Consider element \(113 .\) What is the expected electron configuration for element 113 ? What oxidation states would be exhibited by element 113 in its compounds?

The Aufbau Principle states that electrons in an atom fill the orbitals in order of increasing energy. To find the order in which to fill the orbitals, we can use the diagonal rule. The order is: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

Now we will fill the orbitals with electrons for element 113. As there are 113 electrons, we start filling the orbitals based on the Aufbau Principle. The electron configuration is formed as follows (we stop once we've placed all 113 electrons): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s² 5f¹⁴ 6d^9

From the electron configuration, we can identify the valence electrons. Valence electrons are the electrons in the outermost energy level and are involved in chemical bonding. In this case, valence electrons are found in the outermost energy levels: 7s² 5f¹⁴ 6d^9

Oxidation states for an element are determined by the number of valence electrons it has, which are involved in forming chemical bonds and can be gained, lost, or shared. In element 113, the valence electrons are 7s², 5f¹⁴, and 6d^9. The 7s² orbitals can lose two electrons, the 5f¹⁴ orbitals can lose up to fourteen electrons, and the 6d^9 orbitals can lose up to nine electrons. This gives us the possible oxidation states: +2, +3, +4, +5, +6, +7, +8, +9, +10, +11, +12, +13, +14, +15, and +16. However, it should be noted that oxidation states higher than +8 are extremely rare and usually not observed. So the most likely oxidation states for element 113 could be from +2 up to +8, depending on the specific chemical environment and the elements it forms compounds with.