Me in the oxidation part of an oxidation-reduction reaction, the substance undergoing oxidation: loses electrons gains electrons shares electrons combines protons if any of the reactants or products in a reaction contains oxygen, then the reaction is a redox reaction. true preventing iron corrosion is important because many structures, including bridges and iron railings, are likely to rust over time and become weaker. which of the following conditions would make corrosion more likely? increasing the moisture level near the reducing the concentration of electrolytes in solutions in contact with the structure neutralizing any acidic solutions near the iron painting the iron surface the oxidation number of a metal is always the same for that metal. true the sum of all oxidation numbers: in a neutral molecule = 0 in an ion = a + in an ion = the charges on neutral atoms do not need to be equal on both sides of a chemical equation in the reaction, 2 li (s) + cl2 (g) imported asset 2 licl (s), the reducing agent is: the the cl2 the licl both the li and the cl2 in the reaction, c + 2 s imported asset cs2, the substance that is the oxidizing agent is: the c the the cs2 both the c and the s how many electrons should be added to balance the following oxidation half-reaction, h2o2 imported asset 2 h+ + o2? none one four when balancing the oxidation and reduction half-reactions for acidic solutions, you should: use h+ and oh− equally in order to balance the use h+ only in order to balance the equation use h+ and h2o, as needed to balance the equation use oh− and h2o, as needed to balance the equation the half-reaction occurring at the anode of an electrochemical reaction is comparable to: the oxidation portion of a reaction in a redox the reduction portion of a reaction in a redox reaction both the oxidation and the reduction portions of the redox reaction, at various times the unbalanced portion of either side of a redox equation the voltaic cell produces electric current from a spontaneous chemical reaction, but electrolytic reactions are not spontaneous. false