MORE REACTION TYPES + HOW TO CALCULATE SOLUBILITY AND NET IONIC EQUATION

HOW TO DETERMINE THE STATE OF A COMPOUND (solid, gas, aqueous, liquid)

Here is the SOLUBILITY TABLE that was given during class:

NEGATIVE IONS (ANIONS)	POSITIVE IONS (CATIONS)	SOLUBILITY OF COMPOUNDS (solubility: >0.1mol/L)
ALL	All Alkali ions	Soluble
ALL	Hydrogen ion, H+	Soluble
ALL	Ammonium ion, NH4+	Soluble
Nitrate, NO3¯	ALL cations	Soluble
Acetate, CH3COO¯	ALL cations, except Ag+	Soluble
Chloride, Cl¯ Bromide, Br¯ Iodide, I¯	Ag²+, Pb²+, Hg2²+, Cu+ ALL other cations	Not (low) Soluble Soluble
Sulfate, SO4²¯	Ca²+, Sr²+, Ba²+, Ra²+, Ag+, Pb²+ All other cations	Not (low) Soluble Soluble
Sulfide, S²¯	Alkali ions, H+, NH4+ Be²+, Mg²+, Ca²+, Sr²+, Ba²+, Ra²+ Any other cations	Soluble Soluble Not (low) Soluble
Hydroxide, OH¯	Alkali ions, H+, NH4+, Sr²+ Any other cations	Soluble Not (low) Soluble
Phosphate, PO4³¯ Carbonate, CO3²¯ Sulfite, SO3²¯	Alkali ions, H+, NH4+ ALL other cations	Soluble Not (low) Soluble

Example:

2BeI2(   ) + 1Sn(NO3)4(   ) → 2Be(NO3)2(   ) + 1SnI4(   )

Instructions:

1. Is  2BeI2(   )  a solid or an aqueous substance? First take a look at the Anion, in this case, Iodide. Find Iodide in the left column of the Solubility Table. This is what you should see:

Chloride, Cl¯ Bromide, Br¯ Iodide, I¯

2. When you have found Iodide in the left column, look at the Cation, in this case, Beryllium. On the Solubility Table, look at the box with Iodide, then look at the box to its immediate right, in the middle column. This is what you should see:

Chloride, Cl¯ Bromide, Br¯ Iodide, I¯

Ag²+, Pb²+, Hg2²+, Cu+ ALL other cations

3. Look for Beryllium in the middle column. It if is not stated specifically, the it is considered in the “ALL other cations” category.

Chloride, Cl¯ Bromide, Br¯ Iodide, I¯

Ag²+, Pb²+, Hg2²+, Cu+ ALL other cations

4. Now look to the immediate right of the middle box. This is what you should see:

Chloride, Cl¯ Bromide, Br¯ Iodide, I¯

Ag²+, Pb²+, Hg2²+, Cu+ ALL other cations

Not (low) Soluble Soluble

Look at the one that is directly to the left of the highlighted part, not the other one. It should be like this:

Chloride, Cl¯ Bromide, Br¯ Iodide, I¯

Ag²+, Pb²+, Hg2²+, Cu+ ALL other cations  →

Not (low) Soluble Soluble

When it is SOLUBLE, it means it is an AQUEOUS. When it is NOT (low) SOLUBLE, it means it is a SOLID.

Therefore, 2BeI2( aq )

When you do the whole equation, it should look like this:

2BeI2( aq ) + 1Sn(NO3)4( aq ) → 2Be(NO3)2( aq ) + 1SnI4( s )

DOUBLE REPLACEMENT

• The reaction between 2 ionic compounds
• The positive ions switch places with one another

General formula:

AB + CD → CB + AD

For example:

When a solution of silver nitrate is combined with a solution of sodium chloride, silver chloride and Sodium Nitrate are formed.

AgNO3 + NaCl → AgCl + NaNO3

BUT, how can we determine whether or not a reaction actually occurs?

• Look back at the Solubility Table mentioned earlier.

• There is a reaction if the reactants change states during reaction.
• The change usually forms a precipitate (aqueous).
• There is no reaction if there is no change in states.

When you’ve figured out the states, it should look like this:

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

The reaction changed states, therefore, this reaction can occur.

NEUTRALIZATION

• A special type of Double Replacement
• Happens when an ACID and a BASE reacts to produce WATER and an ionic SALT
• The formula for an ACID always contain H⁺ as the cation
• The formula for a BASE always contain OH¯ as the anion
• An exception to this is H2O, aka. HOH, because it is neutral.

General formula:

HA + BOH → H2O + BA

For example:

Hydrochloric acid combined with Sodium Hydroxide is neutralized to form Sodium Chloride (salt) and water.

