01:694:301 Chapter Notes - Chapter 2: Electronegativity, Hydrophile, Chromatin
11 Mar 2016
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2. 1 the importance of noncovalent interactions in biochemistry. Noncovalent bonds are important because they"re weak: can break & re-form easily, multiple noncovalent bonds sum up in energy. Attract (+-), f = (-: f = kq1q2/ r2. Use energy when considering changes in noncovalent bonding interactions: e = kq1q2/ r. Strong over greater distances compared to other noncovalent interactions. Polar molecules have dipole moment ( : dipole moment expresses magnitude of polarity. Repulsion when 2 nonbonding molecules get too close. Repulsive energy + attractive energies = total e of noncovalent interaction r0 = most stable distance between the centers of the 2 interacting particles rv = r1+r2 ; rv = closest approach. H-bond donor = the atom the h is covalently bonded to: it has an h attached to it. H-bond acceptor = the atom with the nonbonded electron pair: it has lone pairs of electrons. Greater electronegativity = greater h-bond donor: mainly o & n.
