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Ch. 9: Lesson 2 -Intro to Redox Reactions-

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Ch. 9: Lesson 2 -Intro to Redox Reactions-. Brief Charge Reminder. Electrons have a charge Neutral atoms have an overall charge of Adding an e- makes charge go Removing an e- makes charge go. Oxidation and Reduction.

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slide1
Ch. 9: Lesson 2

-Intro to Redox Reactions-

brief charge reminder
Brief Charge Reminder
  • Electrons have a charge
  • Neutral atoms have an overall charge of
    • Adding an e- makes charge go
    • Removing an e- makes charge go
oxidation and reduction
Oxidation and Reduction
  • Reduction is a gain of electrons (charge is reduced)
  • Oxidation is a loss of electrons (charge is increased)
  • Ag  Ag = =
  • Cl  Cl = =

Equation with e-Process

+

-

slide4

Reduction reduces charge

  • Oxidation is just the other one
identifying what s oxidized and what s reduced
Identifying what’s oxidized and what’s reduced
  • First assign oxidation #’s, then see how they change from start to finish

Ex: C + H2O  CO + H2

oxidation reduction practice
Oxidation/Reduction Practice

MnO2 + 4 HCl  MnCl2 + Cl2 + 2 H2O

redox reactions
Redox Reactions
  • Redox reactions involve REDuction and OXidation
  • SAT Word Alert: PORTMANTEAU

-THIS MEANS-

  • Both have to happen at the same time
remembering how redox works
Remembering How Redox Works
  • LEO says GER:
    • Losing e- is
    • Gaining e- is
  • OIL RIG
    • Oxidation is e-
    • Reduction is e-
conclusion questions
Conclusion Questions
  • For Now: Review book page 162, # 11-15, on back of paper slips to hand in before you leave
  • For HW: same page, #16-25, in notebooks
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Ch. 9: Lesson 3

-Recognizing Redox Reactions & Their Parts-

3 forms of redox reactions
3 Forms of Redox Reactions
  • A + B  AB
    • Ex: 2 H2 + O2 2 H2O
  • AB  A + B
    • Ex: 2 NaCl  2 Na + Cl2
  • A + BC  AC + B
    • Ex: Zn + Cu(NO3)2 Zn(NO3)2 + Cu
recognizing redox reactions
Recognizing Redox Reactions
  • 1. Single element(s) on either side of the equation

2 Li + Zn(NO3)2 2 Li(NO3) + Zn

  • 2. Elements change oxidation # from reactant to product
  • 2 K + Cl2 2 KCl
    • Increasing ox # means e- , was
    • Decreasing ox# means e- , was
agents
Agents
  • Reducing agents cause something else to be reduced, but get oxidized themselves
  • Oxidizing agents cause something else to be oxidized, but get reduced themselves

2 Sr + O2 2 SrO

Reduced: Oxidized:

Reducing agent: Oxidizing agent:

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Ox:

Rd:

OxAg:

RdAg:

Ox:

Rd:

OxAg:

RdAg:

Ox:

Rd:

OxAg:

RdAg:

2 Cs + Br2 2 CsBr

3 Mg + N2 Mg3N2

4 Fe + 3 O2 2 Fe2O3

spectator ions
Spectator Ions
  • Spectators are atoms or ions without a charge change, just along for the ride

Cu + 2 AgNO3 Cu(NO3)2 + 2 Ag

labeling things in equations
Labeling Things In Equations

Cu + 2 AgNO3 Cu(NO3)2 + 2 Ag

  • Make sure equation is balanced, find ox# for each species
  • What is being oxidized?
  • What is being reduced?
  • What is the oxidizing agent?
  • What is the reducing agent?

Any spectator ions?

labeling things in equations1
Labeling Things In Equations

Zn + 2 HCl  ZnCl2 + H2

  • Make sure equation is balanced, find ox# for each species
  • What is being oxidized?
  • What is being reduced?
  • What is the oxidizing agent?
  • What is the reducing agent?

Any spectator ions?

labeling things in equations2
Labeling Things In Equations

NaCl + AgNO3 AgCl + NaNO3

  • Make sure equation is balanced, find ox# for each species
  • What is being oxidized?
  • What is being reduced?
  • What is the oxidizing agent?
  • What is the reducing agent?

This is double replacement.

Double replacement’s are

not redox reactions.

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