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anonymous

  • one year ago

Consider Group 5A elements: nitrogen, phosphorus, and arsenic. These elements show an increase in their atomic numbers. Which element has the highest ionization energy?

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  1. anonymous
    • one year ago
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    Hi welcome to Openstudy @independent.Queen! :) To answer your question, you first have to understand what ionization energy is. Ionization energy is the energy required for a neutral atom to \(\sf \large \text{remove an electron}\) in its gaseous phase. Since the metals from the periodic table tend to lose electrons, they have a higher ionization energies than the non-metals which tend to receive electrons. Meanwhile, ionization energy decreases down a group due to electron shielding. From the word itself, it is the ability of electron to 'shield' the nucleues that has positive charge in it. As you go down the group, you'll have more and more electrons that will shield that positive charge, hence lowering the ionization energy. So from the explanation and with the help of a periodic table: |dw:1433980362786:dw| which one do you think will have the highest ionization energy?

  2. anonymous
    • one year ago
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    Data_LG2 Well since you put it in that form now I understand that the one with the highest ionization is Nitrogen. Thank you for clarifying this aspect for me! :)

  3. anonymous
    • one year ago
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    You're welcome :)

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