Advertisements
Advertisements
प्रश्न
Arrange the following as per the instruction given in the bracket:
Potassium, Lithium, Sodium (increasing order of ionization potential).
Advertisements
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.
APPEARS IN
संबंधित प्रश्न
Define the term ‘ionisation potential`.
Name the elements with highest and lowest ionization energies in the first three periods.
Arrange the elements of second and third period in increasing order of ionization energy.
Arrange the elements of group 17 and group 1 according to the given conditions.
Increasing ionization potential
Which element from the following has the highest ionization energy?
Explain your choice.
Ne, He, Ar
State whether the ionization potential increases or decreases on going down a group.
Choose the correct answer from the choice given:
Ionisation potential increases over a period from left to right because the
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 ________
Give reason for the following:
Ionisation potential decreases down a group.
Identify the following:
The energy required to remove an electron from a neutral gaseous atom.
