Unit 4: Chemical Reactions - Oak Park Independent · Unit 4: Chemical Reactions ... > Skeleton...
Transcript of Unit 4: Chemical Reactions - Oak Park Independent · Unit 4: Chemical Reactions ... > Skeleton...
January 11, 2015
Unit 4: Chemical Reactions
What is a chemical reaction?• the process by which the atoms of one or more
substances are rearranged to form different substances
• chemical change
What chemical reactions are important in your life?
Physical change: substance does not change identity
Chemical change: new substances are formed
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Evidence of Chemical Reaction (or chemical change)
1. Temperature change2. Light3. Color change4. Production of gasses5. Production of solids (precipitate)6. Odor change
What evidence of a chemical reaction do you see in a fire?
What evidence of a chemical reaction do you see when you roast a marshmallow?
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Representing Chemical Reactions
• As chemists, we can describe chemical reactions in different ways.> In a sentence> Word equations> Skeleton equation> Chemical equations
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This arrow separates the reactants from the products (kind of like the equal sign in math)
When you have more than one reactant or product, use a plus sign
Representing Chemical Reactions
• Reactants are the starting substances of a reaction.• Products are the substances formed during the
reaction.
reactant 1 + reactant 2 product 1 + product 2
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2. Word Equation
iron(s) + chlorine(g) iron (III) chloride(s)
1. In a sentence
"Solid iron and chlorine gas react to produce solid iron (III) chloride."
The letters in parentheses shows you the state of matter:
(s) = solid state
(l) = liquid state
(g) = gas state
(aq) = water solution
3. Skeleton Equation: uses chemical formulas
Fe(s) + Cl2(g) FeCl3(s)
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Example 1:
Write skeleton equations for these word equations.
1. hydrogen(g) + bromine(g) hydrogen bromide(g)
2. carbon monoxide(g) + oxygen(g) carbon dioxide(g)
3. potassium chlorate(s) potassium chloride(s) + oxygen(g)
HON17: Always diatomic
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4. Chemical equation: Balanced equation that shows the reactants and products, and the relative amounts involved in the reaction.
> Conservation of mass (mass of reactants = mass of products)
> Need to have same # of atoms of each element in the reactants and products.
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How to balance chemical equations
1. Write the unbalanced (skeleton) equation.2. Count the atoms of the elements in the reactants
and products.3. Use coefficients to make the # of atoms of each
element equal on both sides of the equation.> Coefficients:numbers written in front of a
reactant or product. Tells us the number of particles of the substance involved in the reaction.
4. Make sure coefficients are in their lowest possible ratio.
5. Check your work!
unbalanced equation: Fe(s) + Cl2(g) FeCl3(s)
chemical equation: Fe(s) + Cl2(g) FeCl3(s)
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Example 2: Write the balanced chemical equation for each.1. Hydrogen gas and chlorine gas combine to form hydrochloric acid (HCl)
2. __CS2(l) + __O2(g) __CO2(g) + __SO2(g)
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Example 2 (cont): Balance the following
H2(g) + Cl2(g) HCl(g)
CS2(l) + O2(g) CO2(g) + SO2(g)
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Example 2 (cont): Balance the following
CaO(s) + H2O(l) Ca(OH)2(s)
NaOH(aq) + CaBr2(aq) Ca(OH)2(s) + NaBr(aq)
*When balancing equations with Polyatomic Ions that appear in the reactant and product, keep it together as one "unit" and balance.
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