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2. 1. Compare & contrast ionic and covalent bonds in terms of electron position. 2. Predict formulas for stable binary ionic compounds based on balance of charges. 3. Use IUPAC nomenclature for transition between chemical names and chemical formulas of - binary ionic compounds - binary covalent compounds 4. Apply the Law of Conservation of Matter by balancing the following types of chemical equations: Synthesis Decomposition Single Replacement Double ReplacementGOALS 2 34 16

3. Why do Atoms Form Compounds? Stability. What makes an atom stable? Full outer energy level. Eight. Chart page 576. 3

4. A Chemical Bond holds atoms together in a compound. Two basic typesTwo basic types: Ionic Covalent 4

5. Ionic Bonding T r a n s f e r o f e l e c t r o n s f r o m o n e a t o m t o a n o t h e r a t o m. O c c u r s b e t w e e n m e t a l s a n d n o n m e t a l s. Remember: Atoms need a full outer energy level to be stable. EIGHT! 5

6. O c c u r s b e t w e e n m e t a l s a n d n o n m e t a l s. M e t a l s a r e e l e c t r o n d o n o r s. N o n - m e t a l s a r e e l e c t r o n a c c e p t e r s. C a l l e d c o m p o u n d s. 6

7. 7

8. OPPOSITES ATTRACT! 8

9. CLIP 9

10. Covalent Bonding T h e s h a r i n g o f e l e c t r o n s b e t w e e n a t o m s. O c c u r s b e t w e e n n o n m e t a l s a n d n o n m e t a l s. C a l l e d M o l e c u l e s. 10

11. 11

12. Hydrogen and Fluorine Hydrogen and Chlorine 12

13. Single, Double, Triple 13

14. Clip 14

15. Unequal Sharing δ+δ+ Polar δ_δ_ When one atom has a greater positive charge 15

16. 1.CO 2 2.H 2 O 3.NaCl 4.MgCl 2 5.NO 2 6.H 2 SO 4 7.NaF 9.NaPO 4 10.HCl 11.NaF 12.KCl 13.CaCO 3 14.N 2 15.Cl 2 clip 16

17. Goals revisited

18. Writing chemical formulas is a shorthand way of indicating what a substance is made of. These formulas also let you know how many atoms of each type are found in a molecule. The chemical formula for water is H 2 O. Carbon Dioxide is CO 2. Why does oxygen combine in different ratios, in different compounds? The chemical formula for table salt is NaCl. Calcium Chloride is CaCl 2. Why does chlorine combine in different ratios, in different compounds? 17

19. The simplest compounds are ones with only two elements These are called binary KI, CO, H 2 O, NaCl 18

20. +1 +2 -2 -3+3 +4 -4 0 Oxidation numbers 19 Tell you how many electrons an atom must gain, lose or share to become stable.

21. We can predict the ratio of atoms in ionic compounds based on their oxidation numbers Oxidation numbers K Cl +1 KCl Tells you how many electrons an atom must gain, lose or share to become stable. 1 valence electron 7 valence electron All compounds are neutral That means the overall charge is ZERO! 20

22. Subscripts show the number of atoms of that kind in the compound Na Br +1 NaBr Ca Br +2 CaBr 2 To make it ZERO, you need 1 Ca & 2 Br. 21

23. Some elements have more than one oxidation number (Chart p588) Fe O +3 -2 Fe 2 O 3 Fe O +2-2 FeO We call these elements- Multivalent Elements 22

24. Now You Try writing Binary Ionic formulas 1.K + Br 2.Mg + Cl 3.Ca + I 4.K + O 5.K + I 6.Sr + Br 7.Na + O 8.Ga + Br 9.Fe +2 + O 10.Fe +3 + O 11.Cu +2 + F 12.Cr +3 + O 13.Mg + O 14.Al + P

25. Cations:ammonium, NH 4 + Anions: nitrate, NO 3 - sulfate, SO 4 2- hydroxide, OH - phosphate, PO 4 3- carbonate, CO 3 2- chlorate, ClO 3 - permanganate, MnO 4 - chromate, CrO 4 2- Polyatomic Ions Groups of Covalently Bonded atoms that stay together. 24

26. Try these……. 1. Na + SO 4 2. Mg + PO 4 3. Ca + CO 3 4. Na + OH 5. Mg + OH 6. NH 4 + OH 7. K + PO 4 8. NH 4 + NO 3 9. H + SO 4 10. Ca + SO 4 11. K + NO 3 12. Na + PO 4 25

28. Naming Binary Compounds and Molecules Steps: –I–If it is Binary- 1.Decide if it is an ionic or covalent bond. –M–Metal- nonmetal….. »I»Ionic –N–Nonmetal- nonmetal…. »C»Covalent 26 Example: NaCl

