classifying chemical reactions chemistry. classifying chemical reactions essential questions 1. is...
TRANSCRIPT
Classifying Chemical Reactions
Chemistry
Classifying Chemical reactions
Essential Questions
1. Is there a way to organize chemical reactions to make them easier to understand?
2. And maybe easier to balance?
Types of Reactions
We classify reactions to make predicting the products easier
Each type of reaction follows a certain pattern which make balancing easier:)
But…The 5 reactions we talk about are not the only types
And …each reaction does not have to fit into just one type Maybe more than one maybe none
5 types of reactions
1) Synthesis
2) Decomposition
3) Single Replacement
4) Double Replacement
5) Combustion
Video: http://www.youtube.com/watch?v=i-HHvx1VC_8 (1:29 min)
(1) Synthesis Reactions
Synthesis means “to put together”
A + B AB
Two or more reactants react to form
one product
Examples: CaO (s) + H2O (l) Ca(OH)2 (s)
2SO2(g) + O2 (g) 2SO3 (g)
Example of Synthesis
Let’s practice synthesis
Predict the products. Write and balance the following synthesis reaction equations.
• Sodium metal reacts with chlorine gas
Na(s) + Cl2(g) • Solid Magnesium reacts with fluorine gas
Mg(s) + F2(g) • Aluminum metal reacts with fluorine gas
Al(s) + F2(g)
(2) Decomposition Reactions
Opposite of synthesis reactions
A single compound breaks down into two or more elements or simpler compounds
AB A + B
Often need an input of energy (such as heat, light, or electricity) to make the reaction happen
Decomposition Reactions
Example: Car air bags
Sodium azide pellets
decompose to produce
sodium and nitrogen gas
hat inflates the airbag!
2NaN3(s) 2Na(s) + 3N2(g)
Let’s practice decomposition
Predict the products. Then, write and balance the following decomposition reaction equations:
• Solid Lead (IV) oxide decomposes PbO2(s)
• Aluminum nitride decomposes
AlN(s)
Replacement Reactions
Aka displacement reactions
Two types:
Single replacement and Double replacement
(3) Single Replacement
A single element reacts with a compound and displaces another less reactive element from the compound
Like they switch places Example:
Mg + Zn(NO3)2 --> Mg(NO3)2 + Zn
Single replacement reaction
For example:
Zinc metal reacts with aqueous hydrochloric acid
Zn(s) + HCl(aq) ZnCl2 + H2(g)
Zinc replaces the hydrogen ion in the reaction
Single replacement
• A metal can replace hydrogen or another metal (+) OR a nonmetal can replace a nonmetal (-).
Single Replacement
Do single replacement reactions always occur?
NO! A metal will only replace a less reactive metal.
The activity series is a way to predict whether or not certain reactions will occur.
Any specific metal can replace any metal listed below it that is in a compound.
It cannot replace any metal listed above it!
What is the Activity Series?
Activity series a series of elements that have similar properties and that are arranged in descending order of chemical activity
(meaning most reactive at the top) Elements can only “switch” places with
elements below it on the activity series
Activity Series for Metals
Activity series for Halogens
Do single replacement reactions only occur for metals?
No – non metals or halogens can also replace less reactive halogens in single replacement reactions.
Activity Series for Halogens
Each replaces halogens listed below it.
For example, fluorine will replace chlorine, chlorine will replace bromine, etc.
Step for doing single replacement reactions
1) Identify the reactantsDetermine if element is metal or halogenDetermine the element that might be displaced from
compound
2) Check the activity seriesDetermine which element is more active
3) Write the products and balance the equationIf the more active element is already part of the compound
then NO reaction will happen
4) Check your workMake sure the equation is balanced (just like always)
Check for Understanding
Will the following react?
If yes, write the balanced equation.
If no, write NR for no reaction!
1. Cu + ZnSO4 (compare copper and zinc)
2. Fe + CuNO3 (compare iron and copper)
(iron takes +2 charge)
1. Al + Fe2O3 (compare aluminum and iron)
Check for Understanding
Will the following react?
If yes, write the balanced equation.
If no, write no reaction!
1. Cu + ZnSO4 no reaction
2. Fe + 2CuNO3 Fe(NO3)2 + 2Cu
3. 2Al + Fe2O3 Al2O3 + 2Fe
STOP!
Work on identifying and writing the first three types of reactions on the next worksheet both sides.
(4) Double- replacement Reactions
When a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound
A reaction in which a gas, a solid precipitate, or a molecular compound forms from the apparent exchange of atoms or ions between two compounds
Happens in aqueous solutions Must end up with a solid precipitate, gas, or
molecular compound (like water)
Double replacement
Double Replacement
• Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together
• AgNO3(aq) + NaCl(s) AgCl(s) + NaNO3(aq)
Special DD – Acid/Base Reaction
Type of double displacement reaction that takes place when an acid and base react with each other.
The H+ ion in the acid reacts with the OH- ion in the base, causing the formation of water.
Product of this reaction is typically an ionic salt and water:
HA + BOH ---> H2O + BA
Special DD – Acid/Base Reaction
• In double- displacement reactions water, as a product, is often written as HOH so you can more easily see the exchange of atoms/compounds
HCl(aq) + NaOH(aq) -> HOH(l) + NaCl(aq)
• This is a double replacement reaction • The H and the Na changed partners• You formed water (that’s one of the signs!!)
