Monday, March 9, 2015 Homework: NONE! Objective: We will be able to balance chemical equations. Catalyst: Please answer Monday’s question on the back of your catalyst sheet!

Announcements No tutoring today or tomorrow Quiz on THURSDAY!

Agenda Catalyst Announcements Notes Practice Exit Slip

Table of Contents

Review Practice Determine how many of each type of atom you have in the reactants and products

Balancing Chemical Equations Step Description Example 1 Create an atom inventory with elements in the same order as the equation __Na + __MgF2__NaF + __Mg  

Balancing Chemical Equations Step Description Example 1 Create an atom inventory with elements in the same order as the equation __Na + __MgF2__NaF + __Mg   Na – 1 Na – 1 Mg – 1 Mg – 1 F – 2 F – 1

Balancing Chemical Equations Step Description Example 2 Pick an element that is not equal on both sides (save oxygen and hydrogen until last!) __Na + __MgF2__NaF + __Mg   Na – 1 Na – 1 Mg – 1 Mg – 1 F – 2 F – 1

Balancing Chemical Equations Step Description Example 3 Add a coefficient in front of the formula with that element, and adjust the inventory __Na + __MgF2__NaF + __Mg   Na – 1 Na – 1 Mg – 1 Mg – 1 F – 2 F – 1

Balancing Chemical Equations Step Description Example 3 Add a coefficient in front of the formula with that element, and adjust the inventory __Na + __MgF2 2NaF + __Mg   Na – 1 Na – 1 2 Mg – 1 Mg – 1 F – 2 F – 1 2

Balancing Chemical Equations Step Description Example 4 Continue adding coefficients to get the same number of atoms on each side __Na + __MgF2 2NaF + __Mg   Na – 1 Na – 1 2 Mg – 1 Mg – 1 F – 2 F – 1 2

Balancing Chemical Equations Step Description Example 4 Continue adding coefficients to get the same number of atoms on each side 2 Na + 1 MgF2 2 NaF + 1 Mg   Na – 1 2 Na – 1 2 Mg – 1 Mg – 1 F – 2 F – 1 2

Rules 1. You can only change coefficients. 2. All coefficients must be whole numbers. 3. You must end with the same number of all elements on reactants and products. 4. Coefficients should be as simple as possible.

Examples Work through the examples with Ms. Kline.

Practice Complete the practice problems on the back of your notes sheet.

Exit Ticket Create an atom inventory and balance the following equations: ___Fe + __ S  ___ FeS ___O2 + ___H2  ___H2O ___ Fe + ___Cl2___FeCl3

Exit Ticket Thinking about your upcoming test, what are: 3 – things you are confident about 2 – things you are NOT confident about 1 – thing you are going to do tonight to prepare

Tuesday, March 10, 2015 Homework: Study for Quiz! Objective: We practice balancing chemical equations. Catalyst: Please answer Tuesday’s question on the back of your catalyst. 3/10 Classwork: Balancing Chemical Equations 16

Announcements Quiz Thursday!

Agenda Catalyst Announcements Finish worksheet practice Whiteboard practice Exit Ticket

Review: Exit Ticket Create an atom inventory and balance the following equations: ___Fe + __ S  ___ FeS ___O2 + ___H2  ___H2O ___ Fe + ___Cl2___FeCl3

Finish Practice Problems On the back of yesterday’s worksheet, finish the practice problems. You have 10 minutes to solve!

Problem #1 __Na + __ Cl2  __NaCl

Problem #1 2 Na + 1 Cl2  2 NaCl

Problem #2 __SnO2 + __ H2  __Sn + __H20

Problem #2 1 SnO2 + 2 H2  1 Sn + 2 H20

Problem #3 __C2H4 + __ O2  __H2O + __CO2

Problem #3 1 C2H4 + 3 O2  2 H2O + 2 CO2

__TiCl4 + __ H2O  __TiO2 + __HCl Problem #4 __TiCl4 + __ H2O  __TiO2 + __HCl

Problem #4 1 TiCl4 + 2 H2O  1 TiO2 + 4 HCl

Problem #5 __C2H6O + __ O2  __CO2 + __H2O

Problem #5 1 C2H6O + 3 O2  2 CO2 + 3 H2O

Exit Ticket Balance the following equations: ___H2 + __ Cl2  ___ HCl ___ Fe + ___O2___Fe2O3 ___ BaO+ ___H2O___Ba(OH)2

Wednesday, March 11, 2015 Homework: STUDY FOR QUIZ! Objective: We practice balancing chemical equations. Catalyst: Please answer Wednesday’s catalyst question on the back of your catalyst sheet. 3/11 Classwork: Snowman Balancing Practice 17

Announcements Quiz TOMORROW!! Tutoring today after school (after 4pm)!

