Question

The complete orbital notation diagram of an atom is shown.

Answer 1

Answer:

Explanation:

From the description provided by the statement of the problem, we can easily solve for the values of the angular momentum quantum number.

Let us represent the atom as J:

In atom J, we have five sub-orbitals in which there 9 electrons. From the designation used to represent sublevels, we can write the notation as below:

             J = 10 electrons = 1s² 2s² 2p⁵

The s-sublevel can only contain 2 electrons

p-sublevel can contain 6 electrons but we have just 5 electrons in there.

Now, to find the angular momentum quantum number, we need to understand what this quantum number denotes.

This quantum number is also known as azimuthal or secondary quantum number. It gives the shape of the orbitals in subshells accomodating electrons. This quantum number is designated by (l).

         l (n-1)            name of orbital               shape of orbital

             0                     s                                   spherical

             1                     p                                    dumb-bell

             2                    d                                    double dumb-bell

             3                    f                                      complex

J  = 1s² 2s² 2p⁵

where 1 and 2 coefficients are the principal quantum numbers(n).

            s and p are the shape of the orbitals

For 1s², the l vaue is 0 because the electron is in the s orbital

     2s² the l value is 0, 1 and the electron can be in the s or p orbitals

     2p⁵ the l value is 0, 1 and the electrons can be in the s or p orbitals

The quantum number gives the shape of the orbital.