1. Ionic and Covalent Compounds

2. 1)What is the chemical formula? 2)How many valence electrons are being shared total? 3)How many valence electrons are NOT being shared? 4)What type of bond is between H and O? Single? Double? Triple? 5)Are each of the atoms happy? (yes or no) Station 1 H2OH2O 4 4 single yes

3. 1)What is the chemical formula? 2)How many electrons are being shared total? 3)How many electrons are NOT being shared? 4)How many electrons are in the double bond between N and O? 5)Are each of the atoms happy? (yes or no) Station 2 NO 3 8 16 4 yes

4. 1)What is the chemical formula? 2)How many electrons are being shared total? 3)How many electrons are NOT being shared? 4)How many electrons are in the triple bond between C and N ? 5)Are each of the atoms happy? (yes or no) Station 3 HCN 8 2 6 yes

5. 1)What is the chemical formula? 2)How many valence electrons are being shared total? 3)How many valence electrons are NOT being shared? 4)What type of bond is between O and O? Single? Double? Triple? 5)Are each of the atoms happy? (yes or no) Station 4 O2O2 4 8 double yes

6. 1. Look at the examples above. How many bonds does hydrogen form? 2. Hydrogen ALWAYS forms this number of bonds. Why? Station 5 ONE It only needs one more electron to have a full outer shell

7. 4) Compounds have a total charge of zero 5) Atoms share electrons 3) Atoms transfer electrons Ionic Compounds Covalent Compounds 2) Atoms in the compound have charges that balance out. 6) Formed when one atom wants to gain and one atom wants to lose electrons 1) Formed when one or more atoms want to gain electrons Station 6

8. 4) Compounds have a total charge of zero 5) Atoms share electrons 3) Atoms transfer electrons Ionic Compounds Covalent Compounds 2) Atoms in the compound have charges that balance out. 6) Formed when one atom wants to gain and one atom wants to lose electrons 1) Formed when one or more atoms want to gain electrons Station 6 KEY

9. Station 7: Ionic or Covalent Compound? (Just write I or C) 1) CO _______ 2)MgO_______ 3) BN_______ 4) Cl 2 _______ 5) KCl _______ C I I C I

10. Chemical Equations Basics

11. 36 18

15. 22 23 22 2 2 2 2

16. NaCl  Na + Cl 2 Al + HCl  AlCl 3 + H 2 22 2 26 3 Na + HCl  H 2 + NaCl 22 2 Balance these! AND decide what type of reaction… Decomposition Single replacement

17. Classifying Chemical Reactions

18. 1.N 2 + 3H 2  2NH 3 2.2KClO 3  2KCl + 3O 2 3.2NaCl + F 2  2NaF + Cl 2 4.2H 2 + O 2  2H 2 O 5.2AgNO 3 + MgCl 2  2AgCl + Mg(NO 3 ) 2 6.2AlBr 3 +3K 2 SO 4  6KBr + Al 2 (SO 4 ) 3 7.CH 4 + 2O 2  CO 2 + 2H 2 O 8.C 3 H 8 + 5O 2  3CO 2 + 4H 2 O 9.2C 8 H 18 + 25O 2  16CO 2 + 18H 2 O 10.FeCl 3 + 3NaOH  Fe(OH) 3 + 3NaCl 1. S 2. D 3. SR 4. S 5. DR 6. DR 7. C 8. C 9. C 10.DR

19. Characteristic Properties

29. Energy and Rate of Chemical Reactions

30. Exo or endo? Reaction Progress Energy

31. Exo or endo? Reaction Progress Energy

32. Exo or Endo? Reaction Progress Energy What “type” of reaction is this? C 3 H 8 + 5O 2 3CO 2 + 4H 2 O combustion

33. Exo or Endo? Reaction Progress Energy What “type” of reaction is this? 2H 2 + O 2 2H 2 O synthesis

34. Exo or Endo? Reaction Progress What “type” of reaction is this? 2AlBr 3 +3K 2 SO 4 6KBr + Al 2 (SO 4 ) 3 Double replacement

35. Exo or Endo? Reaction Progress What “type” of reaction is this? 2NaCl + F 2 2NaF + Cl 2 Single replacement

36. Exo or Endo? Reaction Progress Energy What “type” of reaction is this? 2KClO 3 2KCl + 3O 2 decomposition

37. Element Math- For Acuity

38. Protons: Neutrons Electrons: 20

39. Protons: Electrons: Neutrons: 19 20

40. Electrons: Protons: Neutrons: 22 26 22

41. Protons = Electrons = Neutrons = 14

42. Protons = Electrons = Neutrons = 15 16

43. Protons = Electrons = Neutrons = 18 22 18