Electron gain enthalpy increases with electro negativity. Chlorine has higher electron gain enthalpy than fluorine (exception).
JEE - 2020
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313176
Electron affinity is a
1 Relative strength to attract the shared electron pair
2 Necessary energy required to remove the electron from the ultimate orbit
3 Energy released when an electron is added to the outermost shell
4 Energy released when an electron is added to the inner shell
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313237
Which element's electronegativity is closest to that of S?
1 O
2 P
3 Cl
4 Se
Explanation:
Sulphur has electronegativity of 2.58. Selenium has electronegativity (2.55) close to 2.58 (E.N.of oxygen is \(3.5, \mathrm{P}\) is \(2.1, \mathrm{Cl}\) is 3.2 on Pauling Scale).
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313177
The correct order of electron gain enthalpy with negative sign of F, Cl, Br and I, having atomic number 9, 17, 35 and 53 respectively, is :
1 F > Cl > Br > I
2 Cl > F > Br > I
3 Br > Cl > I > F
4 I > Br > Cl > F
Explanation:
As we move down in a group electron gain enthalpy becomes less negative because the size of the atom increases and the distance of added electron from the nucleus increases. Negative electron gain enthalpy of F is less than Cl. This is due to the fact that when an electron is added to F, the added electron goes to the smaller n = 2 energy level and experiences significant repulsion from the other electrons present in this level. In Cl, the electron goes to the larger n = 3 energy level and consequently occupies a larger region of space leading to much less electron - electron repulsion. So the correct order is Cl > F > Br > I.
Electron gain enthalpy increases with electro negativity. Chlorine has higher electron gain enthalpy than fluorine (exception).
JEE - 2020
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313176
Electron affinity is a
1 Relative strength to attract the shared electron pair
2 Necessary energy required to remove the electron from the ultimate orbit
3 Energy released when an electron is added to the outermost shell
4 Energy released when an electron is added to the inner shell
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313237
Which element's electronegativity is closest to that of S?
1 O
2 P
3 Cl
4 Se
Explanation:
Sulphur has electronegativity of 2.58. Selenium has electronegativity (2.55) close to 2.58 (E.N.of oxygen is \(3.5, \mathrm{P}\) is \(2.1, \mathrm{Cl}\) is 3.2 on Pauling Scale).
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313177
The correct order of electron gain enthalpy with negative sign of F, Cl, Br and I, having atomic number 9, 17, 35 and 53 respectively, is :
1 F > Cl > Br > I
2 Cl > F > Br > I
3 Br > Cl > I > F
4 I > Br > Cl > F
Explanation:
As we move down in a group electron gain enthalpy becomes less negative because the size of the atom increases and the distance of added electron from the nucleus increases. Negative electron gain enthalpy of F is less than Cl. This is due to the fact that when an electron is added to F, the added electron goes to the smaller n = 2 energy level and experiences significant repulsion from the other electrons present in this level. In Cl, the electron goes to the larger n = 3 energy level and consequently occupies a larger region of space leading to much less electron - electron repulsion. So the correct order is Cl > F > Br > I.
Electron gain enthalpy increases with electro negativity. Chlorine has higher electron gain enthalpy than fluorine (exception).
JEE - 2020
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313176
Electron affinity is a
1 Relative strength to attract the shared electron pair
2 Necessary energy required to remove the electron from the ultimate orbit
3 Energy released when an electron is added to the outermost shell
4 Energy released when an electron is added to the inner shell
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313237
Which element's electronegativity is closest to that of S?
1 O
2 P
3 Cl
4 Se
Explanation:
Sulphur has electronegativity of 2.58. Selenium has electronegativity (2.55) close to 2.58 (E.N.of oxygen is \(3.5, \mathrm{P}\) is \(2.1, \mathrm{Cl}\) is 3.2 on Pauling Scale).
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313177
The correct order of electron gain enthalpy with negative sign of F, Cl, Br and I, having atomic number 9, 17, 35 and 53 respectively, is :
1 F > Cl > Br > I
2 Cl > F > Br > I
3 Br > Cl > I > F
4 I > Br > Cl > F
Explanation:
As we move down in a group electron gain enthalpy becomes less negative because the size of the atom increases and the distance of added electron from the nucleus increases. Negative electron gain enthalpy of F is less than Cl. This is due to the fact that when an electron is added to F, the added electron goes to the smaller n = 2 energy level and experiences significant repulsion from the other electrons present in this level. In Cl, the electron goes to the larger n = 3 energy level and consequently occupies a larger region of space leading to much less electron - electron repulsion. So the correct order is Cl > F > Br > I.
Electron gain enthalpy increases with electro negativity. Chlorine has higher electron gain enthalpy than fluorine (exception).
JEE - 2020
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313176
Electron affinity is a
1 Relative strength to attract the shared electron pair
2 Necessary energy required to remove the electron from the ultimate orbit
3 Energy released when an electron is added to the outermost shell
4 Energy released when an electron is added to the inner shell
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313237
Which element's electronegativity is closest to that of S?
1 O
2 P
3 Cl
4 Se
Explanation:
Sulphur has electronegativity of 2.58. Selenium has electronegativity (2.55) close to 2.58 (E.N.of oxygen is \(3.5, \mathrm{P}\) is \(2.1, \mathrm{Cl}\) is 3.2 on Pauling Scale).
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313177
The correct order of electron gain enthalpy with negative sign of F, Cl, Br and I, having atomic number 9, 17, 35 and 53 respectively, is :
1 F > Cl > Br > I
2 Cl > F > Br > I
3 Br > Cl > I > F
4 I > Br > Cl > F
Explanation:
As we move down in a group electron gain enthalpy becomes less negative because the size of the atom increases and the distance of added electron from the nucleus increases. Negative electron gain enthalpy of F is less than Cl. This is due to the fact that when an electron is added to F, the added electron goes to the smaller n = 2 energy level and experiences significant repulsion from the other electrons present in this level. In Cl, the electron goes to the larger n = 3 energy level and consequently occupies a larger region of space leading to much less electron - electron repulsion. So the correct order is Cl > F > Br > I.