Agenda Catalyst Announcements Snowman Balancing Race! Exit Ticket

Review - Yesterday Balance the following equations: ___H2 + __ Cl2  ___ HCl ___ Fe + ___O2___Fe2O3 ___ BaO+ ___H2O___Ba(OH)2

Snowman Practice You will be working in pairs. One person will draw a snowman card from Ms. Kline. You and your partner will balance the equation and show Ms. Kline. If it is correct, take another! Try to get as many as you can! Earn extra points on the quiz!

Exit Ticket __ P + __ O2 __ P4O10 __ Al2O3 __ Al + __ O2 __ Cl2 + __ NaBr  __NaCl + __ Br2 How well did each member of your group work today?

Thursday, March 12, 2015 You MUST have a pencil!! On the GREEN side of your scantron, bubble in your ENTIRE ID number and write your name.

Exit Ticket What are the FOUR signs of a chemical reaction? __ CH4 + __ O2  __ CO2 + __ H2O What grade do you think you will get on the quiz? What can you do to improve that grade?

Friday, March 13, 2015 Homework: NONE! Objective: We identify the five types of chemical reactions. Catalyst: Please answer Friday’s catalyst question on the back of your catalyst sheet. 3/11 Notes: Types of Chemical Reactions 18

Agenda Catalyst Quiz Notes Exit Ticket

Think + Write What is happening from the reactant side of a chemical equation to the product side of a chemical equation?

Types of Reactions There are millions of different reactions! There are 5 major types of chemical reactions.

Who are these people?

#1 - Synthesis Reactions Description Example Chemical Reactions Synthesis = put together or combine 2 substances combine to make one compound (also called “combination”) Ca + O2 ® CaO SO3 + H2O ® H2SO4

#2 – Decomposition Reactions Description Example Chemical Reactions decompose = fall apart one reactant breaks apart into two or more elements or compounds Energy is usually required NaCl Na + Cl2 CaCO3 CaO + CO2

#3 – Single Replacement Reactions Description Example Chemical Reactions One element replaces another Reactants must be an element and a compound. Products will be a different element and a different compound.

#4 – Double Replacement Reactions Description Example Chemical Reactions Two things replace each other. Reactants must be two ionic compounds, in aqueous (aq) solution

#5 – Combustion Reactions Description Example Chemical Reactions Combustion means “add oxygen” Usually, a compound composed of only C, H, (and maybe O) is reacted with oxygen – usually called “burning” CH + O2  CO2 + H2O

Practice: Name the Type of Reaction 2 H2 + O2 2 H2O 2 H2O  2 H2 + O2 Zn + H2SO4  H2 + ZnSO4 2 HgO  2 Hg + O2 2 KBr + Cl2  2 KCl + Br2 AgNO3 + NaCl  AgCl + NaNO3 2 C2H6 + 7 O2  4 CO2 + 6 H2O Mg(OH)2 + H2SO3  MgSO3 + 2H2O Synthesis Decomposition Single Replacement Decomposition Single Replacement Double Replacement Combustion Double Replacement

Exit Ticket Identify the reactions below as COMBINATION, DECOMPOSITION, SINGLE REPLACEMENT, or DOUBLE REPLACEMENT.   1) ____ P + O2 → P4O10 5) ____ Mg + O2 → MgO 2) ____ HgO → Hg + O2 6) ____ Al2O3 → Al + O2 3) ____ MgCl2 + NaBr → NaCl + MgBr ____ H2 + N2 → NH3 7) __ C2H5 + O2  CO2 + H2O If I were to give you a quiz TOMORROW about identifying types of reactions, how would you do?