Ionization energy explanation questions?Explain why the first ionization energy of aluminum is smaller than the first ionization energy of magnesiumandExplain why the 3rd ionization energy of an element is always larger than its second ionization energy
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The electronic configuration of aluminium is 2, 8, 3; so on the third shell on the first orbital s there are 2 electrons in the only orbit of s (3s?) and one electron on one of the 3 orbits of the orbital p (3p?)The electronic configuration of magnesium is 2, 8, 2; so on the third shell on the first orbital s there are 2 electrons in the only orbit of s (3s?)When you remove an electron from an aluminium atom (ionization) you take it from the p-orbital, which is further away from the core than an s orbital and if an electron is further from the core it takes less energy to remove itThe first electron from a magnesium however comes from the s orbital and thus uses more energyThe ionization energy of an electron is always greater than the one before that because once you have pulled off electrons, your element becomes a positively charged ionBecause of the electrostatic attraction between + and -, it is more difficult to pull an electron away from a positively charged ion than from a neutral atom.
