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Electron Configuration

Electron Configuration. Chemistry I Mr. Pena. 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

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  1. Electron Configuration Chemistry I Mr. Pena

  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 mathematicaly related to the wavelenght: c=λ﹒v Where c=speed of light (3.0 x 108 m/s) λ= wavelenght 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. Electron configuration • Orbital Filling Order (Diagonal Rule)

  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

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