electronic configuration

To write the electronic configuration, we need to know which element you're referring to. Please specify the element. However, I can provide an example for Calcium (Ca) to illustrate the process, as it demonstrates the filling of the 4s orbital before the 3d orbital, a key concept in Advanced Level chemistry. Step 1: Determine the number of electrons for Calcium (Ca). Calcium (Ca) has an atomic number (Z) of 20. This means a neutral calcium atom has 20 electrons. Step 2: Fill the orbitals in increasing order of energy. • The 1s orbital holds 2 electrons: 1s^2 (Remaining: 20 - 2 = 18) • The 2s orbital holds 2 electrons: 2s^2 (Remaining: 18 - 2 = 16) • The 2p orbital holds 6 electrons: 2p^6 (Remaining: 16 - 6 = 10) • The 3s orbital holds 2 electrons: 3s^2 (Remaining: 10 - 2 = 8) • The 3p orbital holds 6 electrons: 3p^6 (Remaining: 8 - 6 = 2) • The 4s orbital holds 2 electrons (before 3d): 4s^2 (Remaining: 2 - 2 = 0) Step 3: Write the full spectroscopic notation. Combining the filled orbitals: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 Step 4: Write the noble gas shorthand notation. The noble gas preceding Calcium is Argon (Ar), which has an electronic configuration of 1s^2 2s^2 2p^6 3s^2 3p^6. We can replace this core configuration with [Ar]. [Ar] 4s^2 The electronic configuration of Calcium is: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 or [Ar] 4s^2 3 done, 2 left today. You're making progress.