To determine the correct electron configuration for nickel (Ni), we need to look at its position in the periodic table. Nickel (Ni) has an atomic number of 28, which means it has 28 electrons. These electrons are arranged in various atomic orbitals according to increasing energy levels.
Let’s step through each option and see which one correctly represents the electron configuration for nickel:
- Option A: [tex]\(1s^2 2s^2 2p^6 3s^2 3p^6 4d^8\)[/tex]
- This configuration shows electrons in the 4-d orbital before all available 3-d orbitals are filled. This is not the correct filling order according to the Aufbau principle.
- Option B: [tex]\(1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10}\)[/tex]
- This configuration suggests that all available 3-d orbitals are filled before moving to higher energy levels. However, for nickel, the valence electrons are in the 3-d orbital and only 8-electrons fill it, not 10.
- Option C: [tex]\(1s^2 2s^2 2p^6 3s^2 3p^6 3d^8\)[/tex]
- This option distributes the 28 electrons properly according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle: 2 electrons in each of the [tex]\(1s\)[/tex], [tex]\(2s\)[/tex], [tex]\(2p\)[/tex], [tex]\(3s\)[/tex], and [tex]\(3p\)[/tex] orbitals, and 8 electrons in the [tex]\(3d\)[/tex] orbital. This corresponds to the correct electron configuration for nickel (Ni).
- Option D: [tex]\(1s^2 2s^2 2p^6 3s^2 3p^6 4d^6 4d^2\)[/tex]
- This configuration indicates an incorrect filling sequence where electrons are incorrectly distributed across orbitals and shells. It does not follow the proper order of orbital filling.
Given these observations, the correct electron configuration for nickel (Ni) is shown in option C: [tex]\(1s^2 2s^2 2p^6 3s^2 3p^6 3d^8\)[/tex]. Therefore, the correct answer is option C.
