1. Section 3.3 – Part A Pg. 91-96 Objective: 1) Apply VSEPR theory to predict molecular shapes

2.  Stereochemistry – is the study of the 3-D spatial configuration of molecules and how this affects their reactions.  The shape of molecules is determined by the repulsion that happens between electron pairs  The theory behind molecular shapes is called VSEPR Theory (Valence Shell Electron Pair Repulsion) Solid = in plane of page Dashed = behind (away) Wedge = ahead (toward)

3.  General Rule: ◦ Pairs of electrons in the valence shell of an atom stay as far apart as possible because of the repulsion of their negative charges ◦ The type, number and direction of bonds to the central atom of a molecule determine the shape of the resulting molecule.  So how do we predict these molecular shapes?

4.  We will be using the following compounds to analyze the 6 shapes possible ◦ BeH 2(s), BH 3(g), CH 4(g), NH 3(g), H 2 O (l), HF (g)  To start, draw a Lewis formula for each of the molecules and then consider the arrangement of all pairs of valence electrons. ◦ (Remember – all pairs of valence e - ’s repel each other and want to get as far apart as possible)

5. Lewis Formula Bond Pairs Lone Pairs Total Pairs General Formula Electron Pair Arrangement Stereochemical Formula 202AX 2 linear X – A – X linear Be This Lewis formula indicates that BeH 2(s) has two bonds and no lone pairs on the central atom. VSPER theory suggests that the two bond pairs will be farthest apart by moving to opposite sides to a bond angle of 180° This gives the molecule a linear orientation * A is the central atom; X is another atom *Exception* Beryllium does not follow OCTET RULE

6. Lewis Formula Bond Pairs Lone Pairs Total Pairs General Formula Electron Pair Arrangement Stereochemical Formula 303AX 3 trigonal planar This Lewis formula indicates that BH 3(g) has three bonds and no lone pairs on the central atom. VSPER theory suggests that the three bond pairs will be farthest apart by moving to a bond angle of 120° to each other. This gives the molecule a trigonal planar orientation. * A is the central atom; X is another atom B *Exception* - Boron Does not follow OCTET RULE

7.  Draw the Lewis Formula for BF 3 Does not obey the octet rule Trigonal Planar F F F

8. Lewis Formula Bond Pairs Lone Pairs Total Pairs General Formula Electron Pair Arrangement Stereochemical Formula 404AX 4 tetrahedral This Lewis formula indicates that CH 4(g) has four bonds and no lone pairs on the central atom. VSPER theory suggests that the four bond pairs will be farthest apart by arranging in three dimensions so that every bond makes an angle of 109.5° with each other. This gives the molecule a tetrahedral orientation. * A is the central atom; X is another atom

9.  Draw the Lewis Formula for SiH 4 H H H H Tetrahedral

10. Lewis Formula Bond Pairs Lone Pairs Total Pairs General Formula Electron Pair Arrangement Stereochemical Formula 314AX 3 E tetrahedral Trigonal pyramidal This Lewis formula indicates that NH 3(g) has three bonds and one lone pair on the central atom. VSPER theory suggests that the four groups of e - ’s should repel each other to form a tetrahedral shape (bond angle = 109.5°) But the lone pair is very repulsive, thus pushes the atoms more to a 107.3° bond angle This gives the molecule a trigonal pyramidal orientation. * A is the central atom; X is another atom, E is a lone pair of electrons

11.  Draw the Lewis Formula for PCl 3 Cl Trigonal pyramidal

12. Lewis Formula Bond Pairs Lone Pairs Total Pairs General Formula Electron Pair Arrangement Stereochemical Formula 224 AX 2 E 2 tetrahedral Angular (Bent) This Lewis formula indicates that H 2 O (l) has two bonds and two lone pairs on the central atom. VSPER theory suggests that the four groups of e - ’s should repel each other to form a tetrahedral shape (bond angle = 109.5°) But the TWO lone pairs are very repulsive, thus pushes the atoms more to a 105° bond angle This gives the molecule an angular (bent) orientation. * A is the central atom; X is another atom, E is a lone pair of electrons

13.  Draw the Lewis Formula for OCl 2 Angular (bent)

14. Lewis Formula Bond Pairs Lone Pairs Total Pairs General Formula Electron Pair Arrangement Stereochemical Formula 134 AXE 3 Linear (Tetrahedral) This Lewis formula indicates that H 2 O (l) has two bonds and two lone pairs on the central atom. VSPER theory suggests that the four groups of e - ’s should repel each other to form a tetrahedral shape (bond angle = 109.5°) But since there are only two atoms with one covalent bond holding them together, by definition, the shape is linear, as is the shape of every other diatomic molecule. * A is the central atom; X is another atom, E is a lone pair of electrons FH

15.  Draw the Lewis Formula for HCl

16.  VSEPR theory describes, explains, and predicts the geometry of molecules by counting pairs of electrons that repel each other to minimize repulsion. The process for predicting the shape of a molecule is summarized below:  Step 1: Draw the Lewis formula for the molecule, including the electron pairs around the central atom.  Step 2: Count the total number of bonding pairs (bonded atoms) and lone pairs of electrons around the central atom.  Step 3: Refer to Table 7, and use the number of pairs of electrons to predict the shape of the molecule.

17. Pg. 95

18.  Draw the Lewis and stereochemical formulas for a sulfate ion, SO 4 2- and predict the shape ◦ See pg. 95  Draw the Lewis and stereochemical formulas for a chlorate ion, ClO 3 - and predict the shape ◦ See pg. 96  On your own: Pg. 96 #3

19.  It is important to remember that a double or triple bond is one bond, and to treat it as such, when predicting the VSEPR shapes of molecules.  Example: Predict the shape of C 2 H 4(g) ◦ Draw the Lewis formula for the molecule ◦ Count the # of pairs of e - ’s around the central carbon atoms.  The carbon atoms have 3 bonds (2 single, 1 double) and no lone pairs.  This is the same as a trigonal planar configuration.trigonal planar  Practice: Predict the shape for C 2 H 2(g). H H H H Answer: See pg. 97

20. 1) Finish pg. 96 #1-3 2) Pg. 98 #6-7 (Multiple Bond Practice) ◦ For 7 c, d, e - If there is more than one central atom involved, tell me the shape around each of the central atoms ◦ Example: 3) Pg. 104 #1, 2, 3  #2: If there is more than one central atom involved, tell me the shape around each of the central atoms trigonal planar—first two carbons tetrahedral—third carbon

21.  Draw the Lewis Formula for PCl 3