Chapter 4 Compounds and Their Bonds
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1 Chapter 4 Compounds and Their Bonds 4.7 Shapes and Polarity of Molecules Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 1
2 VSEPR In the valence-shell electron-pair repulsion theory (VSEPR), the electron groups around a central atom Are arranged as far apart from each other as possible. Have the least amount of repulsion of the negatively charged electrons. Have a geometry around the central atom that determines molecular shape. 2
3 Shapes of Molecules The three-dimensional shape of a molecule Is the result of bonded groups and lone pairs of electrons around the central atom. Is predicted using the VSEPR theory (valence-shellelectron-pair repulsion). 3
4 Guide to Predicting Molecular Shape (VSEPR Theory) STEP 1 Write the electron-dot structure. STEP 2 Arrange the electron groups around the central atom to minimize repulsion. STEP 3 Use the atoms bonded to the central atom to determine the shape of the molecule. 4
5 Two Electron Groups In a molecule of BeCl 2 There are two electron groups bonded to the central atom Be (exception to the octet rule)..... : Cl : Be : Cl :.... To minimize repulsion, the arrangement of two electron groups is 180 or opposite each other. The shape of the molecule is linear. Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 5
6 Two Electron Groups with Double Bonds In a molecule of CO 2 There are two electron groups bonded to C (electrons in each double bond are counted as one group). Repulsion is minimized with the double bonds opposite each other at 180. The shape of the molecule is linear. Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 6
7 Three Electron Groups In a molecule of BF 3 Three electron groups are bonded to the central atom B. (B is an exception to the octet rule)... : F: : F : B : F :.... Repulsion is minimized with 3 electron groups at angles of 120 Has a trigonal planar shape. Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 7
8 Two Electron Groups and One Lone Pair In a molecule of SO 2 S has 3 electron groups; 2 electron groups bonded to O atoms and one lone pair :O :: S : O :.. Repulsion is minimized with the electron groups at angles of 120, a trigonal planar arrangement. With two O atoms bonded to S, the shape is bent (120 ). Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 8
9 Learning Check The shape of a molecule of N 2 O (N N O) is 1) linear 2) trigonal planar 3) bent (120 ) 9
10 Solution The shape of a molecule of N 2 O (N N O) is 1) linear In the electron-dot structure with 16 e -, octets are acquired using two double bonds to the central N atom. The shape of a molecule with two electron groups and two bonded atoms (no lone pairs on N) is linear. two electron groups : N :: N :: O : : N = N=O : linear,
11 Four Electron Groups In a molecule of CH 4 There are four electron groups around C. Repulsion is minimized by placing four electron groups at angles of 109, which is a tetrahedral arrangement. The shape with four bonded atoms is tetrahedral. Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 11
12 Three Bonding Atoms and One Lone Pair In a molecule of NH 3 Three electron groups bond to H atoms and the fourth one is a lone (nonbonding) pair. Repulsion is minimized with 4 electron groups in a tetrahedral arrangement. With three bonded atoms, the shape is pyramidal. Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 12
13 Two Bonding Atoms and Two Lone Pairs In a molecule of H 2 O Two electron groups are bonded to H atoms and two are lone pairs (4 electron groups). Four electron groups minimize repulsion in a tetrahedral arrangement. The shape with two bonded atoms is bent(~109 ). Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 13
14 Shapes with 4 Electron Groups TABLE 4.16 Examples of Shapes of Molecules Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 14
15 Shapes with 2 and 3 Electron Groups Copyright 2007 by Pearson Education, Inc. Publishing as Benjamin Cummings 15
16 Learning Check State the number of electron groups, lone pairs, and use VSEPR theory to determine the shape of the following molecules or ions. 1) tetrahedral 2) pyramidal 3) bent A. PF 3 B. H 2 S C. CCl 4 16
17 Solution A. PF 3 4 electron groups, 1 lone pair, (2) pyramidal B. H 2 S 4 electron groups, 2 lone pairs, (3) bent C. CCl 4 4 electron groups, 0 lone pairs, (1) tetrahedral 17
18 Polar Molecules A polar molecule Contains polar bonds. Has a separation of positive and negative charge called a dipole indicated with δ + and δ -. Has dipoles that do not cancel. δ + δ - H Cl H N H dipole H dipoles do not cancel 18
19 Nonpolar Molecules A nonpolar molecule Contains nonpolar bonds. Cl Cl H H Or has a symmetrical arrangement of polar bonds. O=C=O Cl Cl C Cl Cl dipoles cancel 19
20 Determining Molecular Polarity STEP 1 STEP 2 STEP 3 Write the electron-dot formula. Determine the polarity of the bonds. Determine if dipoles cancel. Example: H 2 O.. H O: H H 2 O is polar dipoles do not cancel 20
21 Learning Check Identify each of the following molecules as 1) polar or 2) nonpolar. Explain. A. PBr 3 B. HBr C. Br 2 D. SiBr 4 21
22 Solution Identify each of the following molecules as 1) polar or 2) nonpolar. Explain. A. PBr 3 1) pyramidal; dipoles don t cancel; polar B. HBr 1) linear; one polar bond (dipole); polar C. Br 2 2) linear; nonpolar bond; nonpolar D. SiBr 4 2) tetrahedral; dipoles cancel; nonpolar 22
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