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 and rubidium have five electron shells/levels.
noble gases have the maximum ionisation energy. helium has the highest ionisation energy
the energy increases as the charge on the cation increases gradually ie1<ie2<ie3
Ionisation energy decreases down the group. It is easy to remove an electron.
no the same,first ionisation contains a slightly differences in isotopes
first ionisation energy is defined as the energy required for removing of one electron from outer shell is called first ionisation energy(IP1)
The first molar ionization energy of rubidium is 403 kJ/mol.
the first ionisation energy is the energy required to remove the first most loosely bound elecctron from a neutral gaseous atom in its ground state.
The outermost principle energy level for strontium is the 5th energy level.
when we go from left to right