Periodic Trends in Chemical Properties of Elements
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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313178 The electron gain enthalpies of halogens are as follows:
F = –332, Cl = – 349, Br = –324,
I=−295kJmol−1
The less negative value for F as compared to that of Cl is due to

1 strong electron-electron repulsions in the compact 2-p subshell of F.
2 weak electron-electron repulsions in the bigger 3-p sub shell of Cl
3 smaller electronegativity value of F than Cl
4 both (1) and (2)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313179 The formation of the oxide ion, O2−(g), from oxygen atom requires first an exothermic and then an endothermic step as shown below:
O(g)+e−→O−(g);ΔHΘ=−141kJmol−1
O−(g)+e−→O2−(g);ΔHΘ=+780kJmol−1
Thus process of formation of O2− in gas phase is unfavourable even though O2− is isoelectronic with neon. It is due to the fact that.

1 Oxygen is more electronegative.
2 Addition of electron in oxygen results in larger size of the ion.
3 Electron repulsion outweighs the stability gained by achieving noble gas configuration.
4 O− ion has comparatively smaller size than oxygen atom.
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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313180 Adding electron a neutral gaseous atom usually leads to
(i) Liberation of energy
(ii) Formation of anion
(iii) Proton/electron ratio decrease
(iv) Proton/electron ratio increase
Identify the correct statement

1 (i), (iv)
2 (ii), (iii), (iv)
3 (i), (ii), (iv)
4 (i), (ii), (iii)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313181 Which of the following species has the highest electron affinity?

1 F
2 O
3 O−
4 Na+
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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313178 The electron gain enthalpies of halogens are as follows:
F = –332, Cl = – 349, Br = –324,
I=−295kJmol−1
The less negative value for F as compared to that of Cl is due to

1 strong electron-electron repulsions in the compact 2-p subshell of F.
2 weak electron-electron repulsions in the bigger 3-p sub shell of Cl
3 smaller electronegativity value of F than Cl
4 both (1) and (2)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313179 The formation of the oxide ion, O2−(g), from oxygen atom requires first an exothermic and then an endothermic step as shown below:
O(g)+e−→O−(g);ΔHΘ=−141kJmol−1
O−(g)+e−→O2−(g);ΔHΘ=+780kJmol−1
Thus process of formation of O2− in gas phase is unfavourable even though O2− is isoelectronic with neon. It is due to the fact that.

1 Oxygen is more electronegative.
2 Addition of electron in oxygen results in larger size of the ion.
3 Electron repulsion outweighs the stability gained by achieving noble gas configuration.
4 O− ion has comparatively smaller size than oxygen atom.
NCERT Exemplar
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313180 Adding electron a neutral gaseous atom usually leads to
(i) Liberation of energy
(ii) Formation of anion
(iii) Proton/electron ratio decrease
(iv) Proton/electron ratio increase
Identify the correct statement

1 (i), (iv)
2 (ii), (iii), (iv)
3 (i), (ii), (iv)
4 (i), (ii), (iii)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313181 Which of the following species has the highest electron affinity?

1 F
2 O
3 O−
4 Na+
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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313178 The electron gain enthalpies of halogens are as follows:
F = –332, Cl = – 349, Br = –324,
I=−295kJmol−1
The less negative value for F as compared to that of Cl is due to

1 strong electron-electron repulsions in the compact 2-p subshell of F.
2 weak electron-electron repulsions in the bigger 3-p sub shell of Cl
3 smaller electronegativity value of F than Cl
4 both (1) and (2)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313179 The formation of the oxide ion, O2−(g), from oxygen atom requires first an exothermic and then an endothermic step as shown below:
O(g)+e−→O−(g);ΔHΘ=−141kJmol−1
O−(g)+e−→O2−(g);ΔHΘ=+780kJmol−1
Thus process of formation of O2− in gas phase is unfavourable even though O2− is isoelectronic with neon. It is due to the fact that.

1 Oxygen is more electronegative.
2 Addition of electron in oxygen results in larger size of the ion.
3 Electron repulsion outweighs the stability gained by achieving noble gas configuration.
4 O− ion has comparatively smaller size than oxygen atom.
NCERT Exemplar
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313180 Adding electron a neutral gaseous atom usually leads to
(i) Liberation of energy
(ii) Formation of anion
(iii) Proton/electron ratio decrease
(iv) Proton/electron ratio increase
Identify the correct statement

1 (i), (iv)
2 (ii), (iii), (iv)
3 (i), (ii), (iv)
4 (i), (ii), (iii)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313181 Which of the following species has the highest electron affinity?

1 F
2 O
3 O−
4 Na+
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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313178 The electron gain enthalpies of halogens are as follows:
F = –332, Cl = – 349, Br = –324,
I=−295kJmol−1
The less negative value for F as compared to that of Cl is due to

1 strong electron-electron repulsions in the compact 2-p subshell of F.
2 weak electron-electron repulsions in the bigger 3-p sub shell of Cl
3 smaller electronegativity value of F than Cl
4 both (1) and (2)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313179 The formation of the oxide ion, O2−(g), from oxygen atom requires first an exothermic and then an endothermic step as shown below:
O(g)+e−→O−(g);ΔHΘ=−141kJmol−1
O−(g)+e−→O2−(g);ΔHΘ=+780kJmol−1
Thus process of formation of O2− in gas phase is unfavourable even though O2− is isoelectronic with neon. It is due to the fact that.

1 Oxygen is more electronegative.
2 Addition of electron in oxygen results in larger size of the ion.
3 Electron repulsion outweighs the stability gained by achieving noble gas configuration.
4 O− ion has comparatively smaller size than oxygen atom.
NCERT Exemplar
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313180 Adding electron a neutral gaseous atom usually leads to
(i) Liberation of energy
(ii) Formation of anion
(iii) Proton/electron ratio decrease
(iv) Proton/electron ratio increase
Identify the correct statement

1 (i), (iv)
2 (ii), (iii), (iv)
3 (i), (ii), (iv)
4 (i), (ii), (iii)
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313181 Which of the following species has the highest electron affinity?

1 F
2 O
3 O−
4 Na+
NEET DIGITAL LIBRARY