Polarity in Molecules!
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1 Chapter 9 part 2: Polarity in Molecules, Valence Bond Theory! Read:!!BLB 9.3 5! W:!!BLB 9.33, 35, 38!!!Packet 9:8-11! Know:! bond angles and geometry! polarity of molecules! Polarity in Molecules! " Just because a molecule possesses polar bonds does not mean the molecule as a whole will be polar.! Dipole Moment (µ) Which Skill Check Test Bonus Deadline is Approaching?? When is EXAM 2??? " ow can we determine the overall dipole moment for the molecule?! 1! 2!
2 Dipole Moment! Which molecules are polar?! or a diatomic molecule: µ = Q r r!!! +Q -Q units = debye (D) = 3.33 x10-30 C-m or two charges (+1 and -1) separated by 1 Å µ = 4.79 D per Å Where Q = 1.6 x10-19 C = charge of an electron or a polyatomic molecule: µ depends on: 1. 2.!! 3! 4
3 Dipole Trends in -X! If the -X bond were ionic, µ(ionic) = Q r If the -Cl bond were ionic (r = 1.27 Å ) µ = 4.79 D /Å x 1.27 Å = 6.08 D owever, experimental data show: µ = 1.08 D Compare the two values: µ(exp) /µ(ionic) x 100 = 1.08/6.08 x 100 = 18% Oxidation Numbers, ormal Charges, and Partial Charges! "!" -Cl -Cl -Cl " = 0.18 oxidation formal partial charges numbers charges (experimental) The bond is only 18% ionic (82% covalent; polar covalent) X bond length Å µ(exp) D µ(ionic) D!EN % ionic % Cl % Br % I % Dipole moment (µ) Measures: 5! 6!
4 Polarity of Molecules! Examples! A molecule is polar if there is a NET charge separation between two "ends" of the molecule: molecule has a negative "end" and a positive "end". CO 2 electronegativity: C = 2.5 O = 3.5 O=C=O Requirements to have a net dipole: 1." 2. To determine the polarity of a molecule that has more than 2 atoms: 1." 2." 3." 4."! 7! EPG: MG: bond dipoles? Net dipole moment? C 4 electronegativity: C = 2.5 = 4.0 EPG: MG: Bond dipoles? Net dipole moment?! C 8!
5 2 O Examples! N 3 Examples! electronegativity: = 2.1 O = 3.5 EPG: MG: bond dipoles? Net dipole moment? C 3 Cl electronegativity: = 2.1 C = 2.5 Cl = 3.0 EPG: MG: Bond dipoles? Net dipole moment? O Cl C 9! electronegativity: = 2.1 N = 3.0 EPG: MG: Net dipole moment? N N 3 vs. N 3 N µ"= 1.47 D µ = 0.24 D [electronegativity: = 2.1 N = 3.0 = 4.0] lone-pairs also have small dipoles partial cancellation of bond dipoles in N 3 10!
6 Chapter 9 part 3: Valence Bond Theory! Read:!!BLB 9.4 6! W:!!BLB 9:43, 47!!!Packet 9:13!!!! Know:! molecular orbitals! orbital hybridization! VBT! ow are bonds made? Lewis structures: location and number of bonding and lone-pair electrons VSEPR: spatial distribution of electrons, shape of molecule ow have we described electron distribution in atoms? What is the electron distribution in molecules? Molecular Orbitals Two models: Valence Bond Theory Valence orbitals on one atom overlap with valence orbitals on another atom: this overlap is a covalent bond. Molecular Orbital Theory a better model that uses wave theory, BUT not covered in Chem 110! [studied in Chem 112 and organic chemistry]! 11! 12!
7 Overlap and Bonding! " Covalent bonds formed through the sharing of electrons by adjacent atoms.! " Only occurs when orbitals on the two atoms overlap.! Overlap and Bonding! Two forces operating: " increased overlap of atomic orbitals (better sharing) brings atoms together closer distance between nuclei increases positive-positive charge repulsion balance of forces! bond length (0.74 Å for 2 )! 13! 14!
8 ow can atomic orbitals overlap to form observed geometries?! Bonding in C 4 Carbon ground-state configuration: Using only open (unpaired) subshell electrons: C Expect:"C 2 " molecule 90 o bond angles. What if we Promote 2 electrons? If all subshell electrons participated in bonding, this "C 4 " molecule would have: ! owever, "" Real molecule is tetrahedral "" o bond angles, "" all bonds are equal length and strength 16!
9 Bonding Orbitals in Be! " Consider beryllium:! " No singly-occupied orbitals! " Can t form Bonds?! ybrid Orbitals! " Mixing the s and p orbitals yields two degenerate orbitals that are hybrids of the two orbitals.! " These sp hybrid orbitals have lobes like a p orbital.! " One of the lobes is larger and more rounded as is the s orbital.! " Absorb Energy! " Now form 2 bonds?! " Bonds equal?! 17!!The sp orbitals are higher in energy than the 1s orbital but lower than the 2p.! 18!
10 ybrid Orbitals on Be! " These two degenerate sp orbitals would align themselves 180 from each other.! " This is consistent with the observed geometry of beryllium compounds: linear.! ybrid orbitals on B! Using a similar model for boron leads to! degenerate sp 2 orbitals.! 19! 20!
11 ybrid Orbitals on C! With carbon we get! degenerate sp 3 orbitals.! Naming ybrid Orbitals! NOTE: 1. start with four atomic orbitals s p x p y p z 2. end up with four hybrid orbitals 4 sp 3 # orbitals name of orbital Each hybrid orbital is composed of: 21! 22!
12 ybrid Orbitals Using d Orbitals! ybrid Orbitals! 23! 24!
13 Deduce the ybridization from Molecular Shape! ormula!structure! ybridization! N N O O B B 25!
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