8.3 Bonding Theories > Chapter 8 Covalent Bonding. 8.3 Bonding Theories. 8.1 Molecular Compounds 8.2 The Nature of Covalent Bonding
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1 Chapter 8 Covalent Bonding 8.1 Molecular Compounds 8.2 The Nature of Covalent Bonding 8.3 Bonding Theories 8.4 Polar Bonds and Molecules 1 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
2 CHEMISTRY & YOU How can you predict where an electron is most likely to be found in a molecule? The lines on a topographic map show you where elevations change. In this lesson, you will learn how to interpret electron maps that show where you are most likely to find electrons. 2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
3 Molecular Orbitals Molecular Orbitals How are atomic and molecular orbitals related? 3 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
4 Molecular Orbitals The model you have been using for covalent bonding assumes the orbitals are those of the individual atoms. There is a quantum mechanical model of bonding, however, that describes the electrons in molecules using orbitals that exist only for groupings of atoms. 4 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
5 Molecular Orbitals When two atoms combine, this model assumes that their atomic orbitals overlap to produce molecular orbitals, or orbitals that apply to the entire molecule. In some ways, atomic orbitals and molecular orbitals are similar. 5 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
6 Molecular Orbitals Just as an atomic orbital belongs to a particular atom, a molecular orbital belongs to a molecule as a whole. A molecular orbital that can be occupied by two electrons of a covalent bond is called a bonding orbital. 6 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
7 Molecular Orbitals Sigma Bonds When two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting two atomic nuclei, a sigma bond is formed. Its symbol is the Greek letter sigma (σ). represents the nucleus s atomic orbital s atomic orbital Sigma-bonding molecular orbital Bond axis 7 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
8 Molecular Orbitals Sigma Bonds In general, covalent bonding results from an imbalance between the attractions and repulsions of the nuclei and electrons involved. The nuclei and electrons attract each other. Nuclei repel other nuclei. Electrons repel other electrons. 8 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
9 Molecular Orbitals Sigma Bonds In a bonding molecular orbital of hydrogen, however, the attractions between the hydrogen nuclei and the electrons are stronger than the repulsions. The balance of all the interactions between the hydrogen atoms is thus tipped in favor of holding the atoms together. The result is a stable diatomic molecule of H 2. 9 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
10 Molecular Orbitals Sigma Bonds Atomic p orbitals can also overlap to form molecular orbitals. A fluorine atom, for example, has a halffilled 2p orbital. When two fluorine atoms combine, the p orbitals overlap to produce a bonding molecular orbital. 10 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
11 Molecular Orbitals Sigma Bonds There is a high probability of finding a pair of electrons between the positively charged nuclei of the two fluorines. The overlap of the 2p orbitals produces a bonding molecular orbital that is symmetrical when viewed around the F F bond axis connecting the nuclei. Therefore, the F F bond is a sigma bond. 11 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
12 Molecular Orbitals Pi Bonds In the sigma bond of the fluorine molecule, the p atomic orbitals overlap end to end. In some molecules, however, orbitals can overlap side to side. 12 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
13 Molecular Orbitals Pi Bonds As shown here, the side-by-side overlap of atomic p orbitals produces what are called pi molecular orbitals. represents the nucleus p atomic orbital p atomic orbital Pi-bonding molecular orbital 13 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
14 Molecular Orbitals Pi Bonds In a pi bond (symbolized by the Greek letter π), the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms. Because atomic orbitals in pi bonding overlap less than in sigma bonding, pi bonds tend to be weaker than sigma bonds. 14 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
15 CHEMISTRY & YOU How can a drawing show where an electron is most likely to be found? 15 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
16 CHEMISTRY & YOU How can a drawing show where an electron is most likely to be found? Drawings can show molecular orbitals, which are the areas where bonding electrons are most likely to be found. 16 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
17 In molecules with sigma bonds, where are the shared electrons most likely to be found? 17 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
