Classification of Elements and Periodicity in Properties
89581
Which of the following elements has the lowest ionisation potential?
1 Sodium
2 Potassium
3 Rubidium
4 Cesium
Explanation:
The ionization energy decreases on moving down the group As we go down in a group, the nuclear charge increases. (2) As we go down in a group the atomic size increases. due to the addition of a new shell to each element. (3) As we go down in a group , the number of inner electrons increases. This increases the shielding effect on outer electrons. The combined effect of the increases in atomic size, and the shielding effect more than the effect of the increases of the nuclear charge. These effects act in such a way that the force of attraction between the nucleus, and the outermost electron decreases as we go down the group.
AMU-2003
Classification of Elements and Periodicity in Properties
89583
The first ionisation energy of magnesium is smaller as compared to that of elements $X$ and $Y$, but higher than that of $Z$. The elements $X, Y$ and $Z$, respectively, are
1 chlorine, lithium and sodium
2 argon, lithium and sodium
3 argon, chlorine and sodium
4 neon, sodium and chlorine
Explanation:
On moving from left to right in a $3^{\text {rd }}$ period ionisaiton energy increases. Ionisation energy of the $3^{\text {rd }}$ period are$\mathrm{Na}<\mathrm{Al}<\mathrm{Mg}<\mathrm{Si}<\mathrm{S}<\mathrm{P}<\mathrm{Cl}<\mathrm{Ar}$ Hence, the element $X, Y$ and $\mathrm{Z}$ are argon, chlorine and sodium respectively.
(JEE Main 2021
Classification of Elements and Periodicity in Properties
89594
The first ionization enthalpies of $\mathrm{Mg}$ and $\mathrm{Al}$ can be expected to be
Ionization enthalpy is defined by the amount of energy an isolated gaseous atom would take to lose an electron in its ground state. (i) $\mathrm{Mg} \longrightarrow \mathrm{Mg}^{+}+\mathrm{e}^{-}$ $\mathrm{I} \cdot \mathrm{E}_1(\mathrm{Mg})=737.7 \mathrm{~kJ} \mathrm{~mole}^{-1}$ (ii) $\mathrm{Al} \longrightarrow \mathrm{Al}^{+}+\mathrm{e}^{-}$ $\mathrm{I} \cdot \mathrm{E}_1(\mathrm{Al})=577.5 \mathrm{~kJ} \mathrm{~mole}{ }^{-1}$
AP EAPCET 20.08.2021 Shift-II
Classification of Elements and Periodicity in Properties
89595
Identify the incorrect order corresponding the mentioned property?
4 $\mathrm{Li}<\mathrm{Be}<\mathrm{B}<\mathrm{C}$ : First Ionization enthaply
Explanation:
Option (1), (2) and (3) are correct. Ionization enthalpy defined as the amount of energy an isolated gaseous atom would take to lose an electron in its ground state. So, the order is - $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}$ (for first ionization energy) $520,801,899,1086, \mathrm{~kJ} /$ mole.
Classification of Elements and Periodicity in Properties
89581
Which of the following elements has the lowest ionisation potential?
1 Sodium
2 Potassium
3 Rubidium
4 Cesium
Explanation:
The ionization energy decreases on moving down the group As we go down in a group, the nuclear charge increases. (2) As we go down in a group the atomic size increases. due to the addition of a new shell to each element. (3) As we go down in a group , the number of inner electrons increases. This increases the shielding effect on outer electrons. The combined effect of the increases in atomic size, and the shielding effect more than the effect of the increases of the nuclear charge. These effects act in such a way that the force of attraction between the nucleus, and the outermost electron decreases as we go down the group.
