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| Atomic orbitals |
| Level 1 1s |
| Level 2 2s 2p |
| Level 3 3s 3p 3d |
| Level 4 4s 4p 4d 4f |
| Level 5 5s 5p 5d 5f 5g |
| Level 6 6s 6p 6d 6f 6g |
| Level 7 7s 7p 7d 7f 7g |
| Hybrid orbitals |
| 2s+2p hybrids sp sp2 sp3 |
| 3s+3p+3d hybrids dsp3 d2sp3 |
| Molecular orbitals |
| H2, dihydrogen σ* σ |
| N2, dinitrogen σp* πx* πy* σp πx πy σs* σs |
| Introduction | Wave function | Electron density | Dots! | Radial distribution | Equations |
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Atomic orbitals: 2s
The shape of the 2s orbital. The blue zone is where the wave function has negative values while the red zone is where values are positive.
For any atom there is just one 2s orbital. The image on the left is deceptively simple as the interesting feature is buried within the orbital. That on the right is sliced in half to show that there is a spherical node in the 2s orbital.
The origin of the spherical node becomes clear if we examine the wave equation, which includes a (2 - ρ) term. When (2 - ρ) = 0, then we must have a node. Since for the 2s orbital ρ = 2Zr/2 = Zr (Z = effective nuclear charge, r = radius in atomic units), then the node is at the radius for which (2 - Zr) = 0, that is, r = 2/Z atomic units.
While still spherical, the higher s-orbitals (3s, 4s, 5s, 6s, and 7s) are more complex since they have more spherical nodes.
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