One common type of rechargeable cell is the nickel–cadmium (NiCad) battery. For each terminal of this battery state the initial and final oxidation number of the element when the cell is delivering a current. Hence deduce which electrode is acting as the anode and which the cathode.

Which of the following batteries is an example of a primary cell?Group of answer choicesNickel-cadmium (NiCd) also known as "nicad"Nickel-metal hydride (NiMH)AlkalineLead acid

These NiCad batteries each have a potential of 1.75 V.The two half reactions occurring are:2Ni(OH)3(s) + 2e- 2Ni(OH)2(s) + 2OH-(aq)Cd(s) + 2OH-(aq) Cd(OH)2(s) + 2e-Which statement is incorrect:Select one:a.Cadmium forms the anode.b.Nickel metal is not involved in the reaction.c.The cadmium becomes eroded as the battery is used.d.The nett battery reaction involves only solid substances.e.The cadmium electrode has the more positive potential.

In an electrochemical cell:

At which electrode does oxidation occur in a voltaic cell?Group of answer choicesanode onlyeither anode or cathode, depending on the metalboth anode and cathodecathode only

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