Question

5)write the full electronic configuration of the element with atomic number 14

Explanation:

Step1: Determine the element

The atomic number is 14, so the element is silicon (Si). The maximum number of electrons an atom can have is equal to its atomic number, so we need to distribute 14 electrons into different orbitals following the Aufbau principle (filling order: 1s, 2s, 2p, 3s, 3p, etc.), Pauli exclusion principle (maximum 2 electrons per orbital with opposite spins), and Hund's rule (electrons fill degenerate orbitals singly first).

Step2: Fill 1s orbital

The 1s orbital can hold a maximum of 2 electrons. So we start with \(1s^2\).

Step3: Fill 2s orbital

Next is the 2s orbital, which also holds 2 electrons. Now we have \(1s^2 2s^2\).

Step4: Fill 2p orbital

The 2p orbital can hold a maximum of 6 electrons (since p orbitals have 3 sub - orbitals, each with 2 electrons). After filling 2s, we fill 2p: \(1s^2 2s^2 2p^6\).

Step5: Fill 3s orbital

The 3s orbital holds 2 electrons. Now our configuration is \(1s^2 2s^2 2p^6 3s^2\).

Step6: Fill 3p orbital

We have used \(2 + 2+6 + 2=12\) electrons so far. We have \(14 - 12 = 2\) more electrons to place in the 3p orbital (since after 3s comes 3p in the filling order for atomic number 14). So the 3p orbital gets 2 electrons, making the full electronic configuration \(1s^2 2s^2 2p^6 3s^2 3p^2\).

Answer:

\(1s^2 2s^2 2p^6 3s^2 3p^2\)