18 In molecules with sigma bonds, where are the shared electrons most likely to be found? In sigma bonds, bonding electrons are most likely found between the positively charged nuclei of the atoms bonded together. 18 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
19 VSEPR Theory VSEPR Theory What do scientists use the VSEPR theory for? 19 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
20 VSEPR Theory Electron dot structures fail to reflect the three-dimensional shapes of molecules. The electron dot structure and structural formula of methane (CH 4 ) show the molecule as if it were flat and merely two-dimensional. Methane (electron dot structure) Methane (structural formula) 20 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
21 VSEPR Theory In reality, methane molecules are three-dimensional. The hydrogens in a methane molecule are at the four corners of a geometric solid called a regular tetrahedron. In this arrangement, all of the H C H angles are 109.5, the tetrahedral angle. 21 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
22 VSEPR Theory In order to explain the threedimensional shape of molecules, scientists use valence-shell electronpair repulsion theory (VSEPR theory). VSEPR theory states that the repulsion between electron pairs causes molecular shapes to adjust so that the valenceelectron pairs stay as far apart as possible. 22 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
23 VSEPR Theory Unshared pairs of electrons are also important in predicting the shapes of molecules. The nitrogen in ammonia (NH 3 ) is surrounded by four pairs of valence electrons. Ammonia (NH 3 ) However, one of the valence-electron pairs is an unshared pair. 23 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
24 VSEPR Theory No bonding atom is vying for these unshared electrons; thus, they are held closer to the nitrogen than are the bonding pairs. The unshared pair strongly repels the bonding pairs, pushing them together. The measured H N H bond angle is only 107, rather than the tetrahedral angle of Unshared electron pair Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
25 VSEPR Theory In a water molecule, the two bonding pairs and the two unshared pairs of electrons form a tetrahedral arrangement around the central oxygen. Thus, the water molecule is planar (flat) but bent. With two unshared pairs repelling the bonding pairs, the H O H bond angle is compressed to about 105. Unshared pairs Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
26 VSEPR Theory The carbon in a carbon dioxide molecule has no unshared electron pairs. The double bonds joining the oxygens to the carbon are farthest apart when the O=C=O bond angle is 180. Thus, CO 2 is a linear molecule. Carbon dioxide (CO 2 ) 180 No unshared electron pairs on carbon 26 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
27 VSEPR Theory Here are some common molecular shapes. Linear Trigonal planar Bent Pyramidal Tetrahedral Trigonal bipyramidal Octahedral Square planar 27 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
28 What causes valence-electron pairs to stay as far apart as possible? 28 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
29 What causes valence-electron pairs to stay as far apart as possible? The repulsion between electron pairs due to their negative charges causes valenceelectron pairs to stay as far apart as possible. 29 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
30 Hybrid Orbitals Hybrid Orbitals In what ways is orbital hybridization useful in describing molecules? 30 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
31 Hybrid Orbitals The VSEPR theory works well when accounting for molecular shapes, but it does not help much in describing the types of bonds formed. 31 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
32 Hybrid Orbitals Orbital hybridization provides information about both molecular bonding and molecular shape. In hybridization, several atomic orbitals mix to form the same total number of equivalent hybrid orbitals. 32 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
33 Hybrid Orbitals Hybridization Involving Single Bonds Recall that the carbon atom s outer electron configuration is 2s 2 2p 2, but one of the 2s electrons is promoted to a 2p orbital to give one 2s electron and three 2p electrons. You might suspect that one bond in methane would be different from the other three. 33 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
34 Hybrid Orbitals Hybridization Involving Single Bonds In fact, all the bonds are identical. The one 2s orbital and three 2p orbitals of a carbon atom mix to form four sp 3 hybrid orbitals at the tetrahedral angle of Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
