Advertisements
Advertisements
Question
Give reason for the following:
Ionisation potential of the element increases across a period.
Advertisements
Solution
As atomic size decreases and nuclear charge increases, it becomes more difficult to remove electrons, requiring more energy and increasing electron potential.
APPEARS IN
RELATED QUESTIONS
Define the term ‘ionisation potential`.
Which element has:
two shells, both of which are completely filled with electrons?
Choose the correct answer.
An element with highest ionization potential
(i) Calesium
(ii) Fluorine
(iii) Helium
(iv) Neon
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?
The metals of group 2 from top to bottom are: Be, Mg, Ca, Sr, Ba. Which of these metals will form ions most readily and why?
Identify the following:
The energy required to remove an electron from a neutral gaseous atom.
Arrange the following in order of increasing ionisation energy:
Ne, He, Ar
Explain your choice.
Give reason:
Ionisation potential of the element increases across a period from left to right.
Ionisation Potential values depend on atomic size. Explain.
