What are the factors that affect IONIC Radius?

Question

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Answer 1

Nuclear charge (actual number of protons).
Number of full levels of electrons (screening).
Number of electrons lost or gained.

Answer 2

The same trends that affect atomic Radius can be applied to ionic radius. As you go down a column in the periodic table the number of atomic orbitals increases therefore the radius increases, and as you go across a row more protons are added to the nucleus therefore the valence orbital gets pulled in closer to the nucleus. However for ions you now must also consider if they are gaining or losing electrons if the atom is losing an electron (Na-->Na+) the ion Na+ ion will have a smaller radius because of the reduced electron repulsion present. The opposite occurs if it gains an electron.

Answer 3

Ionic radius is a concept for expressing the sizes of ions in ionic crystals. The ionic radius is estimated from the distance between cations and anions that are adjacent in ion crystals. It is assumed that the internuclear distance between two ions in the ionic structure is equal to the sum of the radius of those ions, though the ionic radius is not actually constant because it depends on the ionic valency, the coordination number, and the state of spin of the ion. Assuming the radius of 140 picometers for the ion of O2−, the average value of the radius of other ions was set from the distance between ions that were measured for many oxides and from the difference from the radius of O2−. Generally, the ionic radius of the negative ion becomes large and that of the positive ion becomes small compared with the former neutral atom. Ionic radius also refers to the size of an atom after losing all valence electrons (the outer electron shell).

Answer 4

The radius is the well knpwn term used to denote the distance between centre point of a circle to the peripheri.
ATOMIC RADIUS : The atomic radius is the distance between the nucleus to the valence shell electron.
IONIC RADIUS : The distance between the nucleus and the last electron upto which it has its (nuclear attraction) impact.
FACTORS AFFECTING IONIC RADIUS :
A - TOTAL No OF PROTONS IN ITS NUCLEUS : As the no of protons increases in the nucleus the radius of the atom or ion decreases due increasing electrostatic force of attractions. So as we move from left to right in periodic table radius decreases. But as we move downwards it should also be decreases but it not the case why? Because while moving downward there is addition of one shell each time that predominates so radius increses.
B : THE NO OF SCREENED SHELLS (SCREENING EFFECT) : As in inner transition elements (f-block) there are increasing inner shells which works like a screen between nucleus and valence shell electrons. So as the screening effect increases the radius increases.
C : RATIO OF PROTONS /ELECTRONS/ : As this ratio increases (as from Cl atom (17/17 )to < Cl- ion (17/18 ) the radius increases and vice versa in Na (11/11) to > Na+ (11/10). Fe++(26/24) > Fe+++ (26/23).
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Answer 5

a million. C 2. E. The cation is smaller than the anion. All of those have Ar configuration 3. If a trend starts with and E it will strengthen going spectacular and up on the periodic table. E is the respond. 4. B.

Answer 6

1. distance between nucleus
2.atomic number.