CMATT said:Homework Statement
Choose the element in each of the sets you would expect to have the highest IE2.
a. K
b. Be
c. Mg
d. Ca
e. Al
Homework Equations
The correct answer is K
The Attempt at a Solution
I do not understand why it is K ...I kind of guessed by using my Ionization Energy diagram that shows the trend on the periodic table as:
--------> IE increases across a period/row
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IE decreases down a group
Can someone please explain why K is correct?
IE2 stands for second ionization energy. It is the energy required to remove the second electron from an atom or ion.
IE2 is important because it helps determine the stability and reactivity of an element. Elements with high IE2 values are less likely to form ions, making them more stable. This also means they are less reactive and less likely to form compounds with other elements.
The main factor that affects IE2 is the number of protons in the nucleus of the atom. The more protons an atom has, the stronger its attraction for electrons and the higher its IE2 value. Other factors that can affect IE2 include the size of the atom and the electron configuration.
Elements with a high number of protons, such as those in the halogen group (Fluorine, Chlorine, Bromine, Iodine, and Astatine), are expected to have the highest IE2 values. This is because these elements have a strong attraction for electrons due to their high nuclear charge.
IE2 is typically higher than IE1 because it is more difficult to remove a second electron from an atom that has already lost one. This is because the remaining electrons are held more tightly by the positively charged nucleus. However, there are some exceptions where IE1 and IE2 are similar, such as in the case of elements in the alkali metal group (Lithium, Sodium, Potassium, Rubidium, and Cesium).