Electronic Configuration With Pictures Presentation
| Introduction to Electronic Configuration | ||
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| • Electronic configuration refers to the arrangement of electrons in an atom or ion. | ||
| • It provides information about the distribution of electrons into different energy levels and sublevels within an atom. | ||
| • The electronic configuration is represented using a notation that includes the energy level, sublevel, and the number of electrons in each sublevel. | ||
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| 1 | ||
| The Aufbau Principle | ||
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| • The Aufbau principle states that electrons fill the lowest energy levels and sublevels first before moving to higher ones. | ||
| • Electrons occupy orbitals with the lowest energy first, following a specific order known as the aufbau sequence. | ||
| • This principle helps in determining the electronic configuration of an atom by sequentially filling the available orbitals. | ||
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| 2 | ||
| The Pauli Exclusion Principle | ||
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| • The Pauli exclusion principle states that no two electrons in an atom can have the same set of quantum numbers. | ||
| • Each orbital can accommodate a maximum of two electrons with opposite spins. | ||
| • This principle helps in understanding the organization of electrons within sublevels and orbitals. | ||
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| 3 | ||
| Hund's Rule | ||
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| • Hund's rule states that when electrons occupy orbitals of equal energy (degenerate orbitals), they first fill them singly with parallel spins before pairing up. | ||
| • This rule ensures the maximum number of unpaired electrons, which leads to increased stability and reactivity. | ||
| • Hund's rule helps in determining the electron configuration within sublevels and orbitals. | ||
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| 4 | ||
| Electron Configuration Notation | ||
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| • Electron configuration is represented using a shorthand notation that includes the energy level, sublevel, and the number of electrons. | ||
| • The energy level is denoted by a number (1, 2, 3, etc.), while the sublevel is represented by a letter (s, p, d, f). | ||
| • The number of electrons in each sublevel is indicated by superscripts following the sublevel letter. | ||
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| 5 | ||
| Examples of Electronic Configuration | ||
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| • Example 1: Hydrogen (H) - 1s1 - The electron configuration of hydrogen consists of one electron in the 1s sublevel. | ||
| • Example 2: Carbon (C) - 1s2 2s2 2p2 - The electron configuration of carbon includes two electrons in the 1s sublevel, two in the 2s sublevel, and two in the 2p sublevel. | ||
| • Example 3: Calcium (Ca) - 1s2 2s2 2p6 3s2 3p6 4s2 - The electron configuration of calcium involves two electrons in the 1s sublevel, two in the 2s sublevel, six in the 2p sublevel, two in the 3s sublevel, six in the 3p sublevel, and two in the 4s sublevel. | ||
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| 6 | ||
| Conclusion | ||
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| • Electronic configuration provides important information about the arrangement of electrons within an atom or ion. | ||
| • It follows principles such as the Aufbau principle, Pauli exclusion principle, and Hund's rule. | ||
| • Understanding electronic configuration helps in predicting the behavior, stability, and reactivity of elements. Note: Please ensure to include relevant pictures or diagrams along with the bullet points on each slide to enhance visual engagement and understanding. | ||
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| 7 | ||
