Molecular Geometry and Bonding Theories

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1 Molecular Geometry and Bonding Theories
AP Chemistry – Ch 9 Mr. Christopherson

2 CH4 C H C H molecular molecular structural formula shape formula
ball-and-stick model tetrahedral shape of methane tetrahedron

3 Methane & Carbon Tetrachloride
molecular formula structural formula molecular shape ball-and-stick model C H H 109.5o C CH4 The molecular geometry is predicted by first writing the Lewis structure, then using the VSEPR model to determine the electron-domain geometry, and finally focusing on the atoms themselves to describe the molecular structure. space-filling model C Cl CCl4

4 Molecular Geometry Trigonal planar Linear Tetrahedral Bent
Trigonal pyramidal H2O CH4 AsCl3 AsF5 BeH2 BF3 CO2

5 N H .. .. C H O .. H H .. O CH4, methane NH3, ammonia H2O, water O
lone pair electrons O O O3, ozone

6 Molecular Shapes Three atoms (AB2) Four atoms (AB3) B A Linear (180o)
Bent Trigonal planar (120o) Trigonal pyramidal T-shaped B A linear trigonal planar B A Five atoms (AB4) tetrahedral Tetrahedral (109.47o) Square planar Seesaw A Be Ba Six atoms (AB5) Trigonal bipyramidal (BeABe, 120o) & (BeABa, 90o) Square pyramidal B A Seven atoms (AB6) Trigonal bipyramidal Octahedral Bailar, Moeller, Kleinberg, Guss, Castellion, Metz, Chemistry, 1984, page 313.

7 Bonding and Shape of Molecules
Number of Bonds Number of Unshared Pairs Covalent Structure Shape Examples 2 3 4 1 2 -Be- Linear Trigonal planar Tetrahedral Pyramidal Bent BeCl2 BF3 CH4, SiCl4 NH3, PCl3 H2O, H2S, SCl2 B C N : O :

8 Molecular Shapes AB2 Linear AB3 Trigonal planar AB3E Angular or Bent
Tetrahedral AB3E Trigonal pyramidal AB3E2 Angular or Bent AB5 Trigonal bipyramidal AB4E Irregular tetrahedral (see saw) AB3E2 T-shaped AB2E3 Linear AB6 Octahedral AB6E Square pyramidal AB5E2 Square planar

9 The VSEPR Model .. .. .. The Shapes of Some Simple ABn Molecules O S O
Linear Bent Trigonal planar Trigonal pyramidal SF6 F P F S F Cl Students often confuse electron-domain geometry with molecular geometry. You must stress that the molecular geometry is a consequence of the electron domain geometry. The best arrangement of a given number of electron domains is the one that minimizes the repulsions among them. F Xe T-shaped Square planar Trigonal bipyramidal Octahedral Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 305

10 Molecular Shapes AB2 Linear AB3 Trigonal planar AB2E Angular or Bent
Tetrahedral AB3E Trigonal pyramidal AB2E2 Angular or Bent (Source: R.J. Gillespie, J. Chem. Educ., 40, 295, 1963.) AB5 Trigonal bipyramidal AB4E Irregular tetrahedral (see saw) AB3E2 T-shaped AB2E3 Linear AB6 Octahedral AB5E Square pyramidal AB4E2 Square planar

11 Geometry of Covalent Molecules ABn, and ABnEm
Shared Electron Pairs Unshared Electron Pairs Type Formula Ideal Geometry Observed Molecular Shape Examples AB2 AB2E AB2E2 AB2E3 AB3 AB3E AB3E2 AB4 AB4E AB4E2 AB5 AB5E AB6 2 3 4 5 6 1 2 3 Linear Trigonal planar Tetrahedral Trigonal bipyramidal Triangular bipyramidal Octahedral Linear Angular, or bent Trigonal planar Triangular pyramidal T-shaped Tetrahedral Irregular tetrahedral (or “see-saw”) Square planar Triangular bipyramidal Square pyramidal Octahedral CdBr2 SnCl2, PbI2 OH2, OF2, SCl2, TeI2 XeF2 BCl3, BF3, GaI3 NH3, NF3, PCl3, AsBr3 ClF3, BrF3 CH4, SiCl4, SnBr4, ZrI4 SF4, SeCl4, TeBr4 XeF4 PF5, PCl5(g), SbF5 ClF3, BrF3, IF5 SF6, SeF6, Te(OH)6, MoF6 Bailar, Moeller, Kleinberg, Guss, Castellion, Metz, Chemistry, 1984, page 317.

