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CHAPTER 9. AP/HONORS CHEMISTRY. MOLECULAR GEOMETRY. VSEPR - valence-shell electron pair repulsion IDEAL GEOMETRIES Type geometry bond angle AB 2 (2 e- pairs) Linear 180 o example on board
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CHAPTER 9 AP/HONORS CHEMISTRY
MOLECULAR GEOMETRY • VSEPR - valence-shell electron pair repulsion • IDEAL GEOMETRIES • Type geometry bond angle • AB2 (2 e- pairs) Linear 180o example on board • AB3 (3 e- pairs) Triangular 120o example on board Planar • AB4 (4 e- pairs) Tetrahedral 109.5o example on board • AB5(5 e- pairs) Trigonal 120o & 180o example on board bipyramidal • AB6(6 e- pairs) Octahedral 90o example on board
EFFECT OF UNPAIRED ELECTRONS • Type geometry bond angle • AB2E (2 e- pairs, Bent example on board 1 lone pair) • AB2E2 (2 e- pairs, Bent 105o example on board 2 lone pairs) • AB3E (3 e- pairs, Triangular 107o example on board 1 lone pair) pyramidal • the electron pair geometry approximately the same as that observed when only single bonds exist
CONTINUED • the molecular geometry is quite different with lone pairs. Why? • lone pairs take up more space than when bonded • consider NH3 it has a electronic pair geometry of tetrahedral but the angle is 107o • the water molecule is nonlinear because of lone pairs 105o
OTHER LONE PAIR GEOMETRIES • AB4E see-saw SF4 • AB3E2 T-shaped ClF3 • AB2E2 linear XeF2 • AB5E square pyramidal BrF5 • AB4E2 square planar XeF4 • when dealing with geometries multiple bonds behave like single bonds
CONTINUED • the geometry depends upon how many terminal atoms the central atom has around it and the number of unshared electrons • the VSEPR model can be extended to molecules which do not have a single central atom. C2H2 and C2H4
POLARITY OF MOLECULES • Polar • large (not large enough to form ionic bonds) electronegative difference • unequal share of the electrons • nonpolar equal sharing • the degree of polarity is measured by its dipole moment • π = Qr, Q = charge at either end, r = distance • 1 debye = 3.33 x 10-30 coulomb-meters H-Cl 1.03D bond length 1.36 Ǻ
CONTINUED • is it easy to determine whether a diatomic molecule is polar. Why? • check if the elements are the same or different • if a molecule contains more than two atoms, we must decide whether the whole molecule is polar or nonpolar • the are two criteria for determining the polarity of a molecule: bond polarity and molecular geometry
ATOMIC ORBITALS • Sigma bonds σ • single lobe where the electron density is concentrated in the region directly between two bonded atoms • pi bond π • this orbital has two lobes one above the bond axis and one below. The electron density is zero • all single bonds are sigma bonds and any other bond in a double or triple bond will be pi bonds • on board • hybrid orbitals on board
DELOCALIZE BONDING • The bonds are given to all atoms i.e. benzene on board makes it stable (aromaticity) • magnetism - molecules with one or more paired electrons are attracted to a magnetic field • the more unpaired electrons, stronger attraction- paramagnetism • with no unpaired electrons, weak repulsion - dimagnetism