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asdf1
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why is the electron configuration different for Z<20 and Z>90?
Out of curiosity :asdf1 said:Z<20:
1s<2s<2p<3s<3p<4s<3d<4p
but
Z>90
1s<2s<2p<3s<3p<3d<4s<4p ?
Z<20 and Z>90 refer to the atomic number of an element, which determines its placement in the periodic table. Elements with Z<20 have a simpler electron configuration due to their lower number of electrons, while elements with Z>90 have more complex electron configurations.
The number of electrons in an element determines the energy levels and sublevels in which they are arranged. Elements with fewer electrons (Z<20) have complete outermost energy levels and therefore have a more stable electron configuration. Elements with more electrons (Z>90) have incomplete outermost energy levels and therefore have a less stable electron configuration.
Yes, elements with Z<20 and Z>90 can have similar electron configurations. This is because the arrangement of electrons is determined by the number of electrons and their energy levels, not just the atomic number. For example, both carbon (Z=6) and silicon (Z=14) have electron configurations of 1s2 2s2 2p2, even though their atomic numbers are different.
The electron configuration of an element determines its reactivity and chemical properties. Elements with full outermost energy levels (such as those with Z<20) are less likely to react with other elements, while elements with incomplete outermost energy levels (such as those with Z>90) are more reactive and likely to form bonds with other elements.
Yes, the electron configuration of an element can change through various processes such as ionization, where an electron is lost or gained, or through excitation, where an electron is temporarily moved to a higher energy level. However, the number of electrons in the element remains the same, so its placement on the periodic table does not change.