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28 Cards in this Set
- Front
- Back
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NO3- Soluble or insoluble ? |
Soluble no exception |
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C2H3O2- soluble or insoluble ? |
Soluble no exceptions |
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Cl- Soluble or insoluble? |
Soluble with exceptions Ag+, Hg2 (2+), Pb(2+) |
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Br- Soluble or insoluble? |
Soluble exceptions Ag+, Hg2 (2+), Hg(2+), Pb(2+), |
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I- Soluble or insoluble |
Soluble with exceptions Ag+,Hg2(2+), Hg(2+), Pb(2+) |
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SO4 (2-) |
Ca2+, Sr2+, Ba2+, Hg2(2+), Pb2+, Ag+ |
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S2- |
Insoluble Exceptions NH4+, group 1,2 |
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CO3(2-) |
Insoluble with exceptions NH4+, group 1 |
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PO4(3-) |
NH4+, group 1 |
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OH- |
group 1, NH4+, Ca2+, Sr2+, Ba2+ |
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.Milli |
10 ^-3
. |
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killi |
10^3 |
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Net ionic equation |
equation showing only species that happen in the equation |
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limiting reactions |
limits amount of product in reaction |
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theoretical yeild |
maximum amount of product produced in a reaction |
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actual yield |
product actually produced in chemical equations. always equal to or less than theoretical yield. |
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percent yield |
actual yield/theoretical yield *100 |
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Molarity equals |
mols over liters of solution |
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Solvent vs solute |
solvent: majority component of a mixture. ex: in aqueous solution water acts as a solvent. solute: minority component. substance thats dissolved |
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soluble vs insoluble |
soluble: dissolves in water insoluble: doesn't dissolve in water |
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Precipitate reactions |
reaction of a solid is formed. only insoluble compounds form precipitate reactions |
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Strong vs weak electrolytes |
strong. : completely dissociates in water. includes strong acids,bases and salts. ex: HCl, HBr, HI-, Weak: doesn't completely ionize in water, weakly conducts electricity. |
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Acids vs bases |
acids: produces H+ ions in aqueous solutions bases: produces OH- ions in aqueous solutions |
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Acid base reactions usually form |
water and an ionic compound (salt) |
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Titration |
substance in a solution of known concentration is related with another substance in a solution of unknown. great for determining concentration of unknown solutions |
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oxidation-reduction reactions or redox are |
REACTIONS IN WHICH ELECTONS TRANSFER FROM 1 REACTION TO THE OTHER |
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oxidation vs reduction |
oxidation loss of electrons reduction gaining of electrons |
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Rules of assigning oxidation |
1. oxidation state of an atom in a free element is Cu 0 ox state. Cl2 0 ox state 2. The oxidation state of monoatomic ions is equal to the charge. Ca2+ +2 ox state Cl- -1 ox state 3. The sum of oxidation states of allots in: - A neutral or formula unit is 0. H2O 2(H ox states) + 1(O ox states)=0 - An ion is equal to the charge of the ion. NO3- 1(N ox states) + 3(O ox states)=-1 4. In their compounds, metal have positive oxidation states. ~group 1A metal always have an oxidation of +1. NaCl +1 ox state ~group 2A metals always have an oxidation of +2. CaF2 +2 ox state 5. In their compounds, nonmetals are assigned oxidation states according to the table at right. Entries at the top of the table take precedence over entries at the bottom of the table |
