WATER PROPERTIES Supplemental Textbook Material Ch 16 p 349 361 Be sure to attend lab this week Bring the lab manual Must pass lab to pass this class Instructors will give percent lab grade to one another Climate Change by Vicki Hesse The Climate Project Extra credit opportunity for ES 106 Date Time Location Cost Audience Description Sponsoring Group Contact info Wednesday April 11 12 00 noon 1 00 p m Natural Sciences room 103 free Public Natural Science Seminar Series Vicki Hesse MDIV Volunteer Presenter The Climate Project All seminars begin at Noon in NS 103 Free and open to the public Science Department 503 838 8206 Covalent Bonds Overlapping outer shells Silicate minerals have silicon and oxygen joined with covalent bonds Covalent Bonds Need octet of electrons surrounding element in the dot diagram Some bonds are multiple stronger Polar molecules Electro negativity Covalent bonded molecules Like nonmetals form nonpolar covalent bonds Unlike nonmetals form polar covalent molecules Polar molecules have charge concentrated at one end Metals form metallic bonds not covalent bonds Poly atomic ions Covalently bonded compounds Not electrically neutral Maintain covalent bonds within ions as they interact with other ions to form ionic compounds Those bonded to oxygen become ate Common poly atomic ions Hydroxide Bicarbonate Carbonate Sulfate Nitrate Phosphate Chromate OHHCO3CO32SO42NO3PO43CrO42 Chemical Formulas Molecule has specific ratio of elements Subscripts how many Parentheses how many sets Coefficients how many molecules in reaction Chemical Formulas H2SO4 Ca3 PO4 2 Na2O CaCl2 CaO 2 NaCl MgBr2 2Ag NO3 Mg NO3 2 2AgBr Naming Compounds Find subscripts to indicate how many of each atom in the molecule Use chart at right for number of each Geometry of Molecules Molecules Carbon dioxide one carbon two oxygen straight Water one oxygen two hydrogen bent Ammonia one nitrogen three hydrogen pyramid shape Methane one carbon four hydrogen tetrahedron shape Typical Shapes of Molecules Dipole attraction in solid and liquid Dissolution of ionic substance In Class Activity 1 Draw the Bohr diagram electron shell structure for silicon 2 Draw the dot diagram for argon 3 Draw the Lewis diagram dot diagram for lithium 4 Draw the Lewis diagram dot diagram for silicon 5 If an atom gains an electron it is called ANION Its charge is circle POSITIVE NEGATIVE circle one two three 6 If an atom loses two electrons it is called CATION Its charge is circle POSITIVE NEGATIVE circle one two three Elements in Earth s Crust Oxygen Silicon Aluminum Iron Calcium Sodium Potassium Magnesium Mineral Naturally occurring Inorganic Solid Orderly crystalline structure Definite chemical composition Halite Bonding Halite Minerals Silicates most common Silicon Oxygen tetrahedron One oxygen four silicon Feldspar Quartz Hornblende Granite Solute Solvent Water phases and molecules Water Molecule Bent Covalent bonds Polar Dissolves ionic substances Properties of Water Solid water floats on liquid water High specific heat High heat of vaporization Universal solvent Distribution Cycle Animation Hydrologic Cycle Water Drop http www wested org pblnet exp projects H2O html Natural substances in water Impurities in Runoff Atmosphere Dissolved substances Silt etc Radon Organic byproducts in water Contamination of Water Micro organisms Decay products Plant nutrients Petroleum compounds Acid Industry Mining Drinking water standards Pollution Sources Raw Sewage discharge http www nwri ca sande nov dec 2002 e html Plant nutrient pollution http www na fs fed us SPFO pubs n resource riparianforests Tab 20I htm Agricultural Runoff http www na fs fed us SPFO pubs n resource riparianforests Tab 20I htm Oil pollution http www intertanko com tankerfacts sizes pollution htm Mine leachate http www ew govt nz enviroinfo hscs contam Water Pollution http www jvkco com digidare water html Water Pollution Prevention http www jvkco com digidare water html Drinking water standards Heat and Energy Transfer Supplementary Textbook Material Chapter 18 p 410 420 Review Questions 2 4 21 26 Temperature Quantity of hotness Celsius 0o freezing point of pure water at standard pressure 100o boiling point at standard pressure Fahrenheit 0o was lowest attained 32 was his age when he performed experiments 212 is boiling point in those increments Temperature Convert with equations Order of operations Parentheses first Then multiply or divide Add or subtract last Or use adjacent scales such as in the appendix of Earth Science textbook p 683 5 C F 32 9 9 F C 32 5 Temperature Kelvin same size as degree Celsius Absolute Zero is 0 K notice no degree symbol on K 0o C 273 K Equation for Prelab exercise 2 has error K 273 Co change to Heat Calorie Amount of heat required to raise the temperature of 1 mL pure water 1o C Food Calories are kilocalories Joule of calorie 1 cal 4 184 J Specific Heat Capacity Quantity of heat needed to change the temperature of given amount of a substance 1o C Water very high specific heat capacity Maritime areas more mild temperature than continental areas Heat Expansion Random motion causes substance to be bigger Liquids usually have greater heat expansion than solids Thermostats use different expansion of different type of metals Water Expansion Unusual response to cooling Contracts until reaching 4o C Expands slightly upon further cooling to 0o C Expands 9 upon freezing Water Molecule Bent Polar Water Expansion Molecule shape fit together closer in liquid Open structured crystal due to hydrogen bonding of polar molecules upon freezing Water Expansion http www elmhurst edu chm vchembook 122densityice html Heat of Water Supplementary Textbook Materials Chapter 19 Pages 424 435 Electron Structure Diagrams Two ways to correctly do these With elemental symbol in center With number of protons in center Not with circles around symbol and electrons distributed around circle Dot Diagrams Only show VALENCE Electrons Don t show shells Phases of Matter Solid Liquid Gaseous or vapor Plasma Gas Liquid and Solid Gas Liquid Zumdahl Zumdahl DeCoste World of Chemistry 2002 page 441 http www unit5 org christjs Matter 20and 20Energy Unit 202 20PP files frame htm Solid Evaporation Kinetic energy of molecules Taken from liquid cools it Gaseous phase or vapor phase Gas Steam H2O g Steam http www unit5 org christjs Matter 20and 20Energy Unit 202 20PP files frame htm Water vapor http en wikipedia org wiki Water vapor Evaporation or Not http www geology sdsu edu classes
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