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What is a chemical reaction?. When reactants are converted to products, bonds holding the atoms together are broken and new bonds are formed. Reactants Products Recall that atoms themselves are neither created nor destroyed; they are merely rearranged.

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What is a chemical reaction
What is a chemical reaction?

When reactants are converted to products, bonds holding the atoms together are broken and new bonds are formed.

Reactants Products

Recall that atoms themselves are neither created nor destroyed; they are merely rearranged.


What is a word equation
What is a word equation?

Chemical reactions can be described using words.

Either “Iron reacts with oxygen to produce iron (III) oxide (rust)”

Or Iron + Oxygen iron (III) oxide


How do we represent chemical equations
How do we represent chemical equations?

Easier to use chemical shorthand to represent chemical relationships

Reactants on the left of the arrow and products to the right of the arrow

Fe (s) + O2(g) Fe2O3(s)

Where (s)= solid

(l) = liquid

(g) = gas

(aq)= aqueous solution (dissolved in water)

Heat or catalyst added to a reaction would appear above the arrow. See Table 8.1


Balancing chemical equations
Balancing Chemical Equations

H2(g) + O2 (g) H2O(l)

Recall that matter is neither created or destroyed, so what is wrong with this picture?

It’s not balanced, we lost an oxygen, this is not possible so we balance the equation with coefficients, whole numbers that are placed in front representing the relative quantities of each compound.

2 H2(g) + O2 (g) 2 H2O(l)

Now both sides are equal.


Rules for balancing equations
Rules for Balancing Equations

  • Determine the correct formulas for all reactants and products in the reaction. Use parentheses when necessary.

  • Count the number of atoms of each element in the reactants and products.

    • For simplicity, a polyatomic ion appearing unchanged on both sides can be counted as a single unit.

  • Balance the elements one at a time using coefficients.

    • if no coefficient is written, it is assumed to be one.

    • You cannot change the subscripts to balance the equation.

  • Check each atom or polyatomic ion to make sure it is balanced.

  • Finally make sure all the coefficients are in lowest possible ratios.





Plan of the day
Plan of the Day

POD—for extra credit

Questions on lab? Homework?

Types of Reactions Powerpoint


Plan of the day1
Plan of the day

  • Major Reaction Types

  • Get into a 5 groups

  • Make a quick poster (big, bold, letters)

  • These will be your notes for Reaction Types

  • On your poster:

    • Define your reaction

    • Show an example

    • How can you tell a reaction is your type of reaction

    • Show the skeleton reaction!


Plan of the day2
Plan of the day

  • Finish your notes in the lab while I get set up.

  • Finish demos

  • Work on our learning goal:

    • Be able to identify types of reactions!

    • Finish Worksheet from yesterday

  • Please Bring in your Textbooks--Tomorrow!


Plan of the day3
Plan of the day

  • Business

    • Test corrections, retakes.

    • Lab tomorrow—wear appropriate clothing!

  • Thus far in the Reaction Unit?

    • Balancing Equations√

    • Identifying the 5 types of reactions √

  • What is left?

    • Predicting Products

    • Using solubility rules to predict double replacement reactions

    • Net-Ionic Equations


Combination reactions
Combination Reactions

Two or more substances combine to form a single substance, or…

Two or more products combine to form a single product.

Example:

Mg(s) + O2 (g) MgO(s)


Predicting combination reactions
Predicting Combination Reactions

4 Possibilities:

Metal + Non-Metal -- Ionic Compound

K + Cl2  KCl

Non-metal + Non-Metal  (more than one product possible)

S + O2  SO2 or SO3

Non-metal oxide + H2O  acid

SO2 + H2O  H2SO4

Metallic oxide + H2O  metal hydroxide

CaO + H2O  Ca (OH)2


Decomposition reactions
Decomposition Reactions

A decomposition reactionis one in which a single compound breaks down into two or more elements or new compounds.

Decomposition reactions often require an energy source, such as heat, light, or electricity, to occur.

Hard to predict! usually a gas or element!

Example: heat

CaCO3(s) CaO(s) + CO2(g)


Combustion reactions
Combustion Reactions

In a combustion reaction, oxygen combines with a substance and releases energy in the form of heat and light.

Heated hydrogen reacts with oxygen to produce heat and water in a combustion reaction. This is also a combination reaction.


Predicting combustion
Predicting Combustion

Element + Oxygen  oxides

Mg + O2  MgO

Hydrocarbons (or alcohols) + Oxygen  CO2 + H2O

CH4 + O2  CO2 + H2O


Single replacement reactions
Single Replacement Reactions

  • A reaction in which the atoms of one element replace the atoms of another element in a compound is called a single replacement reaction.

