chapter 2: redox reactions

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UNIT 1: CHEMISTRY

Chapter 2: Redox Reactions

NAME:____________________

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Learning Objectives: Chemistry MAJOR CONCEPT #1: Ch.1 - Aqueous Solutions

I CAN…

o Explain how dissolving substances in water is often required for chemical reactions

o Differentiate between electrolytes and non-electrolytes using properties

o Compare, explain and calculate concentration in the following ways: -‐ Molar concentration (mol/L) -‐ Parts per million (ppm) -‐ Percent Volume (%V/V)

o Calculate volumes needed in a dilution using the formula C1V1 = C2V2

MAJOR CONCEPT #2: Ch.2 - Redox Reactions

I CAN…

o Balance single replacement reaction equations; use to predict moles of product & reactants

o Determine the reactivity of metals by comparing their reaction in various aqueous solutions

o Apply mole ratios to predict moles of metals consumed or produced in redox reactions

o Define oxidation and reduction using electron gain or loss

o Define spontaneous and non-spontaneous reactions and explain how each uses/makes electricity

o Use half-reactions to explain and construct/draw voltaic cells

o Identify the anode, cathode, oxidation, reduction, and electron flow on a sketch of Voltaic and Electrolytic cells

o Compare modern and traditional methods for extraction of metals and for protection from corrosion

MAJOR CONCEPT #3: Ch.3 - Organic Chemistry

I CAN…

o Identify materials used in daily life from petrochemicals (e.g., plastics, cosmetics, gasoline)

o Identify the physical characteristics of hydrocarbons (melting point, boiling point, solubility of alkanes, alkenes, alkynes)

o Name simple hydrocarbons (alkanes, alkenes, & alkynes) using IUPAC naming rules

o Draw structural formulas for simple hydrocarbons (alkanes, alkenes, & alkynes)

o Identify hydrocarbons as the source of fossil fuels

o Explain the process of fractional distillation and catalytic cracking

o Classify, balance, and apply mole ratios to hydrocarbon reactions -‐ combustion -‐ catalytic cracking of ethene (production of ethane) -‐ hydrogenation of alkenes to produce alkanes (saturated & non-saturated fats) -‐ polymerization of ethane (ethane to polyethene)

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Learning Objectives:1) balance provided single-replacement reaction equations, building on knowledge from Science 10 Chemistry Unit.

2) relate single-replacement reactions to oxidation-reduction and apply mole ratios from given equations to predict moles of metals consumed or produced

What are "Single Replacement Reactions"

Ch 2.1 “Balancing Reactions & Mole Ratio”

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Gizmo: Balancing Chemical Equations


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Mole Ratio

(formula on page 10 of Data Booklet)


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1)

2) Determine the Mole Ratio

3)


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Video "Time Lapse Rust"

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Practice Questions (p.68 #5-7):


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9

1

Fe2O3why are first nation's rockpaintings usually red?

(pp.69-75)

Read p. 69-70 on how Copper metal is produced

Learning Objectives:

1) determine the reactivity of metals by comparing their reaction in various aqueous solutions.

2) define oxidation and reduction and spontaneous and nonspontaneous reactions

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(p.70)

Ch 2.2 “Gain & Loss of Electrons” (Intro)

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AnswersUse the Periodic Table to complete the above table.

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11

5

(p.72)

6

(p.73)


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7

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13

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(p.74)

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-have a reduction 1/2 reaction and an oxidation 1/2 reaction


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(p.75)


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12#10#31&

1&

•  Recall the reaction:

CuCl2(aq) + Al(s) ! AlCl3(aq)&&&&&&&+&&&&&&&Cu(s)&3 2 2 3 •  The aluminum is more reactive than the copper, so it is able to �steal away� the chloride ions from the copper. •  The aluminum is reactive because is unstable.

The Reactivity Series: •  By doing experiments scientists have ranked the reactivity of many metals and their ions.

Ch 2.3 “Reactivity of Metals”

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12#10#31&

2&

MORE%REACTIVE%ATO

MS%M

ORE

%REA

CTIVE%IONS%

•  The more reactive a metal is, the less reactive its ion is.

Read left-to-right: it�s a(n) _________ reaction

Read right-to-left: it�s a(n) _________ reaction

Li(s) " e- + Li+(aq)


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12#10#31&

3&

• You can use the Activity Series to predict if whether or not a spontaneous reaction will occur. (i.e. a reaction that occurs on its own with no extra energy added.)

e.g. #1. A piece of zinc metal is placed in a solution containing Cu2+

(aq) ions. Will

spontaneous reaction occur?

Zn + Cu+ ! ??

Yes, a spontaneous reaction will occur.

E.g. #1 con�t: The half reactions: Cu2+ + 2e- ! Cu Zn ! Zn2+ + 2e- Combined:


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12#10#31&

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e.g.$#2.$A$piece$of$gold$jewelry$is$dipped$into$a$solu8on$containing$in$H+(aq)$ions.$Will$

spontaneous$reac8on$occur?$

Au + H+ ! ??

Practice: P. 82 Q28, 29 More Practice: P. 83 Q31, 32


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"The Busy Electron" (video)


1) Use half-reactions to explain and construct/draw voltaic cells

2) Identify the anode, cathode, oxidation, reduction, and electron flow on a sketch of Voltaic and Electrolytic cells

(p.88 in textbook)

Ch 2.4 “Voltaic Cells”

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(p.89 in textbook)

The Lowest Electrode on the rightwill be Oxidized [Anode]


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Which has a non-spontaneous chemical reaction?

Video: Electrolysis of Water


1) Define spontaneous and non-spontaneous reactions and explain how each uses/makes electricity

Ch 2.5 “Electrolytic Cells”

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1) Protecting from Corrosion

-Electroplating a metal can increase the life span of the consumer good without having to actually make the entire object out of an expensive metal. (e.g,. gold plated)

2) Electrical Connections

- Stereo equipment is gold plated - conducts electricity well & does not corrode

3) Purify metals

-blister copper (97-99% pure is purified to 99.99% for copper wires)

4) Produce Non-metals

-e.g., chlorine gas produced from NaCl (table salt)

5) Recharging Batteries (voltaic cells)

Uses of Electrolytic Cells:


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chapter 2: redox reactions

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