Rb is larger with a radius of 248 pm while Xe has one of 130 pm. It follows the trend that radii decrease as you move right across the periodic table.
The atomic radius of Sr (Strontium) is larger than that of Rb (Rubidium). This is because atomic radius generally increases down a group in the periodic table, and Sr is located below Rb in the same group.
Potassium's atomic radius is smaller than rubidium's because potassium has fewer energy levels of electrons.
The species with the smallest atomic radius among K, Mg, Rb, and Ca is Rb (Rubidium). This is because atomic radius tends to decrease across a period from left to right in the periodic table, and Rb is located towards the right side of this group of elements.
Ionization energy increase across a period and decreases down a group, therefore the the element with the greater ionization energy would be found in the top right of the periodic table. In this instance fluorine, F would have the greater ionization energy.
a) Sc,Ti,V,Crb) Na,K,Rb,Csc) B,Si,As,Ted) F,Cl,Br,Ie) Na,Mg,Al,SiThe correct answer of these options is a) Sc,Ti,V,Cr because they are the closest elements to each other in the periodic table.
The atomic radius of Sr (Strontium) is larger than that of Rb (Rubidium). This is because atomic radius generally increases down a group in the periodic table, and Sr is located below Rb in the same group.
Rubidium has an atomic radius of 248 picometers.
In the context of atomic physics, the smallest radius for an atomic orbital is typically found in the hydrogen atom, where the radius is defined by the Bohr model. For the ground state (n=1), the Bohr radius is approximately 0.529 angstroms. In multi-electron atoms, the effective nuclear charge and electron-electron interactions can influence the size of the orbitals, but for a hydrogen-like atom (one electron), the smallest radius occurs at n=1.
Potassium's atomic radius is smaller than rubidium's because potassium has fewer energy levels of electrons.
The species with the smallest atomic radius among K, Mg, Rb, and Ca is Rb (Rubidium). This is because atomic radius tends to decrease across a period from left to right in the periodic table, and Rb is located towards the right side of this group of elements.
Ionization energy increase across a period and decreases down a group, therefore the the element with the greater ionization energy would be found in the top right of the periodic table. In this instance fluorine, F would have the greater ionization energy.
A potassium atom has 19 protons and 19 electrons, plus 20-22 neutrons. A rubidium atom has 37 protons and 37 electrons, plus 46-50 neutrons and so is bigger.
85.4678 is the atomic weight of Rb.
Ca, Mg, Be, Fr, Cs, Rb, K, Na, Li, H
the atomic number of any element is the number of protons in its nucleus, so in this case, 31, Gallium
a) Sc,Ti,V,Crb) Na,K,Rb,Csc) B,Si,As,Ted) F,Cl,Br,Ie) Na,Mg,Al,SiThe correct answer of these options is a) Sc,Ti,V,Cr because they are the closest elements to each other in the periodic table.
Rubidium's atomic radius is greater than xenon's because the trend for atomic radius is that it decreases left to right across a period (even though atomic number increases, and generally speaking, atomic mass does as well.) This is a result of the attraction between the protons in the nucleus and the valence electrons, which are all in the same energy level for isoperiodic elements.