Classification of Elements and Periodicity in Properties
89713
The first electron affinity of $C, N$ and $O$ will be of the order
1 $\mathrm{C}<\mathrm{N}<\mathrm{O}$
2 $\mathrm{N}<\mathrm{C}<\mathrm{O}$
3 $\mathrm{C}<\mathrm{O}<\mathrm{N}$
4 $\mathrm{O}<\mathrm{N}<\mathrm{C}$
Explanation:
The electron affinity of an atom or molecules can be defined as the amount of energy released when an electron is attached or gained by an electrically neutral atom. Nitrogen has a stable half-filled p-orbital. Thus, the correct order of first electron affinity of $\mathrm{C}, \mathrm{N}$ and $\mathrm{O}$ will be $$ \mathrm{N}<\mathrm{C}<\mathrm{O} $$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89716
Which of the following has the highest electron affinity?
1 $\mathrm{K}$
2 $\mathrm{O}^{-}$
3 $\mathrm{F}^{-}$
4 $\mathrm{O}$
Explanation:
Electron affinity is defined as the minimum energy released electron add to the valence shell of isolated atom. $\text { Electron affinity } \propto \frac{1}{\text { size }}$ Therefore, $\mathrm{O}^{-}$has less electron affinity due to complete the shell to form stable configuration but in case of oxygen has high electron affinity.
Manipal-2016
Classification of Elements and Periodicity in Properties
89717
Among $P, S, C l, F$, the elements with most negative and least negative electron gain enthalpy respectively are
1 $\mathrm{Cl}, \mathrm{S}$
2 F, S
3 $\mathrm{Cl}, \mathrm{P}$
4 F, P
Explanation:
On moving from left to right in a period generally electron gain enthalpy increases and decrease down the group. But the electron affinity of third period is greater than the electron affinity of second period element due to small atomic size of second period element. Hence, the order is $\mathrm{P}<\mathrm{S}<\mathrm{F}<\mathrm{Cl}$ Therefore, $\mathrm{Cl}$ and $\mathrm{P}$ has more negative and less negative electron gain enthalpy respectively.
J and K CET-(2015)
Classification of Elements and Periodicity in Properties
89721
Which one of the following arrangement represents the correct order of least negative to most negative electron gain enthalpy for $\mathrm{C}$, Ca, Al, $F$ and $O$ ?
The nuclear charge increases, the force of attraction between the nucleus and the incoming electron increase and thus, the electron gain enthalpy becomes more negative. On moving from left to right in a period, the effective nuclear charge increases. Therefore, the order are- $\mathrm{Ca}<\mathrm{Al}<\mathrm{C}<\mathrm{O}<\mathrm{F}$
Karnataka NEET-2013
Classification of Elements and Periodicity in Properties
89728
Which one of the following statements is false
1 The electron affinity of chlorine is less than that of fluorine
2 The electronegativity of fluorine is more than that of chlorine
3 The electron affinity of bromine is less than that of chlorine
4 The electronegativity of chlorine is more than that of bromine
Explanation:
(i) The electron affinity of chlorine is greater than the fluorine. (ii) The $\mathrm{EN}$ of fluorine is greater than chlorine. (iii) The electron affinity of bromine is less than of chlorine. (iv) The electronegative of Chlorine is more than that of bromine.
Classification of Elements and Periodicity in Properties
89713
The first electron affinity of $C, N$ and $O$ will be of the order
1 $\mathrm{C}<\mathrm{N}<\mathrm{O}$
2 $\mathrm{N}<\mathrm{C}<\mathrm{O}$
3 $\mathrm{C}<\mathrm{O}<\mathrm{N}$
4 $\mathrm{O}<\mathrm{N}<\mathrm{C}$
Explanation:
The electron affinity of an atom or molecules can be defined as the amount of energy released when an electron is attached or gained by an electrically neutral atom. Nitrogen has a stable half-filled p-orbital. Thus, the correct order of first electron affinity of $\mathrm{C}, \mathrm{N}$ and $\mathrm{O}$ will be $$ \mathrm{N}<\mathrm{C}<\mathrm{O} $$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89716
Which of the following has the highest electron affinity?
