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Q of the Day

Q of the Day. Day 2 3-30. Write the formula for magnesium chloride. Draw the dot structure for magnesium chloride. Valence-Shell, Electron-Pair Repulsion VSEPR theory. Repulsion between sets of valence-level electrons, causes them to be oriented as far apart as possible. VSEPR THEORY.

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Q of the Day

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  1. Q of the Day Day 2 3-30 • Write the formula for magnesium chloride. • Draw the dot structure for magnesium chloride.

  2. Valence-Shell, Electron-Pair Repulsion VSEPR theory Repulsion between sets of valence-level electrons, causes them to be oriented as far apart as possible

  3. VSEPR THEORY What do electrons do to other electrons? Chapter # 8 VSEPR theory – in a small molecule, the pairs of valence electrons are arranged as far apart from each other as possible

  4. Q of the Day Day 3 4-2 • Draw the dot structure for CH4.

  5. Lewis Dots Draw the Lewis Dot Structures for the following: NaCl, O2, CO2, H2O, BCl3, NH3, CH4

  6. Reds = oxygen short “bonds” = single bonds Blacks = carbon long “bonds” = double bonds Whites = hydrogen Greens = chlorine Blue = nitrogen VSEPR THEORY Build: O2 CO2 *BCl3 CH4 *NH3 H2O  Linear 1st & 5th pd stopped  Trigonal planar  Tetrahedral  Pyramidal 3rd pd stopped  Bent

  7. LINEAR LINEAR BENT TRIGONAL PLANAR PYRAMIDAL TETRAHEDRAL

  8. VSEPR THEORY Carbon compounds form 3 shapes, what are they? WHY? ______________________ ____________________________ ____________________________

  9. VSEPR THEORY For #s 58 + 60 on pages 256-257 DO DOT STRUCTURES AND SHAPES FOR BOTH!!!

  10. Homework Read Section 8.4 (pages 261-264 AND complete #s 61, 63, 64, 66 (only molecular shape not hybrid orbitals) AND # 60 = an optional bonus – must be correct

  11. Hybrid Orbitals Going back: How did we name orbitals? 2p Energy level Shape As atoms come together and bond, orbitals come together, overlap, and mix … hybridization

  12. Hybrid Orbitals As atoms come together and bond, orbitals come together, overlap, and mix … hybridization Hybrid orbitals – mixed orbitals – combo. of properties of the atomic orbitals that formed them

  13. Polarity Polar bonds? Br H Polar Covalent 2.8 2.1

  14. Polarity Intramolecular Forces Forces of attraction within molecules H O H Intermolecular Forces Forces of attraction between molecules

  15. Polarity PERIODS 3 & 6 – 2-18 Intermolecular Forces Forces of attraction between molecules Hydrogen Bonding H H H O O O (-) (+) (-) (+) (-) (+) H H H

  16. Polarity Hydrogen bonding is a direct result of water’s polar nature and leads to … Water sticking to something else Water sticking to water … cohesion … adhesion

  17. Polarity Does a polar bond mean you have a polar molecule? CO2 – Polar bonds? Polar molecule?

  18. Polarity Does a polar bond mean you have a polar molecule? Polar molecules  unequal charge distribution …2 factors are molecular shape and bonds (polar vs. nonpolar)

  19. Polarity PERIODS 1 & 5 – 2-18 Polar bond(s)? Polar molecule? HCl SiS2 BCl3 NH3

  20. Homework Read section 12.2 AND complete the section review on page 414 #s 14-16

  21. Quick Talk Linear VSEPR theory Intermolecular force Cohesion H2SO4 Hydrogen bonding Bent Adhesion Intracellular Octet rule

  22. Homework Read section

  23. H Intracellular O H Br H Polar Covalent 2.8 2.1

  24. H H H O O O (-) (+) (-) (+) (-) (+) H H H H H Intercellular O O (-) (+) (-) (+) H H

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