1. HONORS REVIEW

2.  What are valence electrons?

3.  What are valence electrons Electrons in the outermost energy level

4.  What is the octet rule?

5. Rule that states that atoms will combine in such a way that each atom will have 8 electrons

6.  Exceptions to octet rule?

7. Boron – 6 electrons P or S – 10 or 12 electrons H and He – 2 electrons

8.  How to metals obey octet rule? How do non-metals obey octet rule?

9. Metals – give up electrons Non-metals – gain electrons

10.  What is the formula for ions achieving noble gas configuration? Ca O Br Al

11.  How do you determine the electron configuration for an ion?

12. First calculate number of electrons, then fill orbitals Ex: Mg +2

13.  What is the difference between an ionic bond and a covalent bond?

14. Ionic – opposite charged ions attract Covalent – atoms share electrons

15.  How do ionic bonds form?

16. A bond between metal and nonmetal – metal will give up electrons to non-metal resulting in a cation and anion which are attracted by opposite charges

17.  What are some characteristics of ionic compounds?

18. Made of anions and cations Called salts Higher BP and MP than covalent compounds – why?

19.  How do you name ionic compounds?

20. Cation – keeps name Anion – ending turns to –ide If polyatomic, keeps name

21.  CaBr 2  K 2 SO 4  Magnesium fluoride  Ammonium phosphate

22.  What elements form ionic bonds, covalent bonds, and metallic bonds?

23. Ionic – M and NM Covalent – NM and NM Metallic – M and M

24.  What state are ionic compounds normally in? covalent compounds?

25. Ionic – solid Covalent – gas or liquid

26.  What are some characteristics of metals?

27. Good electrical conductors due to movement of valence e - Ductile – drawn into wires Malleable – hammered into sheets

28.  How many electrons shared in the following bonds: Ionic Single covalent Double covalent Triple covalent

29.  How many electrons shared in the following bonds: Ionic - 0 Single covalent - 2 Double covalent - 4 Triple covalent - 6

30.  What are diatomic molecules?

31. Molecules in which both atoms are the same

32.  How do you determine how many bonds are in a molecule?

33. “Bond order” – calculate has, calculate want (want-has)/2 Example: CO

34.  What type of electrons are found in molecules?

35. Bonding electrons Non-bonding (unshared or lone pair) electrons

36.  What are all the possible types of bonds?

37. Ionic, nonpolar covalent, polar covalent, coordinate covalent, metallic

38.  How do sigma bonds form?

40.  How pi bonds formed?

42.  Draw the Lewis structures for the following: NO 3 -1 CH 2 S C 2 H 2

43.  What does VSEPR stand for? What does it mean?

44. Valence Shell Electron Pair Repulsion Electrons repel each other so shapes will result in them being far apart

45.  What shape has 1 central atom surrounded by 4 atoms, no lone pairs on central atom?

46. Tetrahedral

47.  What shape has 1 central atom surrounded by 3 atoms, one lone pair on central atom?

48. Trigonal pyramidal

49.  What shape has 1 central atom surrounded by 2 atoms, two lone pairs on central atom?

50. Bent

51.  What shape has 1 central atom surrounded by 6 atoms, no lone pairs on central atom?

52. Octahedral

53.  What shape has 1 central atom surrounded by 3 atoms, no lone pairs on central atom?

54. Trigonal planar

55.  How can you determine if a bond is polar covalent, non-polar covalent or ionic?

56. Electronegativity values

57.  What is happening in a polar covalent bond?

58. Electrons are being pulled towards the more electronegative atom resulting in a partial positive and partial negative charges

59.  Would a bond be more polar covalent or less polar covalent if atoms have a large electronegativity difference?

60. More polar covalent

61.  What is a dipole interaction?

62. Attraction between polar molecules

63.  What is a hydrogen bond?

64. Attraction between polar molecules that occurs when H is bound to highly EN atom (N, O, F) and is attracted another highly EN atom