A community for students.

Here's the question you clicked on:

55 members online
  • 0 replying
  • 0 viewing

Photon336

  • one year ago

@rushwr

  • This Question is Closed
  1. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    @Woodward we will need u here lol

  2. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    \[Ca(s) + Cl_{2}(g) --> CaCl_{2}\] Which of the following is true concerning this reaction? Ca is an oxidizing agent Cl2 is the reducing agent Cl2 is an oxidizing agent CaCl2 is an oxidizing agent.

  3. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    I guess CL2 is an oxidising agent

  4. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    Ca goes from +0 to +2 oxidation state goes up so Calcium loses electrons. oxidized Cl goes from 0 to -1 it gains electrons so it's reduced. Oxidizing agent = what causes the other to be oxidized but is reduced itself. Cl2 is an oxidizing agent, because it's reduced causes the other to be oxidized

  5. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    Oxidising agents are the ones that reduce themselves to oxidise some other species. Here Cl2 has gone from 0 oxidation state to -2 oxidation state whereas Ca has gone from 0 to +2. So we can see that Cl has reduced while Ca is oxidised.

  6. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    That is the answer

  7. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    Awesome so what's next !!!!

  8. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    @Woodward @Rushwr could someone explain this to me?

  9. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    \[Cl_{2}(g) +2e --> 2Cl ^{-}\] \[E^(0)\] = +1.36V how does this compare with the other halogens?

  10. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    A) F2 > Cl2 = Br2 > I2 B) F2 = Cl2 > Br2 > I2 C) f2 > Cl2 > Br2 > I2 D) F2<Cl2>Br2>I2

  11. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    I think it's C

  12. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    why?

  13. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    I don't know myself

  14. anonymous
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 0

    Yeah that's what I'm thinking too since their ionic radii are smaller they're able to better hold the charge closer so it takes more energy to ionize them. After all, the highest occupied molecular orbital of \(X_2\) (X is a halogen) will be larger in energy the further you go down the table, so the valence electrons of \(I_2\) are higher energy than \(F_2\) so you don't need to spend as much energy to remove them.

  15. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    @Woodward you're essentially saying that because the radii are smaller, the electrons are more tightly held. so when you move down, a group, the number of shells goes up, the electrons are farther from nucleus and easier to move requiring less energy.

  16. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    Okai I actually didn't know this. but what I thought was When going up an electrochemical series E 0 decreases right? The top elements in the electrochemical cells are having a higher reducing ability. But when going down the series the Eo increases thus the reducing ability is reduced. So the oxidising ability increases. So I arranged it in that order

  17. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    What does this have to do with the E cell though?

  18. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    @Woodward Do u think I'm right ?

  19. anonymous
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 0

    I think @Rushwr is more right in her reasoning than me, I am kind of not sure about the electrical cell stuff, and this is what this question is from. I honestly don't know. But the reason I made that talk about energy is because voltage has units of Energy per Charge. so often times they'll use electron charge * volts to record energy of ionization of electrons.

  20. anonymous
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 0

    Now that I think of it, I don't remember how the sign convention works so idk if they increase or decrease or what haha.

  21. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    right, @Rushwr can you explain the higher reducing ability again? how you would organize that, i'm curious

  22. anonymous
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 0

    I'm gonna read through this, come back here and tell you what I find, probably just going to say, "Yeah I agree with her!" hopefully haha XD

  23. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    You mean as in the ability to cause another substance, as in oxidizing agent, or or the element itself being oxidized as in it's own tendency to lose electrons?

  24. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    Metals at the top of the series are good at giving away electrons. They are good reducing agents. The reducing ability of the metal increases as you go up the series. Elements at the bottom of the series are good at picking up electrons. They are good oxidising agents. The oxidising ability increases as you go down the series.

  25. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    if they are good at giving away their electrons, they are much better reducing agents. okay so as you go to the top reducing ability also goes up. so as you go down the series the metals become better at accepting electrons. |dw:1442549317764:dw|

  26. Photon336
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 1

    it's been a while haha

  27. Rushwr
    • one year ago
    Best Response
    You've already chosen the best response.
    Medals 2

    yep

  28. 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...

23

  • 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.