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Orbitales “ s”

Orbitales “ s”. Orbitales “ p”. 3 O.A. p ( p x p y p z ) de même énergie. Orbitales “ d”. Spin e -. Orbitales électroniques. Tableau périodique des éléments. Valence. Rayon atomique. Rayon atomique. Énergie d’ionisation. Énergie d’ionisation. Énergie d’ionisation.

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Orbitales “ s”

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  1. Orbitales “s”

  2. Orbitales “p” 3 O.A. p (pxpypz) de mêmeénergie

  3. Orbitales “d”

  4. Spin e-

  5. Orbitalesélectroniques

  6. Tableau périodique des éléments

  7. Valence

  8. Rayon atomique

  9. Rayon atomique

  10. Énergie d’ionisation

  11. Énergie d’ionisation

  12. Énergie d’ionisation

  13. Énergie d’ionisation Na : 1s2 2s2 2p6 3s1 Mg : 1s2 2s2 2p6 3s2 Al : 1s2 2s2 2p6 3s2 3p1

  14. Taille ions

  15. Affinitéélectronique

  16. Electronégativité

  17. Electronegativité

  18. Ions • Un atomepossèdenormalement le mêmenombred’électronsque de protons. Autant de charges + que de charges -. La charge net de l’atomeestnulle. • Lorsqu’unatomeperdougagne un ouplusieursélectrons, ildevientionisé. Avec un déficitd’électrons, l’atome a une charge nette positive, avec un excédentd’électrons, ila une charge nette negative.

  19. Foreces Inter Atomiques • Attraction • Répulsion • Vander waals • Dipolaires

  20. Attractive / Repulsive Forces

  21. Energy and Bond Formation http://server.chem.ufl.edu/~chm2040/Notes/Chapter_10/properties.html#e_energies_and_affinities

  22. Types of Chemical Bonds • Covalent bonds • Shared electron, dipole possible • Ionic bonds • Shared electron, but strong dipole • Metallic bonds • Sea of electrons shared by all atoms • Semiconductors • Valence electron can move into band gap

  23. Liaison Ionique

  24. Comparison of Bonding

  25. Ionic Bond • Ionic bonding can be thought of as an ‘extreme dipole moment’ • Atom A (if a cation) loses much of the electron density in a valence shell • Atom B (if a anion) gains much of the electron density in a valence shell • Together, they form a chemical bond, with a strong dipole moment (cation => anion) • Very common in ceramics, salts and minerals

  26. Ionic Bonding • Occurs between + and - ions. • Requires electron transfer. • Large difference in electronegativity required • Example: NaCl

  27. Covalent Bond • Shared electrons • One electron from an orbital in atom A • One electron from an orbital in atom B • They become ‘spin paired’ • Lewis structure model for octet rule • VSERP – how shells form and repel • Chemistry is ‘physics in motion’

  28. Ionic Bond and Electronegativity • Consideration of electronegativity can demonstrate that ionic bonds are nothing more than an extreme case of a polar covalent bond. In fact… • If the electronegativity difference between two atoms is greater than 2.0, then any bond between these two atoms would be (defined as) ionic.

  29. - O H H + + Polar Covalent Bonds in H2O Electronegativity difference between oxygen and hydrogen

  30. Molecular Polarity If a molecule contains polar bonds, and if those polar bonds are located such that the + charges are at one end of the molecule and the - charges are at the other end, then the molecule is a polar molecule. The measure of molecular polarity is a quantity called the dipole moment (D).

  31. Si vous la voyez dans le sens horaire, vous utilisez majoritairement votre cerveau droit, sinon, c’est le gauche. Avec un peu de concentration, il est possible de changer le sens. le cerveau gauche : est utilisé pour la logique, les sciences, le langage, les maths ou encore la sécurité.Le cerveau droit : est quand à lui le lieu de la créativité, la philosophie, l’appréciation et la prise de risque.

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