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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: 7s equations
The symbols used in the following are:
- r = radius expressed in atomic units (1 Bohr radius = 52.9 pm)
- π = 3.14159 approximately
- e = 2.71828 approximately
- Z = effective nuclear charge for that orbital in that atom.
- ρ = 2Zr/n where n is the principal quantum number (7 for the 7s orbital)
- k = a constant (value to follow)
| Function | Equation |
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| Radial wave function, R7s | = (1/k) × (5040 - 15120ρ + 12600ρ2 - 4200ρ3 + 630ρ4 - 42ρ5 + ρ6) × Z3/2 × e-ρ/2 |
| Angular wave function, Y7s | = 1 × (1/4π)1/2 |
| Wave function, ψ7s | = R7s × Y7s |
| Electron density | = ψ7s2 |
| Radial distribution function | = 4πr2ψ7s2 |
| Copyright | Feedback | The images | Acknowledgments | Problems? | References | |
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