Advertisements
Advertisements
Question
Ionisation Potential values depend on the nuclear pull. Explain.
Advertisements
Solution
The ionisation potential is the energy needed to remove an electron from a neutral isolated gaseous atom. 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).
RELATED QUESTIONS
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.
Ne, He, Ar
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.
State whether the ionization potential increases or decreases on going down a group.
Supply the missing word from those in the brackets:
If an element has a low ionization energy then it is likely to be ______ (metallic/ non-metallic).
Choose the correct answer from the choice given:
Ionisation potential increases over a period from left to right because the
Rewrite the following sentence by using the correct > (greater than) or < (less than) in the blank given
The ionization potential of potassium is _______ that of sodium.
Arrange the following in order of increasing ionisation energy:
F, O, Ne
Explain your choice.
Across a period, the ionization potential ______.
Give reason:
Ionisation potential of the element increases across a period from left to right.
