11-1 Notes. Chemical Reactions
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1 11-1 Notes Chemical Reactions
2 Chemical Reactions In a chemical reaction 1 or more substances (the reactants) change into 1 or more new substances (the products). Reactants are always written on the left of an equation Products are always written on the right side of the equation An (read as yields) separates them. Reactants yield products Example: Iron + oxygen iron (III) oxide
3 Word Equations To write a word equation: 1. Write the names of the reactants to the left of the arrow separated by plus signs if necessary 2. Write the names of the products to the right of the arrow separated by plus signs if necessary Example - Hydrogen peroxide water + oxygen
4 Chemical Equations A representation of a chemical reaction The formulas of the reactants on the left The formulas of the products on the right Example: Fe + O 2 Fe 2 O 3 A skeleton equation is a chemical equation that does not indicate the relative amounts of the products and reactants See table 11.1 for symbols used in equations
5 Writing Chemical Equations To write a chemical equation: 1. Write the formulas of the reactants to the left of the arrow 2. Write the formulas of the products to the right of the arrow Indicate the state each element is in. Ex. Gas = (g) Liquid = (l) Solid = (s) Aqueous solution = (aq) A catalyst is a substance that speeds up a reaction but is not used in the reaction. Catalysts are always written over the arrow.
6 Balancing Chemical Equations A balanced equation indicates the quantity of the reactants to make the products. To balance an equation we use coefficients which are small whole numbers that are placed in front of a particular formula in order to balance it. In a balanced chemical reaction the number of atoms on the left side of the equation must equal the number of atoms on the right side of the equation.
7 Balancing Chemical Equations Fe + O 2 Fe 2 O 3 1. Write the # of atoms of each element on each side of the arrow 2. Use coefficients to balance 4Fe + 3O 2 2Fe 2 O 3 Do not forget to reduce the coefficients if possible. Sample Problems #3 & 4 (homework)
8 11-2 Notes Types of Chemical Reactions
9 Classifying Reactions There are five general types of equations Combination Reactions Decomposition Reactions Single-replacement Reactions Double-replacement Reactions Combustion Reactions
10 Combination Reactions A chemical change in which two or more substances react to form a single new substance. Examples: a + b = c 2Mg + O 2 2MgO Generally a combination reaction involves two elements chemically combining, however, two compounds may also combine to form one new substance
11 Decomposition Reactions A chemical change in which a single compound is broken down into two or more simpler products Examples A b + c 2HgO 2Hg + O 2 Decomposition reactions will only have one reactant. The products can be single elements or simple compounds
12 Single-Replacement Reactions A chemical change in which one element replaces a second element in a compound Examples: a + bc ac + b Zn + Cu(NO 3 ) 2 Cu + Zn(NO 3 ) 2 Br 2 + NaI NaBr + I 2 Whether one metal will displace another metal from a compound depends on the relative reactivities of the two metals
13 Single-Replacement Reactions The activity series of metals lists metals in order of decreasing activity See table 11.2 p. 333 A reactive metal will replace any metal listed below it. Halogens decrease in activity as you go down the period. Br 2 + NaI NaBr + I 2 Br 2 + NaCl no reaction It would not react because bromine is less active then chlorine.
14 Double Replacement Reactions A chemical change involving an exchange of positive ions between two compounds Examples ab + cd ad + cb Na 2 S + Cd(NO 3 ) 2 CdS + 2NaNO 3 Ca(OH) 2 + 2HCl CaCl 2 + 2H 2 O
15 Combustion Reactions A chemical change in which an element or compound reacts with oxygen, often producing energy in the form of heat and light Hydrocarbons are often involved in combustion reactions Hydrocarbons react with oxygen to form carbon dioxide and water Examples: C 4 H 10 + O 2 CO 2 + H 2 O 2 Mg + O 2 2MgO also considered a combination reaction.
16 Predicting the Products of a Chemical Reaction The number of elements and/or compounds reacting is a good indicator of possible reaction type and thus possible products. Examples: In a combination reaction you will have at least 2 reactants In a double replacement reaction you will also have 2 reactants but they must be compounds not single elements. Copy Fig
17 11-3 Notes Reactions in Aqueous Solutions
18 Net Ionic Equations Many chemical equations take place in water, scientifically speaking, aqueous solution In the reaction of silver nitrate with sodium chloride, a solid silver chloride precipitates out. AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) This is the correct equation, but it does not show how the ions disassociate out of the solution.
19 Net Ionic Equations In the reaction, the AgNO 3 and the NaCl disassociate into Na +, Cl -, Ag + and NO 3- ions. You can show this happening by writing a complete ionic equation. Ag + (aq) + NO 3- (aq) + Na + (aq) + Cl - (aq) AgCl(s) + Na + (aq) + NO 3- (aq)
20 Net Ionic Equations If an ion appears on both sides of the equation, it means that it is not directly involved in the reaction. These ions are called spectator ions. When you write a net ionic equation you must leave out all spectator ions. Net Ionic Equation: Ag+(aq) + Cl-(aq) AgCl (s)
21 Net Ionic Equations Another Example: Pb(s) + AgNO 3 (aq) Ag(s) + Pb(NO 3 ) 2 (aq) Pb(s) + Ag + (aq) + NO NO - 3 Pb(s) + Ag + Pb(s) + 2Ag + Ag(s) + Pb 2+ (aq) Ag(s) + Pb 2+ (unbalanced) 2Ag(s) + Pb 2+ (balanced) A net ionic equation shows only those particles involved in the reaction and is balanced with respect to both mass and charge.
22 Predicting the formation of a Precipitate A precipitate is a solid that forms or settles out of a liquid mixture. You can predict the formation of a precipitate by using the general rules for the solubility of ionic compounds Copy table 11.3 page 344 Will a precipitate form when aqueous solutions of NaCO 3 (aq) and Ba(NO 3 ) 2 are mixed?
23 Predicting the formation of a Precipitate When these four ions are mixed the cations could change partners. If this happened the following compounds would form: NaNO 3 and BaCO 3 Sodium is an alkali metal. NO 3 is a nitrate salt. According to the table both of these are soluble so the combination will not form a precipitate.
24 Predicting the formation of a Precipitate CO 3 is a carbonate According to the table most carbonates are insoluble. Therefore, BaCO 3 is not soluble so it will form precipitate. Write the net ionic equation. Ba 2+ (aq) + CO 3 2- (aq) BaCO 3 (s)
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