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Electrons are added to the same shell, therefore the nuclear charge is greater. Electrons are closer to the nucleus so have a greater attraction to the neucleus as you go across a period.

(enough to get you 3 marks, use this always for this type of question).

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Related Questions

Do an atom's successive ionization energies increase regularly?

No, an atom's successive ionization energies do not increase regularly. The first ionization energy, which is the energy required to remove the outermost electron, is typically lower than the second ionization energy, which is the energy required to remove the second electron. The ionization energies generally increase as more and more electrons are removed from an atom. However, there can be irregularities due to factors such as electron-electron repulsion and electron shielding.


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Metallic character increases down a group and from right to left across periods on the periodic table. A decrease in first ionization energy corresponds to an increase in metallic character, as it becomes easier for metals to lose electrons and form cations. Metamorphic metals have lower first ionization energies than nonmetals.


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As you move down a group on the periodic table, the first ionization energy generally decreases due to the increasing atomic size and shielding effect of inner electrons. Across a period, the first ionization energy generally increases because the effective nuclear charge increases, making it harder to remove an electron.