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Activity Series & Redox. Metal Reactivity Lab Results. 1. What metal is the most reactive? How do you know?. 2. What metal is the least reactive? How do you know?. 3. Which metal would most likely be found in elemental form in nature? (not in a compound, but just as an element).

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metal reactivity lab results
Metal Reactivity Lab Results

1.What metal is the most reactive? How do you know?

2. What metal is the least reactive? How do you know?

3. Which metal would most likely be found in elemental form in nature? (not in a compound, but just as an element)

4. Design an activity series with these 4 metals. Put the most reactive metal at the top and the least reactive on the bottom

activity series1

Li+!!

Activity Series

p. 121

Which is the most active – Li+ or Au+?

slide5

Yes it reacts

Will a reaction occur between Li & AuCl?

  • For a reaction to occur the pure metal must be higher on the series (more reactive) than the metal in the compound

Au

What is the metal in AuCl?

Is Li+ more reactive than Au+?

Li + AuCl LiCl + Au

which of the following reactions will occur
Which of the following reactions will occur?
  • Al + AgNO3 -->
  • NaCl + Ca-->
  • KBr + Zn -->
  • Li + AgNO3 -->

Is the free element above the element in the compound?

Al(NO3)3 + Ag

Yes

CaCl2 + Na

Yes

No – no reaction

LiNO3 + Ag

Yes

p. 121

reduction making something smaller from ore to pure element

CuS2

Reduction– making something smaller – from ore to pure element.
  • gain of e- gives ion a reduced charge
  • EX: Chlorine (Cl) = 17p+ & 17e-
  • Gains 1 e-… What happens to the chg #? Bigger or smaller?
  • Chloride (Cl-)= 17p+ & 18e- = -1 charge

Example: Formation of pure Cu Metal

Cu 2+ + 2 e- Cu

copper II electrons copper

ion (ore) metal

Where would you find a Cu2+?

oxidation
Oxidation
  • Loss of e- results in ion left with more protons (+ charge)
  • Ex: Copper = 29p+ & 29e-
  • Copper II = 29p+ & 27e- = +2 charge

Formation of Copper II ions

Cu Cu 2+ + 2 e-

copper copper II electrons

metal ion

Which copper is in a compound?

Which is the pure copper?

If metal chemically combines with oxygen, can it remain neutral?

oxidation reduction
Oxidation / Reduction
  • Redox – electrons lost by one element are gained by another
  • ALWAYS happen together!
  • OIL RIG
  • Oxidation is Losing
  • Reduction is Gaining
identify what is being oxidized and reduced

+

2+

Identify what is being oxidized and reduced.

3+

1-

0

1+

1-

0

  • Al + AgNO3 --> Al(NO3)3 + Ag
  • Na + Ca--> Ca + Na

Al

Oxidized is loss of electrons = becomes more positive

Reduction is gain of electrons = # is reduced

Ag

When do elements have a charge?

Elements have a charge when in a compound.

Ca

Oxidized =

Reduced =

Na+

slide11

NO tutorials this Friday!

Tutorials will be Thursday

8:15am in D204

4:15pm in D219

  • Monday, October 24, 2005
  • WU: see OH
  • Check: Check: p109 #1,2,6,8,9,12-17
  • p.126 # 1,2,7,13-16
  • Notes on Redox in Mining & Refining
  • Redox! Where are the electrons? WS
    • (same as MM pp124-125)
  • HW: 1. p127 #9-12
  • 2. Study for Quiz on Wed over
  • Unit 2 Sec AB
redox in mining refining
Redox in Mining & Refining
  • Used to reduce metal cations in a compound to purify metal
  • Cu2S + Na  Cu + Na2S
  • Cu + + e- Cu
how geologists evaluate an ore p 113
How geologists evaluate an ore: (p. 113)
  • Percent of metal in ore !
  • Quantity of available ore
  • Type of mining & processing
  • Distance of mine to refining facility & markets
  • Supply and demand status
techniques used to reduce purify metals
Techniques used to reduce/purify metals
  • Electrometallurgy –use electric current to supply e-
  • Pyrometallurgy – heat causes rxn w/ CO2 which supplies e-
  • Hydrometallurgy – reactants in water solution supply e-
resources are limited
Resources are limited
  • Conservation-preserve, don’t use
  • Reuse-use again in same form
  • Recycle-break down, reform & use for something else
redox ws 1

Pt+2+ Cu

 Pt+ Cu+2

REDOX WS #1

Is pure element above element in cmpd?

  • Will rxn occur?
  • Draw e-dot

c. Reactant oxidized?

Reactant Reduced?

d. Oxidizing reagent?

Reducing Agent?

Yes

Pt+2

CuCharge decreased

Agents are opposite. They caused it to happen.

Pt+2

Cu