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Ch.8 - Periodic Properties of the Elements
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.8 - Periodic Properties of the ElementsProblema 44b
Capitolo 8, Problema 44b

Write the full orbital diagram for each element. b. Ca

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Identify the atomic number of calcium (Ca), which is 20.
Determine the electron configuration of calcium by filling the orbitals in order of increasing energy: 1s, 2s, 2p, 3s, 3p, 4s.
Write the electron configuration for calcium: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2.
Draw the orbital diagram by representing each orbital as a box and each electron as an arrow. Fill the orbitals according to the electron configuration, following Hund's rule and the Pauli exclusion principle.
Ensure that each orbital is filled with a maximum of two electrons with opposite spins, and that electrons are distributed to maximize unpaired electrons in degenerate orbitals.

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Orbital Diagrams

Orbital diagrams visually represent the distribution of electrons in an atom's orbitals. Each orbital can hold a maximum of two electrons with opposite spins, and the diagram uses arrows to indicate the presence and spin of electrons. Understanding how to construct these diagrams is essential for predicting the electron configuration of elements.
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Electron Orbital Diagrams

Electron Configuration

Electron configuration describes the arrangement of electrons in an atom's orbitals, following the principles of the Aufbau principle, Pauli exclusion principle, and Hund's rule. For calcium (Ca), which has 20 electrons, the electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s², indicating how electrons fill the available orbitals in order of increasing energy.
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Electron Configuration Example

Periodic Table and Element Properties

The periodic table organizes elements based on their atomic number and electron configurations, which influence their chemical properties. Calcium, located in Group 2, is an alkaline earth metal, and its electron configuration reveals its tendency to lose two electrons to achieve a stable noble gas configuration, which is crucial for understanding its reactivity and bonding behavior.
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Periodic Table History
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