Types of Reactions Six Types.

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Presentation transcript:

Types of Reactions Six Types

Single Replacement A free element replaces one of the ions in a compound A metal replaces a metal OR a nonmetal replaces a nonmetal The single element replaces one of the ions in the solution and a new element appears from the ion in solution Element + Compound yields element + compound

Examples 2 KI + Cl2 → 2 KCl + I2 2 AgNO3 + Cu → Cu(NO3)2 + 2 Ag

Double Replacement The cations (+ ions) switch places OR anions (- ions) switch places A metal replaces a metal AND a nonmetal replaces a nonmetal Compound + Compound yields Compound + Compound

Double Replacement Often one of the product will be a precipitate – an insoluble solid product that separates from a solution.

Examples AgNO3 + KCl → AgCl + KNO3 Barium chloride + potassium sulfate yields barium sulfate + potassium chloride Make sure to switch the names and then write the formula accordingly, balancing charges BaCl2 + K2SO4 → BaSO4 + 2 KCl

(Acid-Base) Neutralization Special double displacement reaction Acids: compounds that begin with hydrogen Bases: compounds that end with hydroxide Acid + hydroxide compound → Salt (ionic compound) + H2O

Example HCl + NaOH → NaCl + H2O H2SO4 + 2 NH4OH → (NH4)2SO4 + 2 H2O NaCl is not the only salt!!!! H2SO4 + 2 NH4OH → (NH4)2SO4 + 2 H2O

Synthesis Two or more elements or compounds come together to make a single product A + B → AB Element or compound + element or compound yields a single compound

Examples 2 H2 + O2 → 2 H20 H20 + SO3 → H2SO4

Decomposition A coming apart; a single reactant comes apart into 2 or more products AB → A + B Compound yields two or more smaller substances (elements and/or compounds)

Examples 2 KClO3 → 2 KCl + 3O2 2 HgO → 2 Hg + O2

Combustion (of hydrocarbon) Hydrocarbon + oxygen → water + carbon dioxide CxHy + O2 → H2O + CO2 Coefficients will change according to your hydrocarbon subscripts C6H12 + 9 O2 → 6 H2O + 6 CO2

Many reactions will require activation energy - energy required to start a reaction. Some reactions need a catalyst - a subst. which speeds up a reaction without being permanently changed itself.