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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 Reactions. Word Equations. 11.1 Describing Chemical Reactions.

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Chemical Reactions

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  1. Chemical Reactions Chapter 11

  2. 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

  3. 11.1 Describing Chemical Reactions • Word Equations

  4. 11.1 Describing Chemical Reactions • Word Equations Reactants → Products

  5. 11.1 Describing Chemical Reactions • Word Equations Reactants → Products iron + oxygen → iron(III) oxide

  6. Symbols Used in Chemical Reactions + → ↔ (s) (l) (g) (aq) Heat ∆ Pt

  7. 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

  8. Chemical Equations Reactants → Products iron + oxygen → iron(III) oxide Fe + O2 → Fe2O3

  9. →

  10. Chemical Equations Reactants → Products iron + oxygen → iron(III) oxide Fe + O2 → Fe2O3 4Fe(s) + 3O2(g) → 2Fe2O3 (s)

  11. Magnesium + Oxygen → Magnesium oxide

  12. Magnesium + Oxygen → Magnesium oxide Mg + O2 → MgO

  13. Magnesium + Oxygen → Magnesium oxide Mg + O2 → MgO 2Mg + O2 → 2MgO

  14. 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

  15. Do Now - Write the ionic or molecular formula for Lithium Oxide Li2O Aluminum Sulfide Al2S3 Silicon Oxide SiO2

  16. Balancing Chemical Equations 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

  17. 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.

  18. 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.

  19. Iron + oxygen → iron 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.

  20. Iron + oxygen → iron 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.

  21. Iron + oxygen → iron 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.

  22. Iron + oxygen → iron 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.

  23. Iron + oxygen → iron 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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