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Electron_Energy_Level_Notes.ppt
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- 2. Electron Energy LevelNotes ⢠Electrons do not travel around the nucleus of an atom in orbits ⢠They are found in energy levels at different distances away from the nucleus. (kind of like shells or layers).
- 3. The Quantum MechanicalModel of the Atom (cont.) The wave function predicts a three-dimensional region around the nucleus called the atomic orbital.
- 4. Hydrogen Atomic Orbitals Principalquantum number (n) indicates the relative size and energy of atomic orbitals. n specifies the atomâs major energy levels, called the principal energy levels. Electrons cannot exist between energy levels (just like the rungs of a ladder).
- 5. Electron Energy LevelNotes ⢠Energy levels are broken up into sublevels: ⢠There are at least 4 possible types of sublevelsâgiven labels: s, p, d, or f â˘
- 6. Hydrogen Atomic Orbitals(cont.) Energy sublevels are contained within the principal energy levels. 1 = 1sublevel ,s 2 = 2sublevel ,sp 3 = 3sublevel ,spd 4 = 4sublevel ,spdf
- 8. Electron Energy LevelNotes ⢠Only a certain number of electrons may exist in an energy level, but the number varies. It can be determined by: ⢠# of electrons in level = 2 x (# of energy level)2 ⢠Therefore: ⢠energy level 1 = 2 (1)2 = 2 ⢠energy level 2 = 2 (2)2 = 8 ⢠energy level 3 = 18 ⢠energy level 4 = 32 ⢠etc...
- 9. Electron Energy LevelNotes ⢠In each energy level, electrons fill sublevels in a certain order ⢠Level 1: ⢠only has one s sublevel (a spherical shape) ⢠2 electrons may fit in this sublevel--each one has an opposite âspinâ, allowing them to take up the same space ⢠Pauli exclusion principleâno more than 2 electrons may be found in the same orbital (âorbitalâ means a particular location)
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- 11. Electron Energy LevelNotes ⢠Level 2: ⢠has two sublevels: s and p ⢠2 electrons in s ⢠there are 3 different p orbitals, and may hold 2 electrons eachâ6 total. (look at shape on p. 154-- imagine how they can fit together) ⢠total of 8 overall in Level 2
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- 13. Electron Energy LevelNotes ⢠Level 3: ⢠has 3 sublevels: s, p, and d ⢠2 electrons in s ⢠6 electrons in p ⢠there are 5 different d orbitals, and 2 electrons can fit in eachâtotal of 10. (look at picture of d orbitals, imagine how they can fit together) ⢠total of 18
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- 15. Hydrogen Atomic Orbitals(cont.) Each energy sublevel relates to orbitals of different shape.
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- 17. Electron Energy LevelNotes ⢠Level 4: ⢠has 4 sublevels: s, p, d , and f ⢠2 electrons in s ⢠6 electrons in p ⢠10 electrons in d ⢠14 electrons in f (7 different orbitals for f) ⢠total of 32
- 18. Hydrogen Atomic Orbitals(cont.)
- 19. Electron Energy LevelNotes ⢠The order that electrons fill up orbitals does not follow the logical order of all 1âs, then all 2âs, then all 3âs, etc. ⢠They follow the order found based on certain rules.
- 21. ⢠ATOMIC #= #p+ = #e-
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- 23. Electron Energy LevelNotes ⢠An easy way to remember this is to use the periodic table--it is arranged to show how these orbitals are filled.
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- 25. Ground-State Electron Configuration Thearrangement of electrons in the atom is called the electron configuration. The aufbau principle states that each electron occupies the lowest energy orbital available.
- 26. Ground-State Electron Configuration(cont.) The Pauli exclusion principle states that a maximum of two electrons can occupy a single orbital, but only if the electrons have opposite spins. Hundâs rule states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same energy level orbitals.
- 27. Electron Energy LevelNotes ⢠Hundâs rule is used for filling orbitals with electrons. It states that only one electron will be put in each orbital of a sublevel until all of them are filled, and after that, they may be paired up until the sublevel is full.
- 28. Section 5-3 Ground-State ElectronConfiguration (cont.)
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- 30. Section 5-3 Ground-State ElectronConfiguration (cont.) Noble gas notation uses noble gas symbols in brackets to shorten inner electron configurations of other elements.
- 31. Section 5-3 Ground-State ElectronConfiguration (cont.) The electron configurations (for chromium, copper, and several other elements) reflect the increased stability of half-filled and filled sets of s and d orbitals.
- 32. Section 5-3 Valence Electrons Valenceelectrons are defined as electrons in the atomâs outermost orbitalsâthose associated with the atomâs highest principal energy level. Electron-dot structure consists of the elementâs symbol representing the nucleus, surrounded by dots representing the elementâs valence electrons.
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