The chapter delves into atomic structure and periodicity, focusing on electron configurations, trends in ionization energy and electron affinity, electronegativity, and atomic/ionic radii. Key principles such as the Aufbau principle, Hund's Rule, and the Pauli Exclusion Principle are outlined, along with periodic trends that influence an atom's behavior and chemical properties. Additionally, the quantum mechanical model of the atom is introduced, detailing quantum numbers and the importance of photoelectron spectroscopy.
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Sections
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Untitled document (19).pdfClass Notes
Memorization
What we have learnt
- Understanding electron conf...
- Ionization energy and elect...
- Electronegativity and atomi...
Final Test
Revision Tests
Chapter FAQs
What we have learnt
- Understanding electron configuration is essential for predicting an atom's chemical behavior.
- Ionization energy and electron affinity are critical for explaining periodic trends in reactivity and stability.
- Electronegativity and atomic/ionic radii influence the type and strength of chemical bonds.
Key Concepts
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Term: Aufbau Principle
Definition: A rule stating that electrons occupy the lowest energy atomic orbitals first before moving to higher levels.
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Term: Ionization Energy
Definition: The energy required to remove an electron from a gaseous atom or ion.
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Term: Electron Affinity
Definition: The energy change when an electron is added to a neutral gaseous atom to form a negative ion.
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Term: Electronegativity
Definition: A measure of an atom's ability to attract shared electrons in a chemical bond.
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Term: Quantum Numbers
Definition: A set of four numbers that describe the unique state of an electron in an atom, including its energy level and shape.