Practice double replacement
1. HCl(aq) + AgNO3(aq) (hint: silver takes a +1 charge)
2. CaCl2(aq) + Na3PO4(aq) (hint: You can tell that phosphate takes a -3 charge)
3. Pb(NO3)2(aq) + BaCl2(aq) (hint: You can tell that lead takes a +2 charge)
4. HBr + NaOH
(5) Combustion Reactions
Combustion reactionReaction of a hydrocarbon with oxygenAKA “burning!”Products are carbon dioxide and water vaporReleases energy in the form of heat & light
Ex: the lighting in here is because of the combustion of coal
Do you have any others?
Hydrocarbons
Just a fancy way to say the compound only has hydrogen and carbon in it
Let’s try some:
___C3H8 + ___O2 ___CO2 + ___H2O
___C5H12 + ___O2
___ C10H22 + ___ O2
How to identify the type of reaction!
Follow this series of questions. When you can answer "yes" to a question, then stop!
1) Does your reaction have oxygen as one of its reactants and carbon dioxide and water as products? If yes, then it's a combustion reaction
2) Does your reaction have two (or more) chemicals combining to form one chemical? If yes, then it's a synthesis reaction
3) Does your reaction have one large molecule falling apart to make several small ones? If yes, then it's a decomposition reaction
4) Does your reaction have any molecules that contain only one element? If yes, then it's a single displacement reaction
5) If you haven't answered "yes" to any of the questions above, then you've got a double displacement reaction
Check for understanding
List what type the following reactions are:
1) NaOH + KNO3 --> NaNO3 + KOH
2) CH4 + 2 O2 --> CO2 + 2 H2O
3) 2 Fe + 6 NaBr --> 2 FeBr3 + 6 Na
4) CaSO4 + Mg(OH)2 --> Ca(OH)2 + MgSO4
5) Pb + O2 --> PbO2
6) Na2CO3 --> Na2O + CO2
1) double displacement
2) combustion
3) single displacement
4) double displacement
5) synthesis
6) decomposition
Pharaoh's Snakes
Now for something fun
Check this out…
http://www.youtube.com/watch?v=ritaljhhk7s
Pharaoh's Snakes
Igniting mercury(II) thiocyanate Hg(SCN)2
causes it to decompose into an insoluble brown mass that is primarily tricarbon tetranitride, mercury(II) sulfide and carbon disulfide.
Write the decomposition reaction and balance it!
2Hg(SCN)2 → 2HgS + CS2 + C3N4
Pharaoh's Snakes
Then flammable carbon disulfide combusts in oxygen to produce carbon dioxide and sulfur dioxide:
Write the combustion reaction and balance it!
CS2 + 3O2 → CO2 + 2SO2
Stop!
Let’s practice what we have learned with some worksheets!
“Writing Net Ionic Equations”Goals
Write total ionic equations for reactions in aqueous solutions
Identify spectator ions and write ionic equations for reactions in aqueous solutions
Ionic Equations
When ionic compounds dissolve in water, the ions separate form each other and spread throughout the solution
So when you see KI(aq) what it really means is K+
(aq) + I-(aq)
Or if you see Pb(NO3)2(aq) it means Pb+2(aq) +
2NO3-(aq)
More Correct
When we react the two compounds on the last slide we would do this:
KI(aq)+ Pb(NO3)2(aq) -> PbI2(s) + 2KNO3(aq)
But we should put the charges on them and then balance the charges and masses
K+(aq) + I-
(aq) + Pb+2(aq) + 2NO3
-(aq) -> PbI2(s) +
2K+ (aq) + 2NO3
-(aq)
Most Correct
When you mix two solutions all of the ions are present in the combined solution But not all of the ions will react with each other
Spectator ions=> ions that are present in a solution in which a reaction is taking place but that do not participate in the reaction
These spectator ions can be taken out of the total ionic equation
Example
Bottom of page 286
Writing Net Ionic Equations
These equations only show the compounds that change
Displacement Net Ionic
Happens in displacement reactions too Zn(s)+Cu+2
(aq)+SO4-2
(aq)-> Cu(s)+Zn+2 (aq)+ SO4-2
(aq)
Which is the spectator ion? How would we correctly write this?
Skills Toolkit Page 288 1) List what you know
ID each chemical described ID type of reaction
2) Write a balanced equation Predict products Include states (next slide shows how to know!!!)
3) Write total ionic equation Write separated aqueous ions for each aqueous ionic
substance DO NOT split up anything that is a solid, liquid, or gas
4) Find the net ionic equation Cancel out spectator ions Double check numbers and charges
Solubility
All group 1 compounds and NH4
All nitrates All halides (but Ag+ and Pb+2) All sulfates (but Ca+2, Sr+2, Ba+2, Hg+2,
and Pb+2) All carbonates (except group 1 and NH4) are
INSOLUBLE!
Charges
Make sure charges are equal on both sides SO4
-2 (aq) + Ba+2 (aq) -> BaSO4(s)
Notice no charge on reactant side so no charge on product side
Practice
Br2(l) + NaI(aq) -> NaBr(aq) + I(s)
Br2(l) + 2Na+(aq) + 2I-(aq) -> 2Na+(aq) + 2Br-(aq) + I2(s)