Consider Fe3+, Fe2+, and Zn2+:a. Write the electro...

Question

Consider Fe3+, Fe2+, and Zn2+:a. Write the electron configuration for each ionb. Unlike iron, zinc is unlikely to have additional oxidation states, such as Zn+ or Zn3+. Briefly explain why zinc nearly always forms Zn2+ ions.

Jules Bruno · Accepted Answer

We’re being asked to determine the correct noble gas electron configuration for Fe3+, Fe2+, and Zn2+.Part a:For Fe3+:Before we can do that, we have to first write the electron configuration of a neutral ground state iron (Fe).You can determine the ground-state electron configuration of Iron (Fe) by locating its position in the periodic table.You see from the periodic table that FeCr is in Period 4 and d-block• Before reaching Fe, you will pass through the atomic orbitals 1s, 2s, 2p, 3s, 3p, 4s, 3d• In a neutral atom:Atomic number = # of protons = # of electronsFe atomic number = 26 → 26 protons & 26 electrons• Distribute electrons in the atomic orbitals:[readmore]Recall:s           _                1 orbitalp        _ _ _             3 orbitalsd       _ _ _ _ _        5 orbitalss orbital → can hold a maximum of 2 electronsp orbitals → can hold a maximum of 6 electronsd orbitals → can hold a maximum of 10 electronsf orbitals → can hold a maximum of 14 electronsFill up the orbitals with electrons:Aufbau Principle → totally fill in the lowest energy orbital firstHund’s Rule → electron orbitals that are degenerate (same energy)are first half-filled before they are totally filled          Write the electron configuration from the lowest energy level to the highest energy level:Neutral Fe: 1s22s22p63s23p64s23d6Going back to Fe3+:▪ charge = +3 ▪ the +3 charge means that it lost 3 electrons:• subtract 3 e- from the outermost electrons of Fe• subtract the electrons from the highest numbered orbital or higher energy orbital: 4s and 3dFe3+: 1s22s22p63s23p63d5For Fe2+: Fe2+:▪ charge = +2 ▪ the +2 charge means that it lost 2 electrons:• subtract 2e- from the outermost electrons of Fe• subtract the electrons from the highest numbered orbital or higher energy orbital: 4s and 3dFe2+: 1s22s22p63s23p63d6For Zn2+:Before we can do that, we have to first write the electron configuration of a neutral ground state zinc (Zn).You can determine the ground-state electron configuration of Zinc (Zn) by locating its position in the periodic table.You see from the periodic table that Zn is in Period 4 and d-block• Before reaching Zn, you will pass through the atomic orbitals 1s, 2s, 2p, 3s, 3p, 4s, 3d• In a neutral atom:Atomic number = # of protons = # of electronsZn: atomic number = 30 → 30 protons & 30 electrons• Distribute electrons in the atomic orbitals:Recall:s           _                1 orbitalp        _ _ _             3 orbitalsd       _ _ _ _ _        5 orbitalss orbital → can hold a maximum of 2 electronsp orbitals → can hold a maximum of 6 electronsd orbitals → can hold a maximum of 10 electronsf orbitals → can hold a maximum of 14 electronsFill up the orbitals with electrons:Aufbau Principle → totally fill in the lowest energy orbital firstHund’s Rule → electron orbitals that are degenerate (same energy)are first half-filled before they are totally filled          Write the electron configuration from the lowest energy level to the highest energy level:Neutral Zn: 1s22s22p63s23p64s23d10Going back to Zn2+:▪ charge = +2▪ the +2 charge means that it lost 2 electrons:• subtract 2 e- from the outermost electrons of Zn• subtract the electrons from the highest numbered orbital or higher energy orbital: 4s and 3dZn2+: 1s22s22p63s23p63d10Part b:b. Unlike iron, zinc is unlikely to have additional oxidation states, such as Zn+ or Zn3+. This is because if you look at its electron configuration, all of the orbitals are completely filled and all of the electrons are paired making Zn2+ the most stable form a zinc ion. Therefore, zinc nearly always forms Zn2+ ions

Problem: Consider Fe3+, Fe2+, and Zn2+:a. Write the electron configuration for each ionb. Unlike iron, zinc is unlikely to have additional oxidation states, such as Zn+ or Zn3+. Briefly explain why zinc nearly always forms Zn2+ ions.

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Problem: Consider Fe3+, Fe2+, and Zn2+:a. Write the electron configuration for each ionb. Unlike iron, zinc is unlikely to have additional oxidation states, such as Zn+ or Zn3+. Briefly explain why zinc nearly always forms Zn2+ ions.

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