Chemical Reactions: An Introduction
Indicators of a Chemical Reaction A color change A solid forms (precipitate) A gas forms The temperature changes (hot OR cold)
Chemical Equations Reactants – what goes INTO the rxn Products – what comes OUT OF the rxn Reactant A + Reactant B Product A
Law of Conservation of Mass In a chemical reaction, atoms are neither created or destroyed All atoms in the reactants MUST be accounted for in the products.
Physical States After each reactant and product is a symbol representing the physical state of the element or compound (s) – solid (l) – liquid (g) – gas (aq) – aqueous (dissolved in water)
Balancing Chemical Equations Done by trial and error 1.Balance elements that only appear once 2.Keep polyatomic ions together if possible 3.***NEVER EVER EVER EVER CHANGE A SUBSCRIPT!!!*** 4.Balance hydrogen and oxygen last
Diatomic Molecules 7 elements exist in nature as diatomic molecules (2 atoms) –Hydrogen (H 2 ) –Oxygen (O 2 ) –Nitrogen (N 2 ) –Fluorine (F 2 ) –Chlorine (Cl 2 ) –Bromine (Br 2 ) –Iodine (I 2 )
C 2 H 5 OH (l) + O 2 (g) CO 2 (g) + H 2 O(g)
Fe 2 O 3 (s) + HNO 3 (aq) Fe(NO 3 ) 3 (aq) + H 2 O(l)
H 2 S(g) + Pb(NO 3 ) 2 (aq) PbS(s) + HNO 3 (aq)
Types of Reactions
Objectives 1.Give general equations for types of reactions 2.Classify reactions 3.List 3 types of synthesis and 6 decomposition reactions 4.List 4 types of single-replacement and 3 types of double-replacement reactions 5.Predict products of reactions given the reactants
Synthesis Reactions General Formula: A + X AX
Synthesis with Oxygen With metals form metal oxides Ex – Mg(s) + O 2 (g) MgO(s) K(s) + O 2 (g) K 2 O(s) 2Fe(s) + O 2 (g) 2FeO(s) 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 S 8 (s) + 8O 2 (g) 8SO 2 (g) C(s) + O 2 (g) CO 2 (g)
Synthesis with Sulfur With metals produce metal sulfides Ex-16Rb(s) + S 8 (s) 8Rb 2 S(s) 8Ba(s) + S 8 (s) 8BaS(s)
Metals with Halogens Group 1: M + X 2 2MX Ex – Na(s) + Cl 2 (g) 2NaCl(s) Group 2: M + X 2 MX 2 Ex – Mg(s) + F 2 (g) MgF 2 (s)
Metal Oxides with Water Group 1 & 2 form hydroxides Ex – K 2 O(s) + H 2 O(l) 2KOH(aq) CaO(s) + H 2 O(l) Ca(OH) 2 (l)
Non-metal Oxide with Water Form oxyacids Ex – SO 2 (g) + H 2 O(l) H 2 SO 3 (aq) P 2 O 5 (s) + 3H 2 O(l) 2H 3 PO 4 (aq)
Decomposition Reactions AX A + X
Decomposition of Binary Compounds Breaks down into its elements Process called electrolysis
Decomposition of Metal Carbonates Form metal oxides and carbon dioxide
Decomposition of Metal Hydroxides Form metal oxides and water
Decomposition of Acids Break down into non-metal oxides and water
Single Replacement General Formula A + BX AX + B
Metal Replaces Another Metal Aluminum is more reactive than lead
Replacement of Hydrogen in Water by a Metal More Active Metals Less Active Metals
Replacement of Hydrogen in an Acid by a Metal Metals more active than hydrogen
Replacement of Halogens Each halogen can replace the halogen below it on the periodic table
Double Replacement AX + BY AY + BX Formation of a precipitate Formation of a gas Formation of water
Formation of a Precipitate An insoluble product forms
Formation of a Gas Insoluble gas forms Example
Formation of Water Water forms during reaction
Combustion Reaction Substance reacts with oxygen to release heat and light Products are often carbon dioxide and water
Neutralization Reaction HA + BOH AB + HOH Usually these are acid-base reactions Products include salt and water
Activity Series
Objectives 1.Explain the significance of an activity series 2.Use an activity series to predict if a reaction will take place
Metals vs. Nonmetals Greater activity of a metal indicates how easily it loses electrons Greater activity of a nonmetal indicates how easily it gains electrons In a single-replacement reaction, if an element with lower activity is to be replaced, the reaction will take place.