Chem CatalystHow is an ion formed?

Today’s Agenda:1. Do Now2. Intro: New Chapter3. Notes- Oxidation & Reduction4. Practice Worksheet

New Topic: ElectrochemistryChapter 20 (and some Chapter 21)- Oxidation and Reduction- Writing Redox Reactions- Voltaic cells/batteries

Oxidation Reactions- Originally defined as combining

the element with oxygen- Now defined as loss of electrons

(shift of electrons away from an atom)

- Charge becomes more positive (increases)

Reduction Reactions- Originally defined as removing oxygen

from a compound with the element- Now defined as gain of electrons (shift

of electrons toward an atom)- Charge becomes more negative (charge

decreases)- Occurs alongside an oxidation reaction

Redox Reactions- A reaction that includes oxidation and

reduction- The substance that gains electrons is

reduced- The substance that loses electrons is

oxidized

- “LEO the lion goes GER”- Losing Electrons is Oxidation; Gaining

Electrons is Reduction

Redox Reactions: PracticeIdentify the element being reduced and the element

being oxidized:Hint: break apart the ionic compounds

2AgNO3 + Cu Cu(NO3)2 + 2Ag

*Identify the oxidizing agent and the reducing agent

Redox Reactions: PracticeIdentify the element being reduced and the

element being oxidized:

2Na + Br2 2NaBr

Applications of Redox:- Some metals (gold, platinum) are not easily

oxidized- Iron is oxidized by oxygen, causing corrosion- Can be coated w/ aluminum, whose oxide does

not corrode- Connect to an easily oxidized metal (zinc,

magnesium) which will transfer electrons to iron