Your SlideShare is downloading. ×
0
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Chapter 19.1: Oxidation and Reduction
Upcoming SlideShare
Loading in...5
×

Thanks for flagging this SlideShare!

Oops! An error has occurred.

×
Saving this for later? Get the SlideShare app to save on your phone or tablet. Read anywhere, anytime – even offline.
Text the download link to your phone
Standard text messaging rates apply

Chapter 19.1: Oxidation and Reduction

2,633

Published on

Published in: Education, Technology, Business
0 Comments
0 Likes
Statistics
Notes
  • Be the first to comment

  • Be the first to like this

No Downloads
Views
Total Views
2,633
On Slideshare
0
From Embeds
0
Number of Embeds
1
Actions
Shares
0
Downloads
84
Comments
0
Likes
0
Embeds 0
No embeds

Report content
Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
No notes for slide

Transcript

  • 1. Chapter 19.1
  • 2. 1. Assign oxidation numbers to reactant and product species. 2. Define oxidation and reduction. 3. Explain what an oxidation-reduction reaction (redox reaction) is.
  • 3. • The oxidation number assigned to an element in a molecule is based on the distribution of electrons in that molecule. • The rules by which oxidation numbers are assigned are summarized on the next slide. chromium (II) chloride chromium (III) chloride potassium chromate potassium dichromate
  • 4. • Reactions in which the atoms or ions of an element experience an increase in oxidation state are oxidation processes. • A species whose oxidation number increases is oxidized.
  • 5. • Reactions in which the oxidation state of an element decreases are reduction processes. • A species that undergoes a decrease in oxidation state is reduced. Aluminum from Aluminum Oxide Tungsten from Tungsten Oxide
  • 6. • Any chemical process in which elements undergo changes in oxidation number is an oxidation- reduction reaction. • This name is often shortened to redox reaction. • The part of the reaction involving oxidation or reduction alone can be written as a half-reaction.
  • 7. • Equations for the reaction between nitric acid and copper illustrate the relationship between half- reactions and the overall redox reaction. 2+ +20 Cu Cu + 2e – +5 2 +1 +4 2 +1 + 23 2 22NO + 2 + 4H 2NO + 2H Oe  – – – – – +5 + 2+ 3 2 +20 +4 2Cu + 2NO + 4H Cu + 2NO + 2H O– (oxidation half-reaction) (reduction half-reaction) (redox reaction)
  • 8. • When hydrogen burns in chlorine, a covalent bond forms from the sharing of two electrons. • The pair of electrons is more strongly attracted to the chlorine atom because of its higher electronegativity. 2 2 0 0 +1 1 H + Cl 2HCl – • Neither atom has totally lost or totally gained any electrons. • Hydrogen has donated a share of its bonding electron to the chlorine but has not completely transferred that electron.

×