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Why the first ionization energies generally increase from Na to Ar?
Wiki User
∙ 11y ago
(any period)
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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∙ 11y ago
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Fluorine. Ionization energies are a periodic trend and they generally increase as you go up and to the right in the periodic table.See the chart in the Web Links to the left for a complete chart of the ionization energies of all the elements.
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The energy required to remove more than one electron from atoms. After the first electron is removed, there is now a positive charge which is working against removing another electron. So successive ionization energies increase.
Elements that have the highest first ionization energy?
Helium (He) has the highest first ionization energy. Ionization energy increase as you go across the periodic table from left to right
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1. The ionization energy decrease down in the group.2. The cause is that the distance between the nucleus and the electron shell increase and the needed energy to extract an electron decrease.
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What is the differences between first and second ionization energy?
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Which group of the periodic table has the elements with lowest first ionization energies?
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Atomic Radii,Ionic Radii, First Ionization Energy,Second and Higher Ionization Energies, Electron Affinity.
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Which electrons in the first period have higher ionization energies?
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There is no relation ship. They have the lowest ionization energies.
