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### Chemical Reactions

4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)

4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)

4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)

4. Balance the number of atoms of each element by adding coefficients. (The subscripts can’t be changed now)

Chapter 11

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

+ 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 + O2 → Fe2O3

- Chemical Equations
Reactants → Products

iron + oxygen → iron(III) oxide

Fe + O2 → Fe2O3

4Fe(s) + 3O2(g) → 2Fe2O3 (s)

Magnesium + Oxygen → Magnesium oxide

Mg + O2 → MgO

- 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

- Do Now - Write the ionic or molecular formula for OxideLithium Oxide Li2O
Aluminum Sulfide Al2S3

Silicon Oxide SiO2

Balancing Chemical Equations Oxide

Take the time to write the steps you used to balance this problem. If you can write the steps used you can use them to balance any chemical equation.

Fe + O2 → Fe2O3

Iron + oxygen → iron oxide 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 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 Oxide

Fe + O2 → Fe2O3

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 Oxide

Fe + O2 → Fe2O3

Fe 1 Fe 2

O 2 O 3

Fe + O2 → Fe2O3

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.

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 Oxide

Fe + O2 → Fe2O3

Fe 1 Fe 2

O 2 O 3

Fe + O2 → Fe2O3

Fe 1 Fe 2

O 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.

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 Oxide

Fe + O2 → Fe2O3

Fe 1 Fe 2

O 2 O 3

Fe + O2 → Fe2O3

Fe 1 Fe 2

O 2 O 3

4Fe + 3O2→ 2Fe2O3

Fe 4 Fe 4

O 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.

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 Oxide

Fe + O2 → Fe2O3

Fe 1 Fe 2

O 2 O 3

Fe + O2 → Fe2O3

Fe 1 Fe 2

O 2 O 3

4Fe + 3O2→ 2Fe2O3

Fe 4 Fe 4

O 6 O 6

4Fe + 3O2 → 2Fe2O3

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.

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.

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