AMU-2003
Classification of Elements and Periodicity in Properties
89583
The first ionisation energy of magnesium is smaller as compared to that of elements $X$ and $Y$, but higher than that of $Z$. The elements $X, Y$ and $Z$, respectively, are
1 chlorine, lithium and sodium
2 argon, lithium and sodium
3 argon, chlorine and sodium
4 neon, sodium and chlorine
Explanation:
On moving from left to right in a $3^{\text {rd }}$ period ionisaiton energy increases. Ionisation energy of the $3^{\text {rd }}$ period are$\mathrm{Na}<\mathrm{Al}<\mathrm{Mg}<\mathrm{Si}<\mathrm{S}<\mathrm{P}<\mathrm{Cl}<\mathrm{Ar}$ Hence, the element $X, Y$ and $\mathrm{Z}$ are argon, chlorine and sodium respectively.
(JEE Main 2021
Classification of Elements and Periodicity in Properties
89594
The first ionization enthalpies of $\mathrm{Mg}$ and $\mathrm{Al}$ can be expected to be
Ionization enthalpy is defined by the amount of energy an isolated gaseous atom would take to lose an electron in its ground state. (i) $\mathrm{Mg} \longrightarrow \mathrm{Mg}^{+}+\mathrm{e}^{-}$ $\mathrm{I} \cdot \mathrm{E}_1(\mathrm{Mg})=737.7 \mathrm{~kJ} \mathrm{~mole}^{-1}$ (ii) $\mathrm{Al} \longrightarrow \mathrm{Al}^{+}+\mathrm{e}^{-}$ $\mathrm{I} \cdot \mathrm{E}_1(\mathrm{Al})=577.5 \mathrm{~kJ} \mathrm{~mole}{ }^{-1}$
AP EAPCET 20.08.2021 Shift-II
Classification of Elements and Periodicity in Properties
89595
Identify the incorrect order corresponding the mentioned property?
4 $\mathrm{Li}<\mathrm{Be}<\mathrm{B}<\mathrm{C}$ : First Ionization enthaply
Explanation:
Option (1), (2) and (3) are correct. Ionization enthalpy defined as the amount of energy an isolated gaseous atom would take to lose an electron in its ground state. So, the order is - $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}$ (for first ionization energy) $520,801,899,1086, \mathrm{~kJ} /$ mole.
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Classification of Elements and Periodicity in Properties
89581
Which of the following elements has the lowest ionisation potential?
1 Sodium
2 Potassium
3 Rubidium
4 Cesium
Explanation:
The ionization energy decreases on moving down the group As we go down in a group, the nuclear charge increases. (2) As we go down in a group the atomic size increases. due to the addition of a new shell to each element. (3) As we go down in a group , the number of inner electrons increases. This increases the shielding effect on outer electrons. The combined effect of the increases in atomic size, and the shielding effect more than the effect of the increases of the nuclear charge. These effects act in such a way that the force of attraction between the nucleus, and the outermost electron decreases as we go down the group.
AMU-2003
Classification of Elements and Periodicity in Properties
89583
The first ionisation energy of magnesium is smaller as compared to that of elements $X$ and $Y$, but higher than that of $Z$. The elements $X, Y$ and $Z$, respectively, are
1 chlorine, lithium and sodium
2 argon, lithium and sodium
3 argon, chlorine and sodium
4 neon, sodium and chlorine
Explanation:
On moving from left to right in a $3^{\text {rd }}$ period ionisaiton energy increases. Ionisation energy of the $3^{\text {rd }}$ period are$\mathrm{Na}<\mathrm{Al}<\mathrm{Mg}<\mathrm{Si}<\mathrm{S}<\mathrm{P}<\mathrm{Cl}<\mathrm{Ar}$ Hence, the element $X, Y$ and $\mathrm{Z}$ are argon, chlorine and sodium respectively.
