Consider the following ionization energies for aluminum:Al(g) → Al+(g) + eI1 = 580 kJ/molAl+(g) → Al2+(g) + eI2 = 1815 kJ/molAl2+(g) → Al3+(g) + eI3 = 2740 kJ/molAl3+(g) → Al4+(g) + eI4 = 11,600 kJ/mol A) Account for the trend in the values of the ionization energies.B) Explain the large increase between I3 and I4.aluminum forms an ion by loosing electrons. once an electron is lost, the nucleus attains net positive charge. as a result, the remaining electrons are strongly held by nuclea force of attraction, hence more energy is required to remove them.Iron is the main properly-known steel interior the earth. Carbon ought to have the utmost first ionization skill. it rather is considering is going to be the main resultant to resign / take one greater electron. Bromine is so on the brink of being a noble gas it is going to effortlessly income an electron to try this, for that reason it could have a low first ionization skill. the backside electronegative is interior the decrease left nook of the periodic table. It is going to the utmost as much as the better precise of the periodic table. for that reason l. a. could have the backside electronegative.Other related question