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Electric Vehicle Batteries Backgrounder

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Electric Vehicle Batteries Backgrounder This unit is aligned with Chemistry 30 – Unit B: Electrochemical Changes. 1 Start your discussion on EV’s by introducing what they are. Electric vehicles are an emission free form of transportation. These vehicles use an electric motor in place of an internal combustion engines (ICE) – what you find in gasoline cars. These vehicles are essentially large, rechargeable batteries. The description here is for an all-electric vehicle (meaning no gas is used). There are also plug-in hybrids, and hybrid vehicles. Plug-in hybrid cars run on electricity and gas to increase the range. Hybrids run on gas and use electricity to offset the car. Reference: https://www.drive.com.au/motor-news/everything-you-need-to-know-about-electric- cars-119469 2 https://www.plugndrive.ca/electric-cars-available-in-canada/ Image source: https://www.nspower.ca/your-home/energy-products/electric- vehicles/types Hybrids do not travel as far on electricity as an all-electric vehicle does on a single charge. However, hybrids use gasoline to further the distance they travel once the battery runs out of power. All-electric cars do not burn gasoline, do not have gears or a transmission, and do not require oil for the parts (there are no moving parts). On average, all-electric cars can travel 200 – 250 km on a single charge. 3 The very first battery, called the Voltaic Pile, was invented by Alessandro Volta in 1799. This battery was composed of multiple zinc and cooper electrodes, and the electrolyte was a brine-soaked paper. This invention was revolutionary as at the time, people believed that only living beings could make electricity. This theory was debunked with the invention of the Voltaic Pile. Although revolutionary, the Voltaic Pile was not perfect. It was prone to producing hydrogen bubbles, which would collect at the zinc electrode. This decreased the lifespan and usage of the battery. 60 years later, the first rechargeable, lead acid battery was invented. https://www.visualcapitalist.com/evolution-of-battery-technology/ 4 Electric Vehicles (EV) are a large battery that stores chemical energy, which is then converted to electrical energy. The electrical energy is used to turn the wheels of the car and make it move. In another lesson, we learn about energy storage. Electric vehicles are considered a form of energy storage in the sense that they store energy to be used later. Electrons are the basis of batteries. The flow of electrons is what creates electricity. In a voltaic battery (one that produces electricity), electrons flow from the positive terminal to the negative terminal. An easy way to remember the way electrons flow is with the saying “LEO the lion says GER” LEO = lose electrons, oxidation (start) GER = gain electrons, reduction (end) Another saying is “OIL RIG” OIL = oxidation is loss (start) RIG = Reduction is gain (end) It is up to you which saying you use to remember. Can you think of another saying? 5 These sayings lead to the next topic: electrochemistry https://www.youtube.com/watch?v=9OVtk6G2TnQ 5 Every battery undergoes electrochemistry within the cells. By taking a closer look at the chemistry within each cell, we can better understand how electricity is created. Electrochemistry is the study of chemical reactions that result in the movement of electrons. Moving electrons creates a current, which creates electricity. The chemical reactions in electrochemistry are called redox reactions. Redox reactions are made up of two half reactions (oxidation and reduction). The next slide will discuss redox reactions in more detail. Electrochemistry Crash Course: https://www.youtube.com/watch?v=IV4IUsholjg 6 Redox reactions are the basis of electrochemistry. This type of reaction is made up of two half reactions. One half reaction undergoes oxidation and the other undergoes reduction. Together, the reactions combine and a net flow of electrons occurs. An example of a oxidation half reaction is sodium (Na). We know this is oxidation because the oxidation state (the charge) of the species is neutral to start, then is +1. This is a net loss of electrons. A species becomes more negative if electrons are gained. Na is also called an electron donor Chlorine (Cl) is an example of a reduction reaction. The oxidation state of Cl is neutral to begin, then becomes -1, which is in line with a gain of electrons. Cl is called an electron acceptor. You can also tell which species is reduced and oxidized based on where the electron is expressed in the half reaction. In the case of Cl, is it on the left hand side. This means the electron acts as a reactant and is added to Cl to form the new Cl- ion (the electron is consumed). If the electron is on the right hand side, as seen