A ground state atom of As could not have any electrons with which of the following configurations? A) n = 3, ℓ = 1, mℓ = 0, ms = +½ B) n = 4, ℓ = 2, mℓ = 0, ms = +½ C) n = 4, ℓ = 0, mℓ = 0, ms = +½ D) n = 3, ℓ = 2, mℓ = 0, ms = +½ E) n = 4, ℓ = 1, mℓ = 0, ms = +½

A ground state atom of As could not have any electrons with n = 4, ℓ = 2, mℓ = 0, ms = +½ .

The given atom:

The electronic configuration of Arsenic is written as follows;

The group of the given element can be obtained from the electronic configuration as shown below;

From the given options, the ground state atom of Arsenic cannot have electron in the following orbital;

Note:

Thus, we can conclude that a ground state atom of As could not have any electrons with n = 4, ℓ = 2, mℓ = 0, ms = +½ .

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n=4, l= 2, ml=0, ms=+1/2

Explanation:

Arsenic (As) is a group 15 element with ground state electronic configuration; 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3. Note that the outer orbitals are 4s2 4p3(corresponding to ns2np3 for group 15 elements).

We can see that the ground state electronic configuration of arsenic does not contain a 4d orbital from the electronic configuration shown above. However, the option chosen as the answer, portrays an electron in a 4d orbital (n=4, l=2). This implies that the electron cannot be seen in the ground state electronic configuration of arsenic, hence the answer.

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons

the answer is b & c i believe : )