Which of the following concerning second ionization energies is true?

a. that of al is lower than that of mg because mg wants to lose the second electron, thus the energy change is greater.
b. that of al is higher than that of mg because the electrons are taken from the same energy level, but the al atom has one more proton.
c. that of al is lower than that of mg because the second electron taken from al is in a p orbital, thus it is easier to take.
d. that of al is higher than that of mg because mg wants to lose the second electron, so it is easier to take the second electron away.
e. the second ionization energies are equal for al and mg.

D

Explanation:

The fact is that the both elements belong to different groups in the periodic table. Mg is in group 12 while Al is in group 13. The outer most electron configuration for Mg2+=[Ne]3s0

Al+= [Ne]3s13p0

It is evident that in Al+, the second electron is to be removed from a filled 3s subshell which is energetically unfavourable. Unlike In Mg2+ where the two electrons are removed. There is always a tendency towards a quick loss of all the valence electrons in the valence shell. It will be more difficult to remove an electron from a filled shell.

Answer

the unit cost of each product is

Explanation:

                          Moulding   Grinding   FinishingDirect Material           143,700               14,400              9,500Direct Labour              13,900                33,300             23,100Applied Overhead      18,300               136,400            18,500                                   Total cost                     175,900           184,100               51,100Transferred in cost                              175,900              Total Manufacturing    Cost                           175,900         360,000                411,100                                      unit cost = 51100 ÷ 9200 = 5.55