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Download Types of Reactions notes 02 Types of chemical reactions
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Transcript
Chemical Equations Chemical change involves a reorganization of the atoms in one or more substances. Chemical Equation A representation of a chemical reaction: CH4 + O2 CO2 + H2O reactants products Physical States When you see a chemical formula, often the formula is followed by a symbol in parentheses. For example: H2O(l) - the water is liquid H2O(s) - the water is solid (ice) H2O(g)- the water is a gas (steam) NaCl(aq) – means that the chemical is disolved in water. In this case it would be salt dissolved in water. The Magnificent 7 (diatomic molecules) Certain elements do not exist naturally as a single atom. They exist in pairs. So when writing out a chemical equation it is important to write the chemical formula to show that. The 7 are: H2, N2, O2, F2, Cl2, Br2, and I2 Types of Reactions Synthesis Reaction When two or more reactants come together to make one product. Also called Combination. Example: N2 + H2 NH3 Note that diatomic molecules (Magnificent 7!) must be diatomic in their elemental form. Decomposition Reaction When a single compound is broken down into two or more products Example: H2O H2 + O2 Single Displacement Reaction When an element and an ionic compound react and the element takes the place of its comparable ion Metal element takes positive ion’s place Nonmetal element takes negative ion’ place Examples: Mg + FeCl3 MgCl2 + Fe Br2 + FeCl3 FeBr3 + Cl2 Mg + FeCl3 MgCl2 + Fe Br2 + FeCl3 FeBr3 + Cl2 Notice! The neutral atom joins the compound becoming a charged ion. The products MUST be electronically neutral. Since Mg becomes Mg+2, two Cl ions neutralize it. The charge on the transition metal stays the same if it remains as an ion (iron is +3 charge in both the reactant and product) Double Displacement Reaction When two ionic compounds switch their partner ions. Positive goes with other negative and vice versa. Switcheroo! Example: NaCl + MgBr2 MgCl2 + NaBr Pb(NO3)2 + Na2SO4 NaNO3 + PbSO4 NaCl + MgBr2 MgCl2 + NaBr Pb(NO3)2 + Na2SO4 NaNO3 + PbSO4 Notice! The reactants and products MUST be electronically neutral All ions keep their charge from reactants to products Do not get fooled into thinking that if there are a certain number atoms of an element in the reactants, there will be the same number in the products! Polyatomic ions are very common in these types of reactions. Make sure you can spot them! Combustion Reactions When a hydrocarbon (something with C’s and H’s and sometimes O’s – organic molecule) reacts with Oxygen to form water and carbon dioxide and heat energy. Example: CH4 + O2 CO2 + H2O C4H8 + O2 CO2 + H2O Acid/Base reaction When an acid reacts with a base, water forms Acids produce H+ in water Bases produce OH- in water Example: HNO3 + KOH HOH (or H2O) + KNO3 What type of equation are each of the following reactions? P + O2 P2O5 C3H5O + O2 CO2 + H2O NH4NO3 N2O + H2O Fe2O3 + C Fe + CO CO2 + H2O H2CO3 CuNO3 + Na2SO4 Cu2SO4 + NaNO3 Check Your Answers P + O2 P2O5 Synthesis C3H5O + O2 CO2 + H2O Combustion NH4NO3 N2O + H2O Decomposition Fe2O3 + C Fe + CO Single Displacement Check Your Answers CO2 + H2O H2CO3 Synthesis CuNO3 + Na2SO4 Cu2SO4 + NaNO3 Double Displacement
