Classification of Elements and Periodicity in Properties
89649
The pair of elements having approximately equal ionization potential is
1 $\mathrm{Al}, \mathrm{Ga}$
2 $\mathrm{Al}, \mathrm{Si}$
3 $\mathrm{Al}, \mathrm{Mg}$
4 Al, B
Explanation:
The pair of elements having approximately equal ionisaiton energy is $\mathrm{Al}$ and $\mathrm{Ga}$. Ionisation energy increases with a decreases in atomic size and due to the increase in the shielding effect of inner electrons.
UPTU/UPSEE-2009
Classification of Elements and Periodicity in Properties
89650
The ionisation energy of nitrogen is larger than that of oxygen because of
1 greater attraction of electons by the nucleus
2 the size of the nitrogen atom being smaller
3 the half-filled p-orbitals possess extra stability
4 greater penetration effect.
Explanation:
The ionisation energy of nitrogen is larger than of oxygen because of nitrogen has half-filled porbital is more stable thus, it is difficult to remove an electron from it. Hence nitrogen has larger ionisation energy than oxygen.
SRMJEEE - 2008
Classification of Elements and Periodicity in Properties
89651
The first ionization potential of $\mathrm{Al}$, as compared to that of $\mathrm{Mg}$ is :
1 Greater
2 Lower
3 The same
4 Twice as much
Explanation:
The first ionization potential of $\mathrm{Al}$ is lower than that of $\mathrm{Mg}$ because valence shell configuration of $\mathrm{Mg}$ is $3 \mathrm{~s}^2$ and of $\mathrm{Al}$ is $3 \mathrm{~s}^2, 3 \mathrm{p}^1$. As s-orbital is close to nucleus than p-orbital. So removal of $1 \mathrm{st}^{-}$from $\mathrm{Mg}$ is difficult and require more energy as compare to $\mathrm{Al}$.
BITSAT 2008
Classification of Elements and Periodicity in Properties
89652
The first ionization energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?
1 Lesser effective nuclear charge of oxygen then nitrogen
2 Lesser atomic size of oxygen than nitrogen
3 Greater interelectron repulsion between two electrons in the same p-orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen
4 Greater effective nuclear charge of oxygen than nitrogen
5 Higher electronegativity of oxygen than Nitrogen
Explanation:
The first ionization energy of oxygen is less than that of nitrogen because we move from left to right in a period atomic size decrease and ionization energy will be increased due to greater effective nuclear charge of oxygen than nitrogen.
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Classification of Elements and Periodicity in Properties
89649
The pair of elements having approximately equal ionization potential is
1 $\mathrm{Al}, \mathrm{Ga}$
2 $\mathrm{Al}, \mathrm{Si}$
3 $\mathrm{Al}, \mathrm{Mg}$
4 Al, B
Explanation:
The pair of elements having approximately equal ionisaiton energy is $\mathrm{Al}$ and $\mathrm{Ga}$. Ionisation energy increases with a decreases in atomic size and due to the increase in the shielding effect of inner electrons.
UPTU/UPSEE-2009
Classification of Elements and Periodicity in Properties
89650
The ionisation energy of nitrogen is larger than that of oxygen because of
1 greater attraction of electons by the nucleus
2 the size of the nitrogen atom being smaller
3 the half-filled p-orbitals possess extra stability
4 greater penetration effect.
Explanation:
The ionisation energy of nitrogen is larger than of oxygen because of nitrogen has half-filled porbital is more stable thus, it is difficult to remove an electron from it. Hence nitrogen has larger ionisation energy than oxygen.
SRMJEEE - 2008
Classification of Elements and Periodicity in Properties
89651
The first ionization potential of $\mathrm{Al}$, as compared to that of $\mathrm{Mg}$ is :
1 Greater
2 Lower
3 The same
4 Twice as much
Explanation:
The first ionization potential of $\mathrm{Al}$ is lower than that of $\mathrm{Mg}$ because valence shell configuration of $\mathrm{Mg}$ is $3 \mathrm{~s}^2$ and of $\mathrm{Al}$ is $3 \mathrm{~s}^2, 3 \mathrm{p}^1$. As s-orbital is close to nucleus than p-orbital. So removal of $1 \mathrm{st}^{-}$from $\mathrm{Mg}$ is difficult and require more energy as compare to $\mathrm{Al}$.
BITSAT 2008
Classification of Elements and Periodicity in Properties
89652
The first ionization energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?
1 Lesser effective nuclear charge of oxygen then nitrogen
2 Lesser atomic size of oxygen than nitrogen
3 Greater interelectron repulsion between two electrons in the same p-orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen
4 Greater effective nuclear charge of oxygen than nitrogen
5 Higher electronegativity of oxygen than Nitrogen
Explanation:
The first ionization energy of oxygen is less than that of nitrogen because we move from left to right in a period atomic size decrease and ionization energy will be increased due to greater effective nuclear charge of oxygen than nitrogen.
