- 1s.
- 2s.
- All s orbitals.
- All orbitals except 1s.
No category found.
- Nitrogen.
- Oxygen.
- Sulfur.
- Zinc.
- To show the exact position of electrons.
- To represent the electron configuration including electron spins in orbitals.
- To calculate atomic mass.
- To determine the number of protons.
- The highest energy electron configuration.
- The lowest energy electron configuration.
- An ionized electron configuration.
- A configuration with all unpaired electrons.
- [Ar]4s23d2.
- [Ar]3d24s2.
- [Ar]4s13d3.
- 1s22s22p63s23p63d24s2.
- Electrons are very small.
- Electrons move at the speed of light.
- Electron properties are quantized.
- Electrons are negatively charged.
- They represent fixed paths of electrons.
- They are precisely defined regions of space.
- They describe the probability of finding an electron.
- They are visible under a microscope.
- [Ar]4s1.
- 1s22s22p63s23p63d1.
- [Ne]4s1.
- 1s22s22p63s23p64p1.
- The Bohr model.
- The wave nature of electrons.
- The particle nature of electrons.
- Classical mechanics.
- 1s22s22p4.
- 1s22s22p6.
- [Ne].
- Both B and C.
- Some orbitals have more lobes.
- Electrons get closer to the nucleus.
- All orbitals have the same energy in hydrogen.
- Electrons repel each other.
- 1s22s22p63s23p4.
- [Ne]3s23p4.
- Both A and B.
- [Ar]3s23p4.
- Hund's Rule.
- Pauli Exclusion Principle.
- Aufbau Principle.
- Heisenberg Uncertainty Principle.
- [Ar]4s2.
- [Ar]3d2.
- 1s22s22p63s23p63d2.
- [Kr]4s2.
