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Chemistry: Form WS10.1.2A. Name. REDOX AND ELECTROCHEMISTRY. Date. Period _____. Analyzing Oxidation-Reduction Reactions. When chemical bonds form 





03 WS10-1-2 Analyzing Oxidation-Reduction Reactionspdf

Chemistry : Form WS10 1 2AName REDOX AND ELECTROCHEMISTRYDate Period _____ Analyzing Oxidation-Reduction Reactions When chemical bonds form electrons are 



[PDF] Analyzing Oxidation-Reduction Reactions - Evans Chemistry Corner

Chemistry: Form WS10 1 2A Name REDOX AND ELECTROCHEMISTRY When chemical bonds form electrons are either lost gained or shared Metals



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[PDF] Form WS1014A ELECTROCHEMISTRY Name Date Period Redox

Redox equations are often too complex to balance by inspection alone Instead they are balanced by the half-reaction method or ion-electron method

  • What is a redox reaction answers?

    An oxidation-reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron.

  • How is redox reaction connected to electrochemistry?

    Broadly speaking, electrochemistry looks at the interactions between electricity and chemical reactions. The chemical reaction that takes place in an electrochemical reaction causes electrons to move from one side to another, known as redox reactions.

  • Is redox reaction part of electrochemistry?

    Electrochemistry is the interchange of chemical and electrical energy. The key to electrochemistry is a redox reaction. This unique type of reaction produces a flow of electrons that can be used to do work like light a flashlight bulb or perhaps your favorite…
  • Redox (reduction–oxidation, /?r?d?ks/ RED-oks, /?ri?d?ks/ REE-doks) is a type of chemical reaction in which the oxidation states of substrate change. Oxidation is the loss of electrons or an increase in the oxidation state, while reduction is the gain of electrons or a decrease in the oxidation state.
C:Documents and SettingsEvanDesktopChemistryChemistry Go on to the next page.)Chemistry: Form WS10.1.2A Name ______________________________ REDOX AND ELECTROCHEMISTRY Date _________________ Period _____

Analyzing Oxidation-Reduction Reactions

When chemical bonds form, electrons are either lost, gained or shared. Metals lose electrons. This is what happens when iron rusts. When the iron, a metal, combines with oxygen, a non metal, to form rust, it loses electrons. This process is called oxidation even when the nonmetal is not oxygen. Nonmetals gain electrons causing their oxidation states to go down. This is called reduction. It is possible to tell what was oxidized and what was reduced in a chemical reaction by checking the oxidation states of the elements before and after the reaction. The element that has an increase in oxidation state was oxidized while the one that has a decrease in oxidation state was reduced.Example2FeCl + Cl 2FeCl

Iron was oxidized

Chlorine was reduced

For each of the examples below, determine the oxidation states of the elements on both sides of the equation.

Then determine which element was oxidized and wh

ich was reduced. Write your answer in the space provided.

Reaction Element:

Oxidized Reduced

Example: Cu + 2AgNO3

Cu(NO + 2Ag

0 +1 +5 -2 +2 +5 -2 0

Cu + 2AgNO

Cu(NO + 2AgCu Ag

1. 2Mg + O

2MgO

2. Zn + 2HCl ZnCl

+ H 3. Fe + 3CO 2Fe + 3CO 4. 2K + 2H

O + 3S 4KOH + 2Cr

+ 3SO Chemistry: Form WS10.1.2AAnalyzing Oxidation-Reduction Reactions

REDOX AND ELECTROCHEMISTRY Page 2

Reaction Element:

Oxidized Reduced

© Evan P. Silberstein, 2003

5. 2H O + O

6. 2KClO

2KCl + 3O

7. 4NaOH + Ca(OH)

+ C + 4ClO

4NaClO

+ CaCO + 3H

8. 3P + 5HNO

+ 2H

O 5NO + 3H

9. 3Cu + 8HNO

2NO + 3Cu(NO

+ 4H

10. 2PbSO

+ 2H

O PbO

+ Pb + 2H

11. 4HCl + MnO

MnCl + 2H

O + Cl

12. 4NH

+ 5O

4NO + 6H

13. 16HCl + 2KMnO

O +2KCl + 2MnCl

+ 5Cl

14. Cu + 2H

CuSO +SO + H

15. 8HNO

+ 6KI 6KNO + 3I + 2NO + 4H 16. I + 5HClO + H

O 2HIO

+ 5HCl 17. K + 3SnCl + 14HCl 2CrCl + 3SnCl + 2KCl + 7H

18. SnCl

+ 2HgCl SnCl + Hgquotesdbs_dbs7.pdfusesText_5
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