12 Molecules with Expanded Valence Shells
Atoms that have expanded octets have AB5 (trigonal bipyramidal) or AB6 (octahedral) electron domain geometries. Trigonal bipyramidal structures have a plane containing three electron pairs. F P The fourth and fifth electron pairs are located above and below this plane. In this structure two trigonal pyramids share a base. For octahedral structures, there is a plane containing four electron pairs. F S Similarly, the fifth and sixth electron pairs are located above and below this plane. Two square pyramids share a base.

13 Trigonal Bipyramid F P The three electron pairs in the plane are called equatorial. The two electron pairs above and below this plane are called axial. The axial electron pairs are 180o apart and 90o from to the equatorial electrons. The equatorial electron pairs are 120o apart. To minimize electron-electron repulsions, nonbonding pairs are always placed in equatorial positions, and bonding pairs in either axial or equatorial positions.

14 Octahedron F S The four electron pairs in the plane are 90o to each other. The remaining two electron pairs are 180o apart and 90o from the electrons in the plane. Because of the symmetry of the system, each position is equivalent. The equatorial electron pairs are 120o apart. If we have five bonding pairs and one nonbonding pair, it doesn’t matter where the nonbonding pair is placed. The molecular geometry is square pyramidal. If two nonbonding pairs are present, the repulsions are minimized by pointing them toward opposite sides of the octahedron. The molecular geometry is square planar. F Xe

15 Electron-Domain Geometries
Number of Electron Domains Arrangement of Electron Domains Electron-Domain Geometry Predicted Bond Angles 2 3 4 5 6 B A Linear Trigonal planar Tetrahedral Trigonal- bipyramidal Octahedral 180o 120o 109.5o 90o B A B A A Be Ba B A

16 Number of electron domains 4 3 4
Acetic Acid, CH3COOH H O H C C O H H Number of electron domains 4 3 4 Trigonal planar Electron-domain geometry Tetrahedral Tetrahedral Predicted bond angles 109.5o 120o 109.5o Hybridization of central atom sp3 sp2 none Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 314

17 Molecular Polarity Molecular Structure
Courtesy Christy Johannesson

18 + - Dipole Moment H Cl Direction of the polar bond in a molecule.
Arrow points toward the more electronegative atom. H Cl + - Courtesy Christy Johannesson

19 Determining Molecular Polarity
Depends on: dipole moments molecular shape Courtesy Christy Johannesson

20 Determining Molecular Polarity
Nonpolar Molecules Dipole moments are symmetrical and cancel out. BF3 F B Courtesy Christy Johannesson

21 Determining Molecular Polarity
Polar Molecules Dipole moments are asymmetrical and don’t cancel . H2O H O net dipole moment Courtesy Christy Johannesson

22 Determining Molecular Polarity
Therefore, polar molecules have... asymmetrical shape (lone pairs) or asymmetrical atoms CHCl3 H Cl net dipole moment Courtesy Christy Johannesson

23 Dipole Moment Nonpolar m = Q r Polar C O O O H H .. Bond dipoles
In H2O the bond dipoles are also equal in magnitude but do not exactly oppose each other. The molecule has a nonzero overall dipole moment. C O O .. Overall dipole moment = 0 O Bond dipoles Nonpolar H H The overall dipole moment of a molecule is the sum of its bond dipoles. In CO2 the bond dipoles are equal in magnitude but exactly opposite each other. The overall dipole moment is zero. Overall dipole moment m = Q r Dipole moment, m Coulomb’s law Polar Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 315

24 Polar Bonds .. .. .. F O N H Cl H H H B H H F F Polar Polar Nonpolar
Students often confuse electron-domain geometry with molecular geometry. You must stress that the molecular geometry is a consequence of the electron domain geometry. The best arrangement of a given number of electron domains is the one that minimizes the repulsions among them. F F F Cl H Xe C C Cl F F Cl H F F Cl H Polar Nonpolar Nonpolar Polar A molecule has a zero dipole moment because their dipoles cancel one another.

25 How is the electron density distributed in these different molecules?
HF HCl HBr HI How is the electron density distributed in these different molecules? Based on your comparison of the electron density distributions, which molecule should have the most polar bond, and which one the least polar? Arrange the molecules in increasing order of polarity. Using Computational Chemistry to Explore Concepts in General Chemistry Mark Wirtz, Edward Ehrat, David L. Cedeno* Department of Chemistry, Illinois State University, Box 4160, Normal, IL Mark Wirtz, Edward Ehrat, David L. Cedeno*

26 CH3Cl CHCl3 CCl4 CH2Cl2 Describe how is the electron density distributed in these different molecules? Based on your comparison of the electron density distributions, which molecule(s) should be the most polar, and which one(s) the least polar? Arrange the molecules in increasing order of polarity. Using Computational Chemistry to Explore Concepts in General Chemistry Mark Wirtz, Edward Ehrat, David L. Cedeno* Department of Chemistry, Illinois State University, Box 4160, Normal, IL Mark Wirtz, Edward Ehrat, David L. Cedeno*

