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Warm Up:. Why do chemical equations need to be balanced? Balance the following equation: __PbCl 2 + __ AgNO 3 __ Pb (NO 3 ) + __ AgCl. Types of Chemical Reactions. Learning Target: To be able to identify the different type of reactions when looking at skeletal equations. - PowerPoint PPT Presentation
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Warm Up: Why do chemical equations need to be
balanced?
Balance the following equation:
__PbCl2 + __ AgNO3 __Pb(NO3) + __ AgCl
Types of Chemical Reactions
Learning Target: To be able to identify the different type of reactions when looking at skeletal equations
Types of Reactions:
There are 5 types of Reactions:1. Synthesis2. Decomposition3. Single-replacement4. Double-replacement5. Combustion
Synthesis: A chemical rxn in which 2 or more substances (A + B) react to produce a single product (AB)
A + B ⇒ ABNa(s) + Cl2(g) ⇒ NaCl(s)
SO2(g) + O2(g) ⇒ SO3(g)
Decomposition: A rxn in which a single compound (AB) breaks down into 2 or more new substances (A + B…)
AB ⇒ A + B
NH4NO3(s) ⇒ N2O(g) + H2O(g)
Na3N(s) ⇒ Na(s) + N2(g)
Single Replacement: A rxn in which the atoms of one element replace the atoms of another element in a compound
A + BX ⇒ AX + B
Li(s) + H2O(l) ⇒ LiOH(aq) + H2(g)
Cu(s) + AgNO3(aq) ⇒ Ag(s) + Cu(NO3)2
Double Replacement: a rxn which involves an exchange of ions between 2 compounds
AX + BY ⇒ AY + BX*Either the metals change places or the nonmetals change places but not both!!!
Ca(OH)2(aq) + HCl(aq) ⇒ CaCl2(aq) + H2O(l)
*Typically occurs in aqueous solutions (in water)
NaOH(aq) + CuCl2(aq) ⇒ NaCl(aq) + Cu(OH)2(s)
*Precipitate: Is when a solid forms from a solution
3 Types of Double Replacement:
1.Formation of a precipitate
2.Formation of H2O
3.Formation of a product which decomposes into a gas
Double-Replacement: Formation of a precipitate
Solubility Rules: Some compounds will dissolve in water (soluble) Some will NOT dissolve in water (insoluble/ not
soluble)
If during a double-replacement rxn is formed, it will fall out of the solution as a solid, which is called a percipitant.
Double-Replacement: Formation of H2O These occur between Acids and Bases
Acids ALWAYS start with _________ Bases are compounds that end with hydroxides
(OH-) One product will be H2O and one will be an ionic
compound salt
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
*Some people consider this a separate rxn altogether
Combustion: a rxn in which O2 can combine with a substance to release energy Ex: Fire, Burning, Magnesium Stripe, etc.
C(s) + O2(g) ⇒ CO2(g)
CH4(g) + O2(g) ⇒ CO2(g) + H2O(l)
*In most cases, the products will be H2O and CO2
Activity Series: Single Replacement Rxn
Active metals will replace less active metals in reactions.
Pt(s) + Zn2O (aq) → NR
Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)
Na(s) + SnCO3(aq) → Na2CO3(aq) + Sn(s)
Practice Problems: Complete these in your notes and see how many you get right!
1. C2H6(g) + O2(g) → H2O(g) +CO2(g)
2. Br2(l) + LiI(s) → LiBr + I2(s)
3. Fe(s) + H2O(l) →Fe3O4(s) + H2(g)
4. MgCO3(s) → MgO(s) + CO2(g)
5. P4(s) + O2(g) → P4O10(s)
6. KNO3(s) → KNO2(s) + O2(g)
7. KOH + H3PO4 →K3PO4 + H2O
8. Na(s) + O2(g) →Na2O(s)
9. O2(g) + C6H12O6(g) → H2O(g) + CO2(g)