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CHAPTER 5

CHAPTER 5. ELECTRON CONFIGURATION. UNITED STATES  NEW JERSEY  MIDDLESEX COUNTY  EDISON Township  YOUR HOUSE . ATOM ENERGY LEVEL SUBLEVEL ORBITAL LOCATION OF ELECTRON. ANALOGY OF THE ATOM. 1. Principle Energy Levels: (n = 1,2,3….7) a.k.a shells

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CHAPTER 5

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  1. CHAPTER 5 ELECTRON CONFIGURATION

  2. UNITED STATES NEW JERSEY MIDDLESEX COUNTY EDISON Township YOUR HOUSE ATOM ENERGY LEVEL SUBLEVEL ORBITAL LOCATION OF ELECTRON ANALOGY OF THE ATOM

  3. 1.Principle Energy Levels: (n = 1,2,3….7) a.k.a shells • Different values of n = different energy levels & different electron energies • Maximum number of e- each level holds is found by: 2n2 EX: 1st energy level (n=1) 2n2 = 2(1)2= 2 electrons in 1st energy level

  4. 2.Sublevels: s (spherical), p (dumbbell), d, f • Cloud shapes • The # of energy sublevels is the same as the energy level #

  5. 3.Orbitals: • Each sublevel has a different # of orbitals which means a different # of electrons • The # of orbitals in an energy level is found by: n2 EX: 3rd energy level (n=3) 32 = 9 orbitals This makes sense because: • 3rd energy level would have 3 sublevels; • s sublevel with 1 orbital, • p sublevel with 3 orbitals, and • d sublevel with 5 orbitals.  • SO……1 + 3 + 5 = 9, so the formula n2 works!

  6. PRACTICE Principle Energy Level 2p5 Number of Electrons in Sublevel Type of Electron Sublevel

  7. HOW TO DETERMINE ELECTRON CONFIGURATIONS • How electrons are arranged around the nuclei of atoms • 3 RULES: • Aufbau • Pauli Exclusion Principle • Hund’s Rule

  8. Aufbau Principle: • Electrons enter orbitals of lowest energy level 1st • Start at the beginning of each arrow, and then follow it all of the way to the end. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

  9. 2. Pauli Exclusion Principle: • Orbitals can hold only 2 electrons • Each electron in the orbital has an opposite spin 1s2

  10. 1s2 2s2 2p3 • 3. Hund’s Rule: • One electron enters each orbital until all orbitals contain one electron with parallel spins. 1s2 2s2 2p4

  11. Bohr Model- Line Spectra Explained • Electrons can occupy specific energy levels • Excited atoms can emit light • Each orbital they are in has specific energy.

  12. Atomic Emission Spectrum Spectrometer: Breaks up what we see as continuous light into individual bands of light. The individual bands of light represent the exact frequency of light be given off. This corresponds to the quantum of energy that is released when an electron goes from an excited state to the ground state.

  13. Electrons move from ground state to an excited state and back again.

  14. The bands of light are called: ATOMIC EMISSION SPECTRUM This spectrum is unique to every element.

  15. Atomic Emission Spectrum Add energy

  16. Different elements are used to give fireworks their color! • To learn more about the science of fireworks see:http://www.pbs.org/wgbh/nova/kaboom/

  17. Electromagnetic Spectrum

  18. How Does the Atomic Emission Spectrum Correspond to Electron Configuration? 1. Electrons get excited when we introduce ENERGY (fire, electricity, light) 2. Electrons jump from ground state to an excited state

  19. 3. The amount of energy needed to do this is a QUANTUM of energy QUANTUM:is the amount of energy needed to move an electron from one energy level to the next. 4. Electrons go back to the ground state and give off this energy in the form of light (PHOTONS) PHOTON: a quantum of light; a discrete amount of energy that behaves as a particle.

  20. E= h c / l E= Energy h= Planck’s constant c= speed of light l=wavelength

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