Why are the oxidation and reduction half-reactions separated in an electrochemical cell?A.So that electricity will flow through the wire connecting the halves of the cellB.Because different solutions are needed for the oxidation and reduction reactionsC.So that the metals produced can be collected without contaminationD.Because oxidation and reduction cannot happen in the same solution

The electrochemical series ranks elements based on their tendency to undergo oxidation or reduction in electrochemical reactions.If a redox reaction can be split into half reactions it becomes possible to build a device, called an electrochemical cell, that has separate compartments (cells) for the oxidant and reductant. This physically prevents them from contacting each other and reacting, but allows for charge transfer in the form of electrons through an external circuit and in the form of counter ions in a salt bridge that connects the cells.When constructing a voltaic cell, choosing the composition of each half-cell is important in order to achieve a spontaneous reaction that will convert chemical energy to electrical energy. You can use the electrochemical series to determine which of the two selected half-cells will undergo oxidation and which will undergo reduction, relative to each other. When examining the electrochemical series, you will notice that very reactive metals are found at the top of the series as they readily lose one or more of their valence electrons to form positive metal ions—they readily oxidize. At the bottom of the electrochemical series is flourine. It is a very reactive non-metal with a strong tendency to gain an electron and fill its outer electron shell. Because of this strong tendency to gain electrons and become reduced, non-metals high in group 17 are powerful oxidizing agents.MYP -CHEMISTRY 4 AND 5 OXFORDThe further apart the metals are in the electrochemical series, the higher the voltage. Electrons flow along the wire from the metal higher in the electrochemical series to the metal lower down. Your task is to design an electrochemical cell to create electrical energy with maximum voltage. You will be provided with the following:freshly cleaned strips of each of the following metals—copper, lead, zinc, and magnesiumsolutions of copper(II) nitrate, zinc(II) nitrate, lead(II) nitrate and magnesium sulfatetest tubesBent tube saltQ 5.1Formulate a hypothesis with a justification (which combination of metals will generate higher voltage) based on your knowledge of the electrochemical series.B 3the combination of magnesium and copper will generate the highest volatageWords: 11Q 5.2State the three variables and discuss the manipulation of the variables.Independent variableDependent variableControlled variable

Where does reduction occur in an electrochemical cell?A.Conducting wireB.AnodeC.CathodeD.Porous barrier

In an electrochemical cell:

If a redox reaction can be split into half reactions it becomes possible to build a device, called an electrochemical cell, that has separate compartments (cells) for the oxidant and reductant. This physically prevents them from contacting each other and reacting, but allows for charge transfer in the form of electrons through an external circuit and in the form of counter ions in a salt bridge that connects the cells.When constructing a voltaic cell, choosing the composition of each half-cell is important in order to achieve a spontaneous reaction that will convert chemical energy to electrical energy. You can use the electrochemical series to determine which of the two selected half-cells will undergo oxidation and which will undergo reduction, relative to each other. When examining the electrochemical series, you will notice that very reactive metals are found at the top of the series as they readily lose one or more of their valence electrons to form positive metal ions—they readily oxidize. At the bottom of the electrochemical series is flourine. It is a very reactive non-metal with a strong tendency to gain an electron and fill its outer electron shell. Because of this strong tendency to gain electrons and become reduced, non-metals high in group 17 are powerful oxidizing agents.MYP -CHEMISTRY 4 AND 5 OXFORDThe further apart the metals are in the electrochemical series, the higher the voltage. Electrons flow along the wire from the metal higher in the electrochemical series to the metal lower down. Your task is to design an electrochemical cell to create electrical energy with maximum voltage. You will be provided with the following:freshly cleaned strips of each of the following metals—copper, lead, zinc, and magnesiumsolutions of copper(II) nitrate, zinc(II) nitrate, lead(II) nitrate and magnesium sulfatetest tubesBent tube saltQ 5.1Formulate a hypothesis with a justification (which combination of metals will generate higher voltage) based on your knowledge of the electrochemical series.

What allows electrons to flow between electrodes in an electrochemical cell?A.Salt bridgeB.Electrolyte solutionsC.Conducting wireD.Battery