with Na, it is a product and therefore removed from Na. https://www.youtube.com/watch?v=lQ6FBA1HM3s 7 Now that we understand the chemistry that occurs in a battery, we can take a look at the three types of batteries associated with electric cars. The three batteries to note are as follows: - Lead-acid batteries - Nickel metal Hydride batteries - Lithium-ion batteries In the next slides, we will take a deeper dive into the chemistry of each. 8 Lead-acid batteries are a type of rechargeable battery, invented in 1859 by a French physicist named Gaston Planté. This type of battery is commonly used as an automobile starter motor, found in internal combustion engines, but was also used in early electric vehicles. They are usually rated at 12 volts. Their low cost and efficiency make them a popular option. However, one of the major downfalls of a lead-acid battery is that they discharge on their own. If you were to let the battery sit unused for months, the total efficiency would slowly deplete; approximately 5% per month. However; a lead acid battery is more efficient than other alternatives. Lead acid batteries are best suited for high loads for short periods of time (i.e., starting an engine). 9 Here is an example of one cell contained in a lead acid battery. This battery was used in the early models of electric cars. They are still the most common battery used in ICE cars. Each cell has a metal conductor used to transfer electrons and create electricity. There are 6 plates in a lead acid battery. Each are 2.1 volts, the whole battery is 12.6 volts. One plate is spongy lead and the other is lead dioxide (the active material where the electrochemical reaction takes place). Lead acid batteries are composed of multiple layers of “plates” (one plate shown on the slide), all of which are submerged in an electrolyte solution. The electrolyte solution is made up of dilute Sulfuric Acid (H2SO4 and water). When the sulfuric acid comes into contact with the lead plates, a chemical reaction occurs, which results in the transfer of electrons to produce a voltage. These electrons move from the negative electrode to the positive electrode. This occurs because the negative electrode has a surplus of electrons (and repels the electrons), while the positive electrode is lacking electrons. This means that the positive electrode has more affinity to electrons; in other words, it wants electrons more than the negative electrode and has a stronger pull. The discharge is a spontaneous reaction whereas charging requires an external power source. 10 During the reaction, the electrolyte depletes and coats the plates. The plates eventually become fully coated and the battery is fully discharged. When the battery is charged, this process is reversed and the electrolyte is returned to solution. These batteries are heavy and are less stable that the newer batteries (nickel and lithium based batteries). Since this battery creates electricity, it is called a galvanic (or voltaic) cell. In these batteries, the electrons flow from the negative anode to the positive cathode. As the chemical process continues, the anode becomes less negative, and then cathode becomes less positive. A key feature of the lead-acid battery is the electrolyte solution that was not present in the prior battery. The electrolyte solution reacts with both electrodes to transfer the electrons. Watch this video for an explanation on how these cells work: https://www.youtube.com/watch?v=7b34XYgADlM Some more information on lead acid batteries: https://batteryuniversity.com/learn/article/lead_based_batteries 10 This is how a lead-acid battery discharges. Blue boxes are the reactants, orange are the intermediates, pink are the products ** Note at the negative electrode, the H is not shown in the graphic, but is expressed in the reaction. This is because the H breaks apart from HSO4 and remains in solution as a hydrogen ion. It is apart of the reaction, but is omitted from the graphic for simplicity. We can examine a lead acid battery in three parts: the electrolyte, the positive electrode and the negative plate. Electrolyte: The electrolyte solution is dilute sulfuric acid (H2SO4 and water). This graphic shows the solution as ions to help understand how the chemical reaction proceeds. This is a fairly accurate representation as when a substance is mixed with water it dissociates into its ionic forms. Positive Electrode: The positive electrode exists as PbO2 (lead oxide) to start. The electrode reacts with 2- + SO4 , H and two electrons. The resulting product is PbSO4 which forms on the electrode. 11 Negative Electrode: At the negatively charged plate, Pb(s) will give off two electrons. At this point, the Pb 2+ 2- becomes positively charged (Pb ). The SO4 the reacts with the lead cation (positively charged ion) and forms PbSO4 in solution.
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