April 25, 2024, 01:30:02 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Another hard electro-chemistry question  (Read 2929 times)

0 Members and 1 Guest are viewing this topic.

Offline s3a

  • Regular Member
  • ***
  • Posts: 63
  • Mole Snacks: +0/-0
Another hard electro-chemistry question
« on: May 13, 2009, 08:49:49 PM »
I have no idea how to do this since I am used to substances being written down twice, once in normal form and the second time in ionic form. When written that way, I can determine what is being oxidized or reduced but here I can't determine anything! Please *delete me*
Logged

Offline Train

  • Regular Member
  • ***
  • Posts: 68
  • Mole Snacks: +2/-0
Re: Another hard electro-chemistry question
« Reply #1 on: May 14, 2009, 01:08:21 AM »
The solid silver and aluminum have oxidation states of 0.  What are their oxidation states in the sulfides?  Do metals usually have positive or negative oxidation states?
Logged

Offline s3a

  • Regular Member
  • ***
  • Posts: 63
  • Mole Snacks: +0/-0
Re: Another hard electro-chemistry question
« Reply #2 on: May 14, 2009, 07:56:51 PM »
How do you determine oxidation states? I don't know the answer to either of your questions. All I know is electrons are gained when a substance is being reduced and lost when a substance is being oxidized.
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27663
  • Mole Snacks: +1801/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Another hard electro-chemistry question
« Reply #3 on: May 15, 2009, 02:54:30 AM »
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info
Pages: [1]   Go Up
« previous next »
Sponsored Links