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Additional resources for Chemical Kinetics and Reaction Mechanisms: McGraw-Hill Series In Advanced Chemistry

Example text

H Tetrahedral H H .. .. Si Cl T t h d l Tetrahedral Cl Cl .. N Pyramidal H H O H Bent H H 4 4,4 .. H O O H .. 4,4 .. 14 Linear F C H H H .. C H .. H .. H2O2 H .. H C .. H .. 14 H .. H N H .. H .. C2H6 Ethane .. 8 .. .. 4 .. NH4+ F Cl .. O H .. H .. 8 4 4 .. H2O Water Note H .. H N H .. H .. 8 Shape - 4 .. NH3 Ammonia .. 32 N .. Cl .. Si Cl .. Cl .. Cl .. SiCl4 .. .. .. F F .. 14 .. CH4 Methane Lewis formula N H H H C T t h d l Tetrahedral H H H H 2 tetrahedral C H H O O F2 Fluorine gas Total No.

E . Lewis recognised that bonding or o sharing of electrons occurred so that an elemeent tended to acquire eight valence electrons (noble gas present a bond configuration): the octet rule. To rep b between two atoms, a Lewis L i structurre is i written i so as to indicate the position of the valen nce electrons: Group . X .. .. Molecules and compounds form wheen bonds exist between atoms involving the transferr or sharing of valence electrons. The Lewis symbool for an atom is the element symbol surrounded by dots that represent the possible valence electtrons for the atom.

When hybridization occurs, the rearraangement of electrons often results in there being more unpaired valence elecctrons than there were originally. 5. In PCl5 (more than eight electrons bonded), the hybrid orbitals are sp3d. H H In the double C=C bond of C2H 4 onee of the   bonds is the end-to-end overlap of onee of the   sp2 hybrid orbitals (this is called the  sigma C      bond) along the line of the two C atom ms (the 2p 1s 2sp2 2 other two sp orbitals overlap with the s   orbitals of the H atoms), while the other o C C      bond is formed by the side-by-side oveerlap of   the unhybridised (dumbbell shapeed) 2p   orbitals parallel to the plane of the C and H H H atoms (this is called the  pi bond).

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