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Across a period , the nuclear charge increases as the number of protons increases.thus the nuclear attraction on the outer shell electron increases so ionization energy should increase across a period .
**Why the first ionization energy of krypton is higher than that of selenium ?
The electron configurations of the last quantum shells of , Se - 4S2 4P4 & Kr- 4S2 4P6.
As Kr has a completely filled outer shell , it needs more energy to remove it' s ooutermost electron than in Se. Also , Kr has the highest nuclear charge in 4th period ,(Kr & Se both are in 4th period ) the nuclear attraction to the outermost electron becoms even high.
Therefore the first ionization energy of krypton is higher than that of selenium .
Hope this s helpful 😊
Kryptons ionization energy is 1356 kJ/mol
The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom, etc. Ionization energy generally increases for every electron that is removed, and increases from left to right in the periodic table or if moving up the periods. In this case, from the periodic table (or according to Mastering Chemistry) Bromine (Br) has a larger sixth ionization energy than Selenium (Se).
First ionization energy is the energy required to remove the first outermost electron from an atom. The second ionization energy is the energy required to remove the next available electron, and is greater than the first IE. The third IE is that energy needed to remove the third electron, and is greater the the second IE.
Helium (He) has the highest ionization energy.
ionization energy
Kryptons ionization energy is 1356 kJ/mol
potassium is greater in the second ionization energy.
Bromine has the highest.
Krypton has a higher value.
The noble gas, krypton
Neon is a much smaller atom than selenium because neon has fewer occupied energy levels so it has a considerably smaller atomic radius. For that reason, it will be more difficult to remove an electron from Ne than Se, so Ne has the greater ionization energy.
No, it is a noble element, therefore it has very high ionization energy.
Beryllium has greater ionization energy, with 899 kJ/mol versus Germanium's 762 kJ/mol. The general trend (most prominently displayed in the representative elements) in the periodic table is increasing ionization energy across a period, and decreasing ionization energy down a group.
The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom, etc. Ionization energy generally increases for every electron that is removed, and increases from left to right in the periodic table or if moving up the periods. In this case, from the periodic table (or according to Mastering Chemistry) Bromine (Br) has a larger sixth ionization energy than Selenium (Se).
It takes more energy to knock off two electrons
First ionization energy is the energy required to remove the first outermost electron from an atom. The second ionization energy is the energy required to remove the next available electron, and is greater than the first IE. The third IE is that energy needed to remove the third electron, and is greater the the second IE.
sodium because it's the first group and first group are the most