molecular interactions and conformations Flashcards
SAR and pharmacophore
structure activity relationship - relationship between chemical structure of drug and biological activity, pharmacophore - 3D ensemble of steric and electronic features of a molecule necessary to ensure optimal molecular interactions with specific biological target structure in order to bind with sufficient affinity to activate/block biological response
Hund rule
each p orbital must be filled with one electron before they will begin to pair up
molecular orbitals - hydrogen
2 x 1s atomic orbitals form 2 molecular orbitals sigma and sigma*, shared electrons fill lower energy sigma
molecular orbitals - methane
outer shell of carbon has 2 electrons in the 2s orbital and 1 electron in each of the 2/3 of its 3 2p orbitals, in order to share 4 electrons carbon forms 4 degenerate (same energy) hybrid sp3 orbitals, tetrahedral arrangement of sp3 orbitals of carbon can interact with 4 x 1s orbitals from hydrogen to form methane, sp3 and 1s orbitals merge to form atomic orbitals, methane consequently has perfect tetrahedra arrangement of bonds
sp3 hybrid orbitals
4 hybrid sp3 orbitals are formed from 1 x s and 3 x p atomic orbitals
molecular orbitals ammonia
outer shell of nitrogen has 2 electrons in 2s and 1 electron in all of the 3 2p orbitals, unlike carbon one of the sp3 orbitals already have 2 electrons, not available for bonding , other 3 are tho (bond with 3 hydrogens)
molecular orbitals - water
outer shell of oxygen has 2 electrons in its 2s orbitals and 2 electrons in one of its 2p orbitals and 1 electron in its other 2 2p orbitals, 2 of the sp3 orbitals already have 2 electrons so not available for bonding, other two are (bond with hydrogen)
pre-filled sp3 orbitals
result in lone pairs of electrons, closer to central atom compared to shared electrons in the bond, push the bond electrons away so bonds become closer together, result in bond angle less than 109.5 degrees (ammonia - 107, water - 104.5
molecular orbitals - ethane
as we build up to more complex molecules same rules apply, all bond angles of ethane are approximately 109.5 and there are only sigma bonds, sigma bonds can rotate, 3 hydrogens on each carbon in ethane spin like helicopter as central bond rotates
molecular orbitals - ethene
1 x s orbital only hybridises with 2 x p orbitals to give 3 sp2 hybrid orbitals, 1 p orbital remains unchanged, 3 sp2 orbitals arranged in plane and separated by 120 degrees, hence ethene is planar, sp2 orbitals can form sigma bonds with another carbon sp2 and also 1s orbitals of hydrogen to form m molecular orbitals, however still 2 x p orbitals (one on each carbon) with only one electron in, these overlap to for pi bond (only one pi bond - electron cloud partially above and partially below sigma bond - electrons are part wave part particle, easier to imagine them as a cloud that has an over-all charge of -1 but can shift about)
molecular orbitals - benzene
aromatic rings are special case when considering single/double bonds, simplest example benzene has its pi electrons in 3 double bonds shared across all six bonds in the ring, delocalisation, aromatic rings common in drug structures, flat planar structures
molecular orbitals - naphthalene
pi electrons in naphthalene delocalised across 2 aromatic rings
molecular orbitals - formaldehyde
formaldehyde is a central carbon atom with a double bonded oxygen and two hydrogens, combination of common biological elements, follows similar pattern to ethene except oxygen has two lone pair rather than 2 sigma bond to hydrogen (carbon and the oxygen are both sp2), 2 x C-H sigma bonds, 1 x C-O sigma bond, 1 x C-O pi bond
molecular orbitals - amides
a regular 2p orbital (not hybridised) on nitrogen containing lone pair of electrons, next door is pi bond between carbon and oxygen, lone pair on nitrogen can interact with pi orbital of carbonyl group (delocalisation)
molecular orbitals - ethyne
sp (only 2 hybrid sp orbitals other 2 p orbitals remain unchanged) orbitals are 180 degrees apart, one bonds with neighbouring carbon and other with hydrogen, however still 4 x p orbitals (2 on each carbon) with only one electron in each, overlap to form two pi bonds (triple bonded carbons each bonded to one hydrogen)
molecular conformations - ethane
bond angles approximately 109.5, only sigma bonds, all single covalent bonds bonds can spin, doesn’t have any affect for C-H bond, when C-C bond in ethane spins position of hydrogens change (each half of the molecule as propeller)
dihedral angles (torsion angles)
Newman projection is way of defining rotation about a single bond, can define the conformation around that bond using the dihedral angle (portion angle), staggered theta = 60 degrees, eclipse theta = 0 degrees
molecular conformations - butane
3 C-C bonds number of different conformations increases, imagine looking down central C-C bond - as central bond rotates the methyl group at one end of molecule moves closer/further from hydrogens and methyl group at opposite end, energy is highest when two terminal methyl groups are closest, also high when there is clash between terminal methane and terminal hydrogen, molecule prefers to be in one of the 3 lowest energy conformations also referred to as rotomers (anti and gauche), is a choice of conformation for each single bond, also so restraint (side chains of all amino acids in a protein - conformation of each single bond in side chain follows these rules, likewise single bonds in drug molecule also follows the rules)
geometric isomers - 2-butene
inability of double bon ds to rotate means there can be two distinct geometric isomers - trans and cis conformation, major implications to conformation of drug
ring closure - single bonds unable to rotate
ring systems with single bonded carbons found in ligands, simplest version of such ring is cyclohexane - not planar like benzene, is puckered and can form chair or boat conformation, often find oxygen or nitrogen inserted into this puckered ring system (glucose), informs us possible to prevent single bond rotation by inserting ring system, chair conformation moist stable
isomers via ring closure
if any two sp3 carbons in a ring have two different substituent groups (not counting other ring atoms) cis/trans stereoisomerism is possible, if more than two ring carbons have substituents stereo-chemical notion distinguishing various isomers becomes more complex and prefixes cis/trans cannot be used to formally name the molecule