There are many elements with atomic radii larger than that of P. Several examples would be Si, Al, Mg, and Na.
Elements atomic radii increase in size as they run down the columns of the periodic table or across the periodic table from right to left. So, Al is larger than Cl. XP
Although they are all group I atoms, Na and K have a nuclear charge representative of s,p,and d electrons. Once you get to Rb the 4f sublevel comes into play along with the significantly increase nuclear charge. As a result, the does not increase as significantly as the Na and K.
N-- Because it has less electrons, the proton pull is smaller on each individual electron, holding them closer to the nucleus and making the radius smaller
The atomic radius increases from top to bottom in groups 1 and 2 of the modern periodic table. This happens because the number of energy shells increase and are occupied by the increasing number of electrons. As the subsequent shells are completed they are located further from the nucleus due to the decreasing force of attraction between nucleus and the electrons. This leads to an increase in atomic radius. == == Atomic radius is a result of the completion of orbitals as atoms get heavier by adding neutrons and protons to the nucleus. The larger nucleus can hold more electrons. The cloud of electrons determines the atomic radius. Each completed orbital (S,P,D or F) takes up room. The higher orbitals have a greater radius . Unlike the old Bohr theory of atoms (little electrons in orbits around the nucleus), the new probability distribution interpretation of the electrons leads to spherical or hourglass shaped volumes.
Generally it decreases. There are a few exceptions: the noble gases tend to be quite a bit bigger than the corresponding halogens, and there's a smaller bump as you go from d-block elements to p-block elements.
The radius of any anion is larger than the original neutral atom. So phosphide (P^3-) which as gained 3 electrons, has a larger radius than phosphorous (P).
Elements atomic radii increase in size as they run down the columns of the periodic table or across the periodic table from right to left. So, Al is larger than Cl. XP
for hydrogen it is about 37 pico-meters. larger atoms (larger than H or He) have a second, or even 3, 4, 5, 6, or 7 orbitals of electrons. Francium, #87 has an atomic radius of 270 p-m. Much bigger, but way tiny compared to you.
Atomic radius increases down the group
N, P, As and Sb
N, P, As and Sb
Atomic radius increases down the group
Atomic radius increases going down the periodic table and going from right to left, meaning that Fr (Francium) has the largest atomic radius and He (Helium) has the smallest. Therefore, Cl<S<P<Si<Al So the answer is Cl
it's neon
Atomic radius increases down the group
The larger bubble has a larger diameter and therefore less pressure than the smaller bubble since: p(in) = p(out) + 2y/r. p = pressure y = surface tension r = radius Therefore, pressure is inversely proportionate to the radius size. Since the smaller bubble has a smaller radius, and therefore, a greater internal pressure, it would "push" the air through the hollow tube to the larger one until the smaller one ceases to exist.
Although they are all group I atoms, Na and K have a nuclear charge representative of s,p,and d electrons. Once you get to Rb the 4f sublevel comes into play along with the significantly increase nuclear charge. As a result, the does not increase as significantly as the Na and K.