The pair of elements having approximately equal ionisation potential is
Ionisation energy increases with decreases in atomic size and decrease in shielding effect.
Al(13) = 1s2, 2s2, 2p6, 3s2, 3p1
Ga(31) = 1s2, 2s2, 2p6, 3s2, 3p6, 4d10, 4s2, 4p1
As the atomic electronic configuration show there are ten d-electrons in Ga which shield the nuclear charge less effectively than s and p electrons. Hence, the outer electron is held fairly strongly by the nucleus. Consequently ionisation energy slightly increases inspite of the increase in atomic size from Al to Ga. Hence, Al and Ga have approximately equal ionisation potential.
Which of the following transition involves maximum amount of energy?
The formation of the oxide ion O2–(g) requires first an exothermic and then an endothermic step as shown below
This is because
The electronic configuration of four elements are given below. Which element does not belong to the same family?
The least stable ion among the following is
Ist and IInd IE of Mg are 7.646 and 15.035 eV respectively. The amount of energy needed to convert all the atoms of magnesium into Mg2+ ions present in 12 mg of magnesium vapours is [Given, 1 eV = 96.5 kJ mol–1]
Which of the following is the most electropositive element?
Which of the following sequence correctly represents the decreasing acidic nature of oxides?
Which of the following pairs of species have nearly same size?
The set representing the correct order of ionic radius is
Which is not the correct order for the stated property?