Chem II: Block 10.14.14 Infinite Campus: Chemical Reactions Exam Replacement Labs (30pts.) Objectives: I can predict and simplify double replacement reactions

Chem II: Block 10.14.14Infinite Campus:• Chemical Reactions Exam• Replacement Labs (30pts.)Objectives:• I can predict and simplify double replacement

reactions.• I can distinguish between oxidation and reduction

reactions.• I can balance oxidation-reduction (Redox)

reactions.

Double Replacement Reactions

• Complete 4.24 problems.

Chem II Period: 10.30.14Infinite Campus Update:• Single Replacement Lab (12pts.)• Double Replacement Lab (14pts.)

Objectives:• Chemical Reaction Gallery Walk Completion• Distinguish between Aqueous Reactions

Chemical Reaction Gallery Walk:

• Assess peers work and document evidence of participation by recording answers on study guide.

Chemical Reaction Review

Solubility Ranges

• Soluble: > 0.1M concentration of solute dissolved in solution.

• Insoluble: < 0.0001M concentration of solute dissolved in solution.

• Slightly soluble: between 0.0001M and 0.1 M of solute dissolved in solution.

Double Replacement Reactions*Why is it ionic compounds differ in the degree of solubility with water? Use the image below to come up with an educated guess.

Aqueous Reactions

Aqueous Reactions are reactions that occur in solution. Aqueous Reactions: 1. Replacement Reactions2. Oxidation-Reduction (Redox) Reactions3. Acid-Base Reactions

*Distinguish between the three types of reactions above that occur in solution.

Oxidation Reduction Reactions

Oxidation Reduction Reactions•Also called Redox Reactions

•One reactant becomes oxidized (lose electrons) and one reactant becomes reduced (gains electrons).(spontaneous /non-spontaneous).

• Transfer of electrons from the oxidized reactant to the reduced reactant.

LEO goes GER

LEO: lose electron(s) oxidizedGER: gain electron(s) reduced

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Redox Reactions

Ex. 2Ca + O2 -----> 2CaO

How do you know which reactant is oxidized (LEO) and which reactant is reduced (REO) in a redox reaction?

Assigning oxidation numbers for elements in the reaction.

Oxidation Number Rules

1. For an atom that is not combined with any other kind of atom its oxidation number is zero.

Ex. Mg0, Fe0, H20 (all diatomic molecules)

2. A monatomic ion’s oxidation number is equal to its charge.

Ex. Mg2 = oxidation number is 2+ Cl1- = oxidation number is 1-


3. The sum of the oxidation number for all atoms in a compound (ionic or covalent) is zero.

Ex. H21O-2 = zero Ex. NaCl1- = zero

Oxidation Number Rules4. The oxidation number for oxygen in a compound is -2.

Ex. C4O22-

*Exceptions: a. peroxides (O2) 2- the oxidation number is -1

Ex. H2 1O2

1-

b. Bonded to F: oxidation number is positive (1+ or 2+)Ex. O1+F 1- F > O electronegativity

Electronegativity Values


5. Hydrogen:• When bonded to a non-metal it is 1+(most common)Ex. H1Cl1-

• When bonded to a metal it will be 1-. Ex. Mg2+H2

1

Oxidation Number Rules6. Polyatomic Ions:The sum of the oxidation numbers of all atoms in a

polyatomic ion has to equal the charge on that ion.

Ex. (Cl5O32-)1-

Oxidation Number Rules7. In covalent compounds that do not contain

hydrogen or oxygen, the most electronegative element has an oxidation number equal to its charge as an ion.

Ex. P5Cl51-

, Cl> P with electronegativity

Electronegativity Values

Chem II: Block 10.15.14Infinite Campus:• Chemical Reactions Exam• Replacement LabsDue: • Element’s Oxdiation #s: qts. 4.49; 4.50 from textObjectives:• I can distinguish between oxidation and reduction

reactions using oxidations numbers. • I can balance oxidation-reduction (Redox) reactions.

Oxidation Numbers: qts. 4.49a. SO2

b. COCl2

c. (MnO4)- : Mn =7+ O = 2-

d. H(BrO): O = 2-; Br= -1; H = +1 *(BrO)1- =hypobromite ion

e. As4

f. K2O2 : O = 1- (peroxide ion); K= 1+

Oxidation Numbers: 4.50a.b.c.d.e.f.

Oxidation Numbers: AssessmentAssign an oxidation number for each element in the examples below: 1. H2

2. Cu3. Fe2O3

4. N2O5

5. H(NO3)

6. CCl4

8. Cr(CO3)

9. OF2

10. Ca(OH)2

Oxidation Numbers: AssessmentAssign an oxidation number for each element in the examples below: 1. H2

2. Cu3. Fe2O3

4. N2O5

5. H(NO3)

6. CCl4

8. Cr(CO3)

9. OF2

10. Ca(OH)2

Chem II: Block 10.16.14

Due: • Oxidation/Reduction Worksheet

Objectives:• I can distinguish between oxidation and reduction


Redox Reactions

Ex. 2Ca + O2 -----> 2CaO

a. Assign oxidation numbers for each element on on reactant and products side.

b. Identify and explain which element was reduced in this reaction.

c. Identify and explain which element was oxidized in this reaction.

