To answer the questions, interpet the Lewis structure for PCl_4^+1. For the phosphorus atom: a. The number on non bonding electronsb. The number of bonding electrons c. The total number of electrons 2. The central phosphorus atom (choose the correct option)A) obeys the octet tule B) has less than an octect C) has more than and octect

1. The Lewis structure for PCl4^+1 is as follows:

   Cl
   |
   

Cl - P - Cl | Cl

a. The number of non-bonding electrons on the phosphorus atom: Phosphorus in PCl4^+1 does not have any non-bonding electrons. All its valence electrons are involved in bonding with the chlorine atoms.

b. The number of bonding electrons: Each bond to a chlorine atom involves 2 electrons, and since there are 4 chlorine atoms, the phosphorus atom is involved in bonding with 8 electrons.

c. The total number of electrons: Phosphorus normally has 5 valence electrons, but in PCl4^+1, it has lost one electron to have a +1 charge. So, it has 4 electrons of its own involved in bonding, plus the 4 it shares with chlorine, for a total of 8 electrons.

2. The central phosphorus atom:

C) has more than an octet. The phosphorus atom in PCl4^+1 is surrounded by 8 electrons, which is more than the octet rule allows for the second period elements. However, phosphorus is in the third period of the periodic table and can expand its octet to accommodate more than 8 electrons.