6 Basic Types of Reactions

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Presentation transcript:

6 Basic Types of Reactions Combination (Synthesis) Decomposition Single replacement Double replacement Neutralisation Combustion

Combination Reactions reactants join together to form a single product

Magnesium burns in Oxygen

Decomposition Reactions Products split to form 2 or more reactants

Electrolysis of water

Decomposition of Hydrogen Peroxide

Single Replacement Reaction A single compound replaces one element for another (ie. Metals swap positions) AB + C  AC + B

Hydrochloric Acid with Mg metal

Double Replacement Reaction When two ionic compounds swap ions with each other (eg. Cations swap places) AB + CD  AD + CB

Precipitation Reactions

Potassium iodide + lead nitrate  Lead nitrate + potassium iodide

Which one forms a precipitate? Soluble = dissolves, no precipitate (aq) Low solubility = forms a solid precipitate (s)

Solubility Table (pg. 152)

Writing the chemical equation:

___NaOH + ____Pb(NO3) 2 ___ Pb(OH) 2 + ___ NaNO3 Balance the Equation ___NaOH + ____Pb(NO3) 2 ___ Pb(OH) 2 + ___ NaNO3 Balance order: 1st metals 2nd any groups (in brackets) 3rd non-metals 4th oxygen or hydrogen last

Neutralisation Reaction A special type of double replacement reaction involving an acid and base to form an ionic salt and water Eg. HBr + LiOH 

Combustion Reaction

Gasoline vs Diesel

Balance the reaction: hexane + oxygen  carbon dioxide + water C6H14 (l) + O2 (g)  CO2 (g) + H20 (g)