3. In general second ionisation enthalpy of an atom
will be
(a) higher than the first ionisation enthalpy
(b) equal to the first ionisation enthalpy
(c) higher than the third ionisation enthalpy
(d) equal to the third ionisation enthalpy
Answers
Answer:
a)Second ionisation enthalpy is usually greater than the first ionisation energy because after removal of first electron, the remaining electrons are held more firmly by the nucleus and thus the atom has greater nuclear charge which makes the removal of second electron difficult and thus greater second ionisation energy.
b)The first ionisation energy is the energy required to remove one mole of the most loosely held electrons from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of 1+. This is more easily seen in symbol terms. It is the energy needed to carry out this change per mole of X.
c) sorry nahi ata
d)First Ionization Energy:
The first ionization energy of an atom is the energy required to remove the first electron from the outermost shell of an atom. Once the first electron has been removed from the gaseous atom, it is possible to remove second and successive electrons from positive ions one after the other.
Second Ionization Energy:
Once the first ionization electron is removed from the gaseous atom, it is possible to remove second and successive electrons from positive ions one after the other. Removal of the second electron from an already ionized gaseous atom is called as second ionization energy.
A(g)+IE
1
→A
+
(g)+e
−
[First Ionization]
A
+
(g)+IE
1
A
2+
(g)+e
−
[Second ionization]
The number of energies required to remove most loosely bound electron from unipositive, dipositive, tripositive ions of the element in the gaseous state are called second, third, fourth, etc ionization energies respectively.
The second, third and fourth, etc ionization energies are collectively called as successive ionization energies.
It is also seen that IE3 > IE2 > IE1.
So options A & C are correct