Question

Atomic Number, Ionic Radius, and First Ionization Energy help!

Answer 1

I'm working on a chemistry assignment right now and I'm stuck on the last two questions.
Here are the ones I've answered so the last two will make sense.
(Q1: What is the relationship between the atomic numbers and ionic radii of the element in the group?
A1: The relationship between the atomic numbers and ionic radii of the elements is that the line has an upwards trend. That means, the higher the atomic number is, the higher the ionic radii becomes. )
(Q2: What is the relationship between atomic numbers and first ionization energies?
A2: Unlike the first graph, the relationship between the atomic numbers and the energies is that they have a downwards trend instead. So that means the higher the atomic number, the lower the first ionization energy is.)

Answer 2

The questions I'm stuck on are "Why do these relationships exist? Propose an explanation for each of these relationships." and "Are these relationships consistent with the periodic trends that you have been studying?"

Answer 3

The question why do these relationships exist, doesn't just mean well okay if this thing goes up then that thing goes down, the question is how do we explain these trends?

Answer 4

I don't know how to explain the trends though. That's the problem

Answer 5

Why do these relationships exist?:

The higher the atomic number of an element means the atomic radii will be bigger because there are more electrons and shells/orbitals involved which will make the element bigger in size. The more electrons there are means the more shells there are which equals to a bigger atomic radii.

The first energisation energy will be lower the bigger the atomic number because a larger atomic number means more electrons. This means more shells and the electrons will be further away from the nucleus which equals to less nuclear attraction. This means as the electrons get further away from the nucleus (from the larger amount of electrons and more shells and shielding from the shells closer to the nucleus) there will be less attraction holding the electrons to the nucleus which will make it easier to remove.

I'm not sure what the next question means, but I hope this helps explain why the relationships exist :)

Answer 6

@jebonna you're a lifesaver thank you so much. I think I can figure out the second one!

Answer 7

Haha no problem! Glad I could help :)