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प्रश्न
State the trends in ionization energy down the group.
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उत्तर
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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संबंधित प्रश्न
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
Give a reason for the following:
Ionisation potential increases across a period, from left to right.
Arrange the elements of second and third period in increasing order of ionization energy.
Among the elements of the second period, Li to Ne, pick out the element with highest first ionization energy
A, B, C are three elements in which B is an inert gas other than helium.With this information complete the following table.
| Element | Atomic number | No. of electrons in the valence shell | Group to which the element belongs |
| A | Z - 1 | ||
| B | Z | ||
| C | Z + 1 |
Also, explain the following : Ionization energy of element C is less than that of element A.
which element has the highest ionisation potential.
Fill in the blank by selecting the correct word from the option.
If an element has a low ionization energy then it is likely to be ________
Arrange the following as per the instruction given in the bracket
Na,Li,K (Increasing ionization energy)
Arrange the following in order of increasing ionisation energy:
F, O, Ne
Explain your choice.
With reference to the variation of properties in the Periodic Table, which of the following is generally true?
