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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).
RELATED QUESTIONS
Define the term ‘ionisation potential`.
Name the elements with highest and lowest ionization energies in the first three periods.
State whether the ionization potential increases or decreases on going down a group.
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.
which element has the highest ionisation potential.
Arrange the following as per instruction given in the bracket.
Na, K, Cl, S, Si (increasing ionisation potential)
Fill in the blank from the choice given in bracket.
The energy required to remove on electron from a natural isolated gaseous atom and convert it into a positively charged gaseous ion is called ____________
Arrange the following as per instruction given in the bracket.
Na, Mg, Cl, S, Si (increasing ionisation potential)
Across a period, the ionization potential ______.
Give reason:
Ionisation potential of the element increases across a period from left to right.
