Home
Class 11
CHEMISTRY
(N(A))/(2) atoms of X(g) are converted ...

`(N_(A))/(2)` atoms of `X_(g)` are converted into `X_((g))^(+)` by energy `E_(1)` .
`(N_(A))/(2)` atoms of `X_((g))` are converted into `X_((g))^(-)` by energy `E_(2)`. Hence, ionisation potential and electron affinity of `X_((g))` are respectively

A

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

B

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

C

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

D

none is correct

Text Solution

Verified by Experts

The correct Answer is:
B

`(E_(1))/(N_(A)), (2E_(2))/(N_(A))`
Promotional Banner

Similar Questions

Explore conceptually related problems

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 :

The ionisation potential of X_((g))^(-) is numerically equal to

Metals have few electrons in their valence shell while non-metals generally have more electrons in their valence shell. Metallic character is closely related to atomic radius and ionisation enthalpy. Metallic character increases from top to bottom in a group and decreases from let to right in a period of periodic table. metallic character is inversely related to electronegativity of element. Q. 3 N_0//2 atoms of X_((g))^(-) by energy E_(2) . hence, ionisation potential and electron affinity of X_((g)) are: ( N_(0) =Avogadro's number)

X_((g))+e rarr X_((g))^(-) +E , Here ''E'' is

If you are given Avogadro's number of atoms of a gas X . If half of the atoms are converted into X_(g)^(+) by energy Delta H . The IE of X is

The value of int_1^2 {f(g(x))}^(-1)f'(g(x))g'(x) dx , where g(1)=g(2), is equal to

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: