The electronic configuration $1 \mathrm{~s}^2 \quad 2 \mathrm{~s}^2 \quad 2 \mathrm{p}^3$ having a half-filled electronic configuration which is stable. If one electron is removed then the high amount of energy is required.
JIPMER-2016
Classification of Elements and Periodicity in Properties
89623
The correct order of first ionization enthalpies of the following elements is
1 Be $>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ra}>\mathrm{Ba}$
2 Ra $>$ Ba $>$ Sr $>\mathrm{Ca}>\mathrm{Mg}>\mathrm{Be}$
3 Be $>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}>\mathrm{Ra}$
On moving from up to down in a group ionization energy decrease due to effective nuclear charge increase. So, the correct order of first ionization enthalpies of the element is- $\mathrm{Be}>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ra}>\mathrm{Ba}$
Kerala-CEE-2015
Classification of Elements and Periodicity in Properties
89625
Ionization energy and electron affinity are defined at
1 enthalpy
2 spontaneity
3 equilibrium
4 absolute zero.
Explanation:
The electron affinity of an atom or molecule is defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion. The ionisation enthalpy is defined as the change of electron as negative sign when energy released overall say that electron affinity and ionisation energy are defined at absolute zero.
J and K CET-(2014)
Classification of Elements and Periodicity in Properties
89626
The incorrect statements among the following is
1 the first ionization potential of $\mathrm{Al}$ is less than the first ionization potential of $\mathrm{Mg}$
2 the second ionization potential of $\mathrm{Mg}$ is lower than the second ionization potential of $\mathrm{Na}$
3 the first ionization potential of $\mathrm{Na}$ is less than the first ionization potential of $\mathrm{Mg}$
4 the third ionization potential of $\mathrm{Mg}$ is greater than the third ionisation potential of $\mathrm{Al}$
Explanation:
Ionisation energy is the energy required to remove one electron from the atom. The second ionization potential indicates the energy required to remove another electron after the first ionization. Hence, the second ionization potential of $\mathrm{Mg}$ is higher than the second ionization potential of $\mathrm{Na}$.
The electronic configuration $1 \mathrm{~s}^2 \quad 2 \mathrm{~s}^2 \quad 2 \mathrm{p}^3$ having a half-filled electronic configuration which is stable. If one electron is removed then the high amount of energy is required.
JIPMER-2016
Classification of Elements and Periodicity in Properties
89623
The correct order of first ionization enthalpies of the following elements is
1 Be $>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ra}>\mathrm{Ba}$
2 Ra $>$ Ba $>$ Sr $>\mathrm{Ca}>\mathrm{Mg}>\mathrm{Be}$
3 Be $>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}>\mathrm{Ra}$
On moving from up to down in a group ionization energy decrease due to effective nuclear charge increase. So, the correct order of first ionization enthalpies of the element is- $\mathrm{Be}>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ra}>\mathrm{Ba}$
Kerala-CEE-2015
Classification of Elements and Periodicity in Properties
89625
Ionization energy and electron affinity are defined at
1 enthalpy
2 spontaneity
3 equilibrium
4 absolute zero.
Explanation:
The electron affinity of an atom or molecule is defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion. The ionisation enthalpy is defined as the change of electron as negative sign when energy released overall say that electron affinity and ionisation energy are defined at absolute zero.
J and K CET-(2014)
Classification of Elements and Periodicity in Properties
89626
The incorrect statements among the following is
1 the first ionization potential of $\mathrm{Al}$ is less than the first ionization potential of $\mathrm{Mg}$
2 the second ionization potential of $\mathrm{Mg}$ is lower than the second ionization potential of $\mathrm{Na}$
3 the first ionization potential of $\mathrm{Na}$ is less than the first ionization potential of $\mathrm{Mg}$
4 the third ionization potential of $\mathrm{Mg}$ is greater than the third ionisation potential of $\mathrm{Al}$
Explanation:
Ionisation energy is the energy required to remove one electron from the atom. The second ionization potential indicates the energy required to remove another electron after the first ionization. Hence, the second ionization potential of $\mathrm{Mg}$ is higher than the second ionization potential of $\mathrm{Na}$.
The electronic configuration $1 \mathrm{~s}^2 \quad 2 \mathrm{~s}^2 \quad 2 \mathrm{p}^3$ having a half-filled electronic configuration which is stable. If one electron is removed then the high amount of energy is required.
JIPMER-2016
Classification of Elements and Periodicity in Properties
89623
The correct order of first ionization enthalpies of the following elements is
1 Be $>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ra}>\mathrm{Ba}$
2 Ra $>$ Ba $>$ Sr $>\mathrm{Ca}>\mathrm{Mg}>\mathrm{Be}$
3 Be $>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}>\mathrm{Ra}$
On moving from up to down in a group ionization energy decrease due to effective nuclear charge increase. So, the correct order of first ionization enthalpies of the element is- $\mathrm{Be}>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ra}>\mathrm{Ba}$
Kerala-CEE-2015
Classification of Elements and Periodicity in Properties
89625
Ionization energy and electron affinity are defined at
1 enthalpy
2 spontaneity
3 equilibrium
4 absolute zero.
Explanation:
The electron affinity of an atom or molecule is defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion. The ionisation enthalpy is defined as the change of electron as negative sign when energy released overall say that electron affinity and ionisation energy are defined at absