Lec-35-Review - Hydrogen Bonds Lecture 35 Exam 3 Review...

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Lecture 35 – Exam 3 Review – Concepts to Remember – Chapters 4, 5, 9-11, and 16. Hydrogen Bonds • Attraction of hydrogen atom for an electron pair on a small, very electronegative atom • Examples include an H-F, H-O, or H-N bond. Hydrogen bonds are stronger than dispersion forces. • Bond between hydrogen and any of three elements is quite polar, with hydrogen at the positive end. • Energies of bonds: 4-25 kJ/mol . p.413b Double Stranded DNA
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Fig. 9-29, p.423 Non-superimposable mirror image chiral molecules are enantiomers. - Enantiomers rotate polarized light in different directions. Any molecule containing a carbon with 4 different attached groups is chiral . Most amino acids are chiral. Properties of Gases • can be compressed • exert pressure on whatever surrounds them • expand into whatever volume is available • easily diffuse into one another • can be described in terms of their temperatures and pressure,the volume occupied, and the amount (number of molecules or moles) present Pressure pressure = force/area force = mass × acceleration 1 Standard Atmosphere = 1 atm 1 atm = 760 mm Hg(exactly) 760 mm Hg(exactly) = 760 torr 760 torr = 101.325 kPa 100 kPa = 1 bar Kinetic Molecular Theory: Gases • particles in continuous, random, rapid motion • collisions between particles are elastic • volume occupied by the particles is negligibly small effect on their behavior • attractive forces between particles have a negligible effect on their behavior • gases have no fixed volume or shape, take the volume and shape of the container
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Ideal Gas Law V α (n × T)/P V = R × (n × T)/P where R is proportionality constant P × V = n × R × T p.451 How does Kinetic Molecular Theory account for the ideal gas law? Boyle’s
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This note was uploaded on 09/04/2009 for the course CHE 81914-01 taught by Professor Prof.benjaminhsiao during the Spring '06 term at SUNY Stony Brook.

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Lec-35-Review - Hydrogen Bonds Lecture 35 Exam 3 Review...

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