(JEE Main 2021
Classification of Elements and Periodicity in Properties
89594
The first ionization enthalpies of $\mathrm{Mg}$ and $\mathrm{Al}$ can be expected to be
Ionization enthalpy is defined by the amount of energy an isolated gaseous atom would take to lose an electron in its ground state. (i) $\mathrm{Mg} \longrightarrow \mathrm{Mg}^{+}+\mathrm{e}^{-}$ $\mathrm{I} \cdot \mathrm{E}_1(\mathrm{Mg})=737.7 \mathrm{~kJ} \mathrm{~mole}^{-1}$ (ii) $\mathrm{Al} \longrightarrow \mathrm{Al}^{+}+\mathrm{e}^{-}$ $\mathrm{I} \cdot \mathrm{E}_1(\mathrm{Al})=577.5 \mathrm{~kJ} \mathrm{~mole}{ }^{-1}$
AP EAPCET 20.08.2021 Shift-II
Classification of Elements and Periodicity in Properties
89595
Identify the incorrect order corresponding the mentioned property?
4 $\mathrm{Li}<\mathrm{Be}<\mathrm{B}<\mathrm{C}$ : First Ionization enthaply
Explanation:
Option (1), (2) and (3) are correct. Ionization enthalpy defined as the amount of energy an isolated gaseous atom would take to lose an electron in its ground state. So, the order is - $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}$ (for first ionization energy) $520,801,899,1086, \mathrm{~kJ} /$ mole.
Classification of Elements and Periodicity in Properties
89581
Which of the following elements has the lowest ionisation potential?
1 Sodium
2 Potassium
3 Rubidium
4 Cesium
Explanation:
The ionization energy decreases on moving down the group As we go down in a group, the nuclear charge increases. (2) As we go down in a group the atomic size increases. due to the addition of a new shell to each element. (3) As we go down in a group , the number of inner electrons increases. This increases the shielding effect on outer electrons. The combined effect of the increases in atomic size, and the shielding effect more than the effect of the increases of the nuclear charge. These effects act in such a way that the force of attraction between the nucleus, and the outermost electron decreases as we go down the group.
AMU-2003
Classification of Elements and Periodicity in Properties
89583
The first ionisation energy of magnesium is smaller as compared to that of elements $X$ and $Y$, but higher than that of $Z$. The elements $X, Y$ and $Z$, respectively, are
1 chlorine, lithium and sodium
2 argon, lithium and sodium
3 argon, chlorine and sodium
4 neon, sodium and chlorine
Explanation:
On moving from left to right in a $3^{\text {rd }}$ period ionisaiton energy increases. Ionisation energy of the $3^{\text {rd }}$ period are$\mathrm{Na}<\mathrm{Al}<\mathrm{Mg}<\mathrm{Si}<\mathrm{S}<\mathrm{P}<\mathrm{Cl}<\mathrm{Ar}$ Hence, the element $X, Y$ and $\mathrm{Z}$ are argon, chlorine and sodium respectively.
(JEE Main 2021
Classification of Elements and Periodicity in Properties
89594
The first ionization enthalpies of $\mathrm{Mg}$ and $\mathrm{Al}$ can be expected to be
Ionization enthalpy is defined by the amount of energy an isolated gaseous atom would take to lose an electron in its ground state. (i) $\mathrm{Mg} \longrightarrow \mathrm{Mg}^{+}+\mathrm{e}^{-}$ $\mathrm{I} \cdot \mathrm{E}_1(\mathrm{Mg})=737.7 \mathrm{~kJ} \mathrm{~mole}^{-1}$ (ii) $\mathrm{Al} \longrightarrow \mathrm{Al}^{+}+\mathrm{e}^{-}$ $\mathrm{I} \cdot \mathrm{E}_1(\mathrm{Al})=577.5 \mathrm{~kJ} \mathrm{~mole}{ }^{-1}$
AP EAPCET 20.08.2021 Shift-II
Classification of Elements and Periodicity in Properties
89595
Identify the incorrect order corresponding the mentioned property?
4 $\mathrm{Li}<\mathrm{Be}<\mathrm{B}<\mathrm{C}$ : First Ionization enthaply
Explanation:
Option (1), (2) and (3) are correct. Ionization enthalpy defined as the amount of energy an isolated gaseous atom would take to lose an electron in its ground state. So, the order is - $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}$ (for first ionization energy) $520,801,899,1086, \mathrm{~kJ} /$ mole.