A community for students.

Here's the question you clicked on:

55 members online
  • 0 replying
  • 0 viewing


  • one year ago

Answer check

  • This Question is Closed
  1. Ciarán95
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    Everything you've said above seems to be correct @Itsokay - The oxygen goes from a 0 oxidation state in the reactants (on the left) to -2 in both of the products (on the right). So, its oxidation number has decreased, meaning it must have gained electrons. Memory Tip: Oxidation is Loss (of electrons), Reduction is Gain (of electrons) (OIL RIG) So, O has been reduced. If something has been reduced, then another species in the reaction must have been oxidised (loss of electrons). Can you spot what that is? (Hint: Oxygen will nearly always have an oxidation state of -2 when bonded to a less electronegative element, except in the case of H2O2).

  2. Not the answer you are looking for?
    Search for more explanations.

    • Attachments:

Ask your own question

Sign Up
Find more explanations on OpenStudy
Privacy Policy

Your question is ready. Sign up for free to start getting answers.

spraguer (Moderator)
5 → View Detailed Profile

is replying to Can someone tell me what button the professor is hitting...


  • Teamwork 19 Teammate
  • Problem Solving 19 Hero
  • You have blocked this person.
  • ✔ You're a fan Checking fan status...

Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.

This is the testimonial you wrote.
You haven't written a testimonial for Owlfred.