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Among the following least 3rd ionization energy is for
- a)Mn
- b)Co
- c)Fe
- d)Ni
Correct answer is option 'C'. Can you explain this answer?
Most Upvoted Answer
Among the following least 3rd ionization energy is fora)Mnb)Coc)Fed)Ni...
The third ionisation energy of iron is least due to :
as electronic configuration is 3d6 4s2
on removing 2 electrons configuration become 3d6 4s0.
now since removing an electron would result. into stable 3d5 configuration so it would cost least energy consumption.
thus ionisation energy will be least.
as electronic configuration is 3d6 4s2
on removing 2 electrons configuration become 3d6 4s0.
now since removing an electron would result. into stable 3d5 configuration so it would cost least energy consumption.
thus ionisation energy will be least.
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Community Answer
Among the following least 3rd ionization energy is fora)Mnb)Coc)Fed)Ni...
Explanation:
The ionization energy is the energy required to remove an electron from an atom or ion. The third ionization energy refers to the energy required to remove the third electron from an atom or ion.
Ionization Energy Trend:
The ionization energy generally increases across a period (from left to right on the periodic table) due to the increasing nuclear charge and decreasing atomic radius. On the other hand, the ionization energy generally decreases down a group (from top to bottom on the periodic table) due to the increasing atomic size and shielding effect.
Comparing the Elements:
In this case, we are comparing the third ionization energy of Mn, Co, Fe, and Ni.
1. Mn (Manganese):
Manganese is located in period 4 and has an atomic number of 25. It has the electron configuration [Ar] 3d5 4s2. To remove the first three electrons, we would have to remove the 4s2 electrons first, followed by one of the 3d5 electrons. The third ionization energy of Mn would be relatively high.
2. Co (Cobalt):
Cobalt is also located in period 4 and has an atomic number of 27. It has the electron configuration [Ar] 3d7 4s2. To remove the third electron, we would have to remove one of the 3d7 electrons. The third ionization energy of Co would be higher than the first and second ionization energies but lower than Mn.
3. Fe (Iron):
Iron is located in period 4 and has an atomic number of 26. It has the electron configuration [Ar] 3d6 4s2. To remove the third electron, we would have to remove one of the 3d6 electrons. The third ionization energy of Fe would be lower than Mn and Co.
4. Ni (Nickel):
Nickel is also located in period 4 and has an atomic number of 28. It has the electron configuration [Ar] 3d8 4s2. To remove the third electron, we would have to remove one of the 3d8 electrons. The third ionization energy of Ni would be higher than Fe but lower than Mn and Co.
Comparison Result:
Among the given elements, the third ionization energy for Mn (Manganese) is expected to be the highest. Therefore, the correct answer is option 'C' (Fe - Iron).
The ionization energy is the energy required to remove an electron from an atom or ion. The third ionization energy refers to the energy required to remove the third electron from an atom or ion.
Ionization Energy Trend:
The ionization energy generally increases across a period (from left to right on the periodic table) due to the increasing nuclear charge and decreasing atomic radius. On the other hand, the ionization energy generally decreases down a group (from top to bottom on the periodic table) due to the increasing atomic size and shielding effect.
Comparing the Elements:
In this case, we are comparing the third ionization energy of Mn, Co, Fe, and Ni.
1. Mn (Manganese):
Manganese is located in period 4 and has an atomic number of 25. It has the electron configuration [Ar] 3d5 4s2. To remove the first three electrons, we would have to remove the 4s2 electrons first, followed by one of the 3d5 electrons. The third ionization energy of Mn would be relatively high.
2. Co (Cobalt):
Cobalt is also located in period 4 and has an atomic number of 27. It has the electron configuration [Ar] 3d7 4s2. To remove the third electron, we would have to remove one of the 3d7 electrons. The third ionization energy of Co would be higher than the first and second ionization energies but lower than Mn.
3. Fe (Iron):
Iron is located in period 4 and has an atomic number of 26. It has the electron configuration [Ar] 3d6 4s2. To remove the third electron, we would have to remove one of the 3d6 electrons. The third ionization energy of Fe would be lower than Mn and Co.
4. Ni (Nickel):
Nickel is also located in period 4 and has an atomic number of 28. It has the electron configuration [Ar] 3d8 4s2. To remove the third electron, we would have to remove one of the 3d8 electrons. The third ionization energy of Ni would be higher than Fe but lower than Mn and Co.
Comparison Result:
Among the given elements, the third ionization energy for Mn (Manganese) is expected to be the highest. Therefore, the correct answer is option 'C' (Fe - Iron).
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