Chapter 3. Orbitals and Bonding
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1 Chapter 3. Orbitals and Bonding What to master Assigning Electrons to Atomic Orbitals Constructing Bonding and Antibonding Molecular Orbitals with Simple MO Theory Understanding Sigma and Pi Bonds Identifying the Hybridization of Atoms in Molecules Understanding and Using Resonance Recognizing Energy Levels of Molecular Orbitals OrgChem1-Chap3-2ed 1
2 Chapter 3. Orbitals and Bonding Atomic orbitals (AOs): 62 Figure 3.1 orbital: the space occupied by electrons; principal (n), angular (l), magnetic (m) & spin (s) quantum numbers 1s, 2s, 2p x, 2p y, 2p z, 3s, 3p x, 3p y, 3p z, 3d xy, 3d xz, 3d yz, 3d x 2-y 2, 3d z 2 the more the nodes, the higher the energy level Electron configuration: 64 Figure 3.2 distribution of electrons among orbitals: aufbau principle, Pauli exclusion principle & Hund s rule ground state vs excited state OrgChem1-Chap3-2ed 2
3 Molecular Orbitals (I) Molecular orbitals (MOs) the LCAO approximation: e.g., H 2 66 Figure 3.3 energy level diagram of H 2 : 66 Figure 3.4 shape of a sigma (σ) bond: cylindrical; symmetrical around the internuclear axis, 67 Figure 3.5 How about a He 2 molecule? Is it stable enough to exist? OrgChem1-Chap3-2ed 3
4 Molecular Orbitals (II) Valence bond theory (VBT) assumption for complex molecules: MOs localized between two bonded atoms Summary: 68 bottom 2 MOs from 2 AOs of 2 atoms (No. of MOs = No. of AOs) one combination: bonding (σ) MO, the other: antibonding (σ*) MO the same rules for electron assignment to MOs as to AOs E dis No. of electrons x ΔE ΔE degree of overlap of the AOs (too close, too unstable) OrgChem1-Chap3-2ed 4
5 Bonding & Hybridization (I) Single bonds & sp 3 hybridization experimental data for CH 4 : the same bond length & angle hybridization of s & 3 p: 4 sp 3 (to fit the data), 69 Fig. 3.6 (cf.) σ bonds for CH 4 : 70 Figure 3.7 other compounds: CH 3 -CH 3, NH 3, CH 3 -OH; 71 Figure 3.8 σ bonding for a C-C bond: 70 middle OrgChem1-Chap3-2ed 5
6 OrgChem1-Chap3-2ed 6
7 Hybridization (II) Double bonds & sp 2 hybridization experimental data for CH 2 =CH 2 : planar, 72 Figure 3.9 hybridization of s & 2 p: 3 sp 2 & the rest 1 p pi(π) bond from the p-p overlap: 73 Figure 3.10 energy level of π and π*: 74 Figure 3.11 (ΔE π = 64, ΔE σ = 81) difficult rotation around a double bond: 74 Figure 3.12 other molecules with sp 2 : CH 2 NH, CH 2 O; 75 Figure 3.13 OrgChem1-Chap3-2ed 7
8 Hybridization (III) Triple bonds & sp hybridization experimental data for HC CH: linear, 76 Figure 3.14 hybridization of s & 1 p: 2 sp & the rest 2 p perpendicular pi(π) bonds others with an sp orbital: HCN, 76, Problem 3.7 Problems 3.8 & 3.9, 77 OrgChem1-Chap3-2ed 8
9 Resonance (I) Delocalized MOs (= resonance) conjugated parallel p orbitals: carboxylate; 79 Figure 3.15 resonance stabilization: MO theory practice: 79 Practice 3.1 & 80 Practice 3.2 OrgChem1-Chap3-2ed 9
10 Resonance by MO Theory Further stabilization by conjugation π* π* 3 p C C π O p O ΔΔE p C π 2 p O p O π 1 C O - O OrgChem1-Chap3-2ed 10
11 Resonance (II) Rules for applying resonance structures 1. Move only π & nonbonding e - : 82 Problem The same No. of e - and charge: 83 Problem Relative stability by octet rule & charge: 84 Practice 3.5 more bonding, fewer charge, closer unlike charge, farther like chare & negative charge on more electronegative atom 4. Real structure the most stable one (resonance structure) 5. The more the important resonances, the more stable: 85, Problem & 3.15 OrgChem1-Chap3-2ed 11
12 Resonance (III) Types of resonance interactions 1. unshared electrons: carboxylate, enolate, carboxylic acid curved double-headed arrow: 86 Figure one electron: allyl radical curved single-headed arrow: 87 Figure empty p orbitals (no e - ): allyl cation; 87 Figure atoms of different electronegativities: 88 Figure cyclic conjugation: benzene, 89 Figure 3.20 OrgChem1-Chap3-2ed 12
13 Resonance (IV) Combinations of the resonance types the anion of phenol: phenoxide, 90 Figure 3.21 (1&5) conjugated C=C with C=O: 92 Figure 3.22 (3&4) practice: 92 Practice 3.6 & 93 Problem 3.17 OrgChem1-Chap3-2ed 13
14 Resonance (V) Properties predicted from resonance structures naphthalene: 94 Focus On bond length: cf. C-C 1.54 Å, C=C 1.34 Å stability: relatively unstable to benzene (identical, 1.40 Å) bond energy: C-H; ethane vs propene smaller E dis of propene: resonance stabilized radical OrgChem1-Chap3-2ed 14
15 Energy Levels of MOs Relative levels of orbital energies: σ < π < n < π* < σ* ethane: 95 Figure 3.23 (only σ MOs) ethylene: 96 Figure 3.24 (σ & π MOs) formaldehyde: 96 Figure 3.25 (σ & π MOs and n AOs) practice: 97 Problem 3.18 OrgChem1-Chap3-2ed 15
16 그저익숙하도록읽는것뿐이다. 글을읽는사람이, 비록글의뜻은알았으나, 만약익숙하지못하면읽자마자곧잊어버리게되어, 마음에간직할수없을것은틀림없다. 이미읽고난뒤에, 또거기에자세하고익숙해질공부를더한뒤라야비로소마음에간직할수있으며, 또흐뭇한맛도있을것이다. - 퇴계이황 ( 금장태著 ) OrgChem1-Chap3-2ed 16
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