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Electron Configuration Notation with Atomic Structure Review

Electron Configuration Notation with Atomic Structure Review. Chemistry I Mr. Streeter. Bohr’s Atom Model. -Confines electrons in shells -Electrons loses energy due to movement. -Electrons can be in certain levels depending of the energy they have.

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Electron Configuration Notation with Atomic Structure Review

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  1. Electron Configuration Notation with Atomic Structure Review Chemistry I Mr. Streeter

  2. Bohr’s Atom Model -Confines electrons in shells -Electrons loses energy due to movement. -Electrons can be in certain levels depending of the energy they have. -The region where we can find the electron with high probability is called the orbital.

  3. Nature of the electron -Thompson’s work show that e- behave like particles. -In 1924, Louis de Broglie states that e- behave like waves based on Bohr’s model. -This was explained in the electromagnetic spectrum.

  4. Electromagnetic Spectrum • The frequency is mathematically related to the wavelength: c=λv Where c=speed of light (3.0 x 108 m/s) λ= wavelength v= frequency

  5. Electromagnetic Spectrum All the frequencies or wavelenghts of electric radiation.

  6. Electromagnetic Spectrum -The movement of electrons produced light when received and release energy. -In 1905, Albert Einstein proposed that light have properties of light and waves.

  7. Light Emission

  8. Light Emission • Electron in lowest possible energy is in ground state. • Electron that gains energy move to excited state. • Electron release energy as go back to ground state.

  9. Light Emission • E1=Energy in ground state • E2=Energy in excited stated. • Overall energy= E1-E2

  10. Quantum Numbers -Number that specifies the properties of the electrons. -There are 4 quantum numbers: n, , m and ms

  11. Quantum Numbers n= level number (n=1 thru 7).  (n-1)= Shape and type of orbital s=0 p=1 d=2 f= 3 m (from – ,0,+)=Magnetic quantum number ms= Magnetic spin. Only have two possible numbers (+1/2 and -1/2)

  12. Electron configurations -Arrangements of electrons in an atom. -Each orbital can have only 2 electrons and with different quantum numbers. This is known as Pauli exclusion principle.

  13. Electron configuration • Types and shapes of orbitals

  14. Electron configuration • Aufbau principle -Electron fill lowest energy levels first. Ex. 1s<2s<2p<3s<3p

  15. Electron configuration • Notations There are 3 notations: 1) Long notation or electron configuration 1s22s22p6 2) Orbital Notation

  16. Electron configuration • 3) Shorthand Notation or Noble Gas configuration. • [Ne]3s23p4

  17. Electron configuration • Hund’s Rule -For atoms in ground state, the number of unpaired electrons is the maximum possible and have the same spin.

  18. Order in which subshells are filled with electrons 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 3d 4d 5d 6d 4f 5f

  19. Electron configuration • Example What is the electron configuration of an element with atomic number of 9 (Z=9) An element with z=9 is Fluorine. We start with the less energy level and orbital, so then is 1s22s22p5. The orbital notation will be then

  20. Filling Rules for Electron Orbitals Aufbau Principle: Electrons are added one at a time to the lowest energy orbitals available until all the electrons of the atom have been accounted for. Pauli Exclusion Principle: An orbital can hold a maximum of two electrons. To occupy the same orbital, two electrons must spin in opposite directions. Hund’s Rule: Electrons occupy equal-energy orbitals so that a maximum number of unpaired electrons results. *Aufbau is German for “building up”

  21. General Rules • Pauli Exclusion Principle • Each orbital can hold TWO electrons with opposite spins. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  22. General Rules 6d 5f 6d 7s 5f Aufbau Principle • Electrons fill the lowest energy orbitals first. • “Lazy Tenant Rule” 6p 7s 5d 6p 4f 6s 5d 4f 5p 6s 4d 5p 5s 4d 4p 5s 3d 4p 4s 3d 4s 3p Energy 3p 3s 3s 2p 2p 2s 2s 1s 1s Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  23. General Rules • Hund’s Rule • Within a sublevel, place one electron per orbital before pairing them. • “Empty Bus Seat Rule” RIGHT WRONG Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  24. 8 O 15.9994 2s 2p 1s Notation • Orbital Diagram O 8e- • Electron Configuration 1s22s22p4 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  25. 16 S 32.066 Core Electrons Valence Electrons Notation • Longhand Configuration S 16e- 2p6 2s2 1s2 3s2 3p4 • Shorthand Configuration S 16e- [Ne]3s2 3p4 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

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