
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borate
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(BO3)-3
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ferricyanide
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[Fe(CN)6]-3
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phosphate
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(PO4)-3
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phosphite
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(PO3)-3
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ferrocyanide
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[Fe(CN)6]-4
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ammonium
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(NH4)+1
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mercury (I)
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(Hg2)+2
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metal + nonmetal
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ionic compound
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nonmetal + nonmetal
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molecular compound
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metal oxide + water
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metal hydroxide (basic)
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nonmetal oxide + water
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oxyacid (acidic)
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metal oxide + nonmetal oxide
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ionic compound
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metal + metal
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no reaction without current
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decomposition reaction?
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substance breaks down by application of heat or electrical current --> 2+ products
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electrolysis (water)
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2H2O(l) --> 2H2(g) + O2(g)
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decomposition-by-heating of hydroxides [(OH)-1]
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with all hydroxides EXCEPT group 1 metal hydroxides
metal hydroxide --> metal oxide + water gas Ba(OH)2 --> BaO + H2O KOH --> no reaction |
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decomposition-by-heating of carbonates [(CO3)-2]
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for all carbonates EXCEPT group 1 metal carbonates
metallic carbonate --> metal oxide + carbon dioxide CaCO3 --> CaO + CO2 |
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decomposition-by-heating of sulfates [(SO4)-2]
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EXCEPT group 1 and group 2 metallic sulfates
metallic sulfate --> metal oxide + sulfur trioxide Cu2SO4 --> Cu2O + SO3 |
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decomposition-by-heating of nitrates [(NO3)-1]
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group 1 metallic nitrates --> metallic nitrite + oxygen gas
2KNO3 --> 2KNO2 + O2 all other metallic nitrates --> metallic oxide + nitrogen dioxide gas + oxygen gas 2Ba(NO3)2 --> 2BaO + 3O2 + 2NO2 |
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decomposition-by-heating of chlorates [(ClO3)-1]
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metallic chlorate --> metallic chloride + oxygen gas
Ba(ClO3)2 --> BaCl2 + 3O3 |
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decomposition-by-heating of oxides (O)-2
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ONLY metallic oxides that decompose into metals and oxygen are: silver, mercury, platinum, palladium, gold
2HgO --> 2Hg + O2 |
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single replacement reaction
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free element + compound --> new free element + new compound
use table of standard reduction potential, or oxidation potential (HARDEST to reduce is EASIEST to oxidize = give away electrons, form a compound) |
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double replacement
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AX + BY --> BX + AY
two categories: acid/base neutralization, precipitation |
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acid-base neutralization: acid-base reaction
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acid + base --> salt + water
HCl + NaOH --> NaCl + H2O |
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acid-base neutralization: metal oxide - acid reaction
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metal oxide + acid --> salt and water
BaO + 2HCl --> BaCl2 + H2O |
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acid-base neutralization: nonmetal oxide - base reaction
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nonmetal oxide + base --> salt + water
SO3 + KOH --> K2SO4 + H2O |
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precipitation reactions
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require solubility rule memorization, make hypothetical double replacement and kill spectators (using solubility rules to see who dissolves into ions)
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precipitation reactions: molecular equation
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describes everything together, REMEMBER STATE OF MATTER
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precipitation reactions: ionic equation
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aqueous separated
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net ionic reaction
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kill spectators, what ACTUALLY reacts
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