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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.

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Chemical reactions

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 reactions1
11.1 Describing Chemical Reactions

  • Word Equations

    Reactants → Products


11 1 describing chemical reactions2
11.1 Describing Chemical Reactions

  • Word Equations

    Reactants → Products

    iron + oxygen → iron(III) oxide


Symbols used in chemical reactions
Symbols Used in Chemical Reactions

+

(s)

(l)

(g)

(aq)

Heat ∆

Pt


Symbols used in chemical reactions1
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

2Mg + O2 → 2MgO




Balancing chemical equations
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.

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

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

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.

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

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.

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.


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