CONFIGURACIÓN ELECTRÓNICA

Summary

In this video, the concept of electronic configuration in atoms is explored. The instructor explains how to determine an atom's electron arrangement based on its energy levels and orbitals (s, p, d, f), using the Moeller diagram. Through detailed examples, the video demonstrates how to fill orbitals and calculate electronic configurations for atoms with varying atomic numbers and charges. The video also highlights how to use this information to determine an element's position in the periodic table, including its period and group, and how to identify the element itself. The process of understanding and applying electronic configurations is made clear for students.

Takeaways

• 😀 The electronic configuration of an atom explains how electrons are arranged in energy levels and orbitals (s, p, d, f).
• 😀 Electrons must follow a specific order of energy, filling orbitals from lowest to highest energy.
• 😀 The Aufbau principle is used to fill the electron orbitals, following the order outlined in the Moeller diagram.
• 😀 The Moeller diagram helps visualize how electrons fill energy levels (1s, 2s, 2p, 3s, etc.) in an atom.
• 😀 Each orbital type (s, p, d, f) can hold a specific number of electrons: 2 for s, 6 for p, 10 for d, and 14 for f.
• 😀 In the example of an atom with an atomic number of 23, the electron configuration follows the 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d3 pattern.
• 😀 For an atom with an atomic number of 32 and two negative charges, the configuration includes extra electrons, ending with 4p4.
• 😀 An atom with 27 protons and three positive charges (losing 3 electrons) will have 24 electrons, with its configuration ending in 3d4.
• 😀 The position of an element in the periodic table can be determined from its electron configuration, based on the last filled orbital.
• 😀 The last electron added determines both the period (row) and the group (column) of an element in the periodic table.
• 😀 For example, elements with configurations like 3d3, 4p4, and 3d7 correspond to different positions on the periodic table: vanadium, germanium, and cobalt, respectively.