Lose electrons oxidation

Two commonly used redox / V I reaction memorization aids are 1) LEO the lion goes GER (Lose Electrons Oxidation, Gain Electrons Reduction) and OIL RIG (Oxidation Involves Loss of electrons, Reduction Involves Gain of electrons). 

Aluminium oxide is an ionic compound. When it is melted the ions become mobile, as the strong electrostatic forces of attraction between them are broken by the input of heat energy. During electrolysis the negatively charged oxide ions are attracted to the anode (the positive electrode), where they lose electrons (oxidation). 

When concentrated hydrochloric acid is electrolysed, two gases are produced. Both chloride ions and hydroxide ions would be attracted to the anode. The chloride ions are at a much higher concentration than the hydroxide ions and go on to produce chlorine gas by losing electrons (oxidation). 

Although this is generally true for the Group 1(1), 11(2), and 111(13) elements, the Group IV-VII (14-17) elements not only gain electrons to form the characteristic oxidation states (reduction), but can also lose electrons (oxidation) to form the next lower inert gas core, as in Figure 4.2. In each case the difference between the two oxidation states and is 8 electrons. The lower oxidation states obtained by addition of... 

Oxidation-reduction potentials are expressed in volts relative to the standard hydrogen electrode at 0 volts, and represent the tendency of a compound to lose electrons (oxidation) or gain electrons (reduction). Various enzyme systems in respiration reactions (e.g., the cytochromes) utilizing ascorbic acid, hemoglobin, as well as reactions in the Krebs cycle (succinic and fumaric acids) involve electron transfers. Drugs can affect all these systems, and the consequences must be taken into account. 

Electrons flow from the anode to the cathode. This means that the hydrogen electrode is losing electrons (oxidation) this is only possible if the H" (aq)/H2(g) redox couple is undergoing the reaction ... 

When a metal, M, is immersed in a solution containing its ions, M, several reactions may occur. The metal atoms may lose electrons (oxidation reaction) to become metaUic ions, or the metal ions in solution may gain electrons (reduction reaction) to become soHd metal atoms. The equihbrium conditions across the metal-solution interface controls which reaction, if any, will take place. When the metal is immersed in the electrolyte, electrons wiU be transferred across the interface until the electrochemical potentials or chemical potentials (Gibbs ffee-energies) on both sides of the interface are balanced, that is, Absolution electrode Until thermodynamic equihbrium is reached. The charge transfer rate at the electrode-electrolyte interface depends on the electric field across the interface and on the chemical potential gradient. At equihbrium, the net current is zero and the rates of the oxidation and reduction reactions become equal. The potential when the electrode is at equilibrium is known as the reversible half-ceU potential or equihbrium potential, Ceq. The net equivalent current that flows across the interface per unit surface area when there is no external current source is known as the exchange current density, f. 

Conventional electrical current flows in the opposite direction as the electron flow. Because of this, when current is flowing into a solution at the anode, electrons are flowing out of the solution. Remember, if electrons are being pulled away from the metal atoms of the anode, they are losing electrons (oxidation). Therefore, oxidation occurs at the anode. 

To help yourself remember which is oxidation and which is reduction in terms of electrons, memorize the phrase LEO goes GER (Lose Electrons Oxidation Gain Electrons deduction). 

Students may be familiar with two good mnemonics for redox reactions (1) LEO the lion says CER Lose electrons oxidation, gain electrons reduction, and (2) OIL RIG Oxidation /hvolves loss of electrons, reduction /hvolves gain of electrons. 

Many authors have suggested mnemonics for oxidation and reduction. One of the most common is "LEO goes CER," for lose electrons = oxidation, and gain electrons = reduction. 

Gains electrons Ojddation number decreases Becomes reduced Loses electrons Oxidation number increases Becomes oxidized... 

Heipfui mnemonics Oil RiG-Oxidation Is Loss Reduction Is Gain. LEO GER—Lose Electrons Oxidation Gain Electrons Reduction. 

Notice that oxidation and reduction must occur together. If one substance loses electrons (oxidation), then another substance must gain electrons (reduction). For now, you simply need to be able to identify redox reactions. In Chapter 16 we will examine them more thoroughly. 

For example, if zinc metal is immersed in a solution containing copper ions, a redox reaction occurs (Figure 14-1). The zinc loses electrons (oxidation) and the copper ions gain electrons (reduction) ... 

When a magnesium metal is reacted with oxygen, it is thought to lose electrons (oxidize) to form Mg + ions and the element or compound that gained... 

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