Electric Cell

Electric cells are like small inverters that you can carry around. Just like an inverter that can power your home during a blackout, an electric cell is a device that can power small devices without a direct electricity connection. Whether it is your remote control, wristwatch, or flashlight, these compact powerhouses of energy undergo energy conversion in a short span of time. An electric cell, or simply a cell, is one of the most crucial devices that keep your everyday gadgets alive and functional, and is our topic of discussion today.

1.0Electric Cell Definition

An electric cell is an electrochemical device that transforms chemical energy into electrical energy by redox (reduction-oxidation) reactions between its two electrodes. These electrodes remain submerged in an electrolyte. The electrons produced by these reactions produce a potential difference (voltage) between the terminals, enabling current to flow when connected in an external circuit. Although a single cell is unable to provide a large amount of electricity, a combination of several cells forms a battery capable of powering large devices that require more electricity. 

2.0Structure and Components of an Electric Cell: 

The structure of an electric cell, regardless of whether the cell is dry or wet, typically consists of the following common key parts: 

• Electrodes: Electrodes are basically the site of origin of electricity in a cell. These are generally made of different materials to create a potential difference between them, which facilitates the smooth conduction of electricity. These can be: 
• Anode (Negative Terminal): In a common dry cell, the flat end of the cell is typically the negative terminal and is made of zinc. It is denoted with the ( – ) sign. 
• Cathode (Positive Terminal): It is the bulging end of the cell, which is generally made up of a carbon rod, surrounded by a manganese dioxide paste. 
• Electrolyte: It is the chemical medium that allows the movement of free electrons or ions through it. In dry cells, an electrolyte is a paste of ammonium or zinc chloride, whereas in wet cells, it is the liquid acid in which the terminals are immersed. 
• Separator: The separator prevents physical contact between the anode and cathode, thereby preventing the short-circuiting of a cell. It is a porous material placed between the two terminals.

3.0Working of an Electric Cell

The working of an electric cell depends on electrochemical reactions that move electrons, allowing it to supply power to a device. The following is a step-by-step account of how it operates, including EMF:

• Redox Reaction Starts: A chemical reaction begins within the cell between the electrodes and the electrolyte. The oxidation (loss of electrons) occurs at the anode, and the reduction (gain of electrons) happens at the cathode.
• Generation of EMF (Electromotive Force): Because of the variation in the chemical nature between the electrodes, a potential difference is created, which is known as EMF. It is the maximum voltage that the cell will deliver when there is no current flowing through it. 
• Electron Flow Through External Circuit: Electrons discharged at the anode cannot cross the electrolyte, so they move along the outside wire towards the cathode, generating an electric current within the circuit.
• Ion Movement Within the Cell: Within the electrolyte, the positive and negative ions migrate to balance the charges, completing the internal circuit, which ultimately powers the device. 

4.0Types of Electric Cells

Based on the reusability and chemical composition, an electric cell can be classified into two different types, which are: 

1. Primary Cells: Primary cells are non-reusable or non-rechargeable cells. This means that these cells can not be used multiple times, once they lose their EMF. Primary cells are most commonly used in household devices. Examples of electric cells in this type are the dry cell and alkaline battery. 

2. Secondary Cells: These are rechargeable or reusable types of electric cells. This means secondary cells can be used multiple times by reversing the chemical reaction using an electric current. These are commonly used in automobiles and electronic devices. Examples of electric cells in this type are the Lithium-ion battery of smartphones and laptops, and the lead-acid battery. 

Primary and Secondary Cells differ in functions, therefore, in applications. Primary cells are cost-effective in terms of price, whereas secondary cells are cost-effective in the long run due to their reusability. 

5.0Uses of Electric Cells 

The uses of electric cells span a wide range of fields in our everyday lives, especially due to their portable, reliable, and clean sources of electrical energy. Which include: 

• Powering Portable Electronic Devices: Electric cells are the major source of electrical energy for powering a variety of small and everyday gadgets, like wall clocks, wristwatches, and flashlights. 
• Used in Toys and Educational Tools: In toys, sound books, talking dolls and other small gadgets, the main source of electric energy used to operate them is these electric cells. 
• Medical Equipment: Medical devices, such as Hearing aids, glucometers, digital blood pressure monitors, and many more, are typically powered by electric cells. 
• Emergency and Safety Devices: Electric cells are also used in various gadgets that work as emergency devices during electric blackouts. For example, emergency torches, smoke detectors, exit signs, etc. 
• Automotive and Transportation: With advancements in technology, electric cells are also being widely used in automotive and transportation vehicles, which ultimately helps prevent the harmful effects of global warming.