LifeDependsontheUniquePropertiesofWater生命取決于水的獨(dú)特性能精選35張課件

1、All living things are dependent on water. Inside your body, your cells are surrounded by a fluid that is mostly water, and your cells themselves are 70 to 95 percent water. The abundance of water is a major reason Earth can support life. 第1頁，共35頁。The Structure of WaterA water molecule at first may s

2、eem pretty simple. Its two hydrogen atoms are each joined to an oxygen atom by a single covalent bond. 第2頁，共35頁。The key to waters unusual properties is that the electrons of each covalent bond are not shared equally between oxygen and hydrogen atoms. Oxygen pulls electrons much more strongly than do

3、es hydrogen. 第3頁，共35頁。Part of the reason is that the oxygen nucleus has eight protons, and therefore has a stronger positive charge than the hydrogen nucleus, which has one proton. This unequal pull results in the shared electrons spending more of their time in the neighborhood of the oxygen atom. 第

4、4頁，共35頁。The unequal sharing of electrons causes the oxygen end of the molecule to have a slight negative charge, while the end with the two hydrogen atoms is slightly positive. A molecule in which opposite ends have opposite electric charges is called a polar molecule. Water is a compound consisting

5、 of polar molecules. 第5頁，共35頁。Water molecules are attracted to one another in a specific way. The slightly negative oxygen end of one molecule attracts the slightly positive hydrogen ends of adjacent water molecules, causing the molecules to become arranged as you see in Figure 4-12. 第6頁，共35頁。This t

6、ype of weak attraction between the hydrogen atom of one molecule and a slightly negative atom within another molecule is a type of chemical bond called a hydrogen bond. Because the atoms within the water molecules have not transferred an electron (and thus a full unit of charge) to another atom, the

7、 attraction in a hydrogen bond is not as strong as that in an ionic bond. 第7頁，共35頁。Waters Life-Supporting Properties The polar nature of water and the effects of hydrogen bonding explain most of waters unique properties. These properties include cohesion and adhesion, temperature moderation, the low

8、er density of ice compared to liquid water, and waters ability to dissolve other substances. 第8頁，共35頁。Cohesion and Adhesion Each hydrogen bond between molecules of liquid water lasts for only a few trillionths of a second. Yet, at any instant most of the molecules are involved in hydrogen bonding wi

9、th other molecules because new hydrogen bonds form as fast as old ones break. 第9頁，共35頁。This tendency of molecules of the same kind to stick to one another is called cohesion. Cohesion is much stronger for water than for most other liquids. Water molecules are also attracted to certain other molecule

10、s. The type of attraction that occurs between unlike molecules is called adhesion. 第10頁，共35頁。Both cohesion and adhesion are important in the living world. One of the most important effects of these forces is keeping large molecules organized and arranged in a way that enables them to function proper

11、ly in cells. 第11頁，共35頁。Trees depend on cohesion and adhesion to help transport water from their roots to their leaves.The evaporation of water from leaves pulls water upward from the roots through narrow tubes in the trunk of the tree. As a result of cohesion, water moves against the force of gravit

12、y even to the top of a very tall tree. 第12頁，共35頁。第13頁，共35頁。Temperature Moderation Thermal energy is the total amount of energy associated with the random movement of atoms and molecules in a sample of matter. Temperature is a measure of the average energy of random motion of the particles in a subst

13、ance. When two substances differ in temperature, thermal energy in the form of heat is transferred from the warmer substance to the cooler one. 第14頁，共35頁。When you heat a substancesuch as a metal pan or waterits temperature rises because its molecules move faster. But in water, some of the thermal en

14、ergy that is absorbed goes to break hydrogen bonds. That doesnt happen in the metal pan, which has no hydrogen bonds. As a result, the water absorbs the same amount of thermal energy but undergoes less temperature change than the metal. 第15頁，共35頁。Conversely, when you cool a substance, the molecules

