Because, as we know that when we go across the period of the Periodic Table, the number of shells remain the same but the number of electrons and protons increases. So, Rb having its atomic number as 37 and Sr as 38, Strontium has got more nuclear charge as well as more electrons. As a result the first ionisation energy required to remove one electron is more in Strontium than Rubidium.
Strontium
The electronegativity of barium is less than that of strontium.
energy is spread over a larger area
A "D-size" carbon-zinc cell at 100 mA would have about ten times as much "energy" as a 9V carbon-zinc at 8mA. A battery in the AAA series would have about the same energy as a 9V, which should not be surprising since a D is 10 time larger than a AAA.
The Atlantic Ocean is larger than the Indian Ocean.
Strontium
The electronegativity of barium is less than that of strontium.
the 1st ionization energy is 403.03 kJ/mol.. since it's oxidation state is +1, you don't normally take away more than one electron so the 2nd and 3rd ionization energies are much larger and don't usually matter
Both are ions and we should consider the ionic radius, not the atomic radius. Rubidium ion (Rb+) will have a larger IONIC radius than strontium ion (Sr2+). Both ions have the same electronic configuration. But strontium ion has more number of protons in the nucleus. Hence it will have greater force of attraction between the nucleus and the valence electrons, resulting in smaller size.
It is about first ionization energy. It is less than alkaline earth metals.
Rubidium is a neutral atom in its elemental form. The rubidium ion, found in rubidium compounds, is smaller than a neutral rubidium atom.
About twice as large, which is not that much at the first ionization level. Still, Magnesium has a slightly larger, one proton nucleus and one more electron in that valence level to add to the energy needed to pill the first electron out of it's orbital. Electron shielding may have something to do with this also as the other valance electron of this 2+ element may shield the pulled electron.
In rubidium, having a larger atomic radius, the attraction force between the atomic nucleus and and the electron from outermost shell is lower.
The reason the second ionization energy is higher than the first relates to the attraction between the electrons and the nucleus. When one electron is removed from an atom, the neutral atom becomes positive. When one attempts to remove a second electron from a positive ion, there is more attraction between the electrons and the nucleus due to the extra proton. Thus, the second electron is harder to remove and the ionization requires more energy.
(Chlorine, Fluorine, anything that gains an electron when it ionizes) For example: when F becomes F−, it gains one electron but has the same number of protons, meaning the attraction of the protons to the electrons is weaker, creating a larger radius.
sn is larger but si is larger if your talking about ionization energy
The larger the magnitude of the earthquake, the larger the energy to be released by the earthquake.