2.  A chemical reaction is a process.  What does this mean?  Give some examples of processes  Is baking a cake a process?  Name some ingredients of baking a cake  What is the product of this baking a cake process?  The cake – duh!  What symbol do we use to show processes? 

3.  In a chemical reaction, the  can be read as “produces” or “yields”  With a chem. Rx. (chemical reaction) something(s) new is produced from other chemical ingredients.  The arrow indicates the process of burning, combining, exploding, disintegrating….  To the left of the arrow is what goes into the reaction:  Reactants, separated by + signs  On the right: ?  Products, also separated by + signs

4.  Convert baking a cake into a chemical reaction  Flour(s) + water(l) + eggs(s) + milk(l), etc  cake(s) + good aroma filling the kitchen!(g)  Ingredients are reactants  Cake + aroma = products   = heat (produces, yields)  You know a chemical reaction has occurred because you can’t reverse it.

5.  Elements from periodic table  How to write ionic and covalent compound names  How to interpret word problems

6.  (l) = liquid state  (s) = solid state  (g) = gas  (aq) = aqueous (dissolved in water; solution)  The BrINClHOF’s  Guess what elements these are  bromine,  iodine,  nitrogen,  chlorine,  hydrogen,  oxygen,  fluorine

7.  The BrINClHOF’s  Always exist in pairs, when not combined with other elements  Gas at room temp.  Referred to by their normal chemical name even though they’re combined  ie. “chlorine” = Cl 2 (g)  “oxygen” = O 2 (g)  AKA: “HON and the halogens”  Or Hydrogen + 7

8.  When metals are just named (i.e., “lead”) this is simply the solid pure element (i.e., Pb(s))  When things are “bubbled in” that means a gas form of that element is being added:  Ex: “hydrogen is bubbled into a solution of…”  Is written as: H2(g) + …  …  “Solutions” are aqueous. Ex: “ a solution of lead(II)chloride…” =  PbCl2(aq)  Acids are aqueous

9. 1. Figure out which are reactants and which are products. 2. Write chemical formulas for all substances, separated by the  3. Add state of matter to each substance 4. Balance equation (to learn Friday)

10.  Zinc and aqueous lead(II)nitrate are combined in an aqueous solution to produce zinc nitrate and a lead precipitate. 1. zinc and lead(II)nitrate are reactants; zinc nitrate and lead are products 2. Zn + Pb(NO3)2  Zn(NO3)2 + Pb 3. Zn(s) + Pb(NO3)2(aq)  Zn(NO3)2(aq) + Pb(s) 4. Balancing Friday

11.  Carbon tetrachloride may be prepared by the reaction of natural gas, methane, and chlorine in the presence of ultraviolet light. Hydrochloric acid (HCl) is also a product of this reaction. 1. Carbon tetrachloride and hydrochloric acid are the products; methane and chlorine are the reactants 2. CH4 + Cl2  CCl4 + HCl 3. CH4(g) + Cl2(g)  CCl4(s) + HCl(aq) 4. To Balance Friday

12.  Big Idea: Law of Conservation of Matter  Matter cannot be created or destroyed  Number of atoms of a certain element must be equal on reactant and product side.  A balanced chemical equation shows the ratio of elements from one side to other

13.  Write unbalanced equation  Once unbalanced equation is written, NEVER CHANGE THE SUBSCRIPTS  Only add coefficients to front of compound  Coefficients multiply everything in the compound by that amount  Work with most complex molecule first, and save simplest for last  If you have an odd # of elements on one side, multiply entire eqn by 2, and continue

14.  How many oxygen atoms? O2O2 22 H2OH2O 11  PO 4 3- 44  2H 2 SO 4 88  2Ca(OH) 2 44  3Ca 3 (PO 4 ) 2  24

15.  O3  O2  You need the same number of O’s on both sides  2O 3  3O 2  6 = 6  Balance: H 2 + O 2  H 2 O  2H 2 + O 2  2H 2 O  H’s : 4 O’s : 2

16.  Combustion of ethane  C 2 H 6 + O 2  CO 2 + H 2 O  Which is most complex?  Ethane – so balance those elements first  C 2 H 6 + O 2  2CO 2 + 3H 2 O  Now you have odd number of O’s  Multiply entire eqn by 2  2(C 2 H 6 + O 2  2CO 2 + 3H 2 O)  2C 2 H 6 + 2O 2  4CO 2 + 6H 2 O  Balance O’s  2C 2 H 6 + 7O 2  4CO 2 + 6H 2 O  Make a T chart to double check balance of all elements on both sides

17.  SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions. SC2  a. Identify and balance the following types of chemical equations:  Synthesis  Decomposition  Single Replacement  Double Replacement  Combustion

18.  Combustion - “burning” (but not necessarily with flames) to release energy from a compound  The energy is stored in the bonds of the compound being “burned”  Oxygen is almost always one of the reactants  Produces carbon dioxide and water  Ex: cellular respiration  Glucose + oxygen  water + carbon dioxide + ENERGY

19.  Synthesis:  Putting things together  2H2 + O2  2H2O (releases energy)  Can you think of another example from biology?  Decomposition  Breaking compounds down  2H2O  2H2 + O2 (requires much energy)  What other rx type is also decomposition?  combustion

20.  Single replacement:  One element “steals” partner from another  3SrO(s) + 2Al(s)  Sr(s) + Al 2 O 3 (s)  Double replacement:  like “Wife Swap”  CaF 2 + H 2 SO 4  CaSO 4 + 2HF

21.  Soluble dissolves (in water)  Insoluble doesn’t dissolve (in water)  Precipitate solids that form when two ions react in water to form an Insoluble compound  Precipitation/ing forming a solid