    A + BX → AX + B

    Cu + AgNO3  Ag + CuNO3


Single replacement reactions1
Single Replacement Reactions

Predicting Products —

if the activity of the metal is higher than the metal cation in solution there will be a reaction, otherwise there is not a reaction.

What is happening?

The more reactive metal will form a compound with the anion, and the other metal will be pulled out of solution and become a solid metal again.

Ex)

Mg (s) + Zn(NO3)2 (aq) Mg(NO3)2 (aq)+ Zn(s)


Reactivity s
Reactivity's

A metal will not always replace a metal in a compound dissolved in water because of differing reactivity's.

An activity series can be used to predict if reactions will occur.


Double replacement
Double Replacement

Double replacement reactionsoccur when ions exchange between two compounds. A precipitate, gas, or molecule will form.

This figure shows a generic double replacement equation.


Predicting double replacement
Predicting Double Replacement

The solid product produced during a chemical reaction in a solution is called a precipitate.

All double replacement reactions produce either water, a precipitate, or a gas.


Double replacements continued
Double Replacements Continued

This table shows the steps to write double replacement reactions.


Summary of reactions
Summary of Reactions

This table summarizes different ways to predict the products of a chemical reaction.


Pop quiz
Pop Quiz

1)Ca(OH)2 + Al2(SO4)3CaSO4 + Al(OH)3

2)Mg + Fe2O3Fe + MgO

3)C2H4+ O2CO2+ H2O

4)PbSO4PbSO3 + O2


Solutions

Solutions

Net Ionic Equations


Plan of the day4
Plan of the day

Finals

Revisit course expectations

Check your grades to make sure they are accurate.

Homework for Chapter 8: 33-53 (odd) due Friday!


What is a solution
What is a solution?

An aqueous solutioncontains one or more dissolved substances (called solutes) in water.

The solvent is the most plentiful substance in a solution.


Aqueous solutions
Aqueous Solutions

Water is always the solvent in an aqueous solution.

There are many possible solutes—sugar and alcohol are molecular compounds that exist as molecules in aqueous solutions.

Compounds that produce hydrogen ions in aqueous solutions are acids.


Ionic compounds in solution
Ionic Compounds in Solution

Ionic compounds can also be solutes in aqueous solutions.

When ionic compounds dissolve in water, their ions separate in a process called dissociation.


Aqueous reactions continued
Aqueous Reactions Continued

When two solutions that contain ions as solutes are combined, the ions might react.

If they react, it is always a double replacement reaction.

Three products can form: precipitates, water, or gases.


Complete ionic equations
Complete Ionic Equations

  • Aqueous solutions of sodium hydroxide and copper(II) chloride react to form the precipitate copper(II) hydroxide.

    2NaOH(aq) + CuCl2(aq) → 2NaCl(aq) + Cu(OH)2(s)

  • Ionic equations that show all of the particles in a solution as they actually exist are called complete ionic equations.

    2Na+(aq) + 2OH–(aq) + Cu2+ (aq)+ 2Cl–(aq) → 2Na+(aq) + 2Cl–(aq) + Cu(OH)2(s)


What is a chemical reaction

Ions that do not participate in a reaction are called spectator ionsand are not usually written in ionic equations.

  • Formulas that include only the particles that participate in reactions are called net ionic equations.

    2OH–(aq) + Cu2+(aq) → Cu(OH)2(s)


Predicting precipitates
Predicting Precipitates

Using solubility rules for ionic equations we can predict whether a precipitate is formed and thus predicting what the products are.

If the solubility rules predict insolubility we have a reaction, a precipitate!

Example:

Na2SO4 (aq) + BaNO3 (s) ???

Assume double replacement

Look at the products

Any insoluble?


Example1
Example

NaSO4 + BaNO3 ???

Assume double replacement

Look at the products

Any insoluble?

Na2SO4 + Ba(NO3)2 2NaNO3 + Ba(SO4)

Write the complete ionic equation:

2Na+(aq) + SO42- (aq) + Ba2+ (aq) + 2NO3-(aq) 2Na+(aq) + 2NO3-(aq) + Ba(SO4)(s)

Eliminate all of the ions that did not change from the reactant side to the product side.

Ba2+ (aq) + SO42- (aq) Ba(SO4)(s) (net ionic eqn)


Plan of the day5
Plan of the day

Problems of the day

Questions on homework.

Lab Write Up.


Plan of the day6
Plan of the day

Lab write up!

Examples?