chemical reactions: an introduction. indicators of a chemical reaction a color change a solid forms...
DESCRIPTION
Chemical Equations Reactants – what goes INTO the rxn Products – what comes OUT OF the rxn Reactant A + Reactant B Product ATRANSCRIPT
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Chemical Reactions:An Introduction
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Indicators of a Chemical Reaction• A color change
• A solid forms (precipitate)
• A gas forms
• The temperature changes (hot OR cold)
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Chemical EquationsReactants – what goes INTO the rxn
Products – what comes OUT OF the rxn
Reactant A + Reactant B Product A
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Law of Conservation of MassIn a chemical reaction, atoms are neither
created or destroyed
All atoms in the reactants MUST be accounted for in the products.
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Physical StatesAfter 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)
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Balancing Chemical EquationsDone by trial and error
1. Balance elements that only appear once2. Keep polyatomic ions together if possible
3. ***NEVER EVER EVER EVER CHANGE A SUBSCRIPT!!!***
4. Balance hydrogen and oxygen last
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Diatomic Molecules• 7 elements exist in nature as diatomic
molecules (2 atoms)– Hydrogen (H2)– Oxygen (O2)– Nitrogen (N2)– Fluorine (F2)– Chlorine (Cl2)– Bromine (Br2)– Iodine (I2)
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C2H5OH (l) + O2(g) CO2(g) + H2O(g)
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Fe2O3(s) + HNO3(aq) Fe(NO3)3(aq) + H2O(l)
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H2S(g) + Pb(NO3)2(aq) PbS(s) + HNO3(aq)
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Types of Reactions
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Objectives1. Give general equations for types of
reactions2. Classify reactions3. List 3 types of synthesis and 6
decomposition reactions4. List 4 types of single-replacement and 3
types of double-replacement reactions5. Predict products of reactions given the
reactants
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Synthesis ReactionsGeneral Formula:
A + X AX
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Synthesis with OxygenWith metals form metal oxides
Ex – Mg(s) + O2(g) MgO(s)
K(s) + O2(g) K2O(s)
2Fe(s) + O2(g) 2FeO(s)
4Fe(s) + 3O2(g) 2Fe2O3
S8(s) + 8O2(g) 8SO2(g)
C(s) + O2(g) CO2(g)
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Synthesis with SulfurWith metals produce metal sulfides
Ex- 16Rb(s) + S8(s) 8Rb2S(s)
8Ba(s) + S8(s) 8BaS(s)
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Metals with HalogensGroup 1: M + X2 2MX
Ex – Na(s) + Cl2(g) 2NaCl(s)
Group 2: M + X2 MX2
Ex – Mg(s) + F2(g) MgF2(s)
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Metal Oxides with WaterGroup 1 & 2 form hydroxides
Ex – K2O(s) + H2O(l) 2KOH(aq)
CaO(s) + H2O(l) Ca(OH)2(l)
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Non-metal Oxide with WaterForm oxyacids
Ex – SO2(g) + H2O(l) H2SO3(aq)
P2O5(s) + 3H2O(l) 2H3PO4(aq)
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Decomposition ReactionsAX A + X
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Decomposition of Binary CompoundsBreaks down into its elements
(g)O (g)2H O(l)2H 22yelectricit
2
Process called electrolysis
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Decomposition of Metal CarbonatesForm metal oxides and carbon dioxide
(g)CO CaO(s) (s)CaCO 23
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Decomposition of Metal HydroxidesForm metal oxides and water
O(g)H CaO(s) (s)Ca(OH) 22
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Decomposition of AcidsBreak down into non-metal oxides and water
O(g)H (g)CO (aq)COH 2232
O(l)H (g)SO (aq)SOH 2342
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Single ReplacementGeneral Formula
A + BX AX + B
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Metal Replaces Another MetalAluminum is more reactive than lead
(aq))2Al(NO 3Pb(s) (aq))Pb(NO 2Al(s)
33
23
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Replacement of Hydrogen in Water by a MetalMore Active Metals
(g)H 2NaOH(aq) O(l)2H 2Na(s) 22
Less Active Metals
(g)4H (s)OFe O(g)4H 3Fe(s) 2432
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Replacement of Hydrogen in an Acid by a MetalMetals more active than hydrogen
(aq)MgCl (g)H 2HCl(aq) Mg(s) 22
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Replacement of HalogensEach halogen can replace the halogen below it
on the periodic table
reaction no 2NaCl(aq) (g)I(g)Cl 2KF(aq) 2KCl(aq) (g)F
(g)Br 2KCl(aq) 2KBr(aq) (g)Cl
2
22
22
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Double ReplacementAX + BY AY + BX
• Formation of a precipitate• Formation of a gas• Formation of water
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Formation of a Precipitate
An insoluble product forms
(aq)2KNO (s)PbI (aq))Pb(NO KI(aq)2 3223
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Formation of a GasInsoluble gas forms
Example
(aq)FeCl S(g)H 2HCl(aq) FeS(s) 22
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Formation of WaterWater forms during reaction
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Combustion ReactionSubstance reacts with oxygen to release heat
and light
Products are often carbon dioxide and water
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Neutralization ReactionHA + BOH AB + HOH
Usually these are acid-base reactions
Products include salt and water
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Activity Series
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Objectives1. Explain the significance of an activity series
2. Use an activity series to predict if a reaction will take place
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Metals vs. NonmetalsGreater 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.