Smaller
flourine has a smaller atomic radius than iodine
The empirically measured covalent radius of tin is 145 pm; for iodine this radius is 140 pm.
In terms of atomic radius yes, nitrogen is larger than fluorine. However, the common fluorine isotopes have a greater mass than those of nitrogen.
Protons have a larger mass, but it is unclear which (if either) have a larger radius. The electron does not seem to have ANY measurable radius.
Na+ is smaller than Na.
For the representative elements (main group elements), atomic radius generally decreases from left to right across a period. Example: B and Fl: Fl has the smaller atomic radius Li and Be: Be has the smaller atomic radius
Iodine has 53 electrons in its orbitals while fluorine only has nine. This does not even count the proton/neutron variance.
Fluorine because it has a smaller atomic radius.
bromine
Flourine
fluorine i just had it for hw and im not sure
No Bromine does. Bromine-195 Fluorine- 133
The empirically measured covalent radius of tin is 145 pm; for iodine this radius is 140 pm.
In non-isotop state, Fluorine will have a larger atom then Carbon.
Bromine has a SMALLER atomic radius because it has one more electron shell than Iodine. On the periodic table, atomic radius of an atom decreases across a period and increases down a group. Since Bromine and Iodine are in the same group, you know Bromine has a smaller atomic radius because it is in a lower period.
In terms of atomic radius yes, nitrogen is larger than fluorine. However, the common fluorine isotopes have a greater mass than those of nitrogen.
Because fluorine's size is lower than that of iodine, it has a greater ionization energy than iodine. Fluorine, on the other hand, appears to have a smaller shielding effect. As a result, fluorine's nucleus attracts more valence electrons than iodine's.
Protons have a larger mass, but it is unclear which (if either) have a larger radius. The electron does not seem to have ANY measurable radius.