Since the given succesive ionisation energy values are 738, 1451, 7753,10540,13630,17630,17995 and 21703
from the above value there is a sudden increase from second ionisation energy to third ionisation energy i.e., from 1451 to 7753 value
hence after removing two electrons from the valence shell of the element it will get stabl configuration so the valence shell.
so the element may be Mg : 1s2 2s2 2p6 3s2
so after removing 2 electrons from Mg it will get stable configuration as 1s2 2s2 2p6 3s0
hence the electron removed from this stable configuration requires more amount of energy hence the ionisation energy became very large value.
Part A What is the third-row element having the successive ionization energies in kJ/mol: 738, 1451,...
82. A period three element has 738, 1451, and 7733 kJ/mol as its first three ionization energies. What is the symbol of this element?
Which period 3 element has the following ionization energies (kJ/mol)? IE1 = 738 IE2 = 1451 IE3= 7733 Group of answer choices Mg S P Al Si
The figure represents the successive ionization energies of an atom in the third period of the periodic table. - Part A 16,000 14,000 Which atom is this most likely to be? Express your answer as a chemical symbol. 12,000 Energy (kJ/mol = ADP * o a ? Al 6000 4000 Submit Previous Answers Request Answer 2000 X Incorrect; Try Again; 5 attempts remaining E1 E2 E3 E4 E,
The figure represents the successive ionization energies of an atom in the third period of the periodic table. Part A 16,000 14,000 Which atom is this most likely to be? Express your answer as a chemical symbol. 12,000 ΑΣΦ ? 10,000 Energy (kJ/mol 8000 Si 6000 Submit Previous Answers Request Answer 4000 2000 X Incorrect; Try Again; 3 attempts remaining 0 E1 E2 E E4 Es
10.) Below is a list of successive ionization energies (in kJ/mol) for a period 3 element. Identify the element and explain how you came to that conclusion. IE2 = 2250 IE3 - 3360 TE 4 = 4560 IE5 = 7010 IE6 - 8500 IE 7 = 27,100
15. Below is a list of successive ionization energies (in kJ/mol) for a period 3 element, X. What is the most likely formula for a stable ion of X? 151 = 1000 IE2 = 2250 IE3 = 3360 IE4= 4560 E5= 7010 TE6= 8500 IE2 = 27.100 d. X a. X2 b. X30 c. X²
Identify the element of Period 2 (name) which has the following successive ionization energies, in kJ/mol. IE1 = 1314 IE2 = 3388 1E3 = 5301 JE4 = 7469 IE5 = 10989 IE6 = 13327 1E7 = 71330 IE8 = 84078 Answer:
a new element X is discovered that has the following successive ionization energies (kj/mol) IE1=1004 , IE2=1251 IE3=5988 , IE4=6220 , IE5=6803 , IE6=7178 a. what group (column) do you expect this element will belong? explain b. if this element X combined with fluorine , what is the likely molecular formula?( for example XF2, X2F3, etc)
This figure represents the successive ionization energy of an atom in the third period of the periodic table. Part A 12,000 10,000 Which atom is this most likely to be? Express your answer as a chemical symbol. 8000 Energy (kJ/mol) = AEON 2 ? 100 Mg 2000 Submit Previous Answers Request Answer Ei E:2 E 3 E A X Incorrect; Try Again; 5 attempts remaining
Identify the group number of the element that has the following successive ionization energies (in kJ/mol). IE1 = 1,060 IE5 = 6,270 1E4 = 4,950 IE2 = 1,890 IE6 = 21,200 E3 = 2,905 IE7 = 25,400 Group 5A O Group 7A Group 4A Group 3A O Group 6A