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The outer valence electron lies in a 1s orbital in Hydrogen. The effective nuclear charge of hydrogen can be taken as Z = 1. The electron that is being ionised in Oxygen lies in a 2p orbital which has an effective nuclear charge of Z = 8-(3.4 or 4.5 or something). The point is, this nuclear charge at a greater distance from the nucleus means the energies of the electrons are similar and so ionisation energis required are too similar.
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RossThe first ionization energy of hydrogen and oxygen is the same because both elements have one electron in their outermost shell, which is easier to remove compared to other electrons located closer to the nucleus. This results in the same amount of energy required to remove the outermost electron in both elements.
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Why are the ionisation energy of isotopes the same?
The ionization energy of isotopes is the same because isotopes have the same number of protons in their nucleus, which determines the ionization energy. Isotopes differ in the number of neutrons they possess, but neutrons do not contribute significantly to the ionization energy compared to protons.
What atoms have the smallest values for the first ionisation energies?
Helium and hydrogen have the smallest values for the first ionization energies. Helium has the lowest first ionization energy due to its stable electron configuration with a full outer shell, while hydrogen has a low ionization energy because it has only one electron in its outer shell.
What is the relationship between ionization energy and the alkali metals?
There is no relation ship. They have the lowest ionization energies.
Why boron has a lower first-ionization energy than beryllium?
Because in Boron there is a complete 2s orbital and the increased shielding of the 2s orbital reduces the ionisation energy compared to that seen in Beryllium.
Whose first ionization energy is higher oxygen or carbon?
The first ionization energy for carbon is 1 086,5 kJ/mol. The first ionization energy for oxygen is 1 319,9 kJ/mol.
