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Let’s get it on!!!!!!

Let’s get it on!!!!!!. Name the geometry and give the bond angles?. t rigonal pyramidal 107.3. Name the geometry and give the bond angles?. Define covalent bond. The electrostatic force between atoms that results in the sharing of one or more pairs of electrons. Define covalent bond.

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Let’s get it on!!!!!!

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  1. Let’s get it on!!!!!!

  2. Name the geometry and give the bond angles?

  3. trigonal pyramidal 107.3 Name the geometry and give the bond angles?

  4. Define covalent bond.

  5. The electrostatic force between atoms that results in the sharing of one or more pairs of electrons Define covalent bond.

  6. List ALL the common diatomic molecules.

  7. H2 hydrogen N2 nitrogen O2 oxygen F2 fluorine Cl2 chlorine Br2 bromine I2 iodine List ALL the common diatomic molecules.

  8. Draw the Lewis structure and the structural formula for water.

  9. Lewis Structural H O H H O H Draw the Lewis structure and the structural formula for water.

  10. Name 3 ways to tell apart an oxyacid and a binary acid.

  11. Binary H and usually a halogen Oxyacids contain OXYANIONS Binary start with prefix hydro- Some Oxyacids end in –ous Formula of Binary only has 2 capital letters Name 3 ways to tell apart an oxyacid and a binary acid.

  12. E N E R G Y The green line refers to a molecules ____________. Distance

  13. E N E R G Y BOND DISSOCIATION ENERGY The green line refers to a molecules ____________. Distance

  14. The arrow is pointing to a

  15. σsigma bond The arrow is pointing to a

  16. What is the relationship between bond length and bond strength?

  17. The shorter the bond the stronger it is!!! What is the relationship between bond length and bond strength?

  18. Define endothermic! And explain the difference between endothemric and exothermic!!!

  19. Endothermic is used to describe a chemical reaction when you have to put more energy in to break the bonds then you get out when new bonds form!!!! Endothermic- you put more energy in Exothermic- you get more energy out Define endothermic! And explain the difference between endothemric and exothermic!!!

  20. List the rules for naming simple binary molecules

  21. Left to Right • “-ide” be back! • Junkies need their PRE-fix • EXCLUDE MONO on first element List the rules for naming simple binary molecules

  22. Name this H3PO3

  23. phosphorous acid PO33- phosphite ion Name this H3PO3

  24. Define resonance. Draw O3 showing resonance.

  25. A structure has resonance when one or more correct Lewis structures can be draw to show the sharing of electrons. O O O Define resonance. Draw O3 showing resonance.

  26. List the prefixes used in naming covalent molecules for 1-10.

  27. mono - 1 di - 2 tri - 3 tetra - 4 penta - 5 hexa - 6 hepta- 7octa - 8 nona - 9 deca - 10 List the prefixes used in naming covalent molecules for 1-10.

  28. List all 3 exceptions to the octet rule we discussed.

  29. Odd number of e- Fewer than 8 e- Expanded Octet List all 3 exceptions to the octet rule we discussed.

  30. Give an example of each of the exceptions to the octet rule.

  31. O N O NO2 H B H H SF6 BH3 F F F S F F Give an example of each of the exceptions to the octet rule. F

  32. Define bonding orbital.

  33. The region where shared electrons are most likely to be found. Define bonding orbital.

  34. What does VESPR stand for and what does it mean?

  35. Valence S hell E lectron P air R epulsion The VSPER model states that atoms will arrange themselves into molecules in such a way as to minimize the repulsion between pairs of electrons What does VSEPR stand for and what does it mean?

  36. A molecule that is sp3 hybridized with no lonepairs on the central atom would have bond angles of?

  37. 109.5 A molecule that is sp3 hybridized with no lonepairs on the central atom would have bond angles of?

  38. Name all of these molecular structure models.

  39. Stick Ball & Stick Name all of these molecular structure models. Space Filling

  40. Name and describe all IMF discussed in class.

  41. Dipole Dipole Forces Attraction between polar molecules The negative end of a polar molecule is attracted to the positive end of another polar molecule and vice-versa Dispersion Forces Attraction between non-polar molecules Electrons move and create small partial charges allowing for attraction Hydrogen bonding Attractive force between a H on one molecule and the N, F, or O of another molecule Name and describe all IMF discussed in class.

  42. According to the chart what is the bond character ratio of N2?

  43. 100:0 covalent:ionic N=3.04 3.04-3.04=0.00 According to the chart what is the bond character ratio of N2?

  44. Which Molecule is polar and why?

  45. F H N H F C F O F Which Molecule is polar and why?

  46. F H N H F C F O F Oxygen is the most electronegative atom in the molecule and will pull all electrons toward itself. F is more electronegative than C but the geometry cancels out the pull of each F. Which Molecule is polar and why?

  47. Draw the Lewis structure of sulfate.

  48. 2- 2- O O O O S S O O O O Draw the Lewis structure of sulfate.

  49. Explain a coordinate covalent bond and give an example of one.

  50. A coordinate covalent bond occurs when on atom donates both electrons that are involved in making a bond. H H H B H N H H Explain a coordinate covalent bond and give an example of one.

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