HCl + NaOH → NaCl + H2O

COMBUSTION

• a COMBUSTION reaction happens when a compound is burned with oxygen

General formula:

AB + O2 → AO + BO

For example:

When methane burns with oxygen, it produces carbon dioxide and water.

1CH4 + 2O2 → 1CO2 + 2H2O  *don’t forget to balance!!

How to Calculate the Net Ionic Equation 

~JZ

Types of Reactions

Synthesis

• A synthesis reaction is when two or more reactants combine to form a compound.

Formula:  A + B --> C

Examples:

• 1Ca + 1Cl₂ --> 1CaCl₂
• Na + Cl₂ --> 
• 2Na + 1Cl₂ --> 2NaCl
• 1H₂ + 1F₂ -->  2HF
• Al + Cl₂ -->  
• 2Al + 3Cl₂ --> 2AlCl₂
• 6Li + 1N₂ --> 2Li₃N

Decomposition

• A decomposition reaction is when a compound degrades into two or more products.

Formula:  A --> B + C

Examples:

• 2H₂O --> 2H₂ + 1O₂
• KNO₃ -->
• 2KNO₃ --> 2KNO₂ + 1O₂
• NF₃ --> 1N₂ + 3F₂
• MgO -->
• 2MgO --> 2Mg + 1O₂
• 2NaCl --> 2Na + 1Cl₂

Single Replacement

• A single replacement(or displacement) reaction is when one element replaces another element in a compound.

Formula for Metal:  A + BC --> AC + B

Formula for Non-Metal:  A + BC --> BA + C

Examples:

• 6K + 1Al₂O₃ --> 3K₂O + 1Al
• Al + FeCl₂ -->
• 2Al + 3FeCl₂ --> 2AlCl₃ + 3Fe
• 2AgCl + 1Mg --> 2Ag + 1MgCl₂
• Zn + H₂SO₄ -->
• 1Zn + 1H₂SO₄ --> 1ZnSO₄ + 1H₂
• 1Cl₂ + 2KBr --> 2KCl + 1Br₂

Activity Series

• Elements higher on the chart can replace elements below it, but elements lower on the chart cannot replace elements higher on the chart.

For example:

Fe + Al2O3 --> N.R., because iron is lower on the activity series chart than aluminum, it cannot replace it. When this occurs we label it N.R. for no reaction.

Balancing Equations

The number of atoms on the reactant side has to equal to the number of atoms on the product side.

Examples:

• Fe + S --> Fe₂S₃
• 2Fe + 3S --> 1Fe₂S₃
• H₂O -->  H₂ + O₂
• 2H₂O -->  2H₂ + 1O₂
• Al + HCl -->  AlCl₃ + H₂
• 2Al + 6HCl -->  2AlCl₃ + 3H₂
• C₂H₆ + O₂  -->  CO₂   +  H₂O
• 2C₂H₆ + 5O₂  -->  2CO₂   + 6H₂O
• Zn + HCl --> ZnCl₂ + H₂
• 1Zn + 2HCl --> 1ZnCl₂ + 1H₂
• Al + Pb(NO₃)₂ --> Al(NO₃) + Pb
• 2Al + Pb(NO₃)₂ --> 2Al(NO₃) + Pb
• KClO₃ --> KCl + O₂
• 2KClO₃ --> 2KCl + 3O₂
• KOH + H₃PO₄ --> K₃PO₄ + H₂O
• 3KOH + 1H₃PO₄ --> 1K₃PO₄ + 3H₂O
• Al + CuCl₂ --> AlCl₃ + Cu
• 2Al + 3CuCl₂ --> 2AlCl₃ + 3Cu

Translating Word Equations and Naming Compounds

Translating Word Equations

1. First thing is to understand the wording of the word equations.

• The word "and" or "reacts with" means + 
• The phrase "react to," or "produce" means ------>

For example:


Magnesium bromide and chlorine produce magnesium chloride and bromine.


    
    2.  You then look at the Periodic Table for the elements in the equation and criss-cross the numbers in front of the charges on the ions.


MgBr₂  +  Cl₂  ---->   MgCl₂  +  Br₂

Examples:

• Iron and sulfur produces iron(III) sulfide
• Fe + S --> Fe₂S₃
• Water produce hydrogen and oxygen
• H₂O -->  H₂ + O₂
• Potassium and water react to produce potassium hydroxide and hydrogen
• K + H₂O -->  KOH + O₂
• Aluminum and hydrochloric acid produce aluminum chloride and hydrogen
• Al + HCl -->  AlCl₃ + H₂
•  Ethane and oxygen react to produce carbon dioxide and water
• C₂H₆ + O₂  -->  CO₂   +  H₂O

Naming Compounds

• Non-metals end with "ide"

• - ic if the anion name ends in - ate.
• - ous if the anion name ends in - ite.

