CONFIGURACION ELECTRONICA. APRENDE A HACER LA CONFIGURACION ELCTRONICA DE CUALQUIER ATOMO O IÓN.

Introduction to Electronic Configuration

Overview of the Topic

• The speaker welcomes students and expresses enthusiasm for teaching chemistry in an easy and simple manner, focusing on electronic configuration.

• The lesson will cover what electronic configuration is and its importance, as well as how to use diagrams to find configurations for both atoms and ions.

Understanding Electronic Configuration

• The term "configuration" refers to arrangement or order, while "electronic" pertains to electrons. Thus, electronic configuration involves organizing the electrons of an atom by their energy levels.

• To effectively understand electronic configuration, it's essential first to grasp the structure of an atom, which consists of a nucleus at the center and an outer region known as the electron cloud.

Structure of Atoms

Components of Atoms

• Atoms have three fundamental particles: protons (positive charge), neutrons (neutral charge), located in the nucleus; and electrons (negative charge), which orbit around the nucleus.

• Protons carry a positive charge (+1), while neutrons are neutral. Electrons possess a negative charge (-1).

Organization of Electrons

• The organization of electrons is crucial because it determines atomic properties and chemical behavior. Electrons are arranged in energy levels around the nucleus.

• An atom can have between 1 to 7 energy levels; smaller atoms like hydrogen have one level, while larger ones like francium can have seven.

Energy Levels and Sublevels

Division into Sublevels

• Energy levels can be further divided into sublevels represented by letters: s, p, d, f. Each level has different capacities for holding electrons.

• For example:

• Level 1 has only one sublevel (s).

• Level 2 includes two sublevels (s and p).

• Level 3 contains three sublevels (s, p, d).

• Levels from 4 onward include all four sublevels (s, p, d, f).

Maximum Electron Capacity

• Each sublevel has a maximum number of electrons it can hold:

• s: up to 2 electrons

• p: up to 6 electrons

• d: up to 10 electrons

• f: up to 14 electrons

Filling Order for Electron Configuration

Diagonal Filling Method

• When filling electron configurations using diagrams, it’s important not to fill them horizontally or vertically but rather diagonally according to specific arrows indicated in diagrams.

Practical Example with Oxygen Atom

• To determine oxygen's electron configuration:

• First identify its atomic number from the periodic table which indicates its number of electrons.

• Atomic numbers are always whole numbers without signs.

Understanding Electron Configuration

Basics of Electron Configuration

• The atomic number of oxygen is 8, and its electron configuration begins with filling the 1s orbital.

• The 1s orbital can hold two electrons, leading to the notation 1s². This process continues by moving to the next available orbitals.

• After filling the 2s orbital (which also holds two electrons), we move to the 2p orbital, which can hold six electrons but must not exceed a total of eight for oxygen.

Completing Oxygen's Electron Configuration

• For oxygen, after filling up to 2p, we find that four more electrons are needed to reach a total of eight.

• The instructor invites viewers to subscribe for further learning while transitioning to iodine's electron configuration.

Iodine's Electron Configuration Process

• Iodine has an atomic number of 53; thus, we start filling from the beginning again: first filling the 1s and then moving through subsequent orbitals.

• Following this order: after completing the 3p orbital (6 electrons), we fill in the 4S (2 electrons), then proceed to fill in the transition metals starting with 3D (10 electrons).

Verifying Iodine's Total Electrons

• A running total confirms that all filled orbitals add up correctly without exceeding iodine’s atomic number of 53.

• Continuing through additional orbitals like 4d and finally reaching into p orbitals ensures accurate counting.

Understanding Ion Formation

• Transitioning from neutral atoms to ions involves understanding charge; gaining or losing electrons results in negative or positive charges respectively.

• Chlorine as an example shows how gaining one electron leads it to become Cl⁻ with a new effective electron count of eighteen.

Configuring Chlorine Ion

• Starting from chlorine’s atomic number (17), adding one due to its negative charge gives us a working total of eighteen for electron configuration purposes.

• Filling out chlorine’s configuration follows similar steps as before until reaching a complete set for Cl⁻.

Magnesium Ion Configuration

Understanding Electronic Configuration

Key Concepts in Electronic Configuration

• The discussion begins with the configuration of electrons, specifically focusing on magnesium. The speaker emphasizes the importance of understanding how to calculate electron configurations accurately.

• A calculation is demonstrated: "Dos más Dos cuatro más seis tenemos 10," illustrating how to arrive at a total of 10 electrons for magnesium's electronic configuration.

• The speaker invites viewers to share their thoughts and feedback about the class, indicating an interactive approach to learning.

Upcoming Topics

• In the next class, the focus will shift to levels and valence electrons, highlighting their significance in relation to electronic configuration.