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Quantum Wave Model

Dive into the quantum wave model and explore electron configurations across four subshells: s, p, d, and f. Discover the shapes, orientations, and energy levels of these subshells, including their orbital diagrams. Learn about fundamental principles such as Hund’s Rule and the Pauli Exclusion Principle that govern electron placement. This guide simplifies concepts like how many orbitals and electrons are present in each subshell, the significance of energy levels, and how to determine valence electrons using the periodic table.

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Quantum Wave Model

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  1. Quantum Wave Model

  2. Electron Configuration • 4 subshells • S, P, D, F

  3. S Subshell • Spherical in Shape – enables the electrons to surround the nucleus of the atom • Lowest energy level • 1 orbital (each orbital holds 2 e-) • Holds 2 e-

  4. P Subshell • Dumbbell shaped and can be oriented in space in one of three ways. • 3 orbitals (each orbital holds 2 e-) • Holds up to 6e-

  5. D Subshell • Dumbbell shaped • 5 orbitals (each orbital holds 2 e-) • Holds 10 e-

  6. F Subshell • Dumbbell shaped • Greatest energy • 7 orbitals (each orbital holds 2 e-) • Holds 14 e-

  7. Orbital Diagrams • Orbital Diagrams: Electrons enter the electron configuration (orbital diagram) pattern beginning at the lowest energy and filling the pattern to the highest energy.

  8. Hund’s Rule • Hund’s Rule: Electrons enter the each orbital individually until all orbitals are half filled before pairing with other electrons in the subshell. • In other words – one electron per orbital until all orbitals are filled, then 2nd electron can be placed in each orbital.

  9. Pauli Exclusion Principle • Pauli Exclusion Principle: an orbital can contain no more than two electrons and those two electrons must be paired, • In other words, electrons must have opposite spin (usually indicated by one up-arrow and one down-arrow).

  10. Feeling Overwhelmed? "Teacher, may I be excused? My brain is full."

  11. Modern Atomic Structure • Space Filling Model for Scandium

  12. __ 1s __ / __ __ __ 2s 2p __ / __ __ __ __ __ __ __ __ 3s 3p 3d __ / __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 4s 4p 4d 4f __ / __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 5s 5p 5d 5f __ / __ __ __ __ __ __ __ __ __ __ __ __ __ __ __ 6s 6p 6d 6f

  13. How many energy levels are there? • 7

  14. The ___ represents? • The orbital

  15. What is the maximum number of electrons that can be held in one orbital • 2

  16. How many subshells are in the second energy level? • 2 • 2s and 2p How many electrons are in this energy level? 8

  17. How many orbitals are in the f subshell? • 7

  18. How many electrons will the third energy level hold? • 18

  19. What four letters represent the subshells? • S • P • D • F

  20. 1s2, 2s2, 2p6,3s23p6 • This is called the _________Configuration • Electron • What element does this electron configuration represent? • Argon

  21. The number 2 in 2p6represents the • Energy level

  22. The letter p in 2p6 represents the number of • Valence Electrons

  23. What is the maximum number of electrons the 4d subshell can hold? • 10

  24. What is an easy way to determine the number of valence electrons? • Look at the periodic table and determine the family the element is in. Family I – 1 valence electron Family II – 2 valence electrons Family III – 3 valence electrons Family IV – 4 valence electrons Family V – 5 valence electrons Family VI – 6 valence electrons Family VII – 7 valence electrons Family VIII – 8 valence electrons

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