Stuck on a chem problem.. please help

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1

<p>Sorry to bother y'all.. but does anyone know how to do this problem ??</p>

<p>The ionization energies for an element Z are as follows:
IE 1 = 600 kj/mol
IE 2 = 1650 kj/mol
IE 3 = 3330 kj/mol
IE 4 = 15230 kj/mol
IE 5 = 17300 kj/mol</p>

<p>To which group does the element belong? Explain
Give the electron dot symbol for the element
What is the trend for each successive ionization energy,why?
How many kJ of energy would be required to convert 1.55 moles of element Z completely to ions of a +3 charge?
Given the first ionization energy above, calculate the minimum wavelength of light that would be needed to remove an electron from an atom of Z.</p>

<p>Thank you!!!!</p>

2

<p>third because there is such a great increase in IE between IE 3 and IE 4</p>

<p>well this you need to check at your data table to find which element it is....</p>

<p>well, keep increasing and great increase when there is electron removal from more inner shells </p>

<p>IE 1 + IE 2 + IE 3 = 5580kj/mol which is the amount of E needed to remove three electrons per mol. Then 5580 * 1.55 you get the answer</p>

<p>IE 1 is 600kj/mol so every atom needs 600kj/ (6.23 * 10 to the 23rd power) energy... Calculate the amount of E needed per atom and then use the formula E = hf to answer the question</p>

3

<p>Thanks!!!!</p>