1. Bonding

7. ION Charged atom Na + (has lost one electron) O -2 (has gained two electrons)

8. Bonding Covalent share electrons Ionic transfer of electrons (lose or gain)

9. IONIC BOND An atom may lose one or more electrons and become positive (+) An atom may gain one or more electrons and become negative (-) The (+) and (-) ions formed now attract each other and form an ionic bond.

10. Ionic Bonds Sodium losesChlorine gains an electron become +becomes -

11. NaCl: Ionic Bond Tutorial 2.1 Chemical Bond Formation

12. Why do atoms bond? To have filled outer electron shells! Atom Heaven (stable)

13. Why do atoms bond? See the filled electron shells.

14. Filled outer e- shells How many e- fill the first shell (nearest the nucleus)? How many e- fill the next two shells? 2,8,8 nucleus

15. Gain 1 e- or lose 7 e-? If gains 1 e-, then it becomes -1

16. Gain 7 e- or lose 1 e-? If loses 1 e-, the it becomes +1.

17. Gain or Lose ? If it could as easily lose or gain e-, then it will probably share them. It will form a covalent bond.

19. Covalent Bonding = Shared e-

20. Polar Covalent Bonding of Water: Unequal sharing of electrons

22. Nonpolar Covalent Bond Equal sharing of electrons Like with carbon dioxide

23. Bonds Single Bond C-C C:C Double Bond C=C C::C Triple Bond C≡C C:::C

25. Single Bond and Double Bonds

27. Chemical Reaction A process to break or share electrons to form or break bonds Click Here Sodium and Chlorine Chemical ReactionSodium and Chlorine Chemical Reaction Also scroll down for covalent bonding AND polar covalent bonding in water

28. Chemical Reactions Reactants on the left of the arrow Products on the right of the arrow IDENTIFY: 2Mg(s) + O2(g) → 2MgO(s) MgO(s) + H2O(l) → Mg(OH)2(s) N2(g) + 3H2(g) → 2NH3(g)

29. Chemical Reaction Example A silver spoon tarnishes. The silver reacts with sulfur in the air to make silver sulfide, the black material we call tarnish. 2 Ag + S Ag 2 S

30. Chemical Reaction Example An iron bar rusts. The iron reacts with oxygen in the air to make rust. 4 Fe + 3 O 2 2 Fe 2 O 3

31. WATER Polar Covalent Bonds H H O

32. Polarity of Water Uneven sharing of electrons Polar covalent Polar Bonding

33. Contrast Polar Uneven distribution of electrons EX: Water Non-polar Even distribution of electrons EX: CO, oil

34. Hydrogen Bonds O - to H+ to 4 other water

35. Hydrogen Bonds Between slightly (+) H atom to a slightly (-) atom of a different molecule H-bonding of Water (nice animation)H-bonding of Water

36. Hydrogen Bonds Weak bonds But they are strong enough to cause water to needing a lot of heat to boil or to evaporate, and they form a less dense ice open lattice.

37. Cohesion Water is attracted to other water molecules (similar polar molecules) H-bonding between water molecules hold them together

39. Cohesion is why a waterfall, a stream, a water drop forms

40. Adhesion Attraction of unlike substances Like water to the sides of a glass tube Not so much with plastic Strong adhesion to glass

41. Water is a Good Solvent Can dissolve many substances

42. Water is the “Universal Solvent” Dissolving NaCl in water movieDissolving NaCl in water movie dissolve

43. Water is the Universal Solvent WHY? Can dissolve a lot of things What types of compounds are good at dissolving? –Polar –Ionic

44. How does detergent work? Soap has a water-loving (hydrophilic) and a water- hating end (hydrophobic). It attaches to the oil and then the water to wash away the oil.

45. Amphipathic Bipolar A molecule that is water-loving (polar) at one end and water- hating (non-polar, like oils) at the other end

46. Capillary Action The thinner the straw or tube the higher up capillary action will pull the water. Plant Capillarity

47. High Specific Heat Takes a lot of heat to raise the temperature of water (break the H-bonds) This is why coastal areas have mild climates

48. Surface Tension - the attraction of molecules to each other on a liquid's surface --creates a “film” Surface Tension

49. Floating Penny And paper clip H-bonds pull in water molecules and form a “film”

50. Water Strider Can stand on top of water Basilisk Lizard on WaterBasilisk Lizard on Water Water strider skimming across pondWater strider skimming across pond

51. Can exist as... Gas Liquid Solid Note in the solid ice, it is not much denser Due to H-bonds opening a lattice

52. High Heat of Vaporization Takes a high temperature to evaporate, or boil water Need to break those H-bonds

53. High Heat of Fusion Takes a low temperature to freeze water Those H-bonds must form

54. Water expands upon freezing If water worked like other liquids, then there would be no such thing as an ice berg, the ice cubes in your soft drink would sink to the bottom of the glass, and ponds would freeze from the bottom up!

55. Ice forms an Open lattice Below 4 o C Ice floats H-bonds are more stable in the solid form of water

56. Ice Expands

57. Water Molecules Can bond to four other water molecules H+ end attracts the O-ends + + -

59. Solutions A SOLUTE is the substance to be dissolved (sugar). The other is a SOLVENT. The solvent is the one doing the dissolving (water). As a rule of thumb there is usually more solvent than solute.

60. Solution = solvent + solute

61. SOLUTIONS When one substance dissolves another substance. SOLVENT + SOLUTE = SOLUTION Solvent=material in which the other material is being dissolved Solute=what is being dissolved

62. SALT SOLUTION Animation of Salt Dissolving in Water Dissolve Another Nice AnimationDissolve When water is the solvent, the solution is called an aqueous solution.

63. Salt Solution Which is the solvent? Which is the solute? Water is solvent. Salt is the solute.

64. FYI The solvent is defined as the substance that exists in a greater quantity than the solute(s) in the solution. Generally polar or ionic compounds will only dissolve in polar solvents.

65. Can you undissolve a dye? Undeniable Facts: Undeniable Friday: Un-dissolving Dye- a fact a dayUndeniable Facts: Undeniable Friday: Un-dissolving Dye- a fact a day Scroll down web page for explanation.

66. Dissociation (break into its ions) of Water Acids release H+ (hydronium) Bases release OH- (hydroxide)

67. Hydronium Ion = H+ Hydroxide Ion = OH- Animation of Dissociation of Water

68. pH * at pH 7.0, a solution is neutral * at lower pH (1-6), a solution is aacidic * at higher pH (8-14), a solution is basic

69. How much more? For every pH level lower there are 10 X’s more H+ ions So…… pH 2 has how many more H+ ions than pH 3? 10 So…pH 2 has how many more H+ ions than pH 4? 100

71. pH 1-6 = acid (the closer to “1” the stronger the acid) donates lots of H+ ions 8-14 = base (the closer to “14” the stronger the base) donate lots of OH- ions 7 = neutral or equal number of H+ and OH-

72. Buffer A substance that resists a change in pH when small quantities of acid or base are added (they are in the pH solutions for the duckweed)