As you come in, Materials: Plan: Paper, periodic table, and pencil for the test Plan: Complete the Unit Four Bonding test Read the Chemical Literacy #4 article and respond to the questions. (due tomorrow) Go to Edmodo, and begin the assignments. DUE TOMORROW – Balancing Equations note-taking guide DUE THURSDAY – Types of Equations note-taking guide DUE FRIDAY – Predicting Products note-taking guide Begin writing chemical equations on the “Writing Equations from Word Equations” handout.

As you come in, Materials: Chemical Literacy Answers Balancing Equations Note-taking Guide Practice Packet (pick up at front) Periodic table and paper for notes Plan: Learn to write and balance chemical equations Complete the “Writing Equations from Word Equations” handout Continue practicing handouts listed on “1c” of SLA list Tonight: Go to Edmodo. DUE TOMORROW – Types of Equations note-taking guide DUE FRIDAY – Predicting Products note-taking guide

Chemical Reactions Process by which the atoms of one or more substances are rearranged to form different substances Law of Conservation of Matter – Matter is not created or destroyed during a chemical reaction.

Writing Chemical Equations Video Example 1: Combustion of H2 gas Description: Hydrogen gas burns in oxygen gas to produce water vapor. Unbalanced equation: Read a description of the reaction Note what is reacted with what Note what is yielded or produced Write formulas for each compound Use + to represent “and” Use  to represent “produces” or “yields” Include states of matter where available (s) solid (l) liquid (g) gas (aq) dissolved in water Video Example 2: Combustion of methane gas Description: Methane gas burns in oxygen gas to produce carbon dioxide and water vapor. Unbalanced equation:

Balancing Chemical Equations Video Example 1: Combustion of H2 gas Unbalanced equation: H2 + O2  H2O Balanced equation: Write the skeleton equation. BE SURE THE FORMULAS ARE WRITTEN CORRECTLY. Inventory reactants Inventory products Insert coefficients to make atoms of each element equal on both sides of the equation Reduce the coefficients if possible Video Example 2: Combustion of methane gas Unbalanced equation: CH4 + O2  CO2 + H2O Balanced equation:

Guided Example Sodium carbonate reacts with chromium (III) chloride to produce sodium chloride and chromium (III) carbonate. Unbalanced Equation: Na2CO3 + CrCl3  NaCl + Cr2(CO3)3 Balanced Equation: 3Na2CO3 + 2CrCl3  6NaCl + Cr2(CO3)3

Writing Equations from Word Equations handout Work with a partner to write and balance equations. Take 10 minutes to write and balance as many as possible. Use a colored pencil or pen to correct your mistakes.

Writing & Balancing Equations Zn + Pb(NO3)2 --> Zn(NO3)2 + Pb 2 AlBr3 + 3 Cl2 --> 2 AlCl3 + 3 Br2 2 Na3PO4 + 3 CaCl2 --> Ca3(PO4)2 + 6 NaCl 2 K + Cl2 --> 2 KCl 2 Al + 6 HCl --> 2 AlCl3 + 3 H2 3 Ca(OH)2 + 2 H3PO4 --> Ca3(PO4)2 + 6 H2O Cu + 2 H2SO4 --> CuSO4 + 2 H2O + SO2 2 H2 + 2 NO --> 2 H2O + N2

As you come in, a Materials: Types of Reactions Note-taking Guide Periodic table and paper for notes Plan: Balancing more advanced equations Learn about types of equations Practice identifying types of equations and writing equations Practice balancing for tomorrow’s quiz Tonight: Go to Edmodo. DUE TOMORROW– Predicting Products note-taking guide Practice balancing equations for tomorrow’s quiz!

