Answer to Question #209042 in General Chemistry for emmanuel kazeya

Question #209042
1.Explain the trend with reasons in the atomic radii and ionization energy of atoms
(A) As you move left to right within the same period
(B) As you move from top to the bottom within the same group
1
Expert's answer
2021-06-21T05:29:36-0400

a) As we all know, atoms prefer complete valence shells. Therefore, when we move to the right over a period of time, we increase e-. And also add protons. Because we have added protons, the size of the atom will become smaller because the nuclear charge will be stronger. Adding protons over a period of time is better than adding electrons. After all, we have a small atom with a lot of electrons in its valence shell and we don't want to let them go. Especially inert gases and halogens. Ionization energy 

 decreases as we go down because: 

 When we go down, a whole new energy level is added. More electrons means more repulsion. 

 This creates a shielding effect in which a layer is added to protect the outer electrons from the nuclear charge. However, here, adding another energy level is better than adding a proton.

b) Well, when we look at the periodic table, we know that from left to right, the size of the atom decreases in one row of the periodic table, this is the effect of increasing the atomic number 

 Z. The increased nuclear charge acts on the valence electrons and attracts them inwards, causing the atomic radius to decrease.

 On the other hand, when we descend a row, that is, a column of the periodic table, the valence electrons move to the new shell ... and the influence of nuclear charge becomes somewhat weaker, so the atomic radius increases by one group. Of course, we know that the ionization energy, that is, the energy associated with the reaction will decrease with the decrease of the group, but it will increase throughout the cycle due to the increase in nuclear charge.


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