1. Water: Structure and Special Properties

2. 5.1 Why Does Water Have Such Unusual Properties? To understand why water has such unusual properties, you must understand its chemical structure.

4. The Water Molecule A molecule is a group of two or more atoms held together by mutually shared electrons. When atoms combine with other atoms to form molecules they share or trade electrons and establish chemical bonds.

5. The Water Molecule A water molecule consists of a central oxygen atom covalently bonded to the two hydrogen atoms. The covalent bond in a water molecule is due to the sharing of electrons between oxygen and each hydrogen atom. They are relatively strong chemical bonds, so a lot of energy is needed to break them.

6. Instead of water’s atoms being in a straight line, both hydrogen atoms are on the same side of the oxygen atom. This curious bend in the geometry of the water molecule is the underlying cause of most of the unique properties of water.

8. Polarity The bent geometry of the water molecule gives a slight overall negative charge to the side of the oxygen atom and a slight overall positive charge to the side of the hydrogen atoms. This slight separation of charges gives the entire molecule an electrical polarity, and because there is both a positive and negative side of the molecule, water molecules are dipolar.

9. Interconnections of Molecules In water, the positively charged hydrogen area of one water molecule interacts with the negatively charged oxygen end of an adjacent water molecule, forming a hydrogen bond. The hydrogen bonds between water molecules are much weaker than the covalent bonds that hold individual water molecules together.

10. Polarity

11. Interconnections of Molecules Even though hydrogen bonds are weaker than covalent bonds, they are strong enough to cause water molecules to stick to one another and exhibit cohesion. The cohesive properties of water cause it to “bead up” and are responsible for the formation of rain drops.

12. Interconnections of Molecules The cohesive properties also give water its surface tension. Surface tension results from the formation of hydrogen bonds between the outermost layer of water molecules and the underlying molecules.

14. Adhesion Attraction between molecules of different substances. i.e. – water and other substances

15. Water: The Universal Solvent Water molecules stick not only to other water molecules, but also to other polar chemical compounds. In doing so, water molecules can reduce the attraction between ions or opposite charges by as much as 80 times.

16. Water: The Universal Solvent The electrostatic attraction between oppositely charged ions produces an ionic bond. When solid NaCl is placed in water, the electrostatic attraction (ionic bond) between them is reduced by 80 times. This, in turn, makes it much easier for the sodium and chloride ions to separate.

17. Water: The Universal Solvent When the ions separate, the positively charged sodium ions become attracted to the negative ends in the water molecules, and the negatively charged chloride ions become attracted to the positive ends of water molecules, and the salt is dissolved in water.

19. Water: The Universal Solvent The process by which water molecules completely surround ions is called hydration. Because water molecules interact with other water molecules and other polar molecules, water is able to dissolve almost everything. This is why water is called “the universal solvent”.

20. Thermal Properties Water exists on Earth as a solid, a liquid, and a gas. It has the capacity to store and releases great amounts of heat. Water’s thermal properties influence the world’s heat budget and are in part responsible for the development of tropical cyclones, worldwide wind belts, and ocean surface currents.

21. Thermal properties of water Solid, liquid, gas on Earth’s surface Water has high freezing point Water has high boiling point Water has high heat capacity Water has high latent heats

22. Heat capacity The amount of heat required to raise the temperature of 1 gram of any substance by 1 0 centigrade Water has a very high specific heat capacity It takes a lot of energy to increase water temperature

24. Heat capacity Why? It take more energy to increase the kinetic energy of hydrogen-bonded water molecules than it does for substances in which the bonds are from the much weaker van der Waals force.

25. The amount of heat absorbed or released is due to water’s high latent heat Latent ( hidden ) heats of Melting; freezing Vaporization, evaporation Condensation

26. Latent Heat Heat needed to change states of matter Movement of molecules: Ice- hardly any movement Gas- a lot of movement Changes in States of Matter: Add energy from surrounding area Melting, sublimation and vaporization Add heat to surrounding area Condensation, freezing and deposition

27. Heat absorbed or released with changes in state

28. As water evaporates from your skin, it cools your body by absorbing heat (this is why sweating cools your body)

29. Latent heat of Evaporation Heat energy that must be added to one gram of a liquid substance to convert it to a vapor at a given temperature below its boiling point. Surface water- Individual molecules converted from the liquid to the gaseous state have less energy than do water molecules at 100 degrees. So, individual molecules must gain energy from surrounding molecules The molecules left behind have lost heat energy to those that evaporate Cooling effect

30. Latent heat of Condensation When water vapor is cooled sufficiently, it condenses to a liquid and releases heat into the surrounding air. A steamer – small amount of heat is released to cook food Large thunderstorms/ Hurricanes – heat is released to power these storms.

31. Global thermostatic effects Properties that act to moderate changes in temperature, which in turn affect Earth’s climate Evaporation removes heat from oceans Condensation adds heat to atmosphere Heat re-distributed globally

34. Water density Related to how tightly the molecules or ions of a substance are packed together Maximum density at 4 o C Ice less dense than liquid water Atomic structure of ice Ice floats

37. Water density Increased salinity decreases temperature of maximum density Also, dissolved solids reduce the freezing point of water. Most seawater never freezes, Earth’s frigid poles Only at the surface Salt is spread on roads and sidewalks Salt lowers the freezing point of water.

38. Fig. 6-8

39. Salinity The total amount of solid material dissolved in water including dissolved gasses Expressed as parts/thousand o/oo i.e. – 35 0/00 seawater has 35 grams of salt in every 1000 grams of seawater Open ocean varies 33-38 0/00 Brackish (hyposaline) – 10 %0 Baltic Sea The Great Salt Lake – 280 0/00 Hypersaline – 330%0 Dead Sea

42. Dissolved Substances How are “salts” added and removed from the ocean? Added to oceans: River (primary input) Circulation through mid-ocean ridges Volcanic eruptions Removed from the ocean: Salt spray Recycling through mid-ocean ridges Biogenic sediments Evaporites, adsorption, precipitation

43. Measuring salinity Early methods involved evaporating a weighed amount of seawater and weighing the salts that precipitated from it. Chemical analysis Principle of Constant Proportions Chlorinity Electrical conductivity (salinometer)

44. Figure 6.13

45. Principle of Constant Proportions States that the major dissolved constituents responsible for the salinity of seawater occur nearly everywhere in the ocean in the exact same proportions, independent of salinity Basically – the ocean is well mixed!

46. Figure 6.21

47. Surface and Depth Salinity Variation Average seawater salinity is 35 o/oo, but it varies significantly from place to place at the surface and also with depth Surface Salinity- Tropics of Cancer and Capricorn warm, dry air near - increase salinity Little precipitation and runoff – decrease salinity Equator- warm temperatures increase salinity and increase precipitation and runoff offsets high salinity

49. Figure 6.22

50. Why doesn’t the surface of the ocean freeze except near the poles?

51. Fig. 6-7

52. Fig. 6-10

53. Factors affecting seawater density As Temperature increases, seawater density decreases ( due to thermal expansion) As salinity increases, seawater density increases (due to the addition of more dissolved material)

54. Water density and salinity Temperature and density share an inverse relationship As temperature increases density decreases Salinity and density share a positive relationship As salinity increases density increases

55. Figure 6.23