1 $\mathrm{K}$
2 $\mathrm{O}^{-}$
3 $\mathrm{F}^{-}$
4 $\mathrm{O}$
Explanation:
Electron affinity is defined as the minimum energy released electron add to the valence shell of isolated atom. $\text { Electron affinity } \propto \frac{1}{\text { size }}$ Therefore, $\mathrm{O}^{-}$has less electron affinity due to complete the shell to form stable configuration but in case of oxygen has high electron affinity.
Manipal-2016
Classification of Elements and Periodicity in Properties
89717
Among $P, S, C l, F$, the elements with most negative and least negative electron gain enthalpy respectively are
1 $\mathrm{Cl}, \mathrm{S}$
2 F, S
3 $\mathrm{Cl}, \mathrm{P}$
4 F, P
Explanation:
On moving from left to right in a period generally electron gain enthalpy increases and decrease down the group. But the electron affinity of third period is greater than the electron affinity of second period element due to small atomic size of second period element. Hence, the order is $\mathrm{P}<\mathrm{S}<\mathrm{F}<\mathrm{Cl}$ Therefore, $\mathrm{Cl}$ and $\mathrm{P}$ has more negative and less negative electron gain enthalpy respectively.
J and K CET-(2015)
Classification of Elements and Periodicity in Properties
89721
Which one of the following arrangement represents the correct order of least negative to most negative electron gain enthalpy for $\mathrm{C}$, Ca, Al, $F$ and $O$ ?
The nuclear charge increases, the force of attraction between the nucleus and the incoming electron increase and thus, the electron gain enthalpy becomes more negative. On moving from left to right in a period, the effective nuclear charge increases. Therefore, the order are- $\mathrm{Ca}<\mathrm{Al}<\mathrm{C}<\mathrm{O}<\mathrm{F}$
Karnataka NEET-2013
Classification of Elements and Periodicity in Properties
89728
Which one of the following statements is false
1 The electron affinity of chlorine is less than that of fluorine
2 The electronegativity of fluorine is more than that of chlorine
3 The electron affinity of bromine is less than that of chlorine
4 The electronegativity of chlorine is more than that of bromine
Explanation:
(i) The electron affinity of chlorine is greater than the fluorine. (ii) The $\mathrm{EN}$ of fluorine is greater than chlorine. (iii) The electron affinity of bromine is less than of chlorine. (iv) The electronegative of Chlorine is more than that of bromine.
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Classification of Elements and Periodicity in Properties
89713
The first electron affinity of $C, N$ and $O$ will be of the order
1 $\mathrm{C}<\mathrm{N}<\mathrm{O}$
2 $\mathrm{N}<\mathrm{C}<\mathrm{O}$
3 $\mathrm{C}<\mathrm{O}<\mathrm{N}$
4 $\mathrm{O}<\mathrm{N}<\mathrm{C}$
Explanation:
The electron affinity of an atom or molecules can be defined as the amount of energy released when an electron is attached or gained by an electrically neutral atom. Nitrogen has a stable half-filled p-orbital. Thus, the correct order of first electron affinity of $\mathrm{C}, \mathrm{N}$ and $\mathrm{O}$ will be $$ \mathrm{N}<\mathrm{C}<\mathrm{O} $$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89716
Which of the following has the highest electron affinity?
1 $\mathrm{K}$
2 $\mathrm{O}^{-}$
3 $\mathrm{F}^{-}$
4 $\mathrm{O}$
Explanation:
Electron affinity is defined as the minimum energy released electron add to the valence shell of isolated atom. $\text { Electron affinity } \propto \frac{1}{\text { size }}$ Therefore, $\mathrm{O}^{-}$has less electron affinity due to complete the shell to form stable configuration but in case of oxygen has high electron affinity.
