![]() ![]() Labels can be used once, more than once, or not at all. Drag the appropriate labels to their respective targets. In other words, when three electrons begin to fill a p subshell (which consists of three degenerate orbitals, meaning three orbitals with the same energy), the lowest energy configuration consists of one electron in each p orbital, all with either spin up or spin down. Finally, Hund's rule states that the lowest energy electron configuration for an atom is one having the maximum number of electrons with parallel spins in degenerate orbitals. ![]() Similarly, d subshells consist of five separate orbitals, and f subshells consists of seven separate orbitals. Remember that p subshells consist of three separate orbitals (p_x, p_y, and p_z), for a total of up to six electrons in a given p subshell. Since there are only two possibly values for m_s (+ 1/2 and -1/2), only two electrons can occupy any given orbital. The fourth quantum number (m_s) specifies the spin of the electron. The first three quantum numbers (n, l, and m_l) specify a particular orbital, such as 1s. This results in the order 1s2s2p3s3p4s3d4p5s, etc This order is often called the 'aufbau order." The Pauli principle states that no two electrons in an atom can have the same value of all four quantum numbers (n, l, m_l, and m_s). To determine the order in which orbitals fill, read the diagram from top to bottom, left to right. To aid in remembering the energy order of orbitals, draw a diagram with the energy levels (1 through 8) down the left of the diagram, and the subshells of each energy level across in rows, with each row offset by one (so 3s is below 2p, 4p is below 3d, etc). For example, the 4s orbital is lower in energy than the 3d orbital for elements with more than one electron. Aufbau is German for "building up." The aufbau principle simply states that electrons are added to an orbital diagram one at a time to the lowest energy orbital available, and that the orbital diagram is thus "built up." However, due to shielding of the nucleus, the energies of orbitals are not always in order of energy level (n). ![]() Orbital diagrams are filled using the aufbau principle, the Pauli principle, and Hund's rule. Orbital diagrams are a useful tool to aid in the derivation of the electron configuration of an element. Electron configurations can be used to predict most of the chemical properties of an element. The electron configuration of an element is the arrangement of its electrons in their atomic orbitals. To understand how to draw orbital diagrams, and how they are used to write electron configurations. ![]()
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