What is the period 6 element that forms a 4+ ion with a pseudo-noble gas configuration?
How can I find the solution?
Thanks
I'm not sure what you mean by pseudo noble gas configuration. In group VI, the elements that come to mind for +4 ion are Pb and Ce.
To find the element that meets the given criteria, we need to understand the structure of the periodic table and the concept of pseudo-noble gas configuration.
The periodic table is organized based on atomic number, which represents the number of protons in an atom. Periods in the periodic table represent the energy levels (shells) in which the electrons reside. In this case, we are interested in period 6.
The elements in period 6 have atomic numbers ranging from 57 to 71 for the lanthanides and from 89 to 103 for the actinides. However, since we are looking for an element with a 4+ ion, we can omit the lanthanides and actinides because they typically form 3+ ions.
Now, let's discuss the concept of pseudo-noble gas configuration. Noble gases are known for their stable electron configurations, meaning their outermost energy levels are completely filled with electrons. Other elements tend to gain or lose electrons to achieve a noble gas configuration.
In this case, the element we are looking for has 4+ charge, indicating that it has lost four electrons. To achieve a pseudo-noble gas configuration, it must have a completely filled outermost energy level after losing these electrons. In period 6, this corresponds to the 5s and 4d orbitals.
So, to find the solution, we need to identify the element in period 6 that has a 5s and 4d orbital and can form a 4+ ion.
Looking at the periodic table, we find that the element in period 6 with a 5s and 4d orbital is Tungsten (W). Tungsten has an atomic number of 74. To form a 4+ ion, it will lose all four of its 5s and 4d electrons, resulting in a pseudo-noble gas configuration.
Therefore, the element that meets the given criteria is Tungsten (W).