The successive ionization energies for an unknown element are
IE1 = 896 kJ/mol IE2 =1752 kJ/mol IE3 =14,807 kJ/mol IE4 =17,948
kJ/mol To which family in the periodic table does the unknown
element most likely belong?
A period 3 element has the following successive ionization
energies IE1=1012 IE2=1900 IE3=2910 IE4=4960 IE5=6270 IE6=22200
Identify the elements based on these energies
Identify the element of Period 2 that has the following
successive ionization energies, in kJ/mol.
IE1 = 1314 IE2 = 3389 IE3 =
5298 IE4 = 7471 IE5 = 10992 IE6 =
13329 IE7 = 71345 IE8 =
84087
Li
Ne
B
O
A certain main-group element exhibits the following successive
ionization energies in kJ/mol: IE1 = 100; IE2 = 300; IE3 = 700; IE4
= 3100; IE5 = 4200 Select the false statement about this element
below. 1) This element likely ionizes to form a cation when
participating in ionic compound formation. 2)The highest-energy
electron in an atom of this element resides in a p orbital. 3)This
element has four valence electrons. 4)This element is likely a
metallic element.
An element of the third period has the following ionization
energies in KJ/mol: IE1 = 1012, IE2 = 1903, IE3 = 2910, IE4 = 4956,
IE5 = 6278 and IE6 = 22,230. USing only this data determine which
one is the element.
The successive ionization energies of a certain element are:
I1 = 899 kJ/mol, I2 =1,757 kJ/mol, I3= 14,850 kJ/mol, I4 =
21,005 kJ/mol,
This pattern of ionization energies suggests that the unknown
element is:
An element has the following first through fourth ionization
energies (in kJ/mol): 700; 1500; 7700; 10500. Deduce to which
column of the periodic table it porbably belongs. Give your
reasoning