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BIOCHEM EXAM

QuestionAnswer
Weakest to strongest forced 1. London 2. Dip-Dip 3. Hydrogen 4. Ion-Dipole 5. Ionic attraction
Boyle's Law As pressure increases, volume decreases
Charle's Law As volume increases, temperature increases
Gay-Lussac's Law As pressure increases, temperature increases
Stronger intermolecular force= higher boiling point means there is more energy needed to break down these forces
polar vs non polar polar= far away on the periodic table (polar opposites) nonpolar= close on the periodic table
London forces non polar and polar ALL COMPOUNDS HAVE THIS
Dipole-Dipole Polar! Creates a slight charge
Ion-Dipole Ion + a POLAR molecule
Ionic Attraction Oppositely Charged Ions Na-+Cl- Li-+F- K+ I-
Hydrogen Bonding HF, HO, HN
in terms of their attractive forces, explain why fats are solids but oils are liquids under normal conditions, despite the fact that both are triglycerides the large number of cis double bonds in the hydrocarbon tails of oils prevents them from interacting with each other as much as the SAT tails of the fats. More interactions means that the tails move more slowly, becoming more like a solid, forming a fat.
FATS SOLID at room temperature KINKY chains SATURATED with hydrogens
OILS LIQUID at room temperature
Why are melting points for oil lower than fats? The lower melting point of oils is related to the higher degree of unsaturation.
Fewer attractive forces= a lower melting point
Amphipathic Compound Polar + Nonpolar sections in 1 molecule
6 Strong acids 1.HClOv4 2. Hv2SOv4 3. HI 4. HBR 5. HCl 6. HNOv3
4 Strong bases 1. LiOh 2. KOH 3. NaOh 4. Ca (OH)v2
Created by: liladdoyle
 

 



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