as you come in, materials: paper, periodic table, and pencil for the test plan: complete the unit...

As you come in,Materials:

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

Read a description of the reaction

Note what is reacted with whatNote what is yielded or producedWrite formulas for each

compoundUse + 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 1:Combustion of H2 gas•Description: Hydrogen gas burns in oxygen gas to produce water vapor.•Unbalanced equation:

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

Write the skeleton equation. BE SURE THE

FORMULAS ARE WRITTEN CORRECTLY.

Inventory reactantsInventory productsInsert coefficients to make

atoms of each element equal on both sides of the equation

Reduce the coefficients if possible

Video Example 1:Combustion of H2 gas•Unbalanced equation:

H2 + O2 H2O•Balanced equation:

Video Example 2:Combustion of methane

gas•Unbalanced equation:CH4 + O2 CO2 + H2O•Balanced equation:

Guided ExampleSodium 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

WORK WITH A PARTNER TO WRITE AND BALANCE

EQUATIONS.

Writing Equations from Word Equations

handout

• Take 10 minutes to write and balance as many as possible.

• Use a colored pencil or pen to correct your mistakes.

Writing & Balancing Equations

1. Zn + Pb(NO3)2 --> Zn(NO3)2 + Pb

2. 2 AlBr3 + 3 Cl2 --> 2 AlCl3 + 3 Br2

3. 2 Na3PO4 + 3 CaCl2 --> Ca3(PO4)2 + 6 NaCl

4. 2 K + Cl2 --> 2 KCl

5. 2 Al + 6 HCl --> 2 AlCl3 + 3 H2

6. 3 Ca(OH)2 + 2 H3PO4 --> Ca3(PO4)2 + 6 H2O

7. Cu + 2 H2SO4 --> CuSO4 + 2 H2O + SO2

8. 2 H2 + 2 NO --> 2 H2O + N2

aAs you come in, 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


DUE TOMORROW– Predicting Products note-taking guide

Practice balancing equations for tomorrow’s quiz!

Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur

dioxide.

Difficult Equations to Balance

Cu + 2 H2SO4 --> CuSO4 + 2 H2O + SO2

5 Types of Chemical Reactions

Synthesis A + B ABCombustion CxHy + O2 CO2 + H2ODecomposition AB A + BDouble-Replacement AX + BY AY + BXSingle-Replacement A + BX B + AX

Five Types of Reactions Clip

Identify the Type of Reaction

1. Zn + Pb(NO3)2 --> Zn(NO3)2 + Pb

2. 2KClO3 2KCl +3 O2

3. 2 AlBr3 + 3 Cl2 --> 2 AlCl3 + 3 Br2

4. 2 Na3PO4 + 3 CaCl2 --> Ca3(PO4)2 + 6 NaCl

5. 2 K + Cl2 --> 2 KCl

6. 2 Al + 6 HCl --> 2 AlCl3 + 3 H2

7. CH4 + 2O2 CO2 + 2H2O

8. 3 Ca(OH)2 + 2 H3PO4 --> Ca3(PO4)2 + 6 H2O

Single Replacement ReactionsSPECIAL! MORE TO COME!

A + BX --> AX + BA 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

• Take 10 minutes to identify types and write as many as possible.


WORK WITH A PARTNER TO BALANCE THE EQUATIONS. YOUR QUIZ WILL BE SIMILAR

TO THIS TOMORROW.

“Balancing Chemical Equations” handout

• Take 10 minutes to balance as many as possible.



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


DUE MONDAY– Net Ionic Equations note-taking guide Practice identifying the types reactions for Monday’s quiz!

WRITE, BALANCE, AND IDENTIFY THE TYPE OF REACTION FOR THE FOLLOWING ON YOUR “LONG

WORKSHEET”#26-#50

(AS MANY AS YOU CAN)

AFTER YOUR QUIZ

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

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 nitrateReactant formulas: •K2CrO4 + AgNO3 [TIP: Label each element with its charge]Unbalanced Equation: •K2CrO4 + AgNO3 KNO3 + Ag2CrO4

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


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?

Predicting Products & States of Matter for SINGLE REPLACEMENT

REACTIONS Tips to remember:

A + BX CONSULT ACTIVITY SERIES TO BEGIN!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 nitrateReactant formulas: •K + AgNO3 [TIP: Label each element with its charge]

Unbalanced Equation: •K + AgNO3 KNO3 + Ag


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

FOR EACH REACTION:•PREDICT THE PRODUCTS.•WRITE A BALANCED EQUATION.•LIST AS MANY OBSERVATIONS AS POSSIBLE DURING THE REACTION.

DISCOVERING INDICATORS OF A

CHEMICAL REACTION LAB

Reactions in Aqueous Solution

MANY reactions occur in water: More than 70% of earth

is covered by water 66% of the human body

is waterMany 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


52. 2Al(s) + 6HCl(aq) 2AlCl3(aq) + 3H2(g)

56.ZnCl2 + (NH4)2S 2NH4Cl + ZnS


56.ZnCl2 (aq)+ (NH4)2S(aq) 2NH4Cl(aq) + ZnS(s)

59. HgSO4 + 2NH4NO3 Hg(NO3)2 + (NH4)2SO4


59. HgSO4(aq) + 2NH4NO3(aq) Hg(NO3)2(aq) + (NH4)2SO4(aq)

60. Fe + CuSO4 FeSO4 + Cu


60. Fe (s)+ CuSO4 (aq) FeSO4 (aq) + Cu (s)

67. Br2 + 2NaI 2NaBr + I2


67. Br2 (l) + 2NaI(aq) 2NaBr (aq) + I2 (g)

Evidence of a Chemical Reaction

1. Formation of a gas Bubbles Smell

2. Formation of a solid (precipitate) from two aqueous solutions; often solids are colorful

“Snow globe” effect “Paint” look “Jello” consistency

3. Change in temperature Test tube feels colder to you (endothermic

reaction) Test tube feels warmer to you (exothermic

reaction)4. 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

as you come in, materials: paper, periodic table, and pencil for the test plan: complete the unit...

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