The space that constitutes 99% of the area of an atom is primarily occupied by its electron cloud or electron cloud distribution. The electron cloud refers to the region around the nucleus of an atom where the electrons are most likely to be found.
In atomic structure, electrons are negatively charged particles that orbit the positively charged nucleus. However, the exact position and velocity of an electron cannot be determined with precision due to the inherent wave-like behavior of subatomic particles. Instead, scientists describe the probability of finding an electron in a given region around the nucleus using electron orbitals or electron probability clouds.
Electron orbitals are three-dimensional regions where electrons are most likely to exist. The most commonly known orbitals are the s, p, d, and f orbitals, each with a specific shape and energy level. The s orbital is spherical and closer to the nucleus, while the p orbitals have dumbbell shapes and are found further from the nucleus.
The reason why the electron cloud constitutes most of the atom's volume is due to the wave nature of electrons and the uncertainty principle in quantum mechanics. According to the Heisenberg uncertainty principle, it is impossible to simultaneously determine both the position and momentum of a particle with perfect accuracy. As a result, electrons do not follow well-defined paths like planets around the sun, but instead exist in a diffuse cloud of probability.
The electron cloud distribution can be visualized as a region where the probability of finding an electron is high, with higher probabilities near the nucleus and decreasing as you move further away. While the electron cloud is mostly empty space, it is essential in determining an atom's chemical and physical properties as it influences bonding, reactivity, and the interaction of atoms with electromagnetic radiation.