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

`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 :

A

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

B

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

C

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

D

None is correct

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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)

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 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:

Statement-1: First ionisation energy of O^(+)(g) is greater than that of N(g) whereas vice versa is true for the first ionisation energy of N^(+)(g) and N(g) respectively. Statement-2: Electronic configuration of N(g) is more stable than that of N^(+)(g) .

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NTA MOCK TESTS-NEET MOCK TEST 10-CHEMISTRY
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  2. Which of the following is NOT a transquilizer ?

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  3. N(0)//2 atoms of X(g) are converted into X^(+) (g) by energy E(1) . N(...

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  4. Nitrogen forms N(2) but phosphorus forms P(4) due to

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  6. The correct order in which the O-O bond length increases in the follow...

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  7. The seqeunce of ionic mobility in the aqueous solution is

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  8. For which of the following van't Hoff factor cannot be greater than un...

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  9. Which of the following exhibits tautomerism ?

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  10. Among the following solids, Schottky defect is NOT observed in-

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  11. Which of the following relations gives the value of n =

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  12. The following data is obtained during the first order thermal decompos...

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  13. Which of the follwing is the most basic oxide?

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  14. When

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  15. The best reagent to convert pent-3-en-2-ol into pent-3-en-2-one is

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  16. On oxidation of S(2)O(3)^(2-) by MnO(4)^(-) in neutral aqueous medium,...

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  17. Consider the reaction 2NO(g) + O(2)(g) rarr 2NO(2)(g), Predict wheth...

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  20. [X]+H(2)SO(4) rarr [Y] a colourless gas with irritating smell [Y] + K(...

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