Classification of Elements and Periodicity in Properties
89649
The pair of elements having approximately equal ionization potential is
1 $\mathrm{Al}, \mathrm{Ga}$
2 $\mathrm{Al}, \mathrm{Si}$
3 $\mathrm{Al}, \mathrm{Mg}$
4 Al, B
Explanation:
The pair of elements having approximately equal ionisaiton energy is $\mathrm{Al}$ and $\mathrm{Ga}$. Ionisation energy increases with a decreases in atomic size and due to the increase in the shielding effect of inner electrons.
UPTU/UPSEE-2009
Classification of Elements and Periodicity in Properties
89650
The ionisation energy of nitrogen is larger than that of oxygen because of
1 greater attraction of electons by the nucleus
2 the size of the nitrogen atom being smaller
3 the half-filled p-orbitals possess extra stability
4 greater penetration effect.
Explanation:
The ionisation energy of nitrogen is larger than of oxygen because of nitrogen has half-filled porbital is more stable thus, it is difficult to remove an electron from it. Hence nitrogen has larger ionisation energy than oxygen.
SRMJEEE - 2008
Classification of Elements and Periodicity in Properties
89651
The first ionization potential of $\mathrm{Al}$, as compared to that of $\mathrm{Mg}$ is :
1 Greater
2 Lower
3 The same
4 Twice as much
Explanation:
The first ionization potential of $\mathrm{Al}$ is lower than that of $\mathrm{Mg}$ because valence shell configuration of $\mathrm{Mg}$ is $3 \mathrm{~s}^2$ and of $\mathrm{Al}$ is $3 \mathrm{~s}^2, 3 \mathrm{p}^1$. As s-orbital is close to nucleus than p-orbital. So removal of $1 \mathrm{st}^{-}$from $\mathrm{Mg}$ is difficult and require more energy as compare to $\mathrm{Al}$.
BITSAT 2008
Classification of Elements and Periodicity in Properties
89652
The first ionization energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?
1 Lesser effective nuclear charge of oxygen then nitrogen
2 Lesser atomic size of oxygen than nitrogen
3 Greater interelectron repulsion between two electrons in the same p-orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen
4 Greater effective nuclear charge of oxygen than nitrogen
5 Higher electronegativity of oxygen than Nitrogen
Explanation:
The first ionization energy of oxygen is less than that of nitrogen because we move from left to right in a period atomic size decrease and ionization energy will be increased due to greater effective nuclear charge of oxygen than nitrogen.
Classification of Elements and Periodicity in Properties
89649
The pair of elements having approximately equal ionization potential is
1 $\mathrm{Al}, \mathrm{Ga}$
2 $\mathrm{Al}, \mathrm{Si}$
3 $\mathrm{Al}, \mathrm{Mg}$
4 Al, B
Explanation:
The pair of elements having approximately equal ionisaiton energy is $\mathrm{Al}$ and $\mathrm{Ga}$. Ionisation energy increases with a decreases in atomic size and due to the increase in the shielding effect of inner electrons.
UPTU/UPSEE-2009
Classification of Elements and Periodicity in Properties
89650
The ionisation energy of nitrogen is larger than that of oxygen because of
1 greater attraction of electons by the nucleus
2 the size of the nitrogen atom being smaller
3 the half-filled p-orbitals possess extra stability
4 greater penetration effect.
Explanation:
The ionisation energy of nitrogen is larger than of oxygen because of nitrogen has half-filled porbital is more stable thus, it is difficult to remove an electron from it. Hence nitrogen has larger ionisation energy than oxygen.
SRMJEEE - 2008
Classification of Elements and Periodicity in Properties
89651
The first ionization potential of $\mathrm{Al}$, as compared to that of $\mathrm{Mg}$ is :
1 Greater
2 Lower
3 The same
4 Twice as much
Explanation:
The first ionization potential of $\mathrm{Al}$ is lower than that of $\mathrm{Mg}$ because valence shell configuration of $\mathrm{Mg}$ is $3 \mathrm{~s}^2$ and of $\mathrm{Al}$ is $3 \mathrm{~s}^2, 3 \mathrm{p}^1$. As s-orbital is close to nucleus than p-orbital. So removal of $1 \mathrm{st}^{-}$from $\mathrm{Mg}$ is difficult and require more energy as compare to $\mathrm{Al}$.
BITSAT 2008
Classification of Elements and Periodicity in Properties
89652
The first ionization energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?
1 Lesser effective nuclear charge of oxygen then nitrogen
2 Lesser atomic size of oxygen than nitrogen
3 Greater interelectron repulsion between two electrons in the same p-orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen
4 Greater effective nuclear charge of oxygen than nitrogen
5 Higher electronegativity of oxygen than Nitrogen
Explanation:
The first ionization energy of oxygen is less than that of nitrogen because we move from left to right in a period atomic size decrease and ionization energy will be increased due to greater effective nuclear charge of oxygen than nitrogen.