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| Subject keyword(s) | Astronomy, Chemistry, Dipole, Hydrogen bonding, Science, Solvation, Space Science, Space sciences |
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Register | Log In Library MyClassroom About Us Help Library > Chemistry > Water Module Questions & Quizzes Links en español print Water Properties and Behavior by Anthony Carpi, Ph.D. In many ways, water is a miracle liquid. It is essential for all living things (on this planet at least), and it is often referred to as a universal solvent because many substances dissolve in it. These unique properties of water result from the ways in which individual H2O molecules interact with each other. Figure 1: Electronic distribution in H2O. In the Chemical Bonding lesson we discussed the dipole that forms across the water molecule as a result of the polar covalent bonding between hydrogen and oxygen (see our Chemical Bonding module for more information). Because the bonding electrons are shared unequally by the hydrogen and oxygen atoms, a partial negative charge (�-) forms at the oxygen end of the water molecule, and a partial positive charge (�+) forms at the hydrogen ends. Since the hydrogen and oxygen atoms in the molecule carry opposite (though partial) charges, nearby water molecules are attracted to each other like tiny little magnets. The electrostatic attraction between the �+ hydrogen and the �- oxygen in adjacent molecules is called hydrogen bonding. Figure 2: Hydrogen Bonding between Water Molecules. Hydrogen bonding makes water molecules "stick" together. While hydrogen bonds are relatively weak compared to other types of bonds, they are strong enough to give water many unique properties. For example, hydrogen bonds sank the Titanic, and hydrogen bonds allow the Basilisk lizard to walk on water (as a result, the Basilisk has earned the nickname "Jesus" lizard). Just how does hydrogen bonding do this?� Well, let's start with the Titanic.� The Titanic sank because it hit an iceberg - a chunk of ice floating on the surface of the ocean.� The reason ice floats is because of hydrogen bonding.� In water's liquid form, hydrogen bonding pulls water molecules together.� As a result, liquid water has a relatively compact, dense structure.� The animation below illustrates this idea. Liquid Water and Hydrogen Bonding Concept simulation - Reenacts hydrogen bonding between molecules of liquid water. (Flash required) As water freezes into ice, the molecules become frozen in place and begin to arrange themselves in a rigid lattice structure, as shown in the animation linked below.�� Ice and Hydrogen Bonding Concept simulation - Reenacts hydrogen bonding between molecules of solid water. (Flash required) The structure that forms in the solid ice crystal actually has large holes in it.� Therefore, in a given volume of ice, there are fewer water molecules than in the same volume of liquid water.� In other words, ice is less dense than liquid water and will float on the surface of the liquid.� Throw in one really big chunk of ice and a cruise ship, and you begin to see the problems that can arise.�� As we just discussed, neighboring water molecules are attracted to one another.� Molecules at the surface of liquid water have fewer neighbors and, as a result, have a greater attraction to the few water molecules that are nearby.� This enhanced attraction is called surface tension. It makes the surface of the liquid slightly more difficult to break through than the interior.�� Surface tension When a small object that would normally sink in water is placed carefully on the surface, it can remain suspended on the surface due to surface tension.� The Basilisk lizard makes use of the high surface tension of water to accomplish the incredible feat of walking on water's surface.� The Basilisk can't actually walk on water; rather, it runs on water, moving its feet before they break through the surface.� Take a look: The 'Jesus' Lizard (473k movie) Water as a solvent The partial charge that develops across the water molecule helps make it an excellent solvent. Water dissolves many substances by surrounding charged particles and "pulling" them into solution. For example, common table salt, sodium chloride, is an ionic substance that contains alternating sodium and chlorine ions. Figure 3: Sodium chloride contains Na+ and Cl- ions. When table salt is added to water, the partial charges on the water molecule are attracted to the Na+ and Cl- ions.� The water molecules work their way into the crystal structure and between the individual ions, surrounding them and slowly dissolving the salt.� The water molecules will actually line up differently depending on which ions are being pulled into solution.� The negative oxygen ends of water molecules will surround the positive sodium ions; the positive hydrogen ends will surround the negative chlorine ions.�� Figure 4: Table salt dissolving in water. In a similar fashion, any substance that carries a net electrical charge, including both ionic compounds and polar covalent molecules (those that have a dipole), can dissolve in water. This idea also explains why some substances do not dissolve in water. Oil, for example, is anonpolar molecule. Because there is no net electrical charge across an oil molecule, it is not attracted to water molecules and therefore does not dissolve in water. External Resources Water: A Natural History The Secret Knowledge of Water : Discovering the Essence of the American Desert Other Recommended Products Back to top Anthony Carpi, Ph.D. "Water: Properties and Behavior," Visionlearning Vol. CHE-2 (1), 2003. http://www.visionlearning.com/library/module_viewer.php?mid=57 Visionlearning Resources Glossary Library Biology AdaptationCellsCharles Darwin ICharles Darwin IICharles Darwin IIIDNA IDNA IIDNA IIIGenetics IGenetics IITaxonomy ITaxonomy II: Nomenclature Chemistry Acids and BasesAtomic Theory IAtomic Theory IICarbohydratesChemical BondingChemical EquationsChemical ReactionsFats and ProteinsMatterMatter: States of MatterNuclear ChemistryOrganic ChemistryThe MoleThe Periodic Table of ElementsWater Earth Science Earth StructureEarth's AtmosphereMinerals IMinerals IIMinerals IIIPlate Tectonics IPlate Tectonics IIThe Carbon CycleThe Hydrologic CycleThe Nitrogen CycleThe Rock Cycle General Science DensityEnergyTemperatureThe Metric SystemThe Scientific MethodUnit Conversion Physics GravityLight ILight IIWaves and Wave Motion Process of Science Data: Analysis and InterpretationData: StatisticsData: Uncertainty, Error, and ConfidenceData: Using Graphs and Visual DataIdeas in Science: Scientific ControversyIdeas in Science: Theories, Hypotheses, and LawsResearch Methods: ComparisonResearch Methods: DescriptionResearch Methods: ExperimentationResearch Methods: ModelingResearch Methods: The Practice of ScienceScientific Communication: Peer ReviewScientific Communication: The How and Why of Scientific MeetingsScientific Communication: Understanding Scientific Journals and ArticlesScientific Communication: Utilizing the Scientific LiteratureScientific EthicsScientific Institutions and SocietiesScientists and the Scientific CommunityThe Nature of Scientific KnowledgeThe Process of Science Scientific Research Bone Changes in Rock ClimbersClassic Experiment: Meselson and StahlCreativity in ScienceFrom Stable Chromosomes to Jumping GenesStudying Climate Change with Kevin ArrigoThe Case of the Ivory-billed Woodpecker Toxicology & Pharmacology Absorption, Distribution and Storage of Chemicals Trigonometry Wave Mathematics Interactive Animations Bohr's Atom: Quantum Behavior in HydrogenThe reaction of sodium with chlorineAn example of an interactive learning tool: Mid-Ocean RidgesLeaning Tower of Pisa ExperimentThe formation of waterThe Virtual Animal CellNuclear FusionTwo Types of Nuclear Chain ReactionsDalton's PlayhouseDarwin's FinchesThe Illustrated Animal CellStates of MatterThe Illustrated Periodic Table External Resources Water: A Natural History The Secret Knowledge of Water : Discovering the Essence of the American Desert Other Recommended Products Quotes If there is magic on this planet, it is contained in water. -L. 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