name: unit 7- chemical equations _____ unit 7- chemical equations ... 1 5 – 6 balancing ... reacts...

Unit 7: Chemical Equations

Name: _________________________________

Unit 7- Chemical Equations Day Page # Description IC/HW Due Date Completed

ALL 2 Warm-up IC

1 3 – 4 Balancing Equations Notes IC

1 5 – 6 Balancing Chemical Equations

Worksheet HW

1

Chemical Reactions Pre-Lab HW

2

Types of Chemical Reactions Lab IC

3 7 – 8 Type of Chemical Reaction Notes IC

3 9 – 10 Types of Chemical Reactions HW

4 11 Rules for Predicting Products of

Chemical Reactions IC

4 12 – 14 Predicting Products HW

5 15 Unit 7 Test Review HW

5 X Unit 7 Test In Class January 26th and 27th


Warm-up Day 2

1. Which side of the arrow is the product? Which side is the reactant? Day 3 Write the balanced equation for the following:

1. Aluminum metal is oxidized by oxygen (from the air) to form aluminum oxide.

2. Sodium oxide reacts with carbon dioxide to form sodium carbonate.

3. Calcium metal reacts with water to form calcium hydroxide and hydrogen gas.

Day 4 Look at your balanced equations from Day 3. Determine the type of reaction for each equation.

1.

2.

3.

Day 5 Predict the product and write the balanced equation.

1. A solution of nitric acid is poured on solid calcium carbonate.

2. Rubbing alcohol, (CH3)2CHOH, is burned completely in air.


Balancing Equations Notes When writing a chemical equation the phase of matter must also be indicated.

Symbol Meaning

Separates two or more reactants or products

Separates reactants from products

(s) Identifies a solid state

(l) Identifies a ___________ state (pure liquid)

(g) Identifies a ___________ state

(aq) Identifies a _____________

Chemical equations represent a chemical ________________. You ___________ with reactants and

___________ with products. Reactants ⟶ Products

When we write chemical equations, we need to make sure the number of___________ is the same on both sides of the _____________. It is just like a math problem. Think about the formation of water:

H2(g) + O2(g)⟶ H2O(l) Reactant Side Product Side

2H + 2O 2H + 1O

Steps to balance: 1. Since there are 2 oxygens on the reactant side, but only one on the product side, another

oxygen must be added to the product side. You can only __________________, and you can NEVER change the subscript because that would change the ____________ of the compound.

2. 2 waters (H2O) are needed, but now we have 4 hydrogens on the product side, so we also need to multiply H2 by 2.

2H2(g) + O2(g) → 2H2O(l) Reactant Side Product Side

4H + 2O 4H + 2O

Examples: ___ HCl(aq) + ___ Zn(s) →___ ZnCl2(aq) + ___ H2(g)

Reactant Side Product Side

___H + __Cl + __Zn __H + __Cl + __Zn

___ Al(s) + ___ CaS (aq)→ ___ Al2S3(s)+ ___ Ca(aq) Reactant Side Product Side

1Al + 1Ca + 1S 2Al + 3S + 1Ca

Always save monatomic elements (Al, Ca, etc) for last.


Write balanced chemical equations below by writing out the skeleton equation and changing the coefficients to make the number of each element equal on both sides of the equation. Note: Br, I, N, Cl, H, O, and F are always diatomic when they are in their elemental form

1. Solid iron and gaseous chlorine react to produce a solid iron (III) chloride

2. Calcium metal reacts with water to form solid calcium hydroxide and hydrogen gas.

3. Zinc hydroxide solution reacts with lithium to form lithium hydroxide solution and zinc metal.

4. Liquid propanol (C3H7OH) reacts with oxygen gas to form carbon dioxide gas and water vapor.

5. Aluminum metal reacts with oxygen gas to form solid aluminum oxide.

6. Lead (II) nitrate solution reacts with iron (III) chloride solution to form solid lead (II) chloride and Iron (III) nitrate solution.

