Title: Types Of Chemical reactions



NAME: _____________________________________ Date: ________________

Partners: ___________________________________________________________________

TYPES OF CHEMICAL REACTIONS

Background Information:

There are many different types of chemical reactions that can occur between atoms. There are several ways to classify these reactions. In this lab we will classify reactions into 4 major types. These are: synthesis, decomposition, single replacement and double replacement. Not ALL reactions can be placed in these categories, but many of the reactions we will use in regents chemistry can.

Purpose: Observe and classify the 4 major types of chemical reactions and identify the reactants and products.

|CAUTION: |

|Goggles required. Signed:____________________ |

|Tie back long hair. Dated:_____________________ |

|Do not look directly into the flame of the burning magnesium ribbon. |

|Point the open end of a test tube away from people. |

|Put out all burning splints with some water. |

|Do not leave splints or any other solid in the sink. Throw them in the garbage. |

|Clean up any spills. |

Pre-lab. Questions:

1. Explain why the terms synthesis and decomposition are appropriate names for their respective reaction types.

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2. In a single replacement reaction, why do metals replace metals and nonmetals replace nonmetals?

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3. Iron III chloride is a chemical compound used in photography. It can be produced by reacting iron and chlorine.

a. Write out the un balanced chemical equation for the above reaction:

____________________________________________________________

b. Identify the type of reaction: _____________________

4. Aqueous Copper II sulfate reacts with aqueous ammonium sulfide to produce a precipitate, copper II sulfide and aqueous ammonium sulfate.

a. Define the term precipitate.

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b. Write out the un balanced chemical equation for the above reaction:

______________________________________________________________

c. Identify the type of reaction: _____________________

Procedure:

Part A

1. Examine a piece of magnesium ribbon. Place an evaporating dish close to the Bunsen burner.

2. Using the crucible tongs, hold the Magnesium ribbon in the hottest part of the Bunsen burner flame until the magnesium starts to burn and place the burning magnesium into the evaporating dish. DO NOT LOOK DIRECTLY INTO THE FLAME OF THE BURNING MAGNESIUM. Examine the ribbon and note any changes in appearance caused by heating.

Part B

1. Place 2 heaping microspatula of copper (II) carbonate in a clean dry test tube. Note the appearance of the sample in your data page.

2. Using a test tube holder, gently heat the sample in the test tube for 3 – 4 minutes. Insert a burning wood splint into the test tube. Note and record what happens to the flame in your data table. Note all changes to the substance in the test tube on your data table.

Part C

1. Add about 5 ml of .1 M copper (II) chloride solutions to a clean, dry test tube.

2. Place a small amount of aluminum foil into the solution.

3. Note the appearance of the solutions before and after the reaction and record all information in your data table.

Part D

1. Add about 15 drops of Na2CO3(aq) to a clean , dry test tube.

2. Add about 10-15 drops of BaCl2(aq) to a the same test tube.

Note the appearance of the solution before and after the reaction and record all information in your data table.

Data Table: (In the space below each equation, name each reactant and each product)

Observations and Chemical Equations on the Different Types of Reactions

| | |

|Part A | |

| | |

| |Mg(s) + O2(g) → MgO(s) |

| |__________ ___________ ____________ |

| | |

|Part B | |

| | |

| |CuCO3(s) → CO2↑ + CuO(s) |

| |_____________ ____________ __________________ |

| | |

|Part C | |

| | |

| |Al(s) + CuCl2(aq) → AlCl3(aq) + Cu(s) |

| |__________ _____________ _____________ __________ |

| | |

|Part D | |

| | |

| |Na2CO3(aq) + BaCl2(aq) → NaCl(aq) + BaCO3(s) |

| |______________ ___________ ___________ _____________ |

Questions:

Complete the following table:

|Experiment |Type of Reaction |Predict the products and write out the formula equation for the following chemical |

| | |reactions. |

| | | |

|Part A | |Potassium reacts with chlorine gas |

| | |Formula Equation: |

| | |______________________________________________ |

| | | |

|Part B | |The breakdown of calcium bromide into its elements |

| | |Formula Equation: |

| | |________________________________________________ |

| | | |

|Part C | |Aqueous potassium iodide reacts with gaseous nitrogen |

| | |Formula Equation: |

| | |_________________________________________________ |

| | | |

|Part D | |Aqueous silver nitrate reacts with aqueous potassium sulfate. |

| | |Formula Equation: |

| | |_________________________________________________ |

| | |According to Table F-Solubility Guidelines for Aqueous Solutions, all nitrate compounds are|

| | |soluble in water. In general, sulfate compounds are soluble except when combined with Ag+, |

| | |Ca+2, Sr+2, Ba+2, or Pb+2 |

| | |Which product would be insoluble in water and is classified as n example of a precipitate? |

| | |_________________ |

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