Difficult Equations to Balance Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur dioxide. Cu + 2 H2SO4 --> CuSO4 + 2 H2O + SO2

5 Types of Chemical Reactions Synthesis A + B  AB Combustion CxHy + O2  CO2 + H2O Decomposition AB  A + B Double-Replacement AX + BY  AY + BX Single-Replacement A + BX  B + AX Five Types of Reactions Clip

Identify the Type of Reaction Zn + Pb(NO3)2 --> Zn(NO3)2 + Pb 2KClO3  2KCl +3 O2 2 AlBr3 + 3 Cl2 --> 2 AlCl3 + 3 Br2 2 Na3PO4 + 3 CaCl2 --> Ca3(PO4)2 + 6 NaCl 2 K + Cl2 --> 2 KCl 2 Al + 6 HCl --> 2 AlCl3 + 3 H2 CH4 + 2O2  CO2 + 2H2O 3 Ca(OH)2 + 2 H3PO4 --> Ca3(PO4)2 + 6 H2O

Single Replacement Reactions SPECIAL! MORE TO COME! A + BX --> AX + B A metal will not always replace another metal. The reactivity of the metal is important to consider. Reaction: More active metal replaces a less active metal. No Reaction: A less active metal will not replace a more active metal. Use the metal activity series to determine if single replacement reactions occur. Find the element who is alone in the reactants on the series. Identify the element that is most similar to it in the reactant compound. The LONE element must be HIGHER than the compound element.

Work with a partner to Identify type of reaction and write equations. “Long worksheet” #26-50 Work with a partner to Identify type of reaction and write equations. Take 10 minutes to identify types and write as many as possible. Use a colored pencil or pen to correct your mistakes.

“Balancing Chemical Equations” handout Work with a partner to Balance the equations. Your quiz will be similar to this tomorrow. Take 10 minutes to balance as many as possible. Use a colored pencil or pen to correct your mistakes.

As you come in, Materials: Paper for quiz Predicting Products note-taking guide Plan: Balancing Equations Quiz (TIME LIMIT: 30 minutes) Practice writing, balancing, and identifying types of reactions Learn to predict the products of double and single replacement reactions Discovery Lab – Indicators of a Chemical Reaction Tonight: Go to Edmodo. DUE MONDAY– Net Ionic Equations note-taking guide Practice identifying the types reactions for Monday’s quiz!

AFTER YOUR QUIZ Write, balance, and identify the type of reaction for the following on your “LONG worksheet” #26-#50 (as many as you can)

Predicting Products & States of Matter Expectations: To predict the products of DOUBLE REPLACEMENT and SINGLE REPLACEMENT reactions To use the Solubility Rules to predict the states of matter of your products

Let’s add states of matter. Predicting Products & States of Matter for DOUBLE REPLACEMENT REACTIONS Tips to remember: AX + BY  Metals (+) always come first! Criss-cross to get subscripts. Deal with number problems by balancing at the end. Video Example 2: Potassium chromate and silver nitrate Reactant formulas: K2CrO4 + AgNO3  [TIP: Label each element with its charge] Unbalanced Equation: K2CrO4 + AgNO3  KNO3 + Ag2CrO4 Let’s add states of matter.

Last Question on Note-taking Guide DOUBLE REPLACEMENT EXAMPLE: Zinc chloride + ammonium sulfide  Reactant formulas: ZnCl2 + (NH4)2S  Unbalanced equation: ZnCl2 + (NH4)2S  ZnS + NH4Cl Balanced equation: ZnCl2 + (NH4)2S  ZnS + 2NH4Cl Let’s add states of matter.

As you come in, Materials: Practice packet Predicting Products note-taking guide Discovering the Indicators of a Reaction lab Plan: Types of Reactions Quiz (TIME LIMIT: 15 minutes) Predicting Products of Single Replacement & finish lab Learn to write Net Ionic Equations Tonight: Practice predicting products and balancing equations for tomorrow’s quiz! Read over the Student Learning Activities. Have you been working the suggested problems in your practice packet?