Redox Reactions: Half Reactions

Ex. 2Ca + O2 -----> 2CaO

Half-Reactions: Separates/identifies the oxidized and reduced reactions that occur simultaneously in nature-why called Redox reactions.

Oxidized Reaction:

Reduced Reaction:


Due: • Redox Reaction Worksheet

Objectives:• I can distinguish between oxidation and reduction


Redox Reactions Practice Problems

1. Classify each half reaction as oxidation or reduction. a. Ba ----> Ba2+ + 2e-b. 2H1+ + 2e- -----> H2

2. Using oxidation numbers, predict if the reactions below are redox reactions.

a. Fe (s) + Cu(SO4) (aq) ----> Fe(SO4) (aq) + Cu (s)

b. NaCl (aq) + Ag(NO3) (aq) ---> Na(NO3) (aq) + AgCl (s)

Redox Reactions


Objectives:• I can classify reactions as redox reactions using oxidations

numbers. • I identify the redox half-reactions.• I can balance redox reactions.

Balancing Redox Reactions: Acidic Solutions

Cu (s) + NO3- (aq) ----> Cu2+ (aq) + NO2 (g)

a. Validate this is a redox reaction by using oxidation numbers to establish the half-reactions.


Redox Reactions: Half ReactionsGallery Walk

Redox Reactions Quiz

• Complete Redox Reaction Quiz


Infinite Campus:• Redox Reaction Quiz (20pts.)


numbers. • I can identify redox half-reactions. (oxidation/reduction)• I can balance redox reactions. (acidic/basic solutions)


Cu (s) + NO3- (aq) ----> Cu2+ (aq) + NO2 (g)

Balancing Redox Reactions• Assign oxidation numbers to identify half-reactions.• Balance each half reaction with the following steps: a. Balance all elements besides O and H.b. Balance O by adding H2O molecules

c. Balance H atoms by adding H+ ionsd. Balance charge by adding electrons so that the

charge on each side is equal.e. Make sure # of e- being lost = # of e- being gained.f. Add the two half-reactions together and cross out

substances that appear on both sides.

Balancing Redox Reactions• Assign oxidation numbers to identify half-reactions.• Balance each half reaction with the following steps: a. Balance all elements besides O and H.b. Balance O by adding H2O molecules

c. Balance H atoms by adding H+ ionsd. Balance charge by adding electrons so that the

charge on each side is equal.e. Make sure # of e- being lost = # of e- being gained.f. Add the two half-reactions together and cross out

substances that appear on both sides.





Redox Reactions: Gallery Walk

• Complete your redox reaction.• Observe two other redox reactions, checking

your peers answer.

Balancing Redox Reactions: Acid

H2O2 + KMnO4 + H2SO4 --> Mn(SO4) + O2 + H2O

Redox Reactions

Redox Reactions• Ag(NO3) + Cu -->

a. Predict Productsb. Assign Oxidation Numbers to validate if

redox reaction.c. If redox, identify and explain what is oxidized

and what is reduced.

Balancing Redox Reactions: Acidic

(Cr2O7)-2 (aq) + I- (aq)----> Cr3+ (aq) + (IO3 )- (aq)





Balancing Redox Reactions: Basic

NO2- (aq) + Al(s) -----> NH3 (aq) + Al(OH)4

- (aq)

Balancing Redox Reactions: Basic

Balancing Redox Reactions• Balance half reactions with peers via gallery

walk. • Self-assess peers work by making changes

where needed.• Record your answers on a separate sheet of

paper.

Balancing Redox Reactions: Acidic

(Cr2O7)-2 (aq) + I- (aq)----> Cr3+ (aq) + (IO3 )- (aq)



numbers. • I can identify redox half-reactions. (oxidation/reduction)• I can balance redox reactions. (acidic/basic solutions) (Redox Reaction Lab)

Homework:• Complete post-lab qts.

Redox Reaction Lab

Redox Titration Lab

http://www.webassign.net

Redox Titration LabH2O2 + KMnO4 + H2(SO4) Mn(SO4) + K2(SO4) + O2 + H2O

Pre-Lab:1. Practice reading and working stopper on Buret. (Measure out 15 mL of water 3xs from buret, validate

volume with graduated cylinder.

2. Complete pre-lab questions from lab



numbers. • I can identify redox half-reactions. (oxidation/reduction)• I can balance redox reactions. (acidic/basic solutions) (Redox Reaction Lab)

Homework:• Complete post-lab qts.

Redox Reaction LabH2O2 + K(MnO4) + H2(SO4) --> Mn(SO4) + K2(SO4) + O2 + H2O

Oxidized Element: O H2O2 -----> O2

Reduced Element: Mn (MnO4)1- -----> Mn2+

Balanced Equation?