35 Hybrid Orbitals Hybridization Involving Single Bonds In methane, each of the four sp 3 hybrid orbitals of carbon overlaps with a 1s orbital of a hydrogen. Atomic orbitals of two hydrogen atoms Sigma bond Sigma bond Sigma bond Sigma bond Hybrid orbitals of a carbon atom 35 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
36 Hybrid Orbitals Hybridization Involving Single Bonds The sp 3 orbitals extend farther into space than either s or p orbitals, allowing a great deal of overlap with the hydrogen 1s orbitals. The extent of overlap results in unusually strong covalent bonds. Sigma bond Sigma bond Sigma bond Sigma bond 36 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
37 Hybrid Orbitals Hybridization Involving Double Bonds Ethene is a relatively simple molecule that has one carbon-carbon double bond and four carbon-hydrogen single bonds. 37 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
38 Hybrid Orbitals Hybridization Involving Double Bonds In ethene, sp 2 hybrid orbitals form from the combination of one 2s and two 2p atomic orbitals of carbon. As you can see in the figure on the next slide, each hybrid orbital is separated from the other two by Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
39 Hybrid Orbitals Hybridization Involving Double Bonds Hybrid orbitals of two hydrogen atoms Hybrid orbitals of two hydrogen atoms Atomic orbital and hybrid orbitals of a carbon atom Pi bond Sigma bond 39 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
40 Hybrid Orbitals Hybridization Involving Double Bonds In an ethene molecule, two sp 2 hybrid orbitals of each carbon form sigmabonding molecular orbitals with the four available hydrogen 1s orbitals. Sigma bond Pi bond The third sp 2 orbitals of each of the two carbons overlap to form a carbon-carbon sigma-bonding orbital. The 2p carbon orbitals overlap side by side to form a pi-bonding orbital. 40 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
41 Hybrid Orbitals Hybridization Involving Triple Bonds A third type of covalent bond is a triple bond, which is found in ethyne (C 2 H 2 ), also called acetylene. 41 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
42 Hybrid Orbitals Hybridization Involving Triple Bonds Ethyne is a linear molecule. The best hybrid orbital description is obtained if a 2s atomic orbital of carbon mixes with only one of the three 2p atomic orbitals. The result is two sp hybrid orbitals for each carbon. 42 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
43 Hybrid Orbitals Hybridization Involving Triple Bonds Atomic orbital of a hydrogen atom Atomic orbital of a hydrogen atom Atomic orbitals and hybrid orbitals of a carbon atom Pi bond Sigma bonds 43 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
44 Hybrid Orbitals Hybridization Involving Double Bonds In an ethyne molecule, one sp hybrid orbital from each carbon overlaps with a 1s orbital of hydrogen to form a sigma bond. Pi bond Sigma bonds The other sp hybrid orbital of each carbon overlaps to form a carbon-carbon sigma bond. The two p atomic orbitals from each carbon also overlap. 44 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
45 How many hybridized orbitals form when one 2s orbital is hybridized with three 2p orbitals? 45 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
46 How many hybridized orbitals form when one 2s orbital is hybridized with three 2p orbitals? Four sp 3 orbitals form. 46 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
47 Key Concepts Just as an atomic orbital belongs to a particular atom, a molecular orbital belongs to a molecule as a whole. In order to explain the three-dimensional shape of molecules, scientists use the valence-shell electron-pair repulsion theory (VSEPR theory). Orbital hybridization provides information about both molecular bonding and molecular shape. 47 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
48 Glossary Terms molecular orbital: an orbital that applies to the entire molecule bonding orbital: a molecular orbital that can be occupied by two electrons of a covalent bond sigma bond (σ bond): a bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei pi bond (π bond): a covalent bond in which the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms 48 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
49 Glossary Terms tetrahedral angle: a bond angle of that results when a central atom forms four bonds directed toward the center of a regular tetrahedron VSEPR theory: valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible hybridization: the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals 49 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
50 BIG IDEA Bonding and Interactions Shared electrons and the valence electrons that are not shared affect the shape of a molecular compound, as the valence electrons stay as far apart from each other as possible. 50 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
51 END OF Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
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