CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313211
Which of the following has the highest electron affinity?
1 \(\mathrm{F}^{-}\)
2 \(\mathrm{O}^{2-}\)
3 \(\mathrm{O}\)
4 \(\mathrm{Na}\)
Explanation:
\(\mathrm{F}^{-}\)and \(\mathrm{O}^{2-}\) ions have stable electronic configuration, thus they will not accept further electrons, while \(\mathrm{O}\) needs electrons to achieve stable arrangement, thus it has highest electron affinity. Further, \(\mathrm{Na}\) is a metal, thus it does not have any electron affinity.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313212
Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of given atomic species?
1 F< Cl < O < S
2 S < O < Cl < F
3 O < S < F < Cl
4 Cl < F < S < O
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313213
Second electron affinity of an element is
1 Always exothermic
2 Endothermic for few elements
3 Exothermic for few elements
4 Always endothermic
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313214
Electron gain enthalpy of fluorine is less negative than chlorine, because of
1 Higher nuclear charge of chlorine
2 Smaller size of chlorine
3 Increased electron-electron repulsions in the compact 2p-subshell of fluorine
4 Higher electro negativity of fluorine.
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313215
Among the following statements, the one that is incorrect
1 Nitrogen has positive value for electron gain enthalpy
2 Greater the nuclear charge, more exothermic is the electron gain enthalpy
3 Electron gain enthalpy decreases from fluorine to iodine in the group
4 Chlorine has most negative electron gain enthalpy
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313211
Which of the following has the highest electron affinity?
1 \(\mathrm{F}^{-}\)
2 \(\mathrm{O}^{2-}\)
3 \(\mathrm{O}\)
4 \(\mathrm{Na}\)
Explanation:
\(\mathrm{F}^{-}\)and \(\mathrm{O}^{2-}\) ions have stable electronic configuration, thus they will not accept further electrons, while \(\mathrm{O}\) needs electrons to achieve stable arrangement, thus it has highest electron affinity. Further, \(\mathrm{Na}\) is a metal, thus it does not have any electron affinity.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313212
Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of given atomic species?
1 F< Cl < O < S
2 S < O < Cl < F
3 O < S < F < Cl
4 Cl < F < S < O
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313213
Second electron affinity of an element is
1 Always exothermic
2 Endothermic for few elements
3 Exothermic for few elements
4 Always endothermic
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313214
Electron gain enthalpy of fluorine is less negative than chlorine, because of
1 Higher nuclear charge of chlorine
2 Smaller size of chlorine
3 Increased electron-electron repulsions in the compact 2p-subshell of fluorine
4 Higher electro negativity of fluorine.
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313215
Among the following statements, the one that is incorrect
1 Nitrogen has positive value for electron gain enthalpy
2 Greater the nuclear charge, more exothermic is the electron gain enthalpy
3 Electron gain enthalpy decreases from fluorine to iodine in the group
4 Chlorine has most negative electron gain enthalpy
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313211
Which of the following has the highest electron affinity?
1 \(\mathrm{F}^{-}\)
2 \(\mathrm{O}^{2-}\)
3 \(\mathrm{O}\)
4 \(\mathrm{Na}\)
Explanation:
\(\mathrm{F}^{-}\)and \(\mathrm{O}^{2-}\) ions have stable electronic configuration, thus they will not accept further electrons, while \(\mathrm{O}\) needs electrons to achieve stable arrangement, thus it has highest electron affinity. Further, \(\mathrm{Na}\) is a metal, thus it does not have any electron affinity.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313212
Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of given atomic species?
1 F< Cl < O < S
2 S < O < Cl < F
3 O < S < F < Cl
4 Cl < F < S < O
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313213
Second electron affinity of an element is
1 Always exothermic
2 Endothermic for few elements
3 Exothermic for few elements
4 Always endothermic
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313214
Electron gain enthalpy of fluorine is less negative than chlorine, because of
1 Higher nuclear charge of chlorine
2 Smaller size of chlorine
3 Increased electron-electron repulsions in the compact 2p-subshell of fluorine
4 Higher electro negativity of fluorine.
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313215
Among the following statements, the one that is incorrect
1 Nitrogen has positive value for electron gain enthalpy
2 Greater the nuclear charge, more exothermic is the electron gain enthalpy
3 Electron gain enthalpy decreases from fluorine to iodine in the group
4 Chlorine has most negative electron gain enthalpy
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313211
Which of the following has the highest electron affinity?
1 \(\mathrm{F}^{-}\)
2 \(\mathrm{O}^{2-}\)
3 \(\mathrm{O}\)
4 \(\mathrm{Na}\)
Explanation:
\(\mathrm{F}^{-}\)and \(\mathrm{O}^{2-}\) ions have stable electronic configuration, thus they will not accept further electrons, while \(\mathrm{O}\) needs electrons to achieve stable arrangement, thus it has highest electron affinity. Further, \(\mathrm{Na}\) is a metal, thus it does not have any electron affinity.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313212
Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of given atomic species?
1 F< Cl < O < S
2 S < O < Cl < F
3 O < S < F < Cl
4 Cl < F < S < O
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313213
Second electron affinity of an element is
1 Always exothermic
2 Endothermic for few elements
3 Exothermic for few elements
4 Always endothermic
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313214
Electron gain enthalpy of fluorine is less negative than chlorine, because of
1 Higher nuclear charge of chlorine
2 Smaller size of chlorine
3 Increased electron-electron repulsions in the compact 2p-subshell of fluorine
4 Higher electro negativity of fluorine.
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313215
Among the following statements, the one that is incorrect
1 Nitrogen has positive value for electron gain enthalpy
2 Greater the nuclear charge, more exothermic is the electron gain enthalpy
3 Electron gain enthalpy decreases from fluorine to iodine in the group
4 Chlorine has most negative electron gain enthalpy
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313211
Which of the following has the highest electron affinity?
1 \(\mathrm{F}^{-}\)
2 \(\mathrm{O}^{2-}\)
3 \(\mathrm{O}\)
4 \(\mathrm{Na}\)
Explanation:
\(\mathrm{F}^{-}\)and \(\mathrm{O}^{2-}\) ions have stable electronic configuration, thus they will not accept further electrons, while \(\mathrm{O}\) needs electrons to achieve stable arrangement, thus it has highest electron affinity. Further, \(\mathrm{Na}\) is a metal, thus it does not have any electron affinity.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313212
Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of given atomic species?
1 F< Cl < O < S
2 S < O < Cl < F
3 O < S < F < Cl
4 Cl < F < S < O
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313213
Second electron affinity of an element is
1 Always exothermic
2 Endothermic for few elements
3 Exothermic for few elements
4 Always endothermic
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313214
Electron gain enthalpy of fluorine is less negative than chlorine, because of
1 Higher nuclear charge of chlorine
2 Smaller size of chlorine
3 Increased electron-electron repulsions in the compact 2p-subshell of fluorine
4 Higher electro negativity of fluorine.
Explanation:
Conceptual Questions
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313215
Among the following statements, the one that is incorrect
1 Nitrogen has positive value for electron gain enthalpy
2 Greater the nuclear charge, more exothermic is the electron gain enthalpy
3 Electron gain enthalpy decreases from fluorine to iodine in the group
4 Chlorine has most negative electron gain enthalpy
