Classification of Elements and Periodicity in Properties
89702
Which one of the following ionic species has the greatest proton affinity to form stable compound?
1 $\mathrm{NH}_2$
2 $\mathrm{F}^{-}$
3 $\mathrm{I}^{-}$
4 $\mathrm{HS}^{-}$
Explanation:
Proton affinity decreases across a period from left to right and down a group from top to bottom. Hence, the nitrogen family has highest proton followed by oxygen family, followed by halogen. Also the ionic pieces with greatest proton affinity form the strongest base. Therefore, $\mathrm{NH}_2^{-}$has the greatest proton affinity to form a stable compound.
BCECE-2012
Classification of Elements and Periodicity in Properties
89706
Electron affinity is positive when
1 $\mathrm{O}^{-}$is formed from $\mathrm{O}$
2 $\mathrm{O}^{2-}$ is formed from $\mathrm{O}^{-}$
3 $\mathrm{O}^{+}$is formed from $\mathrm{O}$
4 electron affinity is always a negative value
Explanation:
When $\mathrm{O}^{2-}$ formed from $\mathrm{O}^{-}$, change is endothermic because $\mathrm{O}^{-}$repels the incoming electron due to similar charge. Therefore, it needs energy to accept the electron. The second electron affinity of oxygen is particularly high because the electron is being forced into a small, very dense electron. Hence, the electron affinity is positive.
CG PET- 2013
Classification of Elements and Periodicity in Properties
89707
Which of the following elements has the highest value of electron affinity?
1 $\mathrm{O}$
2 $\mathrm{S}$
3 $\mathrm{Se}$
4 $\mathrm{Te}$
Explanation:
Oxygen has exceptionally smaller value of electron affinity $(-141 \mathrm{~kJ})$ due to smaller atomic size then sulphur. Hence $S$ is highest value of electron affinity.
BCECE-2010
Classification of Elements and Periodicity in Properties
89708
What is the value of electron gain enthalpy of $\mathrm{Na}^{+}$if $\mathrm{IE}_1$ of $\mathrm{Na}=5.1 \mathrm{eV}$ ?
1 $-5.1 \mathrm{eV}$
2 $-10.2 \mathrm{eV}$
3 $+2.55 \mathrm{eV}$
4 $+10.2 \mathrm{eV}$
Explanation:
Given that, Ionisation enthalpy of $\mathrm{Na}=5.1 \mathrm{eV}$ Thus, the electron gain enthalpy of sodium cation is equal in magnitude and opposite in sign to the first ionization energy of sodium atom. It is equal to -5.1 $\mathrm{eV}$.
Classification of Elements and Periodicity in Properties
89702
Which one of the following ionic species has the greatest proton affinity to form stable compound?
1 $\mathrm{NH}_2$
2 $\mathrm{F}^{-}$
3 $\mathrm{I}^{-}$
4 $\mathrm{HS}^{-}$
Explanation:
Proton affinity decreases across a period from left to right and down a group from top to bottom. Hence, the nitrogen family has highest proton followed by oxygen family, followed by halogen. Also the ionic pieces with greatest proton affinity form the strongest base. Therefore, $\mathrm{NH}_2^{-}$has the greatest proton affinity to form a stable compound.
BCECE-2012
Classification of Elements and Periodicity in Properties
89706
Electron affinity is positive when
1 $\mathrm{O}^{-}$is formed from $\mathrm{O}$
2 $\mathrm{O}^{2-}$ is formed from $\mathrm{O}^{-}$
3 $\mathrm{O}^{+}$is formed from $\mathrm{O}$
4 electron affinity is always a negative value
Explanation:
When $\mathrm{O}^{2-}$ formed from $\mathrm{O}^{-}$, change is endothermic because $\mathrm{O}^{-}$repels the incoming electron due to similar charge. Therefore, it needs energy to accept the electron. The second electron affinity of oxygen is particularly high because the electron is being forced into a small, very dense electron. Hence, the electron affinity is positive.
CG PET- 2013
Classification of Elements and Periodicity in Properties
89707
Which of the following elements has the highest value of electron affinity?
1 $\mathrm{O}$
2 $\mathrm{S}$
3 $\mathrm{Se}$
4 $\mathrm{Te}$
Explanation:
Oxygen has exceptionally smaller value of electron affinity $(-141 \mathrm{~kJ})$ due to smaller atomic size then sulphur. Hence $S$ is highest value of electron affinity.
BCECE-2010
Classification of Elements and Periodicity in Properties
89708
What is the value of electron gain enthalpy of $\mathrm{Na}^{+}$if $\mathrm{IE}_1$ of $\mathrm{Na}=5.1 \mathrm{eV}$ ?
1 $-5.1 \mathrm{eV}$
2 $-10.2 \mathrm{eV}$
3 $+2.55 \mathrm{eV}$
4 $+10.2 \mathrm{eV}$
Explanation:
Given that, Ionisation enthalpy of $\mathrm{Na}=5.1 \mathrm{eV}$ Thus, the electron gain enthalpy of sodium cation is equal in magnitude and opposite in sign to the first ionization energy of sodium atom. It is equal to -5.1 $\mathrm{eV}$.
