Physical Chemistry and Its Biological ApplicationsPhysical Chemistry and Its Biological Applications ... |
From inside the book
Results 1-3 of 80
Page 289
... bonds are directional and that the number of bonds formed by an atom is limited by the number of orbitals in that atom that are of appropriate energy to over- lap profitably with those of other atoms . A covalent bond can be simply ...
... bonds are directional and that the number of bonds formed by an atom is limited by the number of orbitals in that atom that are of appropriate energy to over- lap profitably with those of other atoms . A covalent bond can be simply ...
Page 296
... bond between the two carbons . Such overlap is possible only if the molecule assumes an overall planar structure . The presence of a 7 bond in ethylene and similar molecules restricts rotation of the two parts of the molecule about the ...
... bond between the two carbons . Such overlap is possible only if the molecule assumes an overall planar structure . The presence of a 7 bond in ethylene and similar molecules restricts rotation of the two parts of the molecule about the ...
Page 319
... bond character of the carbon - oxygen bond . In an a , ẞ - unsaturated aldehyde , the carbonyl absorption appears at 1670 to 1680 cm - 1 , the reduction again being the result of conjugation . If an electronegative atom is substituted ...
... bond character of the carbon - oxygen bond . In an a , ẞ - unsaturated aldehyde , the carbonyl absorption appears at 1670 to 1680 cm - 1 , the reduction again being the result of conjugation . If an electronegative atom is substituted ...
Other editions - View all
Common terms and phrases
absorption acid adsorbed adsorption amino amount behavior benzene Calculate carbon carboxyl cell chain charge Chem chemical chemical shift chloride cm³ coefficient complex components concentration containing corresponding curve described diagram dipole dissociation distance effect electric electrolyte electron energy change enthalpy entropy enzyme equal equation equilibrium constant example force free energy frequency function H₂O heat hydrogen atom hydrogen bonds increase interaction ionic ionization k₁ k₂ kcal kcal/mol kinetic magnetic field magnitude material measured membrane mixture molar mole fraction molecular weight molecules nuclei occurs orbital osmotic pressure oxidation oxygen particles polar potential protein proton quantum number radiation rate constant ratio reactant reaction represented resonance rotation sample shown in Figure sodium solid solubility solvent species spectrum spin structure substance sucrose surface tension temperature tion titration torr transition triplet tube vapor pressure velocity vibrational viscosity volume wavelength zero