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No, the noble gases do not follow the periodic trends (i.e. electronegativity, electron affinity, etc.) the way that the Group 1, 2, and so on elements do. They each have a complete valence shell, so they do not usually attract electrons.
Noble gases have a full octet of electrons in their outermost shell, making them stable and virtually unreactive. Since valence electrons determine the chemistry of the atom, noble gases do not exhibit the trends of ionization energy/electron affinity/etc. that we see with atoms with incomplete outer shells.
Yes, noble gases have ionization energies and electron affinities. Since noble gases are very very stable (inert/won't react), they do not want to gain or lose an electron. Therefore, they will have very high ionization energies and very low electron affinities.
No, they don't because they have all 8 valence electrons. These trends are based on the fact that elements tend to want to have a full valence shell. For example, ionization energy is the amount of energy it takes to remove an electron. Group 1 has low ionization energy because they want to lose their one electron to have a full valence shell, while group 17 has high ionization energy because they want to gain one more electron to complete their valence shell, so removing an electron would make it further from completing its shell. Noble gases are already stable and have full valence shells, so they don't want to change their structure.
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