What is Electron?
Electron in chemistry is a subatomic particle with a negative electrical charge that orbits the nucleus of an atom. Electrons are responsible for the chemical bonds between atoms, and they are also the primary carriers of electricity in solids. Electrons are found around the nucleus of every atom, although the number of electrons can vary depending on the element.
Discovery of Electron
In 1897, J. J. Thomson discovered the electron by using a cathode ray tube containing two metal plates. He observed that when a potential difference was applied across the plates, a beam of negatively charged particles was created which curved when it passed between the plates. From this experiment, Thomson discovered that the particles had a negative charge, which he named the electron. This discovery revolutionized physics and ushered in the age of modern physics.
Types of Electrons
Electrons in chemistry can be divided into two categories: valence electrons and core electrons. Valence electrons are those that are found in the outermost shells of atoms and are involved in chemical bonding. 
On the other hand, core electrons are found in the inner shells of atoms and are not involved in chemical bonding.
Electrons come in several types, each of which has its own characteristic properties. These types include:
• Spin-Up Electrons: These electrons have a spin of +1/2 and an intrinsic magnetic moment. They are the most common type of electron, and are found in all atoms.
• Spin-Down Electrons: These electrons have a spin of -1/2 and an intrinsic magnetic moment. They are less common than spin-up electrons and are typically found in larger atoms.
• Positive Electrons: These electrons have a positive charge and an intrinsic magnetic moment. They are the least common type of electron and are found in only a few atoms.
• Negative Electrons: These electrons have a negative charge and an intrinsic magnetic moment. They are also rare and are found in only a few atoms.
Electronic Configration in Atom
Atoms are the basic building blocks of matter and, as such, understanding their structure is essential for understanding the physical world around us. This structure is determined by the electrons that orbit the nucleus of the atom in a specific configuration. In recent years, researchers have been able to manipulate the arrangement of these electrons to create a variety of different electronic configurations.
The electronic configuration of an atom is determined by the number of electrons in its outer shell. The electrons in the outer shell are called valence electrons and they are responsible for bonding with other atoms and creating molecules. By changing the number and arrangement of these electrons, scientists can create different electronic configurations.
By manipulating the electronic configuration of atoms, scientists can create a variety of different materials and molecules. This process has been used to create new types of semiconductors, transistors, and other electronic components. It also has potential applications in the fields of energy and medicine. As research continues, the possibilities of manipulating the electronic configuration of atoms are sure to expand.
Rules of Electronic Configration
Bohr-Burry Rules for Electronic Configuration
The Bohr-Burry Rules for Electronic Configuration in an atom state that the electrons will fill in the orbitals of an atom in order of increasing energy. This means that the lowest energy level will be filled in first and the highest energy level will be filled in last. The electrons will fill the available orbitals starting with the lowest energy orbital and proceeding in order until all the available orbitals are filled. The orbitals must also be filled in order of increasing orbital angular momentum, so that the lowest energy orbital must be filled first, followed by the second lowest energy orbital and so on.
Aufbau Rules of Electronic Configration
The second rule of electronic configuration in atoms is the Aufbau Principle, which states that electrons fill the lowest energy orbitals first. This means that electrons will fill the 1s orbital before the 2s orbital, and so on. The Aufbau Principle also dictates that electrons fill orbitals of the same energy in a parallel way, with spin-up electrons filling the spin-up orbitals before the spin-down orbitals. The Aufbau Principle applies to all elements in the periodic table.
Characteristics and Applictions of Electron
Electron is an essential component of chemistry, as it helps to construct and bind molecules together. It is a subatomic particle that carries a negative electrical charge and is found in the atom’s outermost shell. Electrons are fundamental to chemistry, as they are responsible for chemical bonding and the formation of molecules.
The charge of an electron in chemistry is a fundamental constant, with a value of -1.602176634 × 10-19 coulombs. The mass of an electron in chemistry is 9.1093837015 × 10-31 kilograms.
The behavior of electrons in a molecule can be accurately described using the quantum mechanical model. This model is based on the concept of orbitals, which are regions of space around the nucleus where electrons are most likely to be found. The electrons occupy different orbitals depending on their energy, and these orbitals are divided into two categories: bonding orbitals and non-bonding orbitals. Bonding orbitals contain electrons that are involved in forming chemical bonds between atoms, while non-bonding orbitals contain electrons that do not participate in bonding.
The number of electrons in a molecule is determined by the number of protons in the nucleus. Electrons are arranged in shells around the nucleus, with the innermost shell containing two electrons and the outermost shell containing eight electrons. The properties of a molecule depend on the arrangement of electrons in the outermost shell. For example, a molecule with four electrons in its outermost shell will have different properties than a molecule with six electrons in its outermost shell.
The electrons in a molecule can also interact with each other. This interaction is known as electron-electron repulsion and can cause molecules to be attracted to each other or repelled from each other. Electron-electron repulsion is an important factor in determining the properties of a molecule.
In conclusion, electron is a fundamental component of chemistry. It is responsible for chemical bonding and the formation of molecules. The behavior of electrons in a molecule can be accurately described using the quantum mechanical model, and the number of electrons in a molecule is determined by the number of protons in the nucleus. Electrons can also interact with each other, resulting in electron-electron repulsion. All of these factors contribute to the properties of a molecule.
FAQs about Electron
What is Electron in chemistry?
How does Electron in chemistry work?
This exchange of electrons is how chemical reactions take place. Electron chemistry is used to understand how elements form bonds to create different molecules. It is also used to understand how molecules interact with each other and how they can be manipulated to create new compounds.
What are the applications of Electron in chemistry?
Electron diffraction is another application of electrons in chemistry, which is used to study the structure and composition of materials. This technique is also used to analyze the structure of proteins and other large molecules.
Electron spin resonance spectroscopy is another application of electrons in chemistry, which is used to study the magnetic properties of molecules.
Finally, Scanning Tunneling Microscopy is used to study the electrical properties of materials at the nanoscale.
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