Chemical Reactions Chapter 11

Do Now- In your own words Write an explanation for what Is happening in this picture. Objective 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 solution heat ∆heat was supplied to reaction Pt Element (Pt) used as catalyst

Chemical Equations Reactants → Products iron + oxygen → iron(III) oxide Fe + O 2 → Fe 2 O 3

→

Chemical Equations Reactants → Products iron + oxygen → iron(III) oxide Fe + O 2 → Fe 2 O 3 4Fe(s) + 3O 2 (g) → 2Fe 2 O 3 (s)

Magnesium + Oxygen → Magnesium oxide

Mg + O 2 → MgO

Magnesium + Oxygen → Magnesium oxide Mg + O 2 → MgO 2Mg + O 2 → 2MgO

Do Now - Write the ionic or molecular formula for Lithium Oxide Aluminum Sulfide Silicon 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 + O 2 → Fe 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 + O 2 → Fe 2 O 3 Fe 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 + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 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 + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 2 O 3 Fe + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 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 + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 2 O 3 Fe + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 2 O 3 Fe + O 2 → Fe 2 O 3 Fe 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 + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 2 O 3 Fe + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 2 O 3 4Fe + 3O 2 → 2Fe 2 O 3 Fe 4 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 + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 2 O 3 Fe + O 2 → Fe 2 O 3 Fe 1 Fe 2 O 2 O 3 4Fe + 3O 2 → 2Fe 2 O 3 Fe 4 O 6 4Fe + 3O 2 → 2Fe 2 O 3