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
Give a reason for Ionisation potential increases across a period, from left to right
State the trends in ionization energy across the period.
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.
F, O, Ne
Among the elements of the second period, Li to Ne, pick out the element with highest first ionization energy
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.
Choose the correct answer from the choice given:
Ionisation potential increases over a period from left to right because the
Identify the following:
The energy required to remove an electron from a neutral gaseous atom.
Across a period, the ionization potential ______.
With reference to the variation of properties in the Periodic Table, which of the following is generally true?
