Atomic radii of elements decrease across a period in a periodic table when read left to right. This is because of increasing electronegativity. The higher the electronegativity of an element, the stronger the nuclear charge. Stronger the nuclear c... read more
By one accounting, they have the same atomic radius. That's because the energy levels get really close together the farther they get from the nucleus and the nuclear charge increases by +32. The bottom line is that it is very likely that if we could measure the atomic radius of Francium we would find that it is essentially the same as that of cesium. read more
Not correct; the covalent radius of francium is 260 pm and the covalent radius of caesium is 244 pm. read more
Trends in atomic radius in Periods 2 and 3. Trends in atomic radius down a group. It is fairly obvious that the atoms get bigger as you go down groups. The reason is equally obvious - you are adding extra layers of electrons. Trends in atomic radius across periods. You have to ignore the noble gas at the end of each period. read more