The wave function of an atom cannot be obtained simply by considering the wave functions of all its subatomic particles. While the wave function of an atom can be expressed as a mathematical combination of the wave functions of its constituent particles, such as electrons and the atomic nucleus, there are additional factors that need to be considered.
In quantum mechanics, the behavior of particles is described by wave functions, which are mathematical functions that encode information about the particle's properties. For multi-particle systems like atoms, the wave function is described by the Schrödinger equation, which takes into account the interactions between the particles.
The wave function of an atom includes contributions from the individual wave functions of the electrons and the nucleus, but it also incorporates the effects of their interactions, such as the electrostatic attraction between the electrons and the nucleus. These interactions are crucial for understanding the behavior of atoms and the formation of chemical bonds.
Moreover, the wave function of an atom also depends on the specific arrangement of its electrons in different energy levels or orbitals. This arrangement is determined by the quantum numbers and the Pauli exclusion principle, which restricts the number of electrons that can occupy a given quantum state.
In summary, while the wave function of an atom does involve considering the wave functions of its subatomic particles, it also incorporates the interactions between these particles and takes into account the specific arrangement of electrons within the atom. These additional factors are essential for accurately describing the behavior of atoms in quantum mechanics.