Chemical Reactions
All chemical reactions involve changes in substances Reactants – starting substances Products – new substances formed Reactants Products
Example: Iron + Oxygen Iron (III) oxide (Rust)
In all chemical reactions: Bonds are broken and new bonds form Law of Conservation of matter is supported Atoms are not created or destroyed – just rearranged During an ordinary chemical change, there is no detectable increase or decrease in the quantity of matter
Symbols in Chemical Reactions + used to separate two products or reactants yields (s) subscript – represents a solid (l) subscript – represents a liquid (aq) subscript – represents an aqueous solution (g) subscript – represents a gas
Symbols (cont.) replaces (s) to represent a precipitate replaces (g) to represent a gas
Symbols (cont.) Fe indicates the use of a catalyst (in this case iron) heat or indicates that heat is supplied to the reaction
Examples: Zn (s) + 2HCl (aq) H 2 + ZnCl 2(aq) O 2(g) + 2HO 2H 2 O 2(l) KI O 2(g) + 2H 2 O (l) Pb(NO 3 ) 2 (aq) + 2KI (aq) PbI 2(s) + 2KNO 3 (aq)
Chemical Equations Use formulas to represent elements and compounds Atoms must balance on both sides of the equation Atom inventories are helpful
Rules for Balancing Chemical Equations Determine the correct formulas for all reactants and products in the reaction Reactants go on the left side of the equation Products on the right side of the equation Count the atoms of each element in the reactants and products Balance the elements one at a time by changing the coefficients (NOT subscripts)
Balancing Equations (cont.) Tricks that help Save uncombined elements for last Use least common multiple to balance elements that have odd and even atoms on opposite sides Remember polyatomic ions often remain intact in a reaction count them as a single part Write water as HOH in acid/base reactions
Balancing Equations (cont.) Check each atom or polyatomic ion to be sure that both sides are equal Make sure coefficients are in the lowest possible ratio
Now lets practice! Potassium chlorate is heated and breaks down into potassium chloride and oxygen gas – Write the balanced equation for this reaction. Hydrochloric acid reacts with zinc to produces hydrogen gas and zinc chloride solution, write the chemical equation for this reaction.
6 Types of Chemical Reactions Synthesis (combination) Decomposition Single Replacement Double Replacement Combustion Acid/Base
Synthesis Reactions Two or more substances react to form a single substance Two or more simple compounds combine to form a more complicated one
Examples of Synthesis Reactions 2Mg (s) + O 2(g) 2MgO (s) 8Fe (s) + S 8(s) 8 FeS (s)
Decomposition Reactions A single compound is broken down into two or more simpler substances a complex molecule breaks down to make simpler ones
Examples of Decomposition Reactions 2 H 2 O (l) 2H 2(g) + O 2(g) 2KClO 3(s) 2KCl (s) + 3O 2(g) CaCO 3(s) CaO (s) + CO 2(g)
Single Replacement Reactions Atoms of an element replace the atoms of a second element in a compound Element 1+ Compound 1 Element 2 + Compound 2 net/stwbwk05/05flashchem/avreaction/ avreaction.html net/stwbwk05/05flashchem/avreaction/ avreaction.html
Examples of Single Replacement Reactions 2Al (s) + 3NiSO 4(aq) Al 2 (SO 4 ) 3(aq) + 3Ni (s) 2Fe (s) + 6HBr (aq) 2FeBr 3 (aq) + 3H 2(g) Cl 2(g) + 2KI (aq) 2KCl (aq) + I 2(s)
Double Replacement Reactions Involves the exchange of the positive ions between two compounds Also called metathesis net/stwbwk03/03hchem/nfreaction/nfre action.html net/stwbwk03/03hchem/nfreaction/nfre action.html
Examples of Double Replacement Reactions CaCl 2 (aq) + K 2 CO 3 (aq) CaCO 3 (s) + 2KCl (aq) 3AgNO 3 (aq) + FeCl 3 (aq) 3AgCl (s) + Fe(NO 3 ) 3 (aq )
Combustion Reactions Oxygen reacts with another substance usually producing energy in the form of heat and/or light
Examples of Combustion Reactions CH 4(g) + 2O 2(g) ---> CO 2(g) + 2H 2 O (g) + heat 2C 2 H 6(g) + 7O 2(g) ---> 4CO 2(g) + 6H 2 O (g) + heat C 6 H 12 O 6(s) + 6O 2(g) ---> 6CO 2(g) + 6H 2 O (g) + heat 4C 2 H 5 OH(l) + 13O 2(g) ---> 8CO 2(g) + 10H 2 O (g) + heat
Acid/Base Reactions acid with a base produces a salt plus water The cation in the salt comes from the base; the anion comes from the acid
Examples of Acid/Base Reactions 2HCl (aq) + Ca(OH) 2 (aq) CaCl 2 (aq) + 2H 2 O (l) Acid + Base Salt + Water 3H 2 SO 4(aq) + 2Fe(OH) 3(s) Fe 2 (SO 4 ) 3(aq) + 6H 2 O (l) Acid + Base Salt + Water