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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
Arrange the following as per the instruction given in the brackets:
Na, Li, K (Increasing Ionisation Energy)
Represent ionisation potential in the form of an equation. In which unit it is measured?
Arrange the elements of second and third period in increasing order of ionization energy.
Which element has:
two shells, both of which are completely filled with electrons?
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.
What is meant by ionization potential?
Arrange the following as per the instruction given in the bracket
Na,Li,K (Increasing ionization energy)
With reference to the variation of properties in the Periodic Table, which of the following is generally true?
Ionisation Potential values depend on the nuclear pull. Explain.
