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प्रश्न
Arrange the following as per the instruction given in the bracket:
Potassium, Lithium, Sodium (increasing order of ionization potential).
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उत्तर
Potassium < Sodium < Lithium.
Explanation:
The ionization potential increases as we move up a group in the periodic table because the atomic size decreases, making it harder to remove an electron. Potassium, Lithium, and Sodium belong to Group 1 (alkali metals).
- Potassium (K): Has the lowest ionization potential because it has the largest atomic size and the outermost electron is farthest from the nucleus.
- Sodium (Na): Has a smaller atomic size than potassium, so its ionization potential is higher.
- Lithium (Li): Has the smallest atomic size and the strongest attraction between the nucleus and the outermost electron, giving it the highest ionization potential.
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संबंधित प्रश्न
Represent ionisation potential in the form of an equation. In which unit it is measured?
Name the periodic property which relates to the amount of energy required to remove an electron from an isolated gaseous atom.
Which element from the following has the highest ionization energy?
Explain your choice.
F, O, Ne
Which element from the following has the highest ionization energy?
Explain your choice.
Ne, He, Ar
Among the elements of the second period, Li to Ne, pick out the element with highest first ionization energy
Arrange the following in increasing order of property indicated
Li, Be, B (ionization energy)
What is meant by ionization potential?
State whether the ionization potential increases or decreases on going down a group.
The changes in the properties of elements on moving from left to right across a period of the Periodic Table. For the property, choose the correct answer.
The ionization potential:
Arrange the following in order of increasing ionisation energy:
Ne, He, Ar
Explain your choice.