Manipal-2016
Classification of Elements and Periodicity in Properties
89717
Among $P, S, C l, F$, the elements with most negative and least negative electron gain enthalpy respectively are
1 $\mathrm{Cl}, \mathrm{S}$
2 F, S
3 $\mathrm{Cl}, \mathrm{P}$
4 F, P
Explanation:
On moving from left to right in a period generally electron gain enthalpy increases and decrease down the group. But the electron affinity of third period is greater than the electron affinity of second period element due to small atomic size of second period element. Hence, the order is $\mathrm{P}<\mathrm{S}<\mathrm{F}<\mathrm{Cl}$ Therefore, $\mathrm{Cl}$ and $\mathrm{P}$ has more negative and less negative electron gain enthalpy respectively.
J and K CET-(2015)
Classification of Elements and Periodicity in Properties
89721
Which one of the following arrangement represents the correct order of least negative to most negative electron gain enthalpy for $\mathrm{C}$, Ca, Al, $F$ and $O$ ?
The nuclear charge increases, the force of attraction between the nucleus and the incoming electron increase and thus, the electron gain enthalpy becomes more negative. On moving from left to right in a period, the effective nuclear charge increases. Therefore, the order are- $\mathrm{Ca}<\mathrm{Al}<\mathrm{C}<\mathrm{O}<\mathrm{F}$
Karnataka NEET-2013
Classification of Elements and Periodicity in Properties
89728
Which one of the following statements is false
1 The electron affinity of chlorine is less than that of fluorine
2 The electronegativity of fluorine is more than that of chlorine
3 The electron affinity of bromine is less than that of chlorine
4 The electronegativity of chlorine is more than that of bromine
Explanation:
(i) The electron affinity of chlorine is greater than the fluorine. (ii) The $\mathrm{EN}$ of fluorine is greater than chlorine. (iii) The electron affinity of bromine is less than of chlorine. (iv) The electronegative of Chlorine is more than that of bromine.
Classification of Elements and Periodicity in Properties
89713
The first electron affinity of $C, N$ and $O$ will be of the order
1 $\mathrm{C}<\mathrm{N}<\mathrm{O}$
2 $\mathrm{N}<\mathrm{C}<\mathrm{O}$
3 $\mathrm{C}<\mathrm{O}<\mathrm{N}$
4 $\mathrm{O}<\mathrm{N}<\mathrm{C}$
Explanation:
The electron affinity of an atom or molecules can be defined as the amount of energy released when an electron is attached or gained by an electrically neutral atom. Nitrogen has a stable half-filled p-orbital. Thus, the correct order of first electron affinity of $\mathrm{C}, \mathrm{N}$ and $\mathrm{O}$ will be $$ \mathrm{N}<\mathrm{C}<\mathrm{O} $$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89716
Which of the following has the highest electron affinity?
1 $\mathrm{K}$
2 $\mathrm{O}^{-}$
3 $\mathrm{F}^{-}$
4 $\mathrm{O}$
Explanation:
Electron affinity is defined as the minimum energy released electron add to the valence shell of isolated atom. $\text { Electron affinity } \propto \frac{1}{\text { size }}$ Therefore, $\mathrm{O}^{-}$has less electron affinity due to complete the shell to form stable configuration but in case of oxygen has high electron affinity.
Manipal-2016
Classification of Elements and Periodicity in Properties
89717
Among $P, S, C l, F$, the elements with most negative and least negative electron gain enthalpy respectively are
1 $\mathrm{Cl}, \mathrm{S}$
2 F, S
3 $\mathrm{Cl}, \mathrm{P}$
4 F, P
Explanation:
On moving from left to right in a period generally electron gain enthalpy increases and decrease down the group. But the electron affinity of third period is greater than the electron affinity of second period element due to small atomic size of second period element. Hence, the order is $\mathrm{P}<\mathrm{S}<\mathrm{F}<\mathrm{Cl}$ Therefore, $\mathrm{Cl}$ and $\mathrm{P}$ has more negative and less negative electron gain enthalpy respectively.
J and K CET-(2015)
Classification of Elements and Periodicity in Properties
89721
Which one of the following arrangement represents the correct order of least negative to most negative electron gain enthalpy for $\mathrm{C}$, Ca, Al, $F$ and $O$ ?
