Molecular shapes. Balls and sticks
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1 Molecular shapes Balls and sticks
2 Learning objectives Apply VSEPR to predict electronic geometry and shapes of simple molecules Determine molecule shape from electronic geometry Distinguish between polar and nonpolar bonds in molecules Predict polarity of simple molecules from bond polarity and molecular shape
3 Roadmap to polarity Establish skeleton of molecule Determine Lewis dot structure using S = N A Determine electronic geometry using VSEPR Identify molecular geometry from molecular Count number of polar bonds Perform polarity analysis
4 Stage 2: Valence shell electron pair repulsion Lewis dot structure provides 2D sketch of the distribution of the valence electrons among bonds between atoms and lone pairs; it provides no information about molecular shape First approach to this problem is to consider repulsion between groups of electrons (charge clouds)
5 Electron groups (clouds) minimize potential energy Valence shell electron pair repulsion (VSEPR) Identify all groups of charge: nonbonding pairs or bonds (multiples count as one) Bonded atoms single, double or triple count as 1 Lone pairs count as 1 Distribute them about central atom to minimize potential energy (maximum separation)
6 Electronic geometry: Counting groups of charge Identify central atom. Many molecules have more than one. Central atom has more than one atom bonded to it
7 Choices are limited Groups of charge range from 2 4 If octet expanded can get 5 or 6 Only one electronic geometry in each case More than one molecular shape follows from electronic geometry depending on number of lone pairs
8 Total number of groups dictates electronic geometry Octet rule: Two linear Three trigonal planar Four tetrahedral Additional possibilities (expand octet): Five trigonal bipyramidal Six - octahedral
9 Stage 3: Molecular shape: What you get from electronic geometry considering atoms only Same tetrahedral electronic geometry different molecular shape 1. Establish electronic structure using Lewis dot model 2. Determine electronic geometry using VSEPR model 3. Determine molecular shape from electronic geometry 4. Determine molecule polarity using symmetry model
10 Two groups: linear Except for BeH 2, all cases with two groups involve multiple bonds
11 Three groups: trigonal planar Two possibilities for central atoms with complete octets: Trigonal planar (H 2 CO) Bent (SO 2 ) BH 3 is example of trigonal planar with three single bonds B is satisfied with 6 electrons
12 Four groups: tetrahedral Three possibilities: No lone pairs (CH 4 ) - tetrahedral One lone pair (NH 3 ) trigonal pyramid Two lone pairs (H 2 O) bent Note: lone pairs need more room: H-N-H angle 107 H-O-H angle Tetrahedral angle 109.5
13 Representations of the tetrahedron
14 Groups of charge Lone electron pairs Electronic geometry Molecular shape 2 0 Linear Linear 3 0 Trigonal planar Trigonal planar 3 1 Trigonal planar Bent 4 0 Tetrahedral Tetrahedral 4 1 Tetrahedral Trigonal pyramid 4 2 Tetrahedral Bent
15 Molecules with multiple centers A central atom is any atom with more than one atom bonded to it Perform exercise individually for each atom Electronic geometry and molecular shape will refer only to the atoms/lone pairs immediately attached to that atom
16 Important properties related to polarity Solubility: polar molecules dissolve in polar solvents; nonpolar molecules dissolve in nonpolar solvents Oil (nonpolar) and water (polar) don t mix Ammonia (polar) dissolves in water Melting and boiling points Polar substances have high intermolecular forces: Melting and boiling points are much higher than with nonpolar substances (H 2 O is a liquid, CO 2 is a gas)
17 Roadmap to polarity Establish skeleton of molecule Determine Lewis dot structure using S = N A Determine electronic geometry using VSEPR Identify molecular geometry from molecular Count number of polar bonds Perform polarity analysis
18 Polar bonds and polar molecules Not all molecules containing polar bonds will themselves be polar. Need to examine the molecular shape Ask the question: Do the individual bond polarities cancel out? If so, non polar. If not, polar.
19 How to determine if polarity cancels out In CO 2 (linear molecule) the two polar bonds oppose each other exactly In chemical tug-o-war there is stalemate
20 H 2 O: The most important polar molecule In BF 3 the three bonds cancel out tug of war stalemate In H 2 O (bent) the polar bonds do not directly oppose no stalemate Lone pair also adds some component Overall net polarity Consequence of polarity: H 2 O is a liquid, CO 2 is a gas
21 Symmetry and polarity If the molecule looks symmetrical it will be nonpolar If the molecule looks non-symmetrical it will be polar
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