- Electrons are too small to define.
- The probability of finding an electron never truly drops to zero.
- Orbitals are always moving.
- The nucleus interferes.
Category: Chemistry
- It decreases.
- It increases.
- It remains the same.
- It depends on the orbital type.
- A sharp boundary.
- A diffuse, spherical cloud.
- A dumbbell shape.
- A cloverleaf shape.
- It decreases.
- It increases.
- It remains the same.
- It depends on the orbital type.
- Radial node.
- Angular node.
- Planar node.
- No nodes.
- Radial node.
- Angular node.
- Spherical node.
- No nodes.
- 2s and 2p.
- 3s and 3p.
- 2px?, 2py?, 2pz?.
- 1s and 2s.
- Orbitals with different shapes.
- Orbitals with the same energy.
- Orbitals with different principal quantum numbers.
- Orbitals with no electrons.
- [Ar]4s23d9.
- [Ar]4s13d10.
- [Ar]4s03d11.
- [Ar]3d104p1.
- To achieve a completely empty s orbital.
- To achieve a completely filled d subshell, which offers extra stability.
- To achieve a half-filled d subshell.
- To balance spins.
- To achieve a completely full s orbital.
- To achieve a half-filled d subshell, which offers extra stability.
- To minimize electron-electron repulsion.
- It is a random phenomenon.
- [Ar]4s23d4.
- [Ar]4s13d5.
- [Ar]4s03d6.
- [Ar]4s23d44p1.
- 1s < 2s < 2p < 3s < 3p < 4s < 3d.
- 1s < 2s = 2p < 3s = 3p = 3d.
- 1s = 2s = 2p.
- 1s < 3d < 4s.
- [Ar]4s23d1.
- [Ar]3d14s2.
- [Ar]4s13d2.
- [Kr]4s23d1.
- 1s < 2s < 2p < 3s < 3p < 3d.
- 1s < 2s = 2p < 3s = 3p = 3d.
- 1s < 2p < 2s.
- 1s = 2s = 2p.
