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UW-Milwaukee BIOSCI 150 - Kinetic Energy

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Outline of Last LectureOutline of Current LectureCurrent LectureI. Watera. Propertiesb. Key termsc. Bondsd. Solutionsi. Molesii. Acids & Bases1. The pH scaleBIO SCI 150 1st Edition Lecture 2Outline of Last Lecture I. Introductiona. What is Biology?b. Living systemsi. Classificationc. Approaches in Biologyd. Major theoriesII. Atoms/Chemistrya. What is an atom?b. How atoms interact…Outline of Current Lecture I. Watera. Propertiesb. Key termsc. Bondsd. Solutionsi. Molesii. Acids & Bases1. The pH scaleCurrent LectureI. Water- Essential for life- Major component of planet surface- Major component of living cells 70-95%a. Properties- H2O- Polar (H δ+, O δ-)- Found in most living things- Because of hydrogen bonding, water has a high specific heat.- Water stabilizes air temperature by storing and releasing heat - Because of hydrogen bonding water has a high heat of vaporization.- At different states…o At high temperatures the hydrogen bonds break and molecules are free as gaso At moderate temperatures hydrogen bonds break and reform, giving a liquido At low temperatures multiple hydrogen bonds produce solid iceb. Key terms- Kinetic Energy – movement of atoms- Temperature – intensity of heat (average)- Amount of Heat – temperature + mass- Specific Heat – amount of heat to raise 1g 1 degree- Hydrogen Bonds Produce:o Cohesion - molecules bound to like molecules, forms streamso Adhesion - molecules bound to different substance produces wettingo Surface tension - hydrogen bonding to each other along surface and below- Celsius- 0° freeze 37° human 100 boil- Calorie- amount of heat energy needed to raise temperature of lg of water 1°C- kilocalorie amount of heat energy needed to raise temp of 1kg water, or liter 1° C- Heat of vaporization - amount of heat a liquid must absorb for lg to be converted to gasc. Bonds- Water absorbs energy to break Hydrogen bonds.- Energy is released when Hydrogen bonds form.- Water freezes when all H bonds form.- This makes a solid and expands the structure, since the rigid hydrogen bonds do not allow molecules to move closer to each other- Water gives off energy as it freezes- Water absorbs energy as it meltsd. Solutions- Polar nature of water makes it a good solvent for polar or ionic solids like salt.o Solution- homogeneous mixture of 2 or more substanceso Solvent- liquid in solutiono Solute- dissolved substance- Polar nature of determines its behavior with other substances.o Hydrophilic likes water dissolve or absorb ionic, polaro Hydrophobic repels water, will not dissolve in water Nonpolar, nonionic, oil, wax “a ducks back”i. MolesMolemolecular weight number (M) Given in grams not daltons1 mole of anything contains 6.02 x 1O23 molecules (“Avogadro’s number”)ii. Acids & BasesIf a hydrogen atom leaves one water molecule, but leaves its electron behind, the water molecule gains a negative charge and is called a hydroxide ion.The hydrogen atom without its electron is a hydrogen ion, a single proton witha charge of +1. If another water molecule acquires this proton it becomes ahydronium ion with a charge of +1. Water exists as equilibrium.- Definition - Substances that cause an unbalance in the ration of hydrogen and hydroxide ions are called acid or baseo Acid increases H+ concentrationo Base increases OH- concentration, decreases H+ concentration- A buffer will maintain a balance by shifting the direction if there is a changein H+ concentration1. The pH scale- The concentration of H+ ions in a solution can be determined using pH.- pH = - log of H+ concentration- Low pH = acid = more hydrogen ions- High pH = base = less hydrogen ions- Increase of 1 pH unit = 10 x increase in H- Increase of 2 pH units = 100 x increase in


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