chapter 9 chemical reactions. 9.1: reactions & equations objectives recognize evidence of...

Chapter 9

Chemical Reactions

9.1: Reactions & Equations

Objectives

• Recognize evidence of chemical change

• Represent chemical reactions with equations

• Balance chemical equations

What is a chemical reaction?

• It is the process by which the atoms of one or more substances are rearranged to form new, different substances.

• A chemical reaction is a chemical change!

The 4 signs

There are 4 kinds of observations that indicate a chemical reaction may have taken place.

1.A change in energy: A temperature change is often used to determine if energy was released or absorbed. In addition, release of light also indicates an energy change.

The 4 signs

• 2. A color change

The 4 signs3. Production of a gas may be observed as bubbling or visible fumes. Detection of an odor also indicates a gas was produced.

The 4 signs

4. Formation of a precipitate (or appearance of a solid) in a solution that was previously clear.

Practice

• Recall burning magnesium as part of a lab activity. What evidence was there that a chemical reaction occurred?

Review• Equations represent chemical reactions.

• Reactants (on the left) are the starting substances.

• Products (on the right) are the substances formed during the reaction.

Review

• An arrow shows the way the reaction progresses; It is found between the reactants and products and is usually read as “yields”.

• “+” signs are placed between each reactant and product; They are read as “and”.

Review

• Symbols are often used after each reactant and product to indicate their state.– (s) for solid - (g) for gas – (l) for liquid - (aq) for water solution

Review• Coefficients are whole

numbers written in front of formulas in the equation. They indicate the number of atoms, molecules, or ions of that substance that are involved in the reaction.

Practice

• Identify the reactants and products and, using words not formulas, interpret the following equations.

Mg (s) + H2SO4 (aq) H2 (g) + MgSO4 (aq)

C(s) + 2ZnO (s) 2Zn (s) + CO2 (g)

Types of Equations

• Word Equation: words are used to summarize the reaction.– Ex.: iron + chlorine iron (III) chloride– Ex.: carbon + sulfur carbon disulfide

• Skeleton equation: Chemical formulas are substituted for words.– Ex.: Fe + Cl2 FeCl3

– Ex.: C + S CS2

Skeleton Equations

• Skeleton equations are also called unbalanced equations because they do not obey the Law of Conservation of Mass.– Fe + Cl2 FeCl3

+

1 iron atom 2 chlorine atoms

1 iron atom

3 chlorine atoms

Practice Problems• Write skeleton equations for the following:

1 - hydrogen + bromine hydrogen bromide2 - carbon monoxide + oxygen carbon dioxide 3 - potassium chlorate potassium chloride +

oxygen

4 – Manganese metal reacts with sulfuric acid to produce manganese (II) sulfate and hydrogen gas.

5 – Silver nitride is produced when silver reacts with atmospheric nitrogen.

Types of Equations

• Balanced chemical equation: This equation shows that the number of atoms of each reactant and each product is equal on both sides of the arrow.– 2Fe + 3Cl2 2FeCl3

+ 2 iron atoms

2 iron atoms 6 chlorine atoms 6 chlorine atoms

Balanced Chemical Equation

• This is defined as a statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a reaction.

• Balanced chemical equations obey the Law of Conservation of Mass.

Steps to Balancing Equations1 - Write a skeleton equation.

Problem: Hydrogen and chlorine combine

to form hydrogen chloride

H2 + Cl2 HCl

*Recall there are 7 elements that

exist as diatomic molecules.

Steps to Balancing Equations

2 - Determine the number and kinds of atoms in the reactants.

3 - Determine the number and kinds of atoms in the products.

H2 + Cl2 HCl

2 H 1 H

2 Cl 1 Cl

Steps to Balancing Equations

4 - Change the coefficients (never the subscripts) until the number of atoms of each element is equal on both sides of the equation.

H2 + Cl2 2HCl

2 H 2 1 H

2 Cl 2 1 Cl

Steps to Balancing Equations5 - Make sure the coefficients are in the lowest

possible ratio. Reduce if necessary.

6 - Go back and add the atoms up again. Make sure the number of atoms of each element is equal on both sides of the arrow.

If you cannot balance the equation, go back and make sure your formulas are written

correctly!!

Practice Problems1 - Sodium hydroxide and calcium bromide react

to produce solid calcium hydroxide and sodium bromide.

2 - Carbon disulfide reacts with oxygen gas to produce carbon dioxide and sulfur dioxide.

3 - Zinc and sulfuric acid react to produce hydrogen gas and zinc sulfate.

4 - Iron (III) chloride reacts with sodium hydroxide to produce iron (III) hydroxide and sodium chloride.