27 NO3- Benzene Nitrobenzene
Using Computational Chemistry to Explore Concepts in General Chemistry Mark Wirtz, Edward Ehrat, David L. Cedeno* Department of Chemistry, Illinois State University, Box 4160, Normal, IL Mark Wirtz, Edward Ehrat, David L. Cedeno*

28 2s Using Computational Chemistry to Explore Concepts in General Chemistry Mark Wirtz, Edward Ehrat, David L. Cedeno* Department of Chemistry, Illinois State University, Box 4160, Normal, IL 2p (x, y, z) carbon Mark Wirtz, Edward Ehrat, David L. Cedeno*

29 Hydrogen Bond Formation
Potential Energy Diagram - Attraction vs. Repulsion Energy (KJ/mol) balanced attraction & repulsion no interaction increased attraction The change in potential energy during the formation of hydrogen molecule. The minimum energy, at 0.74 angstrom, represents the equilibrium bond distance. The energy at this point, -426 kJ/mol, corresponds to the energy change for formation of the H – H bond. Potential energy is based on the position of an object. Low potential energy = high stability. increased repulsion - 436 0.74 A H – H distance (internuclear distance) Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 318

30 First, the formation of BeH2 using pure s and p orbitals.
Be = 1s22s2 H Be BeH2 H s p No overlap = no bond! atomic orbitals atomic orbitals The formation of BeH2 using hybridized orbitals. Be H s p atomic orbitals Be H hybrid orbitals Be s p Be BeH2 sp p All hybridized bonds have equal strength and have orbitals with identical energies.

31 sp hybrid orbitals shown together
Ground-state Be atom 1s 2s 2p Be atom with one electron “promoted” sp hybrid orbitals Energy 1s sp 2p Be atom of BeH2 orbital diagram px py pz n = 1 n = 2 s two sp hybrid orbitals s orbital p orbital hybridize H Be sp hybrid orbitals shown together (large lobes only)

32 sp2 hybrid orbitals shown together
Ground-state B atom 2s 2p 2s 2p B atom with one electron “promoted” sp2 hybrid orbitals Energy sp2 2p px py pz s B atom of BH3 orbital diagram p orbitals H B three sps hybrid orbitals sp2 hybrid orbitals shown together (large lobes only) hybridize s orbital

33 Carbon 1s22s22p2 Carbon could only make two bonds
if no hybridization occurs. However, carbon can make four equivalent bonds. B A sp3 hybrid orbitals Energy px py pz sp3 s C atom of CH4 orbital diagram Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 321

34 Hybridization Involving d Orbitals
promote 3s p d s p d unhybridized P atom P = [Ne]3s23p3 vacant d orbitals hybridize A Be Ba F P five sp3d orbitals 3d degenerate orbitals (all EQUAL) Trigonal bipyramidal

35 Multiple Bonds 2s 2p 2s 2p sp2 2p C2H4, ethene H C
promote hybridize 2s p s p sp p C2H4, ethene C H one s bond and one p bond H C s H C Two lobes of one p bond Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page

36 Multiple Bonds C 2s 2p 2s 2p sp2 2p C2H4, ethene H C H
promote hybridize 2s p s p sp p C2H4, ethene p C H H sp2 one s bond and one p bond H C s H C Two lobes of one p bond Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page

37 p bond Internuclear axis p p

38 Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 326

39 s bonds H H C C H C C H C C H H C6H6 = benzene
Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 329

40 2p atomic orbitals Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 329

41 s bonds and p bonds H H C C H C C H C C H H
Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 329

42 s bonds H C H C H C H C H C H C H C H C
Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 329

43 s bonds H C H C H C H C H C H C H C H C
Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 329

44 N O O N O O N N O O N2O4 2 NO2 hn dinitrogen tetraoxide
nitrogen dioxide (free radical) N O O N O O N N O O colorless red-brown

45 Energy-level diagram for (a) the H2 molecule and (b) the hypothetical He2 molecule
s*1s 1s 1s Energy H atom H atom s1s H2 molecule (b) s*1s 1s 1s Energy He atom He atom s1s He2 molecule Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 332

46 Bond Order Bond order = ½ (# or bonding electrons - # of antibonding electrons) A bond order of 1 represents a single bond, A bond order of 2 represents a double bond, A bond order of 3 represents a triple bond. A bond order of 0 means no bond exists. Because MO theory also treats molecules with an odd number of electrons, Bond orders of 1/2 , 3/2 , or 5/2 are possible.

