CHEM-R REVIEW CHAPTERS 9,11,10,12

CHAPTER 9: Writing and Naming Chemical Formulas

IONIC compounds consist of a _________ and a __________ COVALENT compounds (Molecules) consist of 2 ________________

Which of the following compounds contains the Iron III cation? a. FeO b. FePO4 c. FeF2 d. Fe3N2

-ide ending comes from the periodic table (there are exceptions) -ate and -ite are your polyatomic ions Molecular compounds are named using prefixes

NAMING ACIDS -ate polyatomic ion results in an -ic acid -ite polyatomic ion results in -ous acid monoatomic ions results in Hydro-- acid

TIME TO GET UP AND MOVE!

Chapter 11: Chemical Reactions

Reactions that have energy as a reactant are called _______________ reactions: They require energy for the reaction to occur Reactions that have energy as a product are called _______________ reactions Energy happens as a result of the reaction

Writing and Balancing Chemical Reactions *** DONT forget charges when writing, and to add coefficients ONLY when balancing***

RULES for BALANCING COMBUSTION REACTIONS: 1. Determine the # of Hydrogens in the hydrocarbon molecule ODD- Place the coefficient “4” in front of the molecule EVEN- Place the coefficient “2” in front of the molecule 2. Balance both sides of the equations (Left to Right) with the Carbon atoms 3. Balance (Left to Right) the Hydrogen atoms 4. Balance the Oxygen atoms (Right to Left) 5. Reduce the coefficients (If necessary)

What are the 5 types of Chemical reactions?

TIME TO GET UP AND MOVE!

Chapter 10: Chemical Quantities (The Mole)

1 mole of anything is equal to _____________ of that thing This number is better known as ______________ number

The mole is at the center of your chemical calculations

WHAT IS 1 Mole equal to??? 1 Mole = 6.02 x 1023 (atoms, formula units, or molecules) 1 Mole = molar mass (of an element or compound) 1 Mole = 22.4 L (of a gas at STP)

Percent Composition Percent composition tell us what percent, by mass, each element is in a given compound % by mass of element = mass of element molar mass of compound × 100 K = 40.3% Cr = 26.8% + O = 32.9% 100%

Empirical Formula A compound that gives the lowest whole-number ratio of the atoms or moles of the elements in a compound For example: Hydrogen peroxide has a molecular formula H2O2 but an empirical formula HO Carbon dioxide (CO2) has the same molecular and empirical formula

Calculating Empirical Formula (from percent composition) 1. Percent to mass 2. Mass to moles 3. Divide by small 4. Multiple ‘til whole (sometimes) 1. A compound was found to have a percent composition as follows: 47.0 % potassium, 14.5 % carbon, and 38.5 % oxygen. What is its empirical formula?

So how would you determine which chemical you are dealing with? Molecular Formula: a formula giving the actual number of atoms of each of the elements present in one molecule Methanol (formaldehyde), ethanoic acid (acetic acid), and glucose have the same empirical formula CH2O So how would you determine which chemical you are dealing with?

TIME TO GET UP AND MOVE!

Chapter 12: Stoichiometry “stoicheion” = Greek for element “metron” = measurement

Stoichiometry: a process of relating the quantities of reactants and products in a chemical reaction to one another Mole Ratio: Conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction ** All reaction stoichiometry calculations begin with a balanced chemical equation**

Steps to follow when solving stoichiometry calculations: 1. Write/Balance the chemical equation 2. Determine the mole ratio 3. Determine the given and wanted quantity 4. If necessary, convert the given quantity to moles 5. Use the proper mole ratio to get rid of the given moles and determine the wanted moles 6. If necessary, convert the wanted quantity (in moles) to grams, representative particles, or liters

____KClO3 ____KCl + ____O2 What mass of KClO3 do you need to produce 0.500 moles of O2?

Limiting Reactants

Ideal stoichiometry problems assume that the given quantity is completely used up and therefore we can predict how much product is formed In real stoichiometry calculations, you are given the starting amount of both reactants. One of the reactants is used up before the other and therefore limits the reaction Once the limiting reactant is used up, the reaction will stop

TIME TO GET UP AND MOVE!