Can someone help explain the process of electrolysis?
Electrolysis results in either oxidation or reduction. It is the process of effecting chemical change through the allocation of electric current in a substance. The positively charged ions move towards the negatively charged ions and receive electrodes and vice versa.
During electrolysis: Positively charged ions moves to the negative electrode. -They receive electrons and are known as reduced. Negatively charged ions move to the positive electrode. -They lose electrons and are oxidised. -The substance that is broken down is called the electrolyte.
I hope this helps ELECTROLYSIS Ionic substances contain charged particles called ions. For example, lead bromide contains positively charged lead ions and negatively charged bromide ions. Electrolysis is the process by which ionic substances are decomposed (broken down) into simpler substances when an electric current is passed through them. Electricity is the flow of electrons or ions. For electrolysis to work, the compound must contain ions. Covalent compounds cannot act as electrolytes because they contain neutral atoms. The ions must be free to move, which is possible when an ionic substance is dissolved in water or it is melted. For example, if electricity is passed through molten lead bromide, the lead bromide is broken down to form lead and bromine. Two electrodes connected to a cell. The negative electrode attracts positive ions and the positive electrode attracts negative ions. This is what happens during electrolysis: Positively charged ions move to the negative electrode during electrolysis. They receive electrons and are reduced. Negatively charged ions move to the positive electrode during electrolysis. They lose electrons and are oxidised. The substance that is broken down is called the electrolyte. ELECTROLYTE To be an electrolyte, a substance must be able to conduct electricity. To test for conductivity, include a sample of the substance in a circuit that contains a source of direct current (eg a cell or power pack) and a bulb or an ammeter. If a current flows through the substance when it is molten or dissolved, it is an electrolyte.
Electrolysis is a process by which electrical energy is used to produce a chemical change. Perhaps the most familiar example of electrolysis is the decomposition (breakdown) of water into hydrogen and oxygen by means of an electric current. The electrolysis of water illustrates the changes that take place when an electric current passes through a chemical compound. Water consists of water molecules, represented by the formula H2O. In any sample of water, some small fraction of molecules exist in the form of ions, or charged particles. Ions are formed in water when water molecules break apart to form positively charged hydrogen ions and negatively charged hydroxide ions. The equipment used for electrolysis of a compound consists of three parts: a source of DC (direct) current; two electrodes; and an electrolyte. A common arrangement consists of a battery (the source of current) whose two poles are attached to two strips of platinum metal (the electrodes), which are immersed in water to which a few drops of sulfuric acid have been added (the electrolyte). Electrolysis begins when electrical current (a flow of electrons) flows out of one pole of the battery into one electrode, the cathode. Positive hydrogen ions (H+) in the electrolyte pick up electrons from that electrode and become neutral hydrogen molecules (H2). As the electrolysis of water occurs, one can see tiny bubbles escaping from the electrolyte at the cathode. These are bubbles of hydrogen gas.
In chemistry and manufacturing, electrolysis is a technique that uses a direct electric current (DC) to drive an otherwise non-spontaneous chemical reaction. Electrolysis is commercially important as a stage in the separation of elements from naturally occurring sources such as ores using an electrolytic cell. The voltage that is needed for electrolysis to occur is called the decomposition potential.
Get an answer in 5 minutes from expert tutors at Oxford, Cambridge, Imperial and more.