Redox Reaction Lab

• At least get two trials completed. • Work on pre-lab qts. 5 and post-lab qts.



numbers. • I can identify redox half-reactions. (oxidation/reduction)• I can balance redox reactions. (acidic/basic solutions) (Redox Reaction Lab)• I can apply stoichiometry to balanced chemical equations.

Homework:• Stoichiometry Problems

Redox Reaction LabH2O2 + K(MnO4) + H2(SO4) --> Mn(SO4) + K2(SO4) + O2 + H2O



Balanced Equation?

Chem II: Block 10.29.14Objectives:• I can classify reactions as redox reactions using oxidations

numbers. • I can identify redox half-reactions. (oxidation/reduction)• I can balance redox reactions. (acidic/basic solutions) (Redox Reaction Lab pre/post lab qts.)• I can apply stoichiometry to balanced chemical equations. (Apply to Redox Reactions)Homework:• Stoichiometry Problems• Conclusion to Redox Lab• Redox with Stoichiometry Exam-Friday

Redox Reaction Lab

Redox Reaction Lab: Due Thursday

• pre/post lab qts. complete• Calculate percent error of H2O2 concentration

add to post-lab qts.• Establish a conclusion-paragraph format-addresses purpose of lab-analysis and accuracy of your data/class’s data-what did you learn from the lab-modification(s) if could repeat lab

Redox Reaction Lab: Due Thursday

• pre/post lab qts. complete• Calculate percent error of H2O2 concentration

add to post-lab qts.• Establish a conclusion-paragraph format-addresses purpose of lab-analysis and accuracy of your data/class’s data-what did you learn from the lab-modification(s) if could repeat lab

StoichiometryStoichiometry: • Converting between substances in a balanced

chemical equation using mole conversions.

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http://www.larapedia.com/chemistry_notes/Stoichiometry.html

Stoichiometry

www.larapedia.com

http://www.larapedia.com/chemistry_notes/Stoichiometry.html

Redox Reactions: Stoichiometry Applications

2 H2O + NO2- + 2Al(s) ----> NH4

+ + 2AlO2-

a. If we start with 3.8 moles of NO2- how

many moles of AlO2- could be produced?

b. If we want 13 grams of NH4+ ion, how many

grams of Al would we need to start with?

Redox Reactions: Percent Yield2 H2O + NO2

- + 2Al(s) ----> NH4+ + 2AlO2

-

a. If we start with 3.8 moles of NO2- how many

moles of AlO2- could be produced?

If 7.0 moles AlO2- was actually produced in the lab,

what would the percent yield be?

b. If we want 13 grams of NH4+ ion, how many grams

of Al would we need to start with?If 34.8 g of Al was actually produced in the lab, what

would the percent yield be?

Percent Yield

• Percent Yield: (Actual/Theoretical) x 100

Chem II: Block 10.30.14Due:• Stoichiometry ProblemsObjectives:• I can classify reactions as redox reactions using oxidations

numbers. • I can identify redox half-reactions. (oxidation/reduction)• I can balance redox reactions. (acidic/basic solutions) (Redox Reaction Lab pre/post lab qts.)• I can apply stoichiometry to balanced chemical equations. (Apply to Redox Reactions)Homework:• Redox Reactions and Stoichiometry Review

Redox Titration Lab ResultsLab Group Avg. volume

of KMnO4

% of H2O2 in Solution (Avg.)

% ErrorH2O2

1

2

3

4

5

Redox Reaction Lab: Extension ProblemH2O2 + K(MnO4) + H2(SO4) --> Mn(SO4) + K2(SO4) + O2 + H2O



Balanced Equation?

Redox Reaction Lab: Extension of Lab

Stoichiometry Worksheet

Stoichiometry: Limiting Reactants• Limiting Reactant:

• Excess Reactant:

en.wikipedia.org

Stoichiometry: Limiting Reactants• Limiting Reactant: completely consumed

• Excess Reactant: partially consumed

en.wikipedia.org

Stoichiometry: Limiting Reactant HCl + Mg -------> MgCl2 + H2

1. What type of reactions is this?2. Balance equation if needed.3. If 6.8 moles of Mg react with 7.5 moles of HCl which is

considered the limiting reactant? excess reactant?Reactants Have (moles) Need (moles)

Stoichiometry: Limiting Reactant 2HCl + Mg -------> MgCl2 + H2

1.If 6.8 moles of Mg react with 7.5 moles of HCl how many moles of MgCl2 can be produced?

Reactants Have (moles) Need (moles)

HCl (limited) 7.5 mol 13.6

Mg (excess) 6.8 mol 3.75

Documents

Chem II: Block 10.14.14 Infinite Campus: Chemical Reactions Exam Replacement Labs (30pts.) Objectives: I can predict and simplify double replacement reactions