Bài giảng về Lai Hóa

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14a–1
Figure 14.1: (a) Lewis structure of the methane molecule (b) the tetrahedral molecular geometry
of the methane molecule.
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14a–2
Figure 14.2: valence orbitals on a free
carbon atom
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14a–3
Figure 14.3: native 2s and three 2p atomic orbitals characteristic of a free carbon atome are combined to
form a new set of four sp3 orbitals.
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14a–4
Figure 14.5: Energy-level diagram showing the formation of four sp3 orbitals
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14a–5
Figure 14.7: The nitrogen atom in ammonia
is sp3 hybridized.
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14a–6
Figure 14.8: The hybridization of the s, px, and
py atomic orbitals results in the formation of three
sp2 orbitals centered in the xy plane.
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14a–7
Figure 14.9: An orbital energy-level diagram for sp2 hybridization:
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14a–8
Figure 14.13: (a) The orbitals used to form the bonds in ethylene. (b) The Lewis structure for ethylene.
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14a–9
Figure 14.14: When one s orbital and one
p orbital are hybridized, a set of two sp
orbitals oriented at 180 degrees results.
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14a–10
Figure 14.16: orbital energy level diagram for the formation of sp hybrid orbitals of carbon.
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14a–11
Figure 14.19: (a) Orbitals predicted by the LE model to describe (b) The Lewis structure for carbon dioxide
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14a–12
Figure 14.20: (a) An sp hybridized nitrogen atom
(b) The s bond in the N2 molecule (c) the two p bonds
in N2 are formed when
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14a–13
Figure 14.21: A set of dsp3 hybrid orbitals
on a phosphorous atom
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14a–14
Figure 14.22: The orbitals used to form the bonds in the PCL5 molecule
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14a–15
Figure 14.23: An octahedral set of d2sp3 orbitals on a sulfur atom