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प्रश्न
Which element from the following has the highest ionization energy?
Explain your choice.
Ne, He, Ar
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उत्तर
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.
संबंधित प्रश्न
The energy required to remove an electron from a neutral isolated gaseous atom and convert it into a positively charged gaseous ion is called ____________. (electron affinity, ionization potential,
electronegativity)
Name the periodic property which relates to the amount of energy required to remove an electron from an isolated gaseous atom.
Which element has:
two shells, both of which are completely filled with electrons?
With reference to the variation of properties in the Periodic Table, which of the following is generally true?
Ionization potential increases from left to right across a period.
Supply the missing word from those in the brackets:
If an element has a low ionization energy then it is likely to be ______ (metallic/ non-metallic).
Choose the correct answer from the choice given:
Ionisation potential increases over a period from left to right because the
Rewrite the following sentence by using the correct > (greater than) or < (less than) in the blank given
The ionization potential of potassium is _______ that of sodium.
Arrange the following in order of increasing ionisation energy:
Ne, He, Ar
Explain your choice.
Across a period, the ionization potential ______.
Give reason:
Ionisation potential of the element increases across a period from left to right.
