Respuesta :
Answer:
d) 1s² 2s² 2p⁶ 3s² 3p¹
Explanation:
The lowest ionization energy is found from the predictable nature of ionization energy knowing that we have for ionization energy;
1) The ionization energy becomes progressively larger as we move from left to right along the periodic table
2) The ionization energy becomes progressively larger or increases as we move from the top to the bottom in a particular group within the periodic table
Therefore, atoms which are far right (have more electrons in their valence shells) have higher ionization energies, while the atoms that are at the bottom of a group (with more shells in their electronic configuration) have lower ionization energy which gives;
1s² = Helium
1s² 2s² = Beryllium
1s² 2s² sp⁶ = Neon
1s² 2s² 2p⁶ 3s² 3p¹ = Aluminum
1s² 2s² 2p⁶ 3s² 3p³ = Phosphorus
The ionization energy of 1s² 2s² 2p⁶ has the highest ionization energy, while the atom 1s² 2s² 2p⁶ 3s² 3p¹ which has one electron in the p orbital, has the lowest ionization energy
1s² 2s² 2p⁶ 3s² 3p¹ which is Aluminum represents the atom with the lowest
first-ionization energy
Ionization energy is the energy that is needed to remove an electron from its orbital during chemical reactions.
The atoms with more electrons in their outer shells have higher ionization
energies, while the atoms with lesser electrons in their outer shells have
lower ionization energy.
1s²
1s² 2s²
1s² 2s² 2p⁶
1s² 2s² 2p⁶ 3s² 3p¹
1s² 2s² 2p⁶ 3s² 3p³
The element with the lowest first-ionization energy is therefore 1s² 2s² 2p⁶
3s² 3p¹ and the element with the highest first-ionization energy will be 1s²
2s² 2p⁶ .
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