Chemical Reactions
Chapter 11
Do Now- In your own words Write an explanation for what Is happening in this picture.
Objective- 11.1 Describing Chemical Reactions
HW – Pg 329 # 9-12
11.1 Describing Chemical Reactions
• Word Equations
11.1 Describing Chemical Reactions
• Word Equations
Reactants → Products
11.1 Describing Chemical Reactions
• Word Equations
Reactants → Products
iron + oxygen → iron(III) oxide
Symbols Used in Chemical Reactions
+→↔(s)(l)(g)(aq)Heat ∆Pt
Symbols Used in Chemical Reactions
+ Separates two reactant and two products→ “Yields” Separates reactants from products↔ Reaction is reversible (s) solid(l) liquid (g) gas(aq) aqueous solutionheat ∆ heat was supplied to reactionPt Element (Pt) used as catalyst
• Chemical Equations
Reactants → Products iron + oxygen → iron(III) oxide Fe + O2 → Fe2O3
→
• Chemical Equations
Reactants → Products iron + oxygen → iron(III) oxide Fe + O2 → Fe2O3
4Fe(s) + 3O2(g) → 2Fe2O3 (s)
Magnesium + Oxygen → Magnesium oxide
Magnesium + Oxygen → Magnesium oxide
Mg + O2 → MgO
Magnesium + Oxygen → Magnesium oxide
Mg + O2 → MgO
2Mg + O2 → 2MgO
• Do Now - Write the ionic or molecular formula for Lithium Oxide
Aluminum SulfideSilicon Oxide
• Objective – Balance Chemical Equations
• Homework – finish Pg. 329 # 9 – 12 and handout
Balancing Chemical Equations
→
1. Determine correct formulas for all reactants and products. 2. Write a skeleton equation. 3. Determine the number of atoms of each element on the reactant side and the product side.
4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)
5. Check that the number of atoms of each element is the same on both sides. 6. Check to see that all coefficients are in lowest whole number ratio possible.
Iron + oxygen → iron oxide
Fe + O2 → Fe2O3
1. Determine correct formulas for all reactants and products. 2. Write a skeleton equation. 3. Determine the number of atoms of each element on the reactant side and the product side.
4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)
5. Check that the number of atoms of each element is the same on both sides. 6. Check to see that all coefficients are in lowest whole number ratio possible.
Iron + oxygen → iron oxide
Fe + O2 → Fe2O3
Fe Fe O O
1. Determine correct formulas for all reactants and products. 2. Write a skeleton equation. 3. Determine the number of atoms of each element on the reactant side and the product side.
4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)
5. Check that the number of atoms of each element is the same on both sides. 6. Check to see that all coefficients are in lowest whole number ratio possible.
Iron + oxygen → iron oxide
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
1. Determine correct formulas for all reactants and products. 2. Write a skeleton equation. 3. Determine the number of atoms of each element on the reactant side and the product side.
4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)
5. Check that the number of atoms of each element is the same on both sides. 6. Check to see that all coefficients are in lowest whole number ratio possible.
Iron + oxygen → iron oxide
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
1. Determine correct formulas for all reactants and products. 2. Write a skeleton equation. 3. Determine the number of atoms of each element on the reactant side and the product side.
4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)
5. Check that the number of atoms of each element is the same on both sides. 6. Check to see that all coefficients are in lowest whole number ratio possible.
Iron + oxygen → iron oxide
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
Fe + O2 → Fe2O3
Fe Fe O O
1. Determine correct formulas for all reactants and products. 2. Write a skeleton equation. 3. Determine the number of atoms of each element on the reactant side and the product side.
4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)
5. Check that the number of atoms of each element is the same on both sides. 6. Check to see that all coefficients are in lowest whole number ratio possible.
Iron + oxygen → iron oxide
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
4Fe + 3O2 → 2Fe2O3
Fe 4 Fe 4O 6 O 6
1. Determine correct formulas for all reactants and products. 2. Write a skeleton equation. 3. Determine the number of atoms of each element on the reactant side and the product side.
4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)
5. Check that the number of atoms of each element is the same on both sides. 6. Check to see that all coefficients are in lowest whole number ratio possible.
Iron + oxygen → iron oxide
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
Fe + O2 → Fe2O3
Fe 1 Fe 2O 2 O 3
4Fe + 3O2 → 2Fe2O3
Fe 4 Fe 4O 6 O 6
4Fe + 3O2 → 2Fe2O3