The order of filling of the subshells is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, and 7p. In other words, electrons fill up the shells and subshells in a specific order, starting from the lowest energy state. It states that electrons will occupy the lowest energy level available to them before moving to higher energy levels. The Aufbau principle is a basic rule that describes the order in which electrons fill the energy levels and sublevels of an atom. These levels are further divided into sublevels, which are named s, p, d, and f, and each sublevel has a certain number of orbitals that can hold electrons. The third energy level can hold up to 18 electrons, and the fourth energy level can hold up to 32 electrons. The first energy level can hold up to 2 electrons, while the second energy level can hold up to 8 electrons. Each energy level has a certain capacity for electrons, and the electrons fill these levels in a specific order. Protons and neutrons are found in the nucleus of an atom, while electrons orbit around the nucleus in energy levels or shells. The Basics of Electron ConfigurationĪtoms are composed of protons, neutrons, and electrons. In this article, we will explore the concept of electron configuration, how it is determined, and its significance in chemistry. It describes the distribution of electrons among the energy levels and orbitals in an atom and helps to explain the chemical and physical properties of elements. Electron configuration refers to the arrangement of electrons in an atom, molecule, or ion.
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