Atomic Radius

In recent times, atomic radius has become increasingly relevant in various contexts. I'm curious about how why the bigger the nucleus, smaller the atomic .... I think you're confusing a few periodic trends. Atomic radius generally decreases across a row because the effective nuclear charge increases while the maximum distance of the outer electrons remains the same.

In this context, therefore the valence electrons "feel" the nucleus more strongly and are pulled slightly inwards. It's important to note that, why does Magnesium have a smaller atomic radius than Lithium ... Magnesium has 3 shells while Lithium has 2 shells. Moreover, so, the atomic radius of Magnesium should be greater than Lithium. But from online sources, I found that Lithium has a greater atomic radius.

Can someone explain why this happens? Atomic radius vs Ionic radius confusion : r/Mcat - Reddit. Atomic radius: Moving across a period increases the effective nuclear charge, as the addition of a proton outweighs the addition of an electron (which normally increases electrostatic repulsion, thus decreasing effective nuclear charge). Thus, effective nuclear charge increases, pulling electrons in more strongly and decreasing the atomic radius. Why is the atomic radius of Gallium smaller than Aluminum?

My textbook explains that it is because gallium has 10 3d-electrons and since d orbital has poor shielding effect -> effective nuclear charge increases and hence the size of the atom decreases. [Highschool Chemistry] How does Au have a larger atomic radius ... Comparing should be done as follows (At least in Highschool chemistry): A) check the number of electron layers (shells) around the atom, if one has more shells than the other, it's certainly larger in radius B) if step A returns the same value, the element further to the left has a bigger radius Now for Fe VS Au: Simply but thoroughly explain relationship between atomic radius and .... I understand the basic concept for both of these periodic trends, but I have a hard time understanding why an atom of the last element on a certain row has so much smaller of a radius than an atom of the first element on the next row.

Atomic radius of noble gases : r/askscience - Reddit. Atomic radius of noble gases So I've seen a lot of conflicting information on this. Equally important, there is a trend on the periodic table that atomic radius decreases from left to right. However, there seems to be a lack of consensus in the area of noble gas radii.

Are all atoms the same size? : r/chemistry - Reddit. In relation to this, typically, because of the difficulty to isolate atoms in order to measure their radii separately, atomic radius is measured in a chemically bonded state; however theoretical calculations are simpler when considering atoms in isolation. Moreover, the dependencies on environment, probe, and state lead to a multiplicity of definitions. [High School Chemistry] How can Colomb's law for calculating ...

How is this not circular logic? Similarly, you have no idea what "d^2" is, the value of d^2 is the question, and it's inconstant across atoms. Which has the smallest radius: Ar, Cl^- or K^+?