- [Ar]4s13d10.
- [Ar]4s23d9.
- [Ar]3d104s1.
- 1s22s22p63s23p63d94s2.
Category: Chemistry
- [Ar]4s23d7.
- [Ar]3d74s2.
- [Ar]4s13d8.
- [Ar]4s23d64p1.
- [Ar]4s23d4.
- [Ar]4s13d5.
- [Ar]3d54s1.
- [Ar]4s23d34p1.
- [Ar]4s23d3.
- [Ar]3d34s2.
- [Ar]4s13d4.
- 1s22s22p63s23p63d34s2.
- Aufbau principle.
- Pauli exclusion principle.
- Hund's Rule.
- Octet rule.
- 1s22s22p63s23p2.
- [Ne]3s23p2.
- Both A and B.
- [Ar]3s23p2.
- A point.
- A line.
- A three-dimensional region.
- A two-dimensional circle.
- Nitrogen.
- Oxygen.
- Sulfur.
- Zinc.
- 1s.
- 2s.
- All s orbitals.
- All orbitals except 1s.
- 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.
- Electrons are very small.
- Electrons move at the speed of light.
- Electron properties are quantized.
- Electrons are negatively charged.
- [Ar]4s23d2.
- [Ar]3d24s2.
- [Ar]4s13d3.
- 1s22s22p63s23p63d24s2.
- 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.
