Question

How many quantum numbers are needed to define the probability of finding the electron in a given region of space in the hydrogen atom?

Answer 1

Hint: We are already provided with the element. This question could be simply solved from atomic orbital concepts. It is a part of inorganic chemistry. An electron can be defined using the different quantum numbers.

Complete step by step answer
The probability density of an electron in an atomic orbital is defined as the statistical distribution of where an electron often appears in that orbital.
Each electron in an atom is described by four different quantum numbers. The first three $ \left( n,l,{{m}_{l}} \right) $ specify the particular orbital of interest, and the fourth $ {{m}_{s}} $ specifies how many electrons can occupy that orbital.
Thus, we too require four quantum numbers to define the probability of finding the electron in a given region of space in the hydrogen atom.

Additional Note
The number of protons, neutrons, and electrons in an atom can be determined from a set of simple rules. The number of protons in the nucleus of the atom is equal to the atomic number. The number of electrons in a neutral atom is equal to the number of protons. The radial component contains the quantum numbers n (quantum level, such as n=3 for the 3s atomic orbital, etc) and l (the angular momentum, which for instance is l=2 for a d orbital). Orbitals are commonly represented by the boundary surfaces that encloses the region where there is a $ 90-95% $ probability of finding the electron.
Also, a node is a place where there is zero probability of finding an electron. A radial node has a spherical surface with zero probability.

Note
The common mistake that can be done here is that an orbital is a three- dimensional description of the most likely location of an electron around an atom. Below is a diagram that shows the probability of finding an electron around the nucleus of a hydrogen atom. Notice that the 1s orbital has the highest probability.