2.2 A- Hydrogen Bonds
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1 TOPIC WATER
2 2.2 A- Hydrogen Bonds
3 Understandings U1: Water molecules are polar and hydrogen bonds form between them. Polar Water molecules consists of two types of atoms: Oxygen (8 protons) Hydrogen (1 proton) Because of the difference in protons, oxygen attracts hydrogen s electrons towards it. This creates partially positive and negative sides of the molecule. This is known as being polar. 3
4 Understandings U1: Water molecules are polar and hydrogen bonds form between them. Since water is polar, it has slightly positive and negative poles. In diagrams, this is shown using the delta symbol (δ). 4 Polar Even though electrons are not distributed equally WITHIN the molecule, water is neutral (no charge) overall.
5 Understandings U1: Water molecules are polar and hydrogen bonds form between them. When water molecules are near each other, hydrogen bonds form between them. These H-bonds result from the electric attraction between the slightly-positive H s and slightlynegative O s. 5 Hydrogen Bond H-bonds are weaker than covalent bonds since the molecules are only attracted to each other.
6 Understandings U3: Substances can be hydrophilic or hydrophobic. Since water is polar, it can form H-bonds with other polar molecules. This is seen in the phospholipid bilayer. 6 Hydrophilic Hydrophobic Hydrophilic (water-loving) substances are polar and so are attracted to water. This allows them to dissolve in water. Hydrophobic (water-fearing) substances are not polar and so do NOT form H-bonds with water. They are insoluble.
7 Phospholipid Structure 7 Understandings U3: Substances can be hydrophilic or hydrophobic. Hydrophilic Hydrophobic
8 REVIEW 1. Describe the polar nature of water Define hydrogen bond. 3. Outline the formation of hydrogen bonds between water molecules. 4. Define hydrophilic. 5. Define hydrophobic. 6. Compare the structure of hydrophilic and hydrophobic substances.
9 2.2 B Properties of Water
10 INTRO The hydrogen bonds that form between water molecules give them a number of properties that are vital to organisms. These properties include: Cohesive Adhesive Thermal Solvent 10
11 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. The H-bonds between water molecules results in water being cohesive. This means the molecules naturally stick together. 11 Cohesive Many organisms depend on this property for a habitat. Insects like the one above are able to stand on water due to surface tension that cohesion creates.
12 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. Plants also use cohesion to transport water molecules from the ground through to the top of the plant. As molecules move up through the tissues, hydrogen bonds cause them to pull the molecules behind them. This makes water transportation much easier. 12 Cohesive
13 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. Hydrogen bonding also allows water to 13 stick to other substances. This property is called adhesion. Along with cohesion, adhesion allows plants to transport water in columngs against gravity. Adhesion
14 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. An object s temperature is related to the rate at which molecules vibrate. As energy is added, vibrations and temperature increase. 14 However, H-bonds hold water molecules together and slows vibration. So, more energy is needed to increase the temperature of bodies of water.
15 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. The specific heat of a substance is the energy required to increase 15 1g by 1 C. Water s specific heat is 4.18 J/g C, which is higher than most common materials. Specific Heat
16 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. Water s high specific heat allows it to be a stable environment for marine organisms. Air temperatures can change quickly, but water bodies are slow to cool or warm. 16 Specific Heat
17 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. Because of its hydrogen bonds, water also has a high latent heat of vaporization, which is the energy required for it to evaporate. 17 Latent Heat of Vaporization
18 Applications A2: Use of water in sweat as a coolant. Water s high latent heat of 18 vaporization allows organisms to use it as a coolant. When body temperature increases, sweat builds on the skin. The water molecules absorb heat from the skin until it evaporates. This energy is carried away and the body is cooled. Sweat
19 Applications A1: Comparison of the thermal properties of water with those of methane. The following chart compares the thermal properties of water to that 19 of methane, a non-polar molecule. Since methane is non-polar, it has a lower specific heat and latent heat of vaporization. METHANE WATER Polarity Non-polar Polar Specific Heat (J/gx C) Latent Heat of Vaporization (J/g) Melting Point ( C) Boiling Point ( C)
20 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. Because water is polar, it has the ability to surround and dissolve other ionic or polar molecules. This makes water an effective solvent. 20 Solvent As a result, organisms can use water as a medium for reactions (cytoplasm) and also for transport (blood).
21 Understandings U2: Hydrogen bonding and dipolarity explain the cohesive, adhesive, thermal and solvent properties of water. Solvent PROPERTY Cohesive Reaction / Medium Transport Thermal / Coolant Solvent Water s Properties FUNCTION Allows for organisms to walk on water. Capillary action allows plants to transport water. Many substances dissolve in water, so it makes a good reaction medium Many substances dissolve in water, which allows for easy transport of substances in the blood and in the xylem/phloem. High specific heat creates stable environment (internal and external) for organisms. Evaporation of water (sweating, panting, transpiration) cools down organisms. Polarity allows it to dissolve other polar or ionic compounds 21
22 REVIEW 1. Outline the following properties of water and how they are useful to organisms: 22 - Cohesive - Solvent - Thermal - Adhesive
23 2.2 C Blood Transport
24 INTRO Blood is primarily composed of water, which makes it an effective medium for transporting substances throughout the body. 24
25 Applications A3: Modes of transport of glucose, amino acids, cholesterol, fats, oxygen and sodium chloride in blood in relation to their solubility in water. Glucose Sodium Chloride Glucose is a polar molecule and so is hydrophilic. It can freely dissolve in blood plast and is easily transported through the body. Sodium chloride (NaCl) is an ionic compound. It dissociates into Na+ and Cl- in the blood plasma and then flows freely. 25
26 Applications A3: Modes of transport of glucose, amino acids, cholesterol, fats, oxygen and sodium chloride in blood in relation to their solubility in water. The R group of an amino acid determines how soluble it is. All are soluble, however some are more hydrophilic/phobic than others. 26 Amino Acids
27 Applications A3: Modes of transport of glucose, amino acids, cholesterol, fats, oxygen and sodium chloride in blood in relation to their solubility in water. Oxygen (O 2 ) is non-polar and is not able to efficiently dissolve. To meet the needs of cell respiration, hemoglobin in red blood cells binds to O 2 and transports it throughout the body. 27 Oxygen
28 Applications A3: Modes of transport of glucose, amino acids, cholesterol, fats, oxygen and sodium chloride in blood in relation to their solubility in water. Fats are large and nonpolar, which makes them insoluble. Instead of dissolving, they are carried in lipoprotein complexes. These complexes are surronded by a single layer of phospholipids. 28 Fats Lipoprotein Complex This layer allows it to dissolve and carry the hydrophobic contents throughout the body.
29 Applications A3: Modes of transport of glucose, amino acids, cholesterol, fats, oxygen and sodium chloride in blood in relation to their solubility in water. Cholesterol molecules are small, but they insoluble due to a large hydrophobic region. So, they are carried in lipoprotein complexes along with fats. They are embedded in the tails of phospholipids. 29 Cholesterol
30 REVIEW 1. Outline how the following are transported through the blood: 30 - Glucose - Oxygen - Amino Acids - Sodium Chloride - Fats - Cholesterol
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