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Question
Which element from the following has the highest ionization energy?
Explain your choice.
Ne, He, Ar
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Solution
He
Ionisation energy decreases with an increase in the atomic size, i.e. it decreases as one moves down a group. Ne, He and Ar are inert gases. He - Period 1, Ne - Period 2 and Ar - Period 3.
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
Represent ionisation potential in the form of an equation. In which unit it is measured?
In a group, a particular element has the lowest ionization potential; does it ionize most easily or least easily? Explain with example.
State whether the ionization potential increases or decreases on going down a group.
Arrange the following as per the instruction given in the bracket
Na,Li,K (Increasing ionization energy)
First ionisation enthalpy of two elements X and Y are 500 kJ mol−1 and 375 kJ mol−1 respectively. Comment about their relative position in a group as well as in a period.
Arrange the following in order of increasing ionisation energy:
P, Na, Cl
Explain your choice.
Arrange the following in order of increasing ionisation energy:
F, O, Ne
Explain your choice.
Arrange the following in order of increasing ionisation energy:
Ne, He, Ar
Explain your choice.
Give reason:
Ionisation potential of the element increases across a period from left to right.