7. Aluminum metal reacts with silver sulfate solution to form aluminum sulfate solution and silver metal.

8. Methane gas (CH4) reacts with oxygen gas to form carbon dioxide gas and water vapor.

9. Iron metal reacts with bromine gas to form iron (III) bromide solid.

10. Hydrogen peroxide (H2O2) solution decomposes into water and oxygen gas.


Balancing Chemical Equations Worksheet Balance the following chemical equations using coefficients

1. Al(OH)3(s) + HCl (aq) AlCl3 (aq) + H2O (l)

2. Fe2O3 (s) + CO (g) Fe3O4(s) + CO2 (g)

3. FeO (s) + O2 (g) Fe2O3 (s)

4. C6H6 (l) + O2 (g) CO2 (g) + H2O (g)

5. Ca(OH)2 (aq) + H3PO4 (aq) H2O (l) + Ca3(PO4)2 (s)

6. I4O9 (s) I2O6(s) + I2 (s) + O2 (g)

7. Eu (s) + HF (g) EuF3 (s) + H2 (g)

8. NaHCO3 (aq) + C6H8O7 (aq) CO2 (g) + H2O (l) + Na3C6H5O7 (aq)

9. Ni (s) + CO (g) Ni(CO)4 (g)

10. K2PtCl4 (aq) + NH3 (aq) Pt(NH3)2Cl2 (s) + KCl (aq)

Write the following chemical equations and balance using coefficients. 1. Liquid mercury reacts with liquid bromine to produce solid mercury (II) bromide

2. Solid calcium carbonate decomposes upon heating to produce solid calcium oxide and carbon dioxide gas.


3. Solid calcium will react with liquid water to produce aqueous calcium hydroxide and hydrogen gas. 4. Butane gas (C4H10) will react with oxygen gas to produce carbon dioxide gas and water vapor. 5. Solid aluminum will react with oxygen gas to produce solid aluminum oxide. 6. Aluminum metal is oxidized by oxygen (from the air) to form aluminum oxide. 7. Sodium oxide reacts with carbon dioxide to form sodium carbonate. 8. Calcium metal reacts with water to form calcium hydroxide and hydrogen gas. 9. Potassium nitrate decomposes to form potassium nitrite and oxygen. 10. Barium metal reacts with Iron (III) sulfate to produce barium sulfate and iron metal.


Types of Chemical Reactions Notes

Synthesis- two or more __________ or ____________ combine to form one compound.

o Usually releases energy, ______________

o

4 Fe (s) + 3 O2 (g) → 2 Fe2O3 (s)

CaO (s) + H2O (l) → Ca(OH)2 (s)

Decomposition- a single compound _______________ into two or more elements or smaller compounds.

o Often requires an energy source as an _____________. Energy sources can be heat,

light, or electricity. Usually ____________

o

2 NaN3(s) → 2 Na(s) + 3 N2 (g)

2 KClO3 (s) → 2 KCl (s) + 3O2 (g)

CaCO3 (s) → CaO (s) + CO2 (g)

Single Replacement- a ____________ will replace a less active metal in an __________ compound OR a nonmetal will replace a less active nonmetal.

Ca (s) + NaCO3(aq) CaCO3 (s) + NaCO3 (aq)

Double Replacement- the metals in ionic compounds ____________ places.

AgNO3(aq) + NaCl (aq) AgCl(s) + NaNO3(aq)

Combustion- an organic compound containing ___________, ____________ and sometimes oxygen reacts with oxygen gas to form ____________ and ____________.

o Usually _______________ o

C(s) + O2(g) → CO2(g) + energy

4 Fe (s) + 3O2 (g) → 2Fe2O3 (s) + energy


Types of Chemical Reactions Directions

(a) Write and balance the given equation. (b) Indicate the type of chemical reaction represented.

1. Iron reacts with oxygen gas to produce Iron (III) oxide.

(a)

(b)

2. Propane (C3H8) reacts with oxygen gas to produce carbon dioxide and water.

(a)

(b)

3. Bromine gas reacts with potassium iodide to produce potassium bromide and iodine gas.

(a)

(b)

4. Hydrogen peroxide will produce water and oxygen gas if left in sunlight.

(a)

(b)

5. Phosphorous reacts with oxygen gas to produce tetraphosphorous decoxide.

(a)

(b)

6. Iron (III) Chloride reacts with sodium hydroxide to produce Iron (III) hydroxide and sodium chloride.

(a)

(b)

7. Iron (III) oxide reacts with hydrogen gas to produce iron and water.

(a)

(b)


8. Octane (C8H18) reacts with oxygen gas to produce carbon dioxide and water.

(a)

(b)

9. Calcium carbonate reacts with aluminum phosphate to produce calcium phosphate and aluminum carbonate.

(a)

(b)

10. Aluminum hydroxide decomposes to produce aluminum oxide and water.

(a)

(b)

11. Lead (IV) oxide decomposes into lead (II) oxide and oxygen gas.

(a)

(b)

12. Zinc reacts with silver nitrate.

(a)

(b)