The nuclear charge increases, the force of attraction between the nucleus and the incoming electron increase and thus, the electron gain enthalpy becomes more negative. On moving from left to right in a period, the effective nuclear charge increases. Therefore, the order are- $\mathrm{Ca}<\mathrm{Al}<\mathrm{C}<\mathrm{O}<\mathrm{F}$
Karnataka NEET-2013
Classification of Elements and Periodicity in Properties
89728
Which one of the following statements is false
1 The electron affinity of chlorine is less than that of fluorine
2 The electronegativity of fluorine is more than that of chlorine
3 The electron affinity of bromine is less than that of chlorine
4 The electronegativity of chlorine is more than that of bromine
Explanation:
(i) The electron affinity of chlorine is greater than the fluorine. (ii) The $\mathrm{EN}$ of fluorine is greater than chlorine. (iii) The electron affinity of bromine is less than of chlorine. (iv) The electronegative of Chlorine is more than that of bromine.
Classification of Elements and Periodicity in Properties
89713
The first electron affinity of $C, N$ and $O$ will be of the order
1 $\mathrm{C}<\mathrm{N}<\mathrm{O}$
2 $\mathrm{N}<\mathrm{C}<\mathrm{O}$
3 $\mathrm{C}<\mathrm{O}<\mathrm{N}$
4 $\mathrm{O}<\mathrm{N}<\mathrm{C}$
Explanation:
The electron affinity of an atom or molecules can be defined as the amount of energy released when an electron is attached or gained by an electrically neutral atom. Nitrogen has a stable half-filled p-orbital. Thus, the correct order of first electron affinity of $\mathrm{C}, \mathrm{N}$ and $\mathrm{O}$ will be $$ \mathrm{N}<\mathrm{C}<\mathrm{O} $$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89716
Which of the following has the highest electron affinity?
1 $\mathrm{K}$
2 $\mathrm{O}^{-}$
3 $\mathrm{F}^{-}$
4 $\mathrm{O}$
Explanation:
Electron affinity is defined as the minimum energy released electron add to the valence shell of isolated atom. $\text { Electron affinity } \propto \frac{1}{\text { size }}$ Therefore, $\mathrm{O}^{-}$has less electron affinity due to complete the shell to form stable configuration but in case of oxygen has high electron affinity.
Manipal-2016
Classification of Elements and Periodicity in Properties
89717
Among $P, S, C l, F$, the elements with most negative and least negative electron gain enthalpy respectively are
1 $\mathrm{Cl}, \mathrm{S}$
2 F, S
3 $\mathrm{Cl}, \mathrm{P}$
4 F, P
Explanation:
On moving from left to right in a period generally electron gain enthalpy increases and decrease down the group. But the electron affinity of third period is greater than the electron affinity of second period element due to small atomic size of second period element. Hence, the order is $\mathrm{P}<\mathrm{S}<\mathrm{F}<\mathrm{Cl}$ Therefore, $\mathrm{Cl}$ and $\mathrm{P}$ has more negative and less negative electron gain enthalpy respectively.
J and K CET-(2015)
Classification of Elements and Periodicity in Properties
89721
Which one of the following arrangement represents the correct order of least negative to most negative electron gain enthalpy for $\mathrm{C}$, Ca, Al, $F$ and $O$ ?
The nuclear charge increases, the force of attraction between the nucleus and the incoming electron increase and thus, the electron gain enthalpy becomes more negative. On moving from left to right in a period, the effective nuclear charge increases. Therefore, the order are- $\mathrm{Ca}<\mathrm{Al}<\mathrm{C}<\mathrm{O}<\mathrm{F}$
Karnataka NEET-2013
Classification of Elements and Periodicity in Properties
89728
Which one of the following statements is false
1 The electron affinity of chlorine is less than that of fluorine
2 The electronegativity of fluorine is more than that of chlorine
3 The electron affinity of bromine is less than that of chlorine
4 The electronegativity of chlorine is more than that of bromine
Explanation:
(i) The electron affinity of chlorine is greater than the fluorine. (ii) The $\mathrm{EN}$ of fluorine is greater than chlorine. (iii) The electron affinity of bromine is less than of chlorine. (iv) The electronegative of Chlorine is more than that of bromine.