Go through them in the order given until you have an oxidation number assigned. 1  For atoms in their elemental form, the oxidation number is 0. 2  For ions, the oxidation number is equal to their charge. 3  For single hydrogen, the number is usually +1 but in some cases it is 4  -1. For oxygen, the number is usually  -2.
http://www.shodor.org/UNChem/advanced/redox/index.html
2(g) Write the balanced reduction half‐reaction. 3. Write a balanced half‐reaction for the reduction of hydrogen peroxide to water in an acidic solution. 4. Write a balanced half‐reaction for the reduction of SO42–(aq) to SO2(g) in an acidic solution.
http://www.csus.edu/indiv/m/mackj/chem1b/exam/ex3rp.pdf
Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid-base reactions. Fundamentally, redox reactions are a family of reactions that are concerned with the transfer of electrons between species.
http://www.shodor.org/UNChem/advanced/redox/index.html
B. Mg2+(aq) C. Cl-(aq) D. Zn(s) explanation. The best reducing agent is the compound that is most favorably oxidized. According to the table, Mg2+(aq) is an oxidizing agent, because it has no electrons to lose and can gain two electrons to form the neutral metal.
https://forums.studentdoctor.net/threads/which-is-the-strongest-reducing-agent-help.945434/
(equivalentweight of oxidising / reducing agents = Molecular mass/ Number of electrons lost or gained by one molecule)
https://www.easycalculation.com/formulas/oxidizing-and-reducing-agents.html
Oxidizing agents cause the oxidation state of other substances to become more positive by accepting their electrons.Oxidizing agents are themselves reduced. Common oxidizing agents are listed in Figure 1. Reducing agents cause the oxidation state of other substances to become more negative by releasing electrons to them. Reducing agents are themselves oxidized. Common reducing agents are listed in Figure 1. Click on the buttons to see common oxidizing and reducing agents.
https://www.chem.wisc.edu/deptfiles/genchem/netorial/rottosen/tutorial/modules/electrochemistry/01oxidation_reduction/18_11.htm
Exam 3 Review Problems: Useful Equations: ∆Go = ‐RTlnK ∆Go =∆Ho‐T∆So ∆Go = ‐nFEo ln K = nEo/0.0257. Ecell = Ecell. o –RT/nF lnQ. 1. Assuming the following reaction proceeds in the forward direction, 2 Ni2+(aq) + Zn(s)  2 Ni(s) + Zn2+(aq) a. Zn(s) is the reducing agent and Zn2+(s) is the oxidizing agent.
http://www.csus.edu/indiv/m/mackj/chem1b/exam/ex3rp.pdf
Reducing agent. A reducing agent (also called a reductant or reducer) is an element (such as calcium) or compound that loses (or donates) an electron to another chemical species in a redox chemical reaction. Since the reducing agent is losing electrons, it is said to have been oxidized.
https://en.wikipedia.org/wiki/Reducing_agent
Video transcript. Let's see how to identify the oxidizing and reducing agents in a redox reaction. So here, we're forming sodium chloride from sodium metal and chlorine gas. And so before you assign oxidizing and reducing agents, you need to assign oxidation states. And so let's start with sodium.
https://www.khanacademy.org/science/chemistry/oxidation-reduction/redox-oxidation-reduction/v/oxidizing-and-reducing-agents-1
As a summary, here are the steps to follow to balance a redox equation in acidic medium (add the starred step in a basic medium): 1  Divide the equation into an oxidation half-reaction and a reduction half-reaction. 2  Balance these Balance the elements other than H and O. Balance the O by adding H2O.
http://www.shodor.org/UNChem/advanced/redox/index.html
which is the reducing agent in the formula
A compound is the reducing agent in the formula. The reducing agent in the formula is a compound.