Let’s add states of matter. Predicting Products & States of Matter for SINGLE REPLACEMENT REACTIONS Tips to remember: A + BX  CONSULT ACTIVITY SERIES TO BEGIN! Metals (+) always come first in a compound! Lone metals replace compound metals or hydrogen. Lone nonmetals replace compound nonmetals. Criss-cross to get subscripts. Deal with number problems by balancing at the end. Example: Potassium and silver nitrate Reactant formulas: K + AgNO3  [TIP: Label each element with its charge] Unbalanced Equation: K + AgNO3  KNO3 + Ag Let’s add states of matter.

Predicting Products & States of Matter SINGLE REPLACEMENT “Long Worksheet” example 52. Al + HCl  Who will Al try to replace? Is Al more active than H? Criss-cross to write the products. Look for diatomic elements! Unbalanced Equation: Al + HCl  AlCl3 + H2 Balanced Equation: 2Al + 6HCl  2AlCl3 + 3H2 Let’s add states of matter.

DISCOVERING INDICATORS OF A CHEMICAL REACTION LAB For each reaction: Predict the Products. Write a balanced equation. List as many observations as possible during the reaction.

Reactions in Aqueous Solution MANY reactions occur in water: More than 70% of earth is covered by water 66% of the human body is water Many ionic compounds dissociate in water. They are described as (aq) in reactions. Often aqueous reactions form solids called precipitates

Net Ionic Equations Purpose: Communicate the real action of the reaction and leave out the insignificant ions/elements Begin with a balanced equation and states of matter. Write a complete ionic equation, taking apart all aqueous compounds. Remove spectator ions Leaves a balanced net ionic equation Example: Potassium iodide and lead (II) nitrate Discovering the Indicators of a Reaction: Station 2

Why do I set up the lab with so many aqueous solutions? Rate of Reaction Temperature – warmer = faster reaction; particles are moving faster Concentration - # of particles; more particles = faster reaction State of Matter – dissolved means greater surface area; more surface area = faster reaction Surface Area - Filings, shot, powder, mossy, etc.; greater surface area = faster reaction Catalyst – DOES NOT REACT; lowers the activation energy of the reaction

Predicting Products & States of Matter 52. 2Al(s) + 6HCl(aq)  2AlCl3(aq) + 3H2(g) 56.ZnCl2 + (NH4)2S  2NH4Cl + ZnS

Predicting Products & States of Matter 56.ZnCl2 (aq)+ (NH4)2S(aq)  2NH4Cl(aq) + ZnS(s) 59. HgSO4 + 2NH4NO3  Hg(NO3)2 + (NH4)2SO4

Predicting Products & States of Matter 59. HgSO4(aq) + 2NH4NO3(aq)  Hg(NO3)2(aq) + (NH4)2SO4(aq) 60. Fe + CuSO4  FeSO4 + Cu

Predicting Products & States of Matter 60. Fe (s)+ CuSO4 (aq)  FeSO4 (aq) + Cu (s) 67. Br2 + 2NaI  2NaBr + I2

Predicting Products & States of Matter 67. Br2 (l) + 2NaI(aq)  2NaBr (aq) + I2 (g)

Evidence of a Chemical Reaction Formation of a gas Bubbles Smell Formation of a solid (precipitate) from two aqueous solutions; often solids are colorful “Snow globe” effect “Paint” look “Jello” consistency Change in temperature Test tube feels colder to you (endothermic reaction) Test tube feels warmer to you (exothermic reaction) Produces light

Colored Pencil Corrections Al(NO3)3 + NaOH = Al(OH)3 + NaNO3 KClO3 = KCl + O2 H3PO4 + Mg(OH)2 = Mg3(PO4)2 + H2O NH4NO2 = N2 + H2O BaCl2 + Na2SO4 = NaCl + BaSO4 Fe2O3 + CO = Fe + CO2 Mg(OH)2 + (NH4)3PO4 = Mg3(PO4)2 + NH3 + H2O