3D Molecular Geometry
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1 3D Molecular Geometry
2 Shades and Behaviours of 3D Molecules In order to understand the shapes the molecules form we must adhere to rules that are based on the repulsion of valence shell electrons! VSEPR = Valence Shell Electron Pair Repulsion
3 Reasons for Geometry boils down to 5 things 1. Electrons all have the same negative charge 2. Like charges repel therefore Electrons repel 3. Bonded pairs surrounding the nucleus repel other bonded pairs and other electrons 4. Lone pairs surrounding the nucleus repel other bonded pairs and other electrons 5. Valence electrons are oriented in such a way as to be as far apart from one another as possible For each of the following models,, and
4 Shapes of 3D Molecules Molecule Electron Pair Geometry (includes ALL substituents) Molecular Geometry or Shape (includes only bonded substituents) Reason for Shape BeCl 2 (AX 2 ) Linear The 2 pairs of bonding electrons maximize their distance from each other 180 o apart
5 Shapes of 3D Molecules Molecule Electron Pair Geometry (includes ALL substituents) Molecular Geometry or Shape (includes only bonded substituents) Reason for Shape BF 3 (AX 3 ) (AX 3 E 2 ) Trigonal Planar The bonding pairs must be equally far from each other The 3 bonding pairs maximize distance from each other 120 o
6 Shapes of 3D Molecules Molecule Electron Pair Geometry (includes ALL substituents) Molecular Geometry or Shape (includes only bonded substituents) Reason for Shape CH 4 (AX 4 ) Tetrahedral Tetrahedral The bonding pairs must be equally far from each other Maximize distance from each other
7 Shapes of 3D Molecules Molecule Electron Pair Geometry (includes ALL substituents) Molecular Geometry or Shape (includes only bonded substituents) Reason for Shape NH 3 (AX 3 E) Trigonal pyramidal or Triangular pyramidal Because the lone pairs are closer to the nucleus they have great repulsion, push the H s down Tetrahedral
8 Shapes of 3D Molecules Molecule Electron Pair Geometry (includes ALL substituents) Molecular Geometry or Shape (includes only bonded substituents) Reason for Shape H 2 O (AX 2 E 2 ) Bent The two sets of lone pairs further push the H s down and together Tetrahedral
9 Shapes of 3D Molecules Molecule Electron Pair Geometry (includes ALL substituents) Molecular Geometry or Shape (includes only bonded substituents) Reason for Shape PCl 5 (AX 5 ) To maximize distance 3 equatorial Cl s are 120 o Trigonal bipyramidal or Triangular bipyramidal Trigonal bipyramidal or Triangular bipryamidal Top and bottom Cl s are 90 o apart
10 Shapes of 3D Molecules Molecule Electron Pair Geometry (includes ALL substituents) Molecular Geometry or Shape (includes only bonded substituents) Reason for Shape SF 6 (AX 6 ) As more bonding pairs fill up locations around the nucleus the space between the pairs becomes smaller and smaller Octahedral Octahedral The molecule becomes less stable due to increased repulsion
11 Shapes of 3D Molecules Molecule Electron Pair Geometry (includes ALL substituents) Molecular Geometry or Shape (includes only bonded substituents) Reason for Shape XeF 4 (AX 4 E 2 ) Similar to Octahedral except two lone pairs occupy the axial positions. Octahedral Square Planar
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14 Steps to Make VSEPR Diagrams
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20 Combining two Concepts We are combining two concepts to introduce a new one Polarity
21 Remember Electronegativity Values
22 Polarity Molecules are said to be polar is the electron density is NOT evenly spread around the molecule This causes part of the molecule to be partially positive and part of the molecule to be partially negative Two Factors 1) Electronegativity 2) Symmetry of the Molecule (based on shape)
23 Determining the Dipole + Dipole In the bonding unit we determined if a bond was polar based on the electronegativity difference of the two elements To determine if the entire molecule is polar we must also check the symmetry (or lack there of) of the molecule
24 Symmetry vs. Asymmetry
25 Case 1: Non-Polar
26 Case 2: Polar and Asymmetric
27 Case 3: Polar and Symmetric Polar or not polar?
28 Case 3: Polar and Symmetric Not Polar
29 Case 4: Polar and Asymmetric Polar or not polar?
30 Case 4: Polar and Asymmetric Polar
31 Same Shape, Different Polarity
32 Question to ask yourself Polar or not Polar? Does the molecule contain polar bonds, and if so, do the bond dipoles cancel each other or not?
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36 Polarity The extent of polarity depends on the size of the dipole The size of the dipole depends on the difference in electronegativities and the symmetry (or lack there of) of the molecule
37 Polarity When two substances have opposite polarities, they do not mix. Like mixes with Like
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