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\1)The arrangement of electrons surrounding an atom’s nucleus is called its electron configuration. The energy level of the using principle dictates whether more electrons may be added. So, if the energy level is high, the electrons can move farther away from the nucleus. The energy is low, and there is no room for more electrons, but if the energy level is closer to the nucleus. There are sublevels inside each energy level. The letters s, p, d, and f represent the sublevels corresponding to the first four energy levels. Orbitals, the area of an atom inhabited by electrons, make up each sublevel. Atomic orbitals employ a sublevel letter and an energy level number. For instance, 3p stands for sublevel p of the third energy level. The group number in the periodic table indicates the number of electrons, while the row number displays the greatest primary energy level. The first two electrons will couple up in the 1s orbital, and the next two electrons will pair up in the 2s orbital since the electron configuration for oxygen is 1s2 2s2 p4. Four electrons are left and must be positioned in the 2p orbitals. According to Hund’s rule, all orbitals will be single occupied before becoming double-occupied. In addition, two p orbitals receive one electron, and one will receive two.

2)This week we are working on the electron configuration of an atom. I will be describing the electron configuration of Magnesium (Mg). First, we need to know the number of electrons in Magnesium, which is 12. We know this from the atomic number on the period table. We then can use the periodic table to complete the electron configuration. You will need to use the previous noble gas to complete. The complete configuration for magnesium is 1s² 2s² 2p6 3s². Magnesium can also be expressed as [Ne] 3s2. Magnesium contains three orbitals, two valence electrons, and three valance shells.