An element with the electron configuration [xe] 6s24f145d7 would belong to which class on the periodic table?

If the atom is neutral then, the total number of electrons is the same as the number of protons. We calculate for the total number of electrons given the compressed electron configuration,
   number of electrons of Xenon (Xe) = 54
The total number of electrons after Xenon,
   = 2 + 14 + 7 = 23

Adding up all the number of electrons, we have,
   total number of electrons = 54 + 23 = 77

The identity of this element is Iridium (Ir). This element belongs to the class of Group 9. This is the transition metal. 

Aconductor easily transfer heat