Chemistry

Electron Transfer Theory
Write an label the oxidation and reduction half-reaction equations.
a) Ni(s) + Cu(NO3)2(aq) -> Cu(s)+ Ni(No3)2(aq)
oxidation - Ni(s) -> Ni2+(aq) + 2e-
reduction - Cu2+(aq) + 2e- -> Cu(s)

b) Pb(s) + Cu(NO3)2(aq) -> Cu(s) + Pb(NO3)2(aq)
oxidation - Pb(s) -> Pb2+(aq) + 2e-
reduction - Cu2+(aq) +2e -> Cu(s)

c) Ca(s) + 2HNO3(aq) -> H2(g) + Ca(NO3)2(aq)
oxidation - Ca(s) -> Ca2+(aq) + 2e-
reduction - 2H+(aq) + 2e- -> H2(g)

d) 2Al(g)+ Fe2O3(s) -> 2Fe(l) + Al2O3(s)
oxidation - 2Al ->

I have no idea what to do with the last one. If I made any mistakes or did anything wrong can someone correct them.

Oxidation Numbers
Assign oxidation numbers to chloride in each of the follow chemicals.
HCl = +1?
Cl2 = 0?
NaClO = ?
Cl- = -1?
HClO3 = either +1 or -3?
ClO3- = -3?
KClO2 - +2?
ClO2 = +2?
HClO4 = +4?

I have no idea if I'm doing these right. Can someone explain oxidation numbers and correct those?

Also can someone do an example in this and explain how they got it. I don't understand the concept.

Assign oxidation numbers to manganese in each of the following chemicals.
MnO4^2-(aq)

Use oxidation numbers to identify the oxidation and reduction atoms
MnO4-(aq) + H2Se(g) + H+(aq) -> Se(s) + Mn2+(aq) + H2O(l)

Can someone please do those examples and explain how they got the answers because I don't understand oxidation numbers.

  1. 👍
  2. 👎
  3. 👁
  1. The first three equations are ok.
    d) 2Al(g)+ Fe2O3(s) -> 2Fe(l) + Al2O3(s)
    oxidation - 2Al ->

    Al goes from 0 oxidation state on the left to zero on the right so it is oxidized. Fe goes from +3 on the left to 0 on the right so it is reduced. I assume you can write the half equations.

    have no idea what to do with the last one. If I made any mistakes or did anything wrong can someone correct them.

    Oxidation Numbers
    Assign oxidation numbers to chloride in each of the follow chemicals.
    HCl = +1? No, H is +1 so Cl is -1
    Cl2 = 0? right
    NaClO = ? Na is +1, O is -2; therefore, Cl is what to make NaClO zero. Cl must be +1.
    Cl- = -1? right
    HClO3 = either +1 or -3? H is +1, O is -2, there are 3 of them to make total on O of -6; therefore, what must Cl be to have HClO3 zero. Cl must be +5
    ClO3- = -3? +5. O is -6 and Cl must be +5 to leave a -1 charge on the ion.
    KClO2 - +2? K is +1, O is -4, therefore, Cl must be +3
    ClO2 = +2? Cl must be +4 to zero out the -4 from O2
    HClO4 = +4? H is +1, O is -8; therefore, Cl must be +7

    I have no idea if I'm doing these right. Can someone explain oxidation numbers and correct those?

    Also can someone do an example in this and explain how they got it. I don't understand the concept.

    Assign oxidation numbers to manganese in each of the following chemicals.
    MnO4^2-(aq) O is -8 so Mn must be +7 to leave a -1 charge on the ion.

    Use oxidation numbers to identify the oxidation and reduction atoms
    MnO4-(aq) + H2Se(g) + H+(aq) -> Se(s) + Mn2+(aq) + H2O(l)

    Mn goes from +7 on the left to +2 on the right. Se goes from -2 on the left to 0 on the right.

    Can someone please do those examples and explain how they got the answers because I don't understand oxidation numbers.

    I think you have guessed at some of the answers and we don't want to do that, do we?. I think I have a good site with minimal rules that can clear this up for you if you want it. I hope I turned off the bold for your work and used bold for mine. If I didn't I assume you will know what you typed and what I typed, bold or not

    1. 👍
    2. 👎
  2. Minimal but simple rules to live by for redox. Oxidation numbers are nothing more than a book keeping method.
    http://dbhs.wvusd.k12.ca.us/webdocs/Redox/Meaning-of-Redox.html

    (Broken Link Removed)

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced) i. Write the reduction and oxidation half-reactions (without electrons). (.5 point) ii. Balance the equations for atoms (except O and H). (.5 point) iii. Balance the equations for

  2. chemistry

    2. What is the reduction half-reaction for the following unbalanced redox equation? Cr2O72– + NH4+ Cr2O3 + N2 A.) Cr2O3 -> Cr2O7^2– *B.) Cr2O72– -> Cr2O3 C.) NH4+ -> N2 D.) N2 -> NH4+ 3. Which oxidation-reduction reactions

  3. Chemistry

    the type of reaction in a voltaic cell is best described as 1.spontaneous oxidation reaction only 2.nonspontaneous oxidation reaction only 3.spontaneous oxidation-reduction reaction 4.nonspontaneous oxidation-reduction reaction i

  4. Chemistry

    Write the balanced half reaction for the reduction and oxidation reactions for the redox reaction: 2 Mg (s) + O2 (g) -> 2 MgO (s) Notice: for this question you do not have to include a charge of zero and you do not have to include

  1. Chemistry

    a redox reaction is a reaction in which 1.only reduction occurs 2.only oxidation occurs 3.reduction&oxidation occur at the same time 4.reduction occurs first and then oxidation occurs i think its 3 or 4.

  2. chemistry

    A voltaic cell is contructed in which a copper wire is placed in a 1.0 M Cu(NO3)2 solution and a strip of gold i placed in a 1.0 M AuNO3 solution. The measured potential of the cell is found to be 1.36V and the copper electrode is

  3. Chemistry

    what does Zn( NO3)2 form in a half equation for redox ( reduction and oxidation )??

  4. chemistry

    "Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of the following aqueous solution: CuBr2(aq)" Possible oxidation reactions: 1. 2Br- -> Br2 + 2e- = -1.09 2. 2H2O -> O2 + 4H+ + 4e- =

  1. chemistry

    Which of the following equations does not represent an oxidation-reduction reaction? 3Al + 6HCl → 3H2 + AlCl3 2NaCl + Pb(NO3)2 → PbCl2 + 2NaNO3 2H2O → 2H2 + O2 2NaI + Br2 → 2NaBr + I2 Cu(NO3)2 + Zn → Zn(NO3)2 + Cu

  2. Chemistry

    Dr.Bobb222 please help balance the following oxidation-reduction reactions, which occur in acidic solution, using the half-reaction method. (Use the lowest possible coefficients. Include states-of-matter under the given conditions

  3. chemistry- electrochemical cell

    What makes this an oxidation-reaction? 3Ag2S+2Al(s) -> Al2S3+6 Ag(s)? Write the half-reactions showing the oxidation and reduction reactions. Identify which is the oxidation reaction and which is the reduction reason. What is

  4. chemistry

    Write the balanced net ionic equation for each of the following: 1) The reaction of dilute nitric acid with solid aluminum oxide. 2) The reaction of nitrous acid (HNO2) with potassium permanganate to produce nitrate and Mn(II)

You can view more similar questions or ask a new question.