Summary
Summary Reactions
- Course
- Chemistry
- Institution
- 11th Grade
Balancing Chemical Equations, Synthesis Equations, Decomposition Reactions, Single-Displacement Reactions
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L1: Balancing Chemical Equations● Physical Changes
○ Change in the physical property of a substance
○ No change occurs in the identity of the substance
● Chemical Changes
○ Atoms in the reactants are rearranged to form one or more different substances that are
new
○ Old bonds are broke, new bonds form
○ Example: Fe and O2 form rust (Fe2O3)
● Chemical Reaction
○ A process in which at least one new substance is produced as a result of chemical change
○ Reactants → Products
○ All chemical equations show the reactants on the LEFT and the products on the RIGHT
○ Reactants: The number of atoms in the reactants atoms
○ Products: The number of atoms in the products atoms
● Steps for Balancing Chemical Equations
○ Check for diatomic molecules: H, N, O, F, Cl, Br, I
■ If these elements appear by themselves in an equation, they must be written with
a subscript of 2
○ Balance metals
○ Balance non-metals
○ Balance oxygen
○ Balance hydrogen
L2: Synthesis Equations
● Two or more simple substances combine to produce a more complex substance
● Two or more reactants to make on product
● A+B → AB
○ Example: H2+I2 → 2HI
○ HCL + NH3 → NH4Cl
● Oxide: element composed of oxygen and one other element
○ MgO
○ 2MG + O → 2MgO
● Acidic Oxides
○ Acidic oxides (non-metal oxide) react with water to form acids
○ CO2 + H2O → H2CO3
○ Other non-metal oxides are sulfur trioxide, dinitrogen pentoxide
● Basic Oxides
○ Basic oxides (metal oxides) reacts with water to form bases
○ CaO + H2O → Ca(OH)2
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