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CHEM 1210 Lecture Notes - Lecture 4: Molecular Mass, Oxidation State, Carbon-12

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28 Feb 2018

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Oxidation: the loss of electrons, the gain of oxygen and/or loss of hydrogen. Oxidation number = the charge on an element we will add the make the oxidat equal to 0. Leo = lose an electron, it"s oxidation. Reduction: the gain of electrons, the loss of oxygen and/or gain of hydrogen. Oxidation-reduction (redox) reaction: any reaction in which electrons are transferre one species to another. The products of complete combustion of carbon compounds are co2 and h2o. Respiration: the process by which living organisms use o2 to oxidize carbon- containing compounds to produce co2 and h2o. The importance of these reac not the co2 produced, but the energy released. Rusting: the oxidation of iron to a mixture of iron oxides. Bleaching: the oxidation of colored compounds to products which are colorle. Batteries: in all cases, the reaction taking place in a battery is a redox-reaction: formula weight.

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Related Questions

Answer true or false.

(a) When a substance is oxidized, it loses electrons.

(b) When a substance gains electrons, it is reduced.

(c) In a redox reaction, the oxidizing agent becomes reduced.

(d) In a redox reaction. the reducing agent becomes oxidized.

(e) When Zn is converted to Zn²⁺ ion, zinc is oxidized.

(f) Oxidation can also be defined as the loss of oxygen atoms and/or gain of hydrogen atoms.

(g) Reduction can also be defined as the gain of oxygen atoms and/or loss of hydrogen atoms.

(h) When oxygen, O₂, is converted to hydrogen peroxide, H₂O₂, we say that O₂ is reduced.

(i) Hydrogen peroxide, H₂O₂, is an oxidizing agent.

(j) All combustion reactions are redox reactions.

(k) The products of complete combustion (oxidation) of hydrocarbon fuels are carbon dioxide, water, and heat.

(l) In the combustion of hydrocarbon fuels, oxygen is the oxidizing agent and the hydrocarbon fuel is the reducing agent.

(m) Incomplete combustion of hydrocarbon fuels can produce significant amounts of carbon monoxide.

(n) Most common bleaches are oxidizing agents.

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1. What is meant by the term oxidation?

a. The loss of electrons by the compounds in chemicalreactions.

b. The gain of electrons by the compounds in chemicalreactions.

c. The combining of elements with O in chemical reactions.

2. On which side of an oxidation half-reaction do theelectrons appear?

a.	On the left side (reactants).
b.	On the right side (products).

3. What is meant by the termoxidant?

a.	It is the reactant that's being oxidized.
b.	It is oxygen in any oxidation reactions.
c.	It is the reactant that's being combined with O.

4. What is meant by the term oxidizingagent?

The compound which loses electrons in the redox reaction.

b. The compound which gains electrons in the redoxreaction.

c. It is oxygen in any oxidation reactions.

d. The compound which reacts with oxygen in the redoxreaction

I need help with questions 2-4 I can't figure them out.

Introduction An important type of reaction mechanism is the transfer of electrons from one species to another effecting a change in oxidation state. This gain or loss of electrons is referred to as reduction and oxidation, respectively. For example, consider the two balanced, chemical equations (1 & 2) that follow Cu (s) D Cu (aq) 2e (1) Cl2(aq) 2e D 2Cl (aq) (2) The first equation (1) shows elemental copper metal with a oxidation state of zero forming aqueous copper(Il) ions having an oxidation state of +2. This gain in oxidation number, 0 to +2, is called oxidation. The second equation (2) show elemental chlorine having an oxidation state of zero forming chloride ions in aqueous solution with an oxidation state of This decrease in oxidation number, 0 to -1, is called reduction. In any chemical reaction, the electrons gained or lost are conserved, i.e.. there is no net gain or loss of electrons. In fact, the two reactions illustrated above could occur simultaneously with the electrons lost by copper, gained by the chlorine in aqueous solution. Since the copper provides the electrons that subsequently reduce the chlorine copper is referred to as the reducing agent. Likewise, since the chlorine is accepting the electrons from copper, which subsequently oxidizes the copper, chlorine is referred to as he oxidizing agent. The two reactions above (1 & 2) are called half-reactions, as much as they each constitute one-half of the total reaction Equation 1 is the oxidation half reaction showing Cu(s) losing two electrons. In Equation 2, Cla(aq) gains two electrons and is the reduction half-reaction. If these two half-reaction are added together the result is the total oxidation-reduction reaction or "redox" reaction. Adding the two equations yields (3). Cu(s) Cl2(aq) D Cu (aq) 2CI (aq) (3) Whether or not the above reaction is spontaneous proceeds from reactants to products without input of energy into the system, may be determined by observing the reaction mixture if the reactants and products differ greatly in their appearance. Copper metal is a bright copper color and chlorine in aqueous solution will appear yellow. The Cu ion may turn the liquid part of the mixture blue, however, the Cris colorless and cannot be observed directly. Copper, like many of the transition metals, exhibits a variety of oxidation states depending upon the chemical environment in which it is found. In a strong reducing environment copper may exist as the free metal, Cu(s). An example of such a situation is illustrated in the following chemical equation (4). 4Cuo(s) CH4(g) D 4Cu(s) CO2(g) 2H2O(l) (4)