29. If ionic ……. 2.C heck to see if any elements are multivalent. 3.I f all single valent, write the name of the positive ion first. 4.W rite the root of the negative ion and add –ide. Examples: 1.NaCl 2.K 2 O 3.AlCl 3 4.BaF 2 5.KI 6.Li 2 O

30. If ionic ……. 2.Check to see if any elements are multivalent. 3.If multivalent ions, determine the oxidation number of the element. 4.Use Roman numerals in parentheses after the name of the element. 5.Write the root of the negative ion and add –ide. Examples: 1.FeO 2.Fe 2 O 3 3.CuO 4.Cu 2 O 5.PbCl 4 6.PbI 2 30

31. If Covalent... 2.Use Greek prefix to indicate how many atoms of each element are in the molecule 3.Add -ide to the more electronegative element Greek Prefixes 1- mono- 2- di- 3- tri- 4- tetra- 5- penta- 6- hexa- 7- hepta- 8- octa- Example: NO Nitrogen Monoxide PCl 3 Phosphorous trichloride 31

32. If it contains a polyatomic ion... 2.Write the name of the positive ion. 3.Write the name of the polyatomic ion. Examples: 1.NaCO 3 2.KNO 3 3.NaC 2 H 3 O 2 Example: KOH Potassium Hydroxide CaCO 3 Calcium Carbonate 32

33. Name the following: 1.KBr 2.HCl 3.MgO 4.CaCl 5.H 2 O 6.NO 2 7.CuSO 4 8.CaSO 4 9.NH 4 OH 10.CaCO 3 11.Cu(ClO 3 ) 2 12.Cr 2 O 3 13.SrI 2 14.CCl 4 33

34. 34 Goals revisited

35. Chemical Reactions A chemical reaction is a change in which one or more substances are converted into new substances. –R–Rearrangement of bonds in compounds and molecules. Chemical Equations make it possible to see clearly what is happen during a chemical reaction 35

36. Chemical equations are a shorthand way to show chemical reactions. ReactantsProducts H 2 + O 2 H 2 O 36

37. Conservation of Mass T h e m a s s o f t h e p r o d u c t s a l w a y s e q u a l s t h e m a s s o f t h e r e a c t a n t s 37

38. H 2 + O 2 H2OH2O 2 Hydrogen atoms 2 Oxygen atoms 2 Hydrogen atoms & one Oxygen atom Does this meet the Conservation of Mass Law? Must Balance the Equation to show Conservation of Mass. 38

39. 2 H 2 + O 2 H2OH2O 2 4122 2 4 Balanced!! Can add coefficients to Balance equations. Steps: 1. Count Atoms on both sides 2. If not Balanced, add coefficients to balance. 3. Recount atoms after adding each coefficient. 2 4. Keep adding coefficients until balanced. 39

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41. 1.Synthesis 2.Decomposition 3.Single Replacement (Single Displacement) 4.Double Replacement (Double Displacement) 41

42. Synthesis “to make” A + B AB Cu + O CuO 2H 2 + O 2 2H 2 O

43. Decomposition “to breakdown” 2H 2 O 2H 2 + O 2 AB A + B NaOH Na + OH

44. Single Replacement When one element replaces another element in a compound A + BC AC + B Cu+AgNO 3 Cu(NO 3 ) 2 + 2Ag The more reactive metal will always replace the less reactive metal. (p749)

45. Clip Single Replacement

46. Double Replacement Positive Ion of One compound replaces the positive ion of another compound and a Precipitate is formed. AB + CD AD + CB Ba(NO 3 ) 2 +K 2 SO 4 BaSO 4 2KNO 3 Clip

49. Chemical Reactions and Energy All chemical reactions release or absorb energy. –H–Heat, light, sound Chemical reactions are the making and breaking or bonds. 51

50. 1. Exergonic Chemical reactions that releases energy are called exergonic. –G–Glow sticks If heat is released, it is called exothermic.

51. 2. Endergonic Chemical reactions that require energy are called endergonic. Ex: Cold Packs If heat is absorbed, it is called endothermic

52. Catalysts and Inhibitors Some reactions proceed slowly. They can be sped up by a catalysts. –C–Catalysts are not used up in the reaction. –E–EX: enzymes (biological catalysts) Some reactions proceed too fast. They can be slowed down by inhibitors. –E–EX: Preservatives in food

53. 1. Compare & contrast ionic and covalent bonds in terms of electron position. 2. Predict formulas for stable binary ionic compounds based on balance of charges. 3. Use IUPAC nomenclature for transition between chemical names and chemical formulas of binary ionic compounds binary covalent compounds 4. Apply the Law of Conservation of Matter by balancing the following types of chemical equations: Synthesis Decomposition Single Replacement Double Replacement GOALS Revisited…..