No, it is not possible for a hydrogen atom to have all the possible orbitals filled.
In the context of the hydrogen atom, the term "orbital" refers to a specific energy state that an electron can occupy. Each orbital can accommodate a maximum of two electrons, according to the Pauli exclusion principle, which states that no two electrons in an atom can have the same set of quantum numbers.
The hydrogen atom has only one electron. Therefore, it can occupy the lowest energy level, known as the 1s orbital. This 1s orbital can hold a maximum of two electrons with opposite spins.
The energy levels of the hydrogen atom are described by the principal quantum number (n). The 1s orbital corresponds to n=1, and as the value of n increases, higher energy orbitals become available. For example, the n=2 level has additional orbitals like 2s and 2p, each capable of holding two electrons.
As you move to higher energy levels, such as n=3, 4, and so on, more orbitals become available, and the number of possible electron configurations increases. However, at any given energy level, each orbital can only accommodate a maximum of two electrons.
Therefore, in a hydrogen atom, it is not possible to fill all the possible orbitals because there are an infinite number of energy levels with an infinite number of orbitals available. With only one electron, the hydrogen atom can occupy the lowest energy orbital, the 1s orbital, leaving the other higher energy orbitals unoccupied.