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Which of the following pairs has the highest difference in their first ionization energy?
- a)Xe, Cs
- b)Kr, Rb
- c)Ar, K
- d)Ne, Na
Correct answer is option 'D'. Can you explain this answer?
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Which of the following pairs has the highest difference in their first...
Explanation:
First ionization energy is defined as the energy required to remove one electron from an isolated gaseous atom in its ground state. The higher the ionization energy, the more difficult it is to remove an electron from the atom.
To determine which pairs have the highest difference in their first ionization energy, we need to compare their ionization energies. The larger the difference in ionization energy, the higher the difference between the two elements.
Comparing the ionization energies of the given pairs:
a) Xe (1170 kJ/mol), Cs (376 kJ/mol) = 794 kJ/mol
b) Kr (1160 kJ/mol), Rb (403 kJ/mol) = 757 kJ/mol
c) Ar (1520 kJ/mol), K (419 kJ/mol) = 1101 kJ/mol
d) Ne (1310 kJ/mol), Na (496 kJ/mol) = 814 kJ/mol
Therefore, the pair with the highest difference in their first ionization energy is Ne and Na, with a difference of 814 kJ/mol. Therefore, option D is correct.
First ionization energy is defined as the energy required to remove one electron from an isolated gaseous atom in its ground state. The higher the ionization energy, the more difficult it is to remove an electron from the atom.
To determine which pairs have the highest difference in their first ionization energy, we need to compare their ionization energies. The larger the difference in ionization energy, the higher the difference between the two elements.
Comparing the ionization energies of the given pairs:
a) Xe (1170 kJ/mol), Cs (376 kJ/mol) = 794 kJ/mol
b) Kr (1160 kJ/mol), Rb (403 kJ/mol) = 757 kJ/mol
c) Ar (1520 kJ/mol), K (419 kJ/mol) = 1101 kJ/mol
d) Ne (1310 kJ/mol), Na (496 kJ/mol) = 814 kJ/mol
Therefore, the pair with the highest difference in their first ionization energy is Ne and Na, with a difference of 814 kJ/mol. Therefore, option D is correct.
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Which of the following pairs has the highest difference in their first...
- I.E. increases from left to right and decreases from top to bottom in the periodic table.
- Ne (noble gas) and Na (alkali metal) belong to 2nd and 3rd period respectively and show highest difference in their first I.E.
- Subsequent members of the same group show lower I.E. on moving down in the group
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Which of the following pairs has the highest difference in their first ionization energy?a)Xe, Csb)Kr, Rbc)Ar, Kd)Ne, NaCorrect answer is option 'D'. Can you explain this answer?
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