N(0)//2 atoms of X((g)) are converted in...

`N_(0)//2` atoms of `X_((g))` are converted into `X_((g))^(o+)` by energy `E_(1), N_(0)//2` atoms of `X_((g))` are converted inot `X_((g))^(ɵ)` by energy `E_(2)`. Hence ionisation potential and electron affinity of `X_((g))` per atom are

`(2E_(1))/(N_(0)),(2(E_(2)-E_(1)))/(N_(0))`

`(2E_(1))/(N_(0)), (2E_(2))/(N_(0))`

`((E_(1)-E_(2)))/(N_(0)), (2E_(2))/(N_(0))`

None is correct.

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The correct Answer is:

Let the ionisation energy of `X_((g)) = IE` per atom and electron affinity of `X_((g)) = -EA` per atom.
`X_((g)) rarr X_((g))^(o+) + e^(-)`
Energy required to ionise `(N_(0))/(2)` atoms of `X_((g)) = (N_(0))/(2) xx IE = E_(1)` (given)
`:. IE = (2E_(1))/(N_(0))`
`X_((g)) rarr X_((g))^(o+) ("Energy" = (N_(0))/(2) xx IE)` ...(iii)
`X_((g)) + e^(-) rarr X_((g))^(ɵ)[["Energy released to"],["add electrons to" (N_(0))/(2)],["atoms of" X_((g)) = -(N_(0))/(2) xx EA]]` ...(iv)
Energy for the process `X_((g))` to `X_((g))^(ɵ) = E_(2)` (given). Therefore, adding Eq. (iii) and (iv), we give
`((N_(0))/(2) xx IE - (N_(0))/(2) xx EA) = E_(2)` (given) ...(v)
Substitute the value of `IE` from Eq. (ii) in Eq. (v).
`(cancel(N_(0))/(cancel(2)) xx (cancel(2)E_(1))/(cancel(N_(0))) -(N_(0))/(2) xx EA) = E_(2)`
`-(N_(0))/(2) xx EA = E_(2) - E_(1)`
`:. -EA = (2(E_(2)-E_(1)))/(N_(0))`
`:. IE = (2E_(1))/(N_(0))"atom"^(-1)` and `-EA = (2(E_(2)-E_(1)))/(N_(0))`

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N_(0)//2 atoms of X(g) are converted into X^(+) (g) by energy E_(1) . N_(0)//2 atoms of X(g) are converted into X^(-) (g) by the energy E_(2) . Hence ionisation potential and electron affinity of X(g) are :

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The amount of energy required to remove the most loosely bound electron from an isolated gaseous atom is called as first ionization energy (IE_(1)) . Similarly the amount of energies required to knock out second, third etc. electrons from the isolated and IE_(3)gt IE_(2)gt IE_(1) . (i) Nuclear charge (ii) Atomic size (iii) penetration effect of the electrons (iv) shielding effect of the inner electrons and (b) electronic configurations (exactly half filled and completely filled configurations are extra stable) are the important factors which affect the ionisation energies. Similarly, the amount of energy released when a neutral isolated gaseous atom accepts an extra electron to from gaseous anion is called electron affinity. (X(g)+e^(-)(g)rarr X^(-)(g)+ energy A positive elecrton affinity idicates that the ion X^(-) has a lower more negative energy than the neutral atom X. The second electron affinity for the addition of a second electron to an initially neutral atom is negative because the electron replusion outweights the nuclear attraction, e.g., O(g)+e^(-)overset("Exothermic")rarr O^(-)(g),E_(a)=+141 kJ mol^(-) ....(i) O^(-)(g)+e^(-)overset("Excothermic")rarr, E_(a)=-780 kJ mol^(-) ...(ii) The electron affinity of an element depends upon (i) atomic size (ii) nuclear charge and (iii) electronic configuration. In general, in a group, ionisation energy and electron affinity decrease as the atomic size increases. The members of third period have some higher (e.g., S and Cl) electron affinity values than the members of second period (e.g., O and F) because second period elements have very small atomic size. Hence, there is tendency of electron-electron repulsion, which resultss in less evolution of energy in the formation of correcsponding anion. The first ionisation energy of Na, Mg,AI and Si are in the order of:

The amount of energy required to remove the most loosely bound electron from an isolated gaseous atom is called as first ionization energy (IE_(1)) . Similarly the amount of energies required to knock out second, third etc. electrons from the isolated and IE_(3)gt IE_(2)gt IE_(1) . (i) Nuclear charge (ii) Atomic size (iii) penetration effect of the electrons (iv) shielding effect of the inner electrons and (b) electronic configurations (exactly half filled and completely filled configurations are extra stable) are the important factors which affect the ionisation energies. Similarly, the amount of energy released when a neutral isolated gaseous atom accepts an extra electron to from gaseous anion is called electron affinity. (X(g)+e^(-)(g)rarr X^(-)(g)+ energy A positive elecrton affinity idicates that the ion X^(-) has a lower more negative energy than the neutral atom X. The second electron affinity for the addition of a second electron to an initially neutral atom is negative because the electron replusion outweights the nuclear attraction, e.g., O(g)+e^(-)overset("Exothermic")rarr O^(-)(g),E_(a)=+141 kJ mol^(-) ....(i) O^(-)(g)+e^(-)overset("Excothermic")rarr, E_(a)=-780 kJ mol^(-) ...(ii) The electron affinity of an element depends upon (i) atomic size (ii) nuclear charge and (iii) electronic configuration. In general, in a group, ionisation energy and electron affinity decrease as the atomic size increases. The members of third period have some higher (e.g., S and Cl) electron affinity values than the members of second period (e.g., O and F) because second period elements have very small atomic size. Hence, there is tendency of electron-electron repulsion, which resultss in less evolution of energy in the formation of correcsponding anion. Which one of the following statements is incorrect in relation to ionisation enthalpy?

The amount of energy required to remove the most loosely bound electron from an isolated gaseous atom is called as first ionization energy (IE_(1)) . Similarly the amount of energies required to knock out second, third etc. electrons from the isolated and IE_(3)gt IE_(2)gt IE_(1) . (i) Nuclear charge (ii) Atomic size (iii) penetration effect of the electrons (iv) shielding effect of the inner electrons and (b) electronic configurations (exactly half filled and completely filled configurations are extra stable) are the important factors which affect the ionisation energies. Similarly, the amount of energy released when a neutral isolated gaseous atom accepts an extra electron to from gaseous anion is called electron affinity. (X(g)+e^(-)(g)rarr X^(-)(g)+ energy A positive elecrton affinity idicates that the ion X^(-) has a lower more negative energy than the neutral atom X. The second electron affinity for the addition of a second electron to an initially neutral atom is negative because the electron replusion outweights the nuclear attraction, e.g., O(g)+e^(-)overset("Exothermic")rarr O^(-)(g),E_(a)=+141 kJ mol^(-) ....(i) O^(-)(g)+e^(-)overset("Excothermic")rarr, E_(a)=-780 kJ mol^(-) ...(ii) The electron affinity of an element depends upon (i) atomic size (ii) nuclear charge and (iii) electronic configuration. In general, in a group, ionisation energy and electron affinity decrease as the atomic size increases. The members of third period have some higher (e.g., S and Cl) electron affinity values than the members of second period (e.g., O and F) because second period elements have very small atomic size. Hence, there is tendency of electron-electron repulsion, which resultss in less evolution of energy in the formation of correcsponding anion. Identify the least stable ion amongst the following:

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