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Question
State the trends in ionization energy down the group.
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Solution
The greater the nuclear charge, the stronger the attraction between valence electrons and the nucleus and the greater the energy needed to remove the electron(s).
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RELATED QUESTIONS
Choose the correct answer from the options given below:
Ionisation potential increases over a period from left to right because of the
(A) Atomic radius increases and nuclear charge increases
(B) Atomic radius decreases and nuclear charge decreases
(C) Atomic radius increases and nuclear charge decreases
(D) Atomic radius decreases and nuclear charge increases
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Define the term ‘ionisation potential`.
What do you understand by successive ionization energies?
Which element from the following has the highest ionization energy?
Explain your choice.
F, O, Ne
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Among the elements of the second period, Li to Ne, pick out the element with highest first ionization energy
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The ionization potential of potassium is _______ that of sodium.
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The energy required to remove an electron from a neutral gaseous atom.
Across a period, the ionization potential ______.
