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Expanding on Lewis Structures

Expanding on Lewis Structures. Lewis Structures. You can use lewis structures to predict some patterns in bonding. Example : Nitrogen Lewis Structure: How many unpaired electrons? 3 How many bonds will it form? 3. Practice Lewis Structures. Draw the Lewis Structures for: SeF 2 SnCl 4

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Expanding on Lewis Structures

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  1. Expanding on Lewis Structures

  2. Lewis Structures • You can use lewis structures to predict some patterns in bonding. • Example : Nitrogen • Lewis Structure: • How many unpaired electrons? • 3 • How many bonds will it form? • 3

  3. Practice Lewis Structures • Draw the Lewis Structures for: • SeF2 • SnCl4 • BF3 • Octet rule exception • B is fine with 3 bonds – it has 3 valence, so 3 bonds are expected • F NEVER FORMS A DOUBLE BOND

  4. Practice Lewis Structures • Draw the Lewis Structures for: • NO • Odd electron molecules can’t obey the octet rule… why? • ClO2 • Free Radicals – chemical species with an unpaired electron

  5. Practice Lewis Structures • Draw the Lewis Structures for: • SF4 • Expanded octet… empty 3d orbitals in S • I3- • F3- • Can’t happen… no “d” orbitals to hold electrons • Only elements of the 3rd or higher periods in the periodic table may form compounds or ions in which an octet is exceeded

  6. Practice Lewis Structures • SiF5- • PF5 • ClF3 • XeF2

  7. Molecular Shapes VESPER… oh yeah…

  8. Molecular Shapes • Lewis dot structures can help us to predict the 3-dimensional geometry of molecules and ions. • The shape of a molecule plays an important role in its reactivity. • By noting the number of bonding and nonbonding electron pairs we can easily predict the shape of the molecule.

  9. Valence Shell Electron Pair Repulsion Theory (VESPER) • Electron pairs in molecules (either bonding or nonbonding) want to maximize the distance between them. • Bond and lone electron pairs in the valence shell of an element repel each other and seek to be as far apart as possible.

  10. Valence Shell Electron Pair Repulsion Theory (VESPER) “The best arrangement of a given number of electron domains is the one that minimizes the repulsions among them.”

  11. Electron Domains • We can refer to the electron pairs as electrondomains. • In a double or triple bond, all electrons shared between those two atoms are on the same side of the central atom; therefore, they count as one electron domain. • The central atom in this molecule, A, has four electron domains.

  12. Electron-Domain Geometries These are the electron-domain geometries for two through six electron domains around a central atom.

  13. Electron-Domain Geometries • All one must do is count the number of electron domains in the Lewis structure. • The geometry will be that which corresponds to the number of electron domains.

  14. Molecular Geometries • The electron-domain geometry is often not the shape of the molecule, however. • The molecular geometry is defined by the positions of only the atoms in the molecules, not the nonbonding pairs.

  15. Molecular Geometries Within each electron domain, then, there might be more than one molecular geometry.

  16. Linear Electron Domain • In the linear domain, there is only one molecular geometry: linear. • NOTE: If there are only two atoms in the molecule, the molecule will be linear no matter what the electron domain is.

  17. Trigonal Planar Electron Domain • There are two molecular geometries: • Trigonal planar, if all the electron domains are bonding • Bent, if one of the domains is a nonbonding pair.

  18. Nonbonding Pairs and Bond Angle • Nonbonding pairs are physically larger than bonding pairs. • Therefore, their repulsions are greater; this tends to decrease bond angles in a molecule.

  19. Multiple Bonds and Bond Angles • Double and triple bonds place greater electron density on one side of the central atom than do single bonds. • Therefore, they also affect bond angles.

  20. Tetrahedral Electron Domain

  21. Tetrahedral Electron Domain • There are three molecular geometries: • Tetrahedral, if all are bonding pairs • Trigonal pyramidal if one is a nonbonding pair • Bent if there are two nonbonding pairs.

  22. Trigonal Bipyramidal Electron Domain • There are two distinct positions in this geometry: • Axial • Top and bottom positions • Equatorial • Middle positions

  23. Trigonal Bipyramidal Electron Domain Lower-energy conformations result from having nonbonding electron pairs in equatorial, rather than axial, positions in this geometry.

  24. Trigonal Bipyramidal Electron Domain • There are four distinct molecular geometries in this domain: • Trigonal bipyramidal • Seesaw • T-shaped • Linear

  25. Trigonal Bipyramidal Electron Domain

  26. Octahedral Electron Domain • All positions are equivalent in the octahedral domain. • There are three molecular geometries: • Octahedral • Square pyramidal • Square planar

  27. Octahedral Electron Domain

  28. Larger Molecules In larger molecules, it makes more sense to talk about the geometry about a particular atom rather than the geometry of the molecule as a whole.

  29. Larger Moleules This approach makes sense, especially because larger molecules tend to react at a particular site in the molecule.

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