Atomic physics is to fill the physics studying atoms, class and atomic nucleus in the system of the electron. It mainly deals with the way electrons are arranged around the atomic nucleus and how they change. It further includes an atom's energy space and how it interacts with outside particles and the electromagnetic field. Atomic physics is one of the most successful applications it comes in the chain. Atomic theory goes back to the ancient Greek philosophers, Lucicetus Amelokos and Dematetus of Grey, in about 440 BC. The atomicous school of ancient Greek philosophers proposed the idea that matter is made of very small, indivisible, and indestructible atoms. These atoms were seen as beings in continual motion through a surrounding void and colliding with each other like these both. The boys between the atoms, he don't put in question that the atom has to not answer. This caused the idea of the atoms to be rejected by Aristotle in favor of a continuous matter idea. The atom was not seen again for 400 years when the Roman poet Lucritius wrote about it. In 1887, Sir Isaac Newton showed that Voli's law, the principle that at a constant temperature, the products of a gas whose volume and pressure is constant. Such for the idea that a gas is made of particles. In 1808, John Dalton suggested that the atoms of each element were identical. In 1811, Imidu Vodydrow suggested that each element's particles, maybe two or more atoms, stuck together in what it's called molecules. Next during the 19th century, King of Theory, that there were a finite number of elements, each made up of a different type of atoms. With mere infinite ways that these atoms can be combined, the form chemical compounds. According to the today's theory of gases, that shows that pressure in this concept is also the motions of atoms' immoletual. As is on the accepted atomic model, which one known as the pump-putting model, proposed by Joseph John Thompson. This model has negative recharge to the electrons invented in a relatively large, positive charge mass. The rubber-fired gold foil external was first suggested by Ernest Rutherford. It conducted in 1911 by Hans Gardner and Ernest Marston. The experiment involved shooting apaparticles at a gold foil to blur how they were scattered by the gold on a screen. The gold foil external form the structure of the atom. Because if it were a solid mass, you with any apaparticle would get through. It's as excessive. The atom consisted of negative electrons that were embedded in a thin positive mass, all of the apaparticles would get through. However, what they found was that most of the apaparticles get cruel, with some of them being scattered by the small positive nucleus. Rutherford posed that the atom is mostly in space, consisting of a small positive nucleus surrounded by electrons scattered throughout the space. This leads to the planetary model of the atom. In such a model, the electrons cannot stand still. Because if they did, they would fall into the nucleus. This leads to modern the atom having solar systems, with electrons orbiting the nucleus like planets around the star. The planetary model of the atom leads to quantum atomic models. In fact, the planetary model's problems help lead to the development upon the planet, and it's still used to illustrate the atom. The problem with the planetary model is that it had the major flaw. The problem with the planetary model is that electrons are charged particles, and in accelerating charge, it makes light losing energy. This would cause the electrons to spiral into the nucleus. This leads to the four atomic monies. Probably had shown earlier that particles such as electrons have wave-like properties. More than showed that these waves could be bent into orbit, like those expected for an electron. For further shows, the electrons can only occupy those orbits, with exactly a whole number of wavelength. In these orbits, the waves are added together, with constructive interference. A fractional number of wavelengths would destructively interfere and not persist, when electron cannot occupy such an orbit. The reason is that the electrons jump from orbit to orbit, which photons emitted when going to a lower orbit and photon being absorbed when going to a higher orbit. It turns out that the transitions between the possible electron orbits match the spectral lines actually observed in hydrogen. This was a major step in the development of quantum mechanics. Further development have come from studying elements other than hydrogen, including the effects of multiple electrons. These studies resulted in the electron orbitals shown here. The other place is in an atom where electrons can actually be found. The shade to these orbitals were originally found mathematically. They have long been viewed as purely mathematical abstraction. The orbitals were never expected to be seen. These students have long been told this. However, field emission electron microscopy has changed this. Here is a mathematical generated S orbital image. Here is a field emission electron microscopy S orbital image. Here is a mathematical generated B orbital image. Here is a field emission electron microscopy C orbital image. The imaging of actual electron orbitals was a surprise, but the difference shows the accuracy of the quantum atomic model and the quantum mechanics as a whole. The electron configuration is the distribution of electrons in an atom or molecule in terms of atomic and molecular orbital. Here is an example of some electron configurations. The atomic sector are the emission and absorption lines of each element and compound. They result from electrons changing the atomic or molecular orbital. They are fully explained by the quantum atomic model. Think inclusion of the atomic physics study guide. The observed mainly with the electrons around the atomic machines. It also deals with how electrons are varying and how those are ranging to change. Understanding of the atom took over 2,000 years to develop. However, that understanding has survived it many days.