Question

section 2 - orbital diagrams
(2 points each) draw an orbital diagram for the following elements:

1. silicon (si)
2. iron (fe)

Explanation:

Step1: Determine electron - configuration of Silicon

Silicon (Si) has an atomic number of 14. Its electron - configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{2}$.

Step2: Draw orbital diagram for Silicon

For the 1s orbital, it has 2 electrons with opposite spins (represented by up - and down - arrows). The 2s orbital also has 2 electrons with opposite spins. The 2p sub - shell has 3 orbitals, and it is filled with 6 electrons (2 in each orbital with opposite spins). The 3s orbital has 2 electrons with opposite spins. In the 3p sub - shell (3 orbitals), 2 electrons are placed with parallel spins (following Hund's rule) in separate orbitals.

For Iron (Fe):

Step1: Determine electron - configuration of Iron

Iron (Fe) has an atomic number of 26. Its electron - configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{6}$.

Step2: Draw orbital diagram for Iron

The 1s, 2s, 2p, 3s, and 3p orbitals are filled as in the case of lower - atomic - number elements. The 4s orbital has 2 electrons with opposite spins. The 3d sub - shell has 5 orbitals. According to Hund's rule, the first 5 electrons are placed with parallel spins in separate orbitals, and the 6th electron is placed in one of the 3d orbitals with an opposite spin to one of the previously filled 3d electrons.

Answer:

Orbital diagrams are drawn as described above for Silicon and Iron following the rules of electron - filling (Aufbau principle, Pauli exclusion principle, and Hund's rule).