15、slow and the temperature drops. But as water cools, it forms hydrogen bonds. This releases thermal energy in the form of heat, so there is less of a drop in temperature than in metal. 第16頁，共35頁。One result of this property is that it causes oceans and large lakes to moderate the temperatures of nearb

16、y land areas. In other words, coastal areas generally have less extreme temperatures than inland areas. 第17頁，共35頁。Water also moderates temperature through evaporation, such as when you sweat. Evaporation occurs when molecules at the surface of a liquid escape to the air. As water molecules evaporate

17、, the remaining liquid becomes cooler. 第18頁，共35頁。Low Density of Ice Density is the amount of matter in a given volume. A high-density substance is more tightly packed than a low-density substance. In most substances, the solid state is more dense than the liquid state. 第19頁，共35頁。Water is just the op

18、positeits solid form (ice) is less dense than the cold liquid form. Once again, hydrogen bonds are the reason. Because the molecules in liquid water are moving faster than those in ice, there are fewer and more short-lived hydrogen bonds between molecules. 第20頁，共35頁。The liquid water molecules can fi

19、t more closely together than the molecules in ice. Since substances of lesser density float in substances of greater density, ice floats in liquid water.第21頁，共35頁。Ice floats because its molecules are less densely packed than those in liquid water. 第22頁，共35頁。How is the fact that ice floats important

20、to living things? If ice sank, it would form on the bottom of a body of water as the water was cooling. Ponds and lakes would freeze from the bottom up, trapping the fish and other organisms in a shrinking layer of water without access to the nutrients from the muddy bottom. 第23頁，共35頁。Waters Ability

21、 to Dissolve Other Substances When you stir table salt into a glass of water, you are forming a solution, a uniform mixture of two or more substances. The substance that dissolves the other substance and is present in the greater amount is the solvent (in this case, water). The substance that is dis

22、solved and is present in a lesser amount is the solute (in this case, salt). When water is the solvent, the result is called an aqueous solution (from the Latin word aqua, water). 第24頁，共35頁。Sodium chloride dissolves as Na+ and Cl- ions become attracted to water molecules and break away from the surf

23、ace of the solid. Water is the main solvent inside all cells, in blood, and in plant sap. Water dissolves an enormous variety of solutes necessary for life. Figure 4-16 illustrates how water dissolves ionic compounds such as table salt (sodium chloride). 第25頁，共35頁。Acids, Bases, and pHIn aqueous solu

24、tions, a very small percentage of the water molecules themselves break apart into ions. The ions formed are positively charged hydrogen ions (H+) and negatively charged hydroxide ions (OH-). 第26頁，共35頁。Some chemical compounds contribute additional H+ ions to an aqueous solution while others remove H+

25、 ions from it. A compound that donates H+ ions to a solution is called an acid. An example is hydrochloric acid (HCl), the acid in your stomach. 第27頁，共35頁。In an aqueous solution, hydrochloric acid breaks apart completely into H+ and Cl- ions. A compound that removes H+ ions from an aqueous solution

26、is called a base. Some bases, such as sodium hydroxide (NaOH), do this by adding OH- ions, which then combine with H+ ions and form water molecules. 第28頁，共35頁。The pH Scale The pH scale describes how acidic or basic a solution is. The scale ranges from 0 (most acidic) to 14 (most basic).Each pH unit

27、represents a tenfold change in the concentration of H+ ions. For example, lemon juice at pH 2 has 10 times more H+ ions than an equal amount of grapefruit juice at pH 3. 第29頁，共35頁。Pure water and aqueous solutions that have equal amounts of H+ and OH- ions are said to be neutral. They have a pH of 7 and are neither acidic nor basic. The pH of the solution inside most living cells is close to 7. 第30頁，共35頁。A solution having a pH of 7 is neutral. Many fruits have pH values less than 7, making them acidic. Various household cleaners have pH values gr