3.6.6 - Distribuição eletrônica completa dos elétrons do oxigênio magnésio, titânio e estanho

Summary

This video tutorial teaches viewers how to solve electronic configuration problems using the periodic table and orbital diagrams. The instructor demonstrates the process step by step, starting with oxygen and progressing through elements like magnesium, titanium, and tin. The video explains how to determine the number of electrons, fill orbitals, and understand the electron distribution based on energy levels and sublevels. Emphasis is placed on visualizing the diagram and correctly assigning electrons to different orbitals. This practical guide helps viewers grasp the fundamentals of electron configuration for various elements.

Takeaways

• 😀 Understanding how to use the periodic table and orbital diagrams is crucial for determining electronic configurations.
• 😀 The electron configuration of an element can be written by filling orbitals according to their energy levels, following specific rules.
• 😀 The orbital diagram is organized by layers (1 to 7) and sublevels (S, P, D, F) based on quantum numbers.
• 😀 The S sublevel has only one orbital and can hold a maximum of two electrons.
• 😀 The P sublevel has three orbitals, each capable of holding two electrons, for a total of six electrons.
• 😀 The D sublevel has five orbitals, each holding up to two electrons, totaling ten electrons.
• 😀 The F sublevel has seven orbitals, each holding two electrons, totaling fourteen electrons.
• 😀 The electron configuration is done by filling the lowest energy orbitals first, following the diagonal method from the upper-right to the lower-left of the diagram.
• 😀 In the periodic table, the atomic number represents the number of electrons in a neutral atom, which determines its configuration.
• 😀 The electron configuration of an atom in its ground state fills orbitals with the lowest possible energy, ensuring stability.
• 😀 The process of filling orbitals continues as new elements are discovered, and the diagrams evolve with each new orbital type (such as G or H).

Q & A

What is the main goal of this video series?

The main goal of this video series is to help viewers understand how to use the periodic table and orbital diagrams to determine electron configurations for various elements.

What does the atomic number represent in the periodic table?

The atomic number represents the number of protons in an atom and, in a neutral atom, it also indicates the number of electrons.

What is the correct order of orbital filling based on the energy levels?

The correct order of orbital filling is: 1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p, and so on.

How many electrons can the 's' orbital hold?

The 's' orbital can hold a maximum of 2 electrons.

What is the maximum number of electrons that the 'p' orbital can hold?

The 'p' orbital can hold a maximum of 6 electrons because it has 3 suborbitals, and each can hold 2 electrons.

How many orbitals are there in the 'd' sublevel, and what is the maximum number of electrons it can hold?

The 'd' sublevel has 5 orbitals, and it can hold a maximum of 10 electrons (5 orbitals × 2 electrons each).

What rule is used to determine the order in which electrons fill orbitals?

Electrons fill orbitals in order of increasing energy, starting with the lowest energy level, and this can be visualized by filling the orbitals diagonally from top-right to bottom-left.

What is the electronic configuration of Oxygen (O), and how is it derived?

Oxygen (O) has an atomic number of 8, so its electron configuration is 1s² 2s² 2p⁴. This is derived by filling the 1s orbital with 2 electrons, the 2s orbital with 2 electrons, and the 2p orbital with 4 electrons.

How do you calculate the electron configuration of an element like Magnesium (Mg)?

Magnesium (Mg) has an atomic number of 12. Its electron configuration is 1s² 2s² 2p⁶ 3s². This is done by filling up the orbitals sequentially until the total number of electrons equals 12.

What is a key difference in filling the orbitals for elements in higher periods (like Titanium or Tin)?

For elements in higher periods, such as Titanium and Tin, additional orbitals like 3d, 4s, and 4p come into play. It's important to ensure that electrons fill these orbitals in the correct order, following the diagonal rule for orbital filling.