47 Energy-level diagram for the Li2 molecule
s*2s Li = 1s22s1 2s1 2s1 Energy s2s s*1s 1s2 1s2 Li Li s1s Li2 Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 334

48 Energy-level diagram for molecular orbitals
of second-row homonuclear diatomic molecules. s*2p p*2p 2p 2p p2p s2p s*2s 2s 2s s2s Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 337

49 Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 338

50 Increasing 2s – 2p interaction
p2p Energy of molecular orbitals s2p s*2s s2s O2, F2, Ne2 B2, C2, N2 Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 338

51 Large 2s – 2p interaction Small 2s – 2p interaction B2 C2 N2 O2 F2 Ne2
p*2p p*2p s2p p2p p2p s2p s*2s s*2s s2s s2s Bond order Bond enthalpy (kJ/mol) Bond length (angstrom) Magnetic behavior Paramagnetic Diamagnetic Diamagnetic Paramagnetic Diamagnetic _____ Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 339

52 s2s p2px p2py s2p s*2s p*2px p*2py s*2p C2
Using Computational Chemistry to Explore Concepts in General Chemistry Mark Wirtz, Edward Ehrat, David L. Cedeno* Department of Chemistry, Illinois State University, Box 4160, Normal, IL Arrange the atomic and molecular orbitals in order of increasing energy. How many orbitals are per molecule? Can you distinguish the bonding from the antibonding MOs? Mark Wirtz, Edward Ehrat, David L. Cedeno*

53 Magnetic Properties of a Sample
PARAMAGNETISM – molecules with one or more unpaired electrons are attracted into a magnetic field. (appears to weigh MORE in a magnetic field) DIAMAGNETISM – substances with no unpaired electrons are weakly repelled from a magnetic field. (appears to weigh LESS in a magnetic field)

54 Experiment for determining the magnetic properties of a sample
The sample is first weighed in the absence of a magnetic field. When a field is applied, a diamagnetic sample tends to move out of the field and appears to have a lower mass. A paramagnetic sample is drawn into the field and thus appears to gain mass. Paramagnetism is a much stronger effect than is diamagnetism. Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 339

55 Experiment for determining the magnetic properties of a sample
The sample is first weighed in the absence of a magnetic field. When a field is applied, a diamagnetic sample tends to move out of the field and appears to have a lower mass. A paramagnetic sample is drawn into the field and thus appears to gain mass. Paramagnetism is a much stronger effect than is diamagnetism. Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 339

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58 Electron Domains Lone Pair Single bond Double bond Triple bond

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62 Molecular Geometry Courtesy Christy Johannesson

63 VSEPR Theory Valence Shell Electron Pair Repulsion Theory
Electron pairs orient themselves in order to minimize repulsive forces. Courtesy Christy Johannesson

64 Lone pairs repel more strongly than bonding pairs!!!
VSEPR Theory Types of e- Pairs Bonding pairs - form bonds Lone pairs - nonbonding electrons Lone pairs repel more strongly than bonding pairs!!! Courtesy Christy Johannesson

65 VSEPR Theory Lone pairs reduce the bond angle between atoms.
Courtesy Christy Johannesson

66 Determining Molecular Shape
Draw the Lewis Diagram. Tally up e- pairs on central atom. double/triple bonds = ONE pair Shape is determined by the # of bonding pairs and lone pairs. Know the 8 common shapes & their bond angles! Courtesy Christy Johannesson

67 Common Molecular Shapes
2 total 2 bond 0 lone B A BeH2 LINEAR 180° Courtesy Christy Johannesson

68 Common Molecular Shapes
3 total 3 bond 0 lone B A BF3 TRIGONAL PLANAR 120° Courtesy Christy Johannesson

69 Common Molecular Shapes
3 total 2 bond 1 lone SO2 BENT <120° Courtesy Christy Johannesson

70 Common Molecular Shapes
4 total 4 bond 0 lone B A CH4 TETRAHEDRAL 109.5° Courtesy Christy Johannesson

71 Common Molecular Shapes
4 total 3 bond 1 lone NH3 TRIGONAL PYRAMIDAL 107° Courtesy Christy Johannesson

72 Common Molecular Shapes
4 total 2 bond 2 lone H2O BENT 104.5° Courtesy Christy Johannesson

73 Common Molecular Shapes
Be Ba 5 total 5 bond 0 lone PCl5 TRIGONAL BIPYRAMIDAL 120°/90° Courtesy Christy Johannesson

74 Common Molecular Shapes
6 total 6 bond 0 lone B A SF6 OCTAHEDRAL 90° Courtesy Christy Johannesson

75 F P F F 107° TRIGONAL PYRAMIDAL Examples 4 total 3 bond 1 lone PF3
Courtesy Christy Johannesson

76 O C O 180° LINEAR Examples 2 total 2 bond 0 lone CO2
Courtesy Christy Johannesson