{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Chapter 18 Lecture 1

Chapter 18 Lecture 1 - Chapter 18 Lecture 1...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
Chapter 18 Lecture 1 Electrochemistry: DP’s Favorite (As usual, DP holds the minority opinion) Oxidation – Reduction Reactions How do we ID? Look for changes in oxidation numbers on individual atoms. From Chem 1: Memorize the charges on the ions. For monatomic ions the charge is the oxidation number for the atom: Br - , S 2 - , Al 3+ , Fe 2+ , …. etc. Oxidation number for elements is zero: N 2 (g), O 2 (g), As(s) , Cu(s), C(s) For polyatomic ions you figure them out from knowing that Oxide is 2 - , and the charge on the ion Cl - ClO - ClO 2 - ClO 3 - CrO 4 2 - Cr 2 O 7 2 - S 2 O 3 2 - SO 4 2 - If an oxidation number for an atom changes between products and reactants then a oxidation-reduction reaction has occurred.
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Which of the following is an oxidation reduction reaction? AgNO 3 + KI AgI + KNO 3 KClO + 3KI + 2H + KI 3 + KCl + H 2 O + 2K + Oxidation reduction 1) After identifying what is oxidized and reduced, divide the reaction in to two half-reactions 2) Balance all of the atoms but oxygen and hydrogen
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

Page1 / 5

Chapter 18 Lecture 1 - Chapter 18 Lecture 1...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon bookmark
Ask a homework question - tutors are online