How can RnCl4 have no lone pairs. I did the calculation there’s a total of 36 electrons when everything is filled it only has 32 electrons I am missing 4 electrons
The molecular formula of RnCl4 suggests that the central atom (Rn) is bonded to four chlorine atoms (Cl). In order to determine the electronic structure of RnCl4, we need to consider the number of valence electrons of each atom.
Rn (radon) is a noble gas located in Group 18 of the periodic table, meaning it has a full valence shell of electrons. Therefore, Rn has 8 valence electrons.
Each chlorine atom (Cl) has 7 valence electrons.
Total valence electrons in RnCl4 = 8 (Rn) + 4(7) (4 Cl) = 36
From this calculation, you are correct that there are 36 valence electrons present in RnCl4.
In the case of RnCl4, the central Rn atom forms covalent bonds with four Cl atoms, resulting in the full utilization of all 36 valence electrons. This means that all the valence electrons are involved in bonding, and there are no lone pairs present on the central Rn atom. Thus, RnCl4 can have no lone pairs.