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46 Cards in this Set
- Front
- Back
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Aqueous solutions |
Formed when solvent is water Ionic compounds break down into positive and negative ions |
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Hydrated |
Ions are surrounded by water molecules |
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Precipitate |
Insoluble compound Attraction between ions is greater than the force of water, compound will not dissociate |
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Precipitation reaction |
Type of double displacement reaction, precipitate is formed |
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Spectator ions |
Remaining ions in solution Don’t participate in reaction |
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Ionic equation |
All ions in dissociated form Includes spectator ions |
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Net ionic equation |
Resulting equation Spectator ions cancelled out Reaction that forms the precipitate |
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If all products are soluble |
No precipitate formed Reaction doesn’t exist No net ionic equation exists |
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If all products are soluble |
No precipitate formed Reaction doesn’t exist No net ionic equation exists |
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If a product is insoluble |
Precipitate formed Reaction exists Net ionic equation is written Positive ion first |
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Neutralization Reaction |
Double displacement reaction between acid and base Product if water and a salt |
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Salt |
Negative ion from acid and positive ion from base |
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Salt |
Negative ion from acid and positive ion from base |
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Acid |
always have at least one hydrogen atom Releases hydrogen ions in water Sour pH < 7 Reacts with carbonate(CO3) to make CO2 Corrosive to metals, H2 gas is formed |
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Binary Acid |
HX x = non metal Hydro-anion root-ic |
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Ternary Acids (Oxyacids) |
HX x = polyatomic ion “Ate” ending- anion root-ic “Ite” ending - anion root-ous |
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Monoprotic acid |
Releases one hydrogen ion in water |
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Monoprotic acid |
Releases one hydrogen ion in water |
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Polyprotic acid |
Releases more than one hydrogen ion in water Can change “poly” with prefixes like “di” and “tri” |
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Polyprotic acid |
Releases more than one hydrogen ion in water Can change “poly” with prefixes like “di” and “tri” to specify the number of hydrogen ions released |
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Base |
Slippery and bitter Releases hydroxide ions pH > 7 Degrades animal tissue NH3 is a base, must react with water and form ammonium hydroxide |
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Monohydroxic Bases |
Release one hydroxide ion in water |
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Polyhydroxic Bases |
Releases more than one hydroxide ion in water Can replace “poly” with “di” and “tri” to specify the number of hydroxide ions released |
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Stoichiometry of neutralization |
Determine how much acid must be added to a given base to neutralize it |
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Oxidation-reduction reaction |
Aqueous environments |
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Oxidation |
Burning Corrosion When substances are combined with oxygen |
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Joseph Priestley |
Discovered oxygen |
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Antoinne Levoisier |
Father of modern chemistry Discovered that substances burn because they combine with oxygen substances burned to form oxides, mass increased oxides heated mass decreased |
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Burning |
Rapid oxidation |
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Chemiluminescence |
Redox reaction that gives off light |
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Bioluminescence |
Light produced in living things |
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Redox reactions that don’t give off light |
Metabolism of food Bleaching to remove stains Development of black and white photos Discharging of batteries |
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5 types of reactions |
Combustion Synthesis Single replacement Double replacement (Neutralization and precipitation) |
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Two reaction families |
Redox - have an exchange of electrons
Non redox - no exchange of electrons |
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oxidation |
atom is losing one or more electrons |
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reduction |
atom is gaining one or more electrons |
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OIL RIG |
Oxidation Is Losing Reduction Is Gaining |
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oxidation states |
keep track of loss and gain of electrons imaginary charge an atom has, electron pair belongs to the most electronegative element of that compound |
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oxidation numbers |
+/- numbers related to an atoms oxidation state more electro(-) atoms are - least electro(-) atoms are + represents the charge if every bond were ionic |
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determining oxidation number |
1. Number assigned per atom 2. atom is by itself, number is 0 3. neutral compounds, sum of ox # is 0 4. ox # of many elements corresponds to position of element on the periodic table 5. polyatomic ion charge is the sum of ox # |
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recognizing redox reactions |
if there are electrons lost in one element and gained in another (ie. ox # changed) |
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oxidizing agent |
is the substance that becomes reduced makes the other substance oxidized |
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reducing agents |
is the substance that becomes oxidized makes other substance reduced |
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electrons transferred |
1. ox #s
2. determine oxidized and reduced 3. multiply e- lost and gained by # of atoms |
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balancing redox reactions: ox # method |
1. assign ox #, identify ox and red substances 2. balance atoms gaining and losing e- 3. balance e- transferred 4. balance rest by inspection |
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balancing redox reactions: acidic half reaction |
1. assign ox # 2. identify ox and red substances and write ox+red half reactions 3. balance elements except for H and O 4. add e- lost and gained 5. balance O atoms by adding H2O to opp side 6. balance H atoms by adding H+ on opp side 7. balance electrons transferred 8. combine reactions |