Classification of Elements and Periodicity in Properties
89702
Which one of the following ionic species has the greatest proton affinity to form stable compound?
1 $\mathrm{NH}_2$
2 $\mathrm{F}^{-}$
3 $\mathrm{I}^{-}$
4 $\mathrm{HS}^{-}$
Explanation:
Proton affinity decreases across a period from left to right and down a group from top to bottom. Hence, the nitrogen family has highest proton followed by oxygen family, followed by halogen. Also the ionic pieces with greatest proton affinity form the strongest base. Therefore, $\mathrm{NH}_2^{-}$has the greatest proton affinity to form a stable compound.
BCECE-2012
Classification of Elements and Periodicity in Properties
89706
Electron affinity is positive when
1 $\mathrm{O}^{-}$is formed from $\mathrm{O}$
2 $\mathrm{O}^{2-}$ is formed from $\mathrm{O}^{-}$
3 $\mathrm{O}^{+}$is formed from $\mathrm{O}$
4 electron affinity is always a negative value
Explanation:
When $\mathrm{O}^{2-}$ formed from $\mathrm{O}^{-}$, change is endothermic because $\mathrm{O}^{-}$repels the incoming electron due to similar charge. Therefore, it needs energy to accept the electron. The second electron affinity of oxygen is particularly high because the electron is being forced into a small, very dense electron. Hence, the electron affinity is positive.
CG PET- 2013
Classification of Elements and Periodicity in Properties
89707
Which of the following elements has the highest value of electron affinity?
1 $\mathrm{O}$
2 $\mathrm{S}$
3 $\mathrm{Se}$
4 $\mathrm{Te}$
Explanation:
Oxygen has exceptionally smaller value of electron affinity $(-141 \mathrm{~kJ})$ due to smaller atomic size then sulphur. Hence $S$ is highest value of electron affinity.
BCECE-2010
Classification of Elements and Periodicity in Properties
89708
What is the value of electron gain enthalpy of $\mathrm{Na}^{+}$if $\mathrm{IE}_1$ of $\mathrm{Na}=5.1 \mathrm{eV}$ ?
1 $-5.1 \mathrm{eV}$
2 $-10.2 \mathrm{eV}$
3 $+2.55 \mathrm{eV}$
4 $+10.2 \mathrm{eV}$
Explanation:
Given that, Ionisation enthalpy of $\mathrm{Na}=5.1 \mathrm{eV}$ Thus, the electron gain enthalpy of sodium cation is equal in magnitude and opposite in sign to the first ionization energy of sodium atom. It is equal to -5.1 $\mathrm{eV}$.
Classification of Elements and Periodicity in Properties
89702
Which one of the following ionic species has the greatest proton affinity to form stable compound?
1 $\mathrm{NH}_2$
2 $\mathrm{F}^{-}$
3 $\mathrm{I}^{-}$
4 $\mathrm{HS}^{-}$
Explanation:
Proton affinity decreases across a period from left to right and down a group from top to bottom. Hence, the nitrogen family has highest proton followed by oxygen family, followed by halogen. Also the ionic pieces with greatest proton affinity form the strongest base. Therefore, $\mathrm{NH}_2^{-}$has the greatest proton affinity to form a stable compound.
BCECE-2012
Classification of Elements and Periodicity in Properties
89706
Electron affinity is positive when
1 $\mathrm{O}^{-}$is formed from $\mathrm{O}$
2 $\mathrm{O}^{2-}$ is formed from $\mathrm{O}^{-}$
3 $\mathrm{O}^{+}$is formed from $\mathrm{O}$
4 electron affinity is always a negative value
Explanation:
When $\mathrm{O}^{2-}$ formed from $\mathrm{O}^{-}$, change is endothermic because $\mathrm{O}^{-}$repels the incoming electron due to similar charge. Therefore, it needs energy to accept the electron. The second electron affinity of oxygen is particularly high because the electron is being forced into a small, very dense electron. Hence, the electron affinity is positive.
CG PET- 2013
Classification of Elements and Periodicity in Properties
89707
Which of the following elements has the highest value of electron affinity?
1 $\mathrm{O}$
2 $\mathrm{S}$
3 $\mathrm{Se}$
4 $\mathrm{Te}$
Explanation:
Oxygen has exceptionally smaller value of electron affinity $(-141 \mathrm{~kJ})$ due to smaller atomic size then sulphur. Hence $S$ is highest value of electron affinity.
BCECE-2010
Classification of Elements and Periodicity in Properties
89708
What is the value of electron gain enthalpy of $\mathrm{Na}^{+}$if $\mathrm{IE}_1$ of $\mathrm{Na}=5.1 \mathrm{eV}$ ?
1 $-5.1 \mathrm{eV}$
2 $-10.2 \mathrm{eV}$
3 $+2.55 \mathrm{eV}$
4 $+10.2 \mathrm{eV}$
Explanation:
Given that, Ionisation enthalpy of $\mathrm{Na}=5.1 \mathrm{eV}$ Thus, the electron gain enthalpy of sodium cation is equal in magnitude and opposite in sign to the first ionization energy of sodium atom. It is equal to -5.1 $\mathrm{eV}$.
