Respuesta :
This is an incomplete question, here is a complete question.
A (+3) cation of a certain transition metal has three electrons in its outermost d-subshell. Which transition metal could this be?
Answer : The transition metal could be, chromium, molybdenum and tungsten.
Explanation :
Transition elements : They are the elements which lie between 's' and 'p' block elements. These are the elements which lie in group 3 to 12. The valence electrons of these elements enter d-orbital.
Their general electronic configuration is: [tex](n-1)d^{1-10}ns^{0-2}[/tex] where 'n' is the outermost shell.
As we are given that a (+3) cation of a certain transition metal has three electrons in its outermost d-subshell.
The general electronic configuration of group 6 transition elements is: [tex](n-1)d^5ns^1[/tex] where 'n' is the outermost shell (n = 4 to 6)
The group 6 elements are, chromium, molybdenum and tungsten.
The group 6 elements show variable oxidation states and the most stable oxidation state of group 6 is, (+3) an (+6).
The group 6 elements have tendency to lose 3 electrons.
When group 6 elements lose 3 electrons then their oxidation state will be, (+3).
Thus, the transition metal could be, chromium, molybdenum and tungsten.
