Based on Heisenberg's uncertainty principle, there is no way possible to have a quantum number for position since the electron's second quantum number already gives you an exact value for its angular momentum.
Bohr calculated the most probable radius of the electron cloud (which he mistakenly thought was an actual distance) getting the number 5.29X10-11 m.
What I think the asker is speaking of is the quantum number that refers to energy level, n. Though not a physical distance it may be interpreted, using the Bohr model, how "far" away an electron is from the ground state, which some would believe (incorrectly) that this is a function of distance from the nucleus.
The principal quantum number represents the distance between an electron shell and the nucleus. The principal quantum number is represented as n.
The atomic radius is the distance from the nucleus of an atom to the outermost orbital of electron.
Bromine has less valence shells than lead making the distance between its valence electron and its nucleus less than that of lead. This means that there is greater attraction between the nucleus and electron for bromine and it requires a higher ionisation energy to remove its electron.
Direction with respect to the nucleus
It's because as atomic radius increases, so do the number of electron shells. The full electron shells closer to the nucleus act like a barrier or shield that reduces the pulling force exerted by the Nucleus on the outer electron. Since the nucleus's pulling force is reduced, an electron on the outer shell can escape much more easily.
The atomic radii is an estimation of the radius of an atom. The value of the atomic radii is based off an approximation of the distance from the atom's nucleus to the edge of the atom's electron cloud.
Each shell represents a distinct state of electron energy.
Shell
It would not depend on the direction with respect to the nucleus. The direction of the electron has no effect on the distance of the electron from the nucleus.
Attraction gets smaller.
The Bohr radius, is the estimated distance between protons in the nucleus and electrons - but electrons aren't solid, stationary particles... The simple answer would be about one-twentieth of a nanometre. But this would only be reasonable if the electron were a solid particle.
The atomic radius is the distance from the nucleus of an atom to the outermost orbital of electron.
No. The greater distance from the nucleus the more energy an electron has.
The nucleus has a width on the order of 10^(-15) meters, while an electron is (on average) a distance of 10^(-10) meters from the nucleus. If you were to magnify the nucleus to the size of a baseball, the electrons would be orbiting at a distance of around 1000 meters. That is, there are about 50,000-100,000 nucleus diameters to the electron's average radius.
Bromine has less valence shells than lead making the distance between its valence electron and its nucleus less than that of lead. This means that there is greater attraction between the nucleus and electron for bromine and it requires a higher ionisation energy to remove its electron.
The distance between the nucleus an this electron is higher.
shell
shell