13. Potassium oxide reacts with water to produce potassium hydroxide.

(a)

(b)

14. Glucose (C6H12O6) reacts with oxygen gas.

(a)

(b)

15. Hydrochloric acid (hydrogen chloride) reacts with barium hydroxide.

(a)

(b)


Rules for Predicting Products of Chemical Reactions 1. Hydrocarbon + O2 CO2 + H2O

a. 2C4H10 + 13 O2 8 CO2 + 10 H2O

2. Metal Carbonate Metal Oxide + CO2

a. MgCO3 MgO + CO2

b. Synthesis: Metal Oxide + CO2 Metal Carbonate

3. Metal Sulfites Metal Oxide + SO2

a. CaSO3 CaO + SO2

b. Synthesis: Metal Oxide + SO2 Metal Sulfite

4. Metal Hydride + H2O Metal Hydroxide + H2

a. KH + H2O KOH + H2

5. Metal + H2O Metal Hydroxide + H2

a. 2Na + 2H2O 2NaOH + H2

6. Metal Oxide + H2O Metal Hydroxide

a. MgO + H2O Mg(OH)2

7. Non-metal oxide + H2O ternary acid

a. N2O3 + H2O 2 HNO2

b. N2O5 + H2O 2 HNO3

c. CO2 + H2O H2CO3


Predicting Products: Write the COMPLETE balanced equation 1. Hydrochloric acid (HCl) reacts with sodium hydroxide.

2. Sodium reacts with oxygen

3. Mercury (II) oxide

4. Zinc reacts with lead (II) Nitrate

5. Silver nitrate reacts with calcium chloride

6. C7H16 reacts with oxygen

7. CH3OH reacts with oxygen

8. Magnesium reacts with Fluorine

9. Copper (II) Chloride

10. Aluminum reacts with Calcium Sulfide

11. Potassium Hydroxide reacts with Zinc Chloride



13. Sodium Iodide reacts with chlorine

14. Aluminum reacts with sulfur

15. Aluminum Oxide

16. Sodium reacts with water

17. Iron (II) Sulfide reacts with hydrochloric acid

18. C3H8O reacts with oxygen

19. Lithium reacts with nitrogen

20. Calcium reacts with phosphorous

21. Fluorine reacts with sodium chloride

22. Copper (II) Chloride reacts with sodium phosphate


24. Calcium reacts with HCl

25. Lithium Hydroxide reacts with Iron (III) Nitrate


Unit 7 Quiz Review Balance the following equations: _____ HCl + _____ Al _____ AlCl3 + _____ H2 _____ HNO3 + _____ Zn _____ Zn(NO3)2 + _____ NO2 + _____ H2O _____ HNO3 + _____ Sn _____SnO2 + _____ NO2 + _____ H2O Write the balanced equation for the following chemical reaction AND the type of reaction that has occurred. Sodium metal is added to sulfuric acid (H2SO4). Hydrogen gas is produced, along with sodium sulfate. White phosphorus (P4) reacts with chlorine to make phosphorus trichloride. Magnesium chlorate, is heated strongly until it decomposes into magnesium chloride and oxygen gas. Write the balanced equation for the following chemical reaction (you must predict the product) AND the type of reaction that has occurred. Butane gas (C4H10) is burned completely in air. Iron metal is added to bromine- Iron (III) product. Calcium metal is added to phosphoric acid (H3PO4). Aluminum metal is added to a solution of iron (III) chloride. A piece of iron metal is exposed to oxygen gas (Fe3+ product would form). Calcium metal is added to water.


Predicting Products: Write the COMPLETE balanced equation

1. Potassium metal reacts with chlorine gas.

2. Iron (III) Sulfate reacts with barium chloride. 3. Lithium metal reacts with water

4. Copper metal reacts with iron (II) nitrate 5. Sucrose (C5H10O5) reacts with oxygen. 6. Solid calcium carbonate reacts with acetic acid


Extra Practice : Predicting Products: Write the COMPLETE balanced equation

1. Chlorine gas reacts with aluminum metal.

2. C6H6 reacts with oxygen.

3. Ammonium chloride reacts with potassium nitrate

4. Zinc reacts with sulfuric acid

5. Iron (III) chloride

6. Potassium metal reacts with water.

7. Lithium sulfite reacts with nitric acid

8. Copper reacts with hydrochloric acid (Copper (II) product)

9. Aluminum reacts with bromine gas.

name: unit 7- chemical equations _____ unit 7- chemical equations ... 1 5 – 6 balancing ... reacts...

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