OWL NOTES TEST 1- Tetrahedral local electron geometry corresponds to sp3 hybridization.- Trigonal planar local electron geometry corresponds to sp2 hybridization.- Linear local electron geometry corresponds to sp hybridization.- Unshared electron pairs are considered to be hybridized with the bonding pairs on each atom.Electronic geometry at an atom is determined by the sum of its attached atoms(sometimes called ligands) and unshared electron pairs.- If they total four, the local geometry is tetrahedral , and bond angles will be near 109.5o.- If they total three, the local geometry is trigonal planar or simply trigonal, and bond angles will be near 120o.- If they total two, the local geometry is linear or digonal, and the bond angle will be near 180o.MOLECULAR GEOMETRIES-TETRAHEDRAL: 4 bond pairs, no lone pairs, 109.5 degrees-TRIGONAL PYRAMIDAL: 3 bond pairs, 1 lone pair, 107.5 degrees-BENT: 2 bond pairs, 2 lone pairs, 105 degreesELECTRON PAIR GEOMETRY-corresponds directly with how many bonds there are regardless of if they are bonded to an atom or are lone pairs. If two bonds and 2 lone pairs- TETRAHEDRAL, not bent (molecular geometry)There is a carbon at each line intersection and at each line terminus. Heteroatoms(atoms that are not carbon or hydrogen) are written explicitly with their attached hydrogens, e.g. -NH2. Hydrogens attached to carbon are not explicit. They must be deduced by the viewer using valence rules. For example, a carbon at the intersection of three lines(bonds) needs to make one more bond to satisfy its valence offour. This bond is to an unshown hydrogen, see examples below.As the electronegativity difference between the bonded atoms increases, bond polarity increases. Bond polarity influences chemical properties profoundly.You may be able to determine the relative electronegativity differences using your knowledge that electronegativity increases from left to right across a row of the periodic table and decreases from top to bottom down a column.YES permanent electric dipole moment IF not equal CALCULATION OF FORMAL CHARGE:F.C.= periodic group number- unpaired electrons- ½ (b.p electrons)F.C.= valence electrons in neutral atom- valence electrons assigned to atom in a structural formulaHYDROGEN BONDSHydrogen bond donors typically have hydrogen(s) directly bonded to electronegative aoms like oxygen, nitrogen, fluorine, and chlorineHydrogen bond acceptors typicall yahve atleast one unshared 9one pair) of electrons and are measurably basic. The last requirement excludes organic halidesCombination of a donor and an acceptor can give a hydrogen bondTable: Structures of Some Common Functional GroupsName Structure Name StructureAlkene (double bond)NitrileAlkyne (triple bond)NitroArene ThiolHalide AldehydeAlcohol KetoneEther Carboxylic AcidAmine EsterAmideCarboxylic Acid Chloride None of the following molecules display much solubility in waterat room temperature. However, two of the molecules display appreciable solubility in boiling water. Based on its structure, which molecule will be the least soluble in