Be able to write chemical reactions based on the reactants using the 5 types of reactions.
Be able to balance equations.
Be able to calculate stoichiometric quantities using mass to mole, mole to mole, mole to particle conversions.
Be able to identify and explain limiting reactants in stoichiometric data.
Reactants--> Products
The reactants will always be on the left and the products on the right.
Using the 5 Types of Chemical Reactions you can correctly predict the products of a chemical reaction.
Synthesis A + B --> AB Mg + O2-->MgO Whenever there are compounds by themselves that are fused together this is synthesis.
Decomposition AB--> A + B H2O2 --> H2O + O2 Synthesis is the opposite of decomposition. Going from one compound to more than one
Single Displacement A + BC --> AC + B Al + CuCl2 --> AlCl3 + Cu Any element by itself replaces one of the elements inside of an ionic bond
Double Displacement AB + CD --> AD + CB PbNO3 + KI --> KNO3 + PbI Looking at this reaction you see the metals and non-metals switch partners. Remember metal must be bonded to a nonmetal. You cannot put two metals together!
Combustion Fuel + O2 --> CO2 + H2O Usually a hydrocarbon (CH4 for example) reacts with oxygen and in most cases makes CO2 and H2O and a large release of energy. (FIRE!!!)
Please find the Stoichiometry Road Map in the Class Resource Materials.
Try this stoichiometry problem. If you struggle re-watch the video paying close attention to each conversion.
How many grams of H2O, can be made from the combustion of 20.5 grams of Methane (CH4)?
50.6 grams of water can be made!
Think about Bicycle workshop. If you went into business and the supply chain gave you 5 bike frames, but only 8 wheels. How many bicycles could you make? With the 5 bike frames you could make 5 bikes. However with the 8 wheels (2wheels/bike), you could only create 4 bikes. Based on that information you would have an extra bike frame with no wheels to go on it. Therefore even though you have an extra bike bike frame the wheels are limiting how many bikes you could actually make. So in this example you can only make 4! This applies to chemicals too. Watch the video below for an example how this works!
Here is a video of a limiting reactant problem being completed. Please watch carefully and use this as an example for the homework problems.
The last 3 skills of chapter 3 are calculating percent composition, empirical formulas and molecular formulas. Please see this video on how to do each of these. You can find an empirical formula from a % composition, or a molecular formula from an empirical formula so they are all related to each other.
Empirical formula- the simplest whole number ratio of the atoms in a compound
Molecular Formula- The actual number of atoms in a compound
Percent Composition- The percent by weight of a particular atom in a compound
Calculate the percent of Hydrogen in CH4?
4/16 *100=25%
If the molecular formula weighed 64g/mol, what would be its molecular formula?
Empirical Formula (CH4) weighs: 16g/mol, so 64/16=4
4 (CH4) ---> C4H16
Be sure to head over to google classroom and complete all related assignments!