Acid	Ion	Name
H2SO4	SO4 2-	sulfuric acid (anion, sulfate)
HClO3	ClO3 -	perchlorous acid (anion, perchlorite)

• Roman numerals are needed when naming elements with more than one ion.

Element	Cation	Preferred Name
copper	Cu+	copper (I)
	Cu2+	copper (II)
iron	Fe2+	iron (II)
	Fe3+	iron (III)
lead	Pb2+	lead (II)
	Pb4+	lead (IV)
mercury	Hg22+	mercury (I)
	Hg2+	mercury (II)
tin	Sn2+	tin (II)
	Sn4+	tin (IV)

Roman Numeral Prefixes:

Greek Prefixes	Number
mono-	1
di-	2
tri-	3
tetra-	4
penta-	5
hexa-	6
hepta-	7
octa-	8
nona-	9
deca-	10

Examples:

• Zn + HCl --> ZnCl₂ + H₂
• Zinc + hydrochloric acid --> zinc chloride + hydrogen
• Al + Pb(NO₃)₂ --> Al(NO₃) + Pb
• Aluminum + lead(II) nitrate -->  aluminum nitrate + lead
• KClO₃ --> KCl + O₂
• Potassium chlorate -->  Potassium chloride + oxygen gas
• KOH + H₃PO₄ --> K₃PO₄ + H₂O
• Potassium hydride + phosphoric acid --> potassium phosphate + water
• Al + CuCl₂ --> AlCl₃ + Cu
• Aluminum + copper(II) chloride --> aluminum chloride + copper

Molar Volume of a Gas at STP

Molar Volume:

• The volume occupied by one of a gas is called as molar volume.
• One mole of any gas at STP will have a volume of 22.4 L.
• S.T.P. = Standard Temperature and Pressure
• Standard Temperature = 0^oC or 273 K

Formula:
Molar Volume :  22.4 L of gas / 1 mol of gas  


                                       OR


                       1 mol of gas / 22.4 L of gas

Example:
For the information on Molar Volume, skip to 5:20 of the video:
http://www.youtube.com/watch?v=mwVBg9SMKPg


By: Hikari Hoshika

Diluting Solutions to Prepare Workable Solutions



Moles of solute stays the same,
concentration depend on amount of water



Chemicals are shipped around the world in their most concentrated form, like powder, making it easier and lost costly because then we wouldn’t be shipping all that extra water.

This is why we need to be able to make solutions of any concentration from a more concentrated source.

The moles of the solute is always constant.

The concentration is based on the amount of water present.

MOLES OF SOLUTE BEFORE  =  MOLES OF SOLUTE AFTER

or

M1L1  =  M2L2

Where:

M = Moles

L = Litres

Eg.  15.0mL of 0.70M KCl  solution is diluted to a final volume of 150.0mL. What is the new concentration?

M1 =  0.70M

L1  =  15.0mL

M2 = ?

L2  = 150.0mL

M1L1  =  M2L2

0.70M  x 15.0mL = M2  x 150.0mL

0.70M x 15.0mL  =   M2

150.0mL          .

0.070M  =  M2

Eg.   A 0.275M solution is concentrated by evaporating the a reduced volume of 250.0mL and a molarity of 0.720M. What is the original volume?

M1 =  0.275M

L1  =  ?

M2 = 0.720M

L2  = 250.0mL

M1L1  =  M2L2

0.275M  x  L1 = 0.720M  x  250.0mL

L1  =  0.720M  x  250.0mL

       0.275M

L1  =  912mL

By:  JZ

molar concentration/molarity

Molar Concentration or molarity is the #of moles  of solute dissolved in a 1 L of solution.
- represented by M and it has the units of "mols/L."
The formula of Molarity = moles of solute (mol)
                                         volume of solution (L)
 M = mol/L.
 mol = M x L and L = mol/M are ways to find the mol and volume.


1) Calculate molar concentration that has a solution of 0.620 moles of CaCl2 in 1.7 L of solution.
2)Calculate the number of grams of sodium hydroxide in 3200mL of a 1.2 M KF solution.
3) Calculate the volume of L of 0.780 M NaCl solution that contains 55.21 g NaCl.


Answers:
1) M =0.620mol/ 1.7L 
=0.36(remember your sigfigs) 

2) 3200ml = 3.2 L
1.2M x 3.20L= 3.84 mols
convert mols to grams -------> 3.84 mols x 58.1g   = 223.104g--------------->220g
                                                                      1 mol
3) MM of NaCl = 58.5 g/mol
    55.21 g x 1 mol / 58.5 g
    = 0.944
L solution = 9.44444 moles of NaCl / 0.780
                = 12.108L




Post: JN 

bobby with snow :)