AmmoniumNH 4 + Chlorate ClO 3 - AcetateCH 3 CO 2 - PerchlorateClO 4 - ChromateCrO 4 2- NitrateNO 3 - Permanganate MnO 4 - Dichromate Cr 2 O 7 2- NitriteNO 2 - Carbonate CO 3 2- Hydroxide OH - Sulfate SO 4 2- Phosphate PO 4 3- HypochloriteClO - SulfiteSO 3 2- ChloriteClO 2 - Oxalate CyanideCN - Thiocyanate SCN - Hydrogen carbonate HCO 3 - Hydrogen sulfate HSO 4 - Hydrogen sulfite HSO 3 - C 2 O 4 2- Manganate MnO 4 2- IodateIO 3 - BrO 3 - Bromate SilicateSiO 3 2- AsO 4 2- Arsenate

 Naming is a big part of this.  You can’t finish these problems if you can’t get them started.  These are easy points you don’t want to let go. 3

 Synthesis Reactions pg 42  Metals and nonmetals combine to form salts. CHECK CHARGES OF IONS!!!!!  Metal Oxides and water form bases, bases have OH attached  Nonmetal oxides and water form acids  Metal oxides and nonmetal oxides form salts (you will make an oxyanion- just move one oxygen over)

 Magnesium burns in oxygen  Calcium reacts with chlorine gas  Potassium oxide reacts with water  Carbon dioxide is bubbled through water  Lithium oxide is added to carbon dioxide

 Decomposition Reactions pg 42  CHECK CHARGES OF IONS!!!!!  Carbonates decompose into oxides and CO 2  Chlorates decompose into chlorides and O 2  A binary compound may break down to produce two elements.  Hydrogen peroxide with decompose into water and oxygen gas

 Titanium (IV) chlorate decomposes  Copper (III) carbonate is heated  Magnesium chloride is electrolyzed  Carbonic acid is heated  Hydrogen peroxide decomposes

 A + BX  AX + B  You will have a chart of activity series  More active metals will replace less active metals from their compound in a solution  A less active element will have no reaction when added to a more active element!  Active metals replace hydrogen in water  Active metals replace hydrogen in acids  Active nonmetals replace less active nonmetals from their compounds in solutions

 Zinc is added to a solution of cobalt (II) chloride  Cadmium is added to a solution of barium iodide  Lithium is added to a solution of copper (II) chlorate  Chromium is left in water

 Potassium is added to sulfuric acid  Silver is added to hydrochloric acid  Chlorine gas is bubbled through a solution of sodium bromide

 AY + BX  AX + BY  These reactions occur in solution  Remember in solution the ions are free floating. For a reaction to occur, the ions have to come together and leave their dissolved state.  Formation of a precipitate  Formation of a gas  Formation of a molecular species

 Acids are soluble.  Compounds of: alkali metals, ammonium, nitrate, chlorate and acetate are soluble.  Halogens and sulfates are soluble except with silver mercury, lead, and large alkaline earth metals (calcium and up)  With the exception of the first two bullets carbonates, chromates, phosphates, sulfites, oxalates and sulfides are insoluble.  Hydroxides are insoluble with the exception of calcium, strontium and barium (lightning bolt)

 Hydrochloric acid reacts with silver nitrate  Potassium carbonate reacts with calcium chlorate  Sodium chloride reacts with ammonium oxalate  Scandium acetate reacts with lithium chromate

 Acid base neutralization reactions will produce water.  NaOH + HNO 3  H 2 O (l) + NaNO 3 (aq)  Net ionic is  H + + OH -  H 2 O

AcidformulaAcidFormula Hydrochloric acid HClSulfuric Acid H 2 SO 4 Hydrobromic acid HBrNitric AcidHNO 3 Hydriodic acid HIPerchloric Acid HClO 4 Chloric Acid HClO 3

NameFormulaNameFormula Sodium Hydroxide NaOHCalcium Hydroxide Ca(OH) 2 Potassium Hydroxide KOHStrontium Hydroxide Sr(OH) 2 Barium Hydroxide Ba(OH) 2 these make a lightning bolt on the periodic table!

 Strong acids and bases are not at equilibrium, there is no reverse reaction.  Strong acids and bases will never be formed in a net ionic equation.  All other acids/bases can be formed, and will be formed by reacting the appropriate ion with a strong acid/base.  *Most other bases are insoluble

 Calcium hydroxide reacts with chloric acid  Hydrochloric acid reacts with calcium nitrite  Nitric acid reacts with sodium chlorite  Sodium hydroxide is mixed with zinc chloride

 H 2 S (hydrogen sulfide) is formed from any sulfide reacting with an acid  CO 2 (Carbon dioxide) is formed from any carbonate reacting with an acid, water is also produced  SO 2 (sulfur dioxide) is formed from any sulfite reacting with an acid, water is also produced  NH 3 (ammonia) is formed from ammonium reacting with a soluble hydroxide

 Ammonium chloride reacts with calcium hydroxide  Sodium sulfide is combined with nitric acid  Ammonium carbonate is combined with barium chlorate  Lithium sulfite reacts with phosphoric acid

 Alkanes- straight chain hydrocarbons with all single bonds C x H 2x+2  Alkenes- hydrocarbons with a double bond C x H 2x+2 -2 or C x H 2x  Alkynes- hydrocarbons with a triple bond C x H 2x+2 -4 or C x H 2x-2  Cyclic hydrocarbons- rings  C x H 2x+2 -2 or C x H 2x

# of C atoms Meth1Hex6 Eth2Hept7 Prop3Oct8 But4Non9 Pent5Dec10

 Combustion- reacts with O 2 makes H 2 O + CO 2  hexane is burned in air  C 5 H O 2  5 CO 2 + 6H 2 O  Addition- halogen added to place of a double bond  Butene reacts with fluorine  C 4 H 8 + F 2  C 4 H 8 F 2  Substitution- halogen replaces one hydrogen  Ethane reacts with chlorine  C 2 H 6 + Cl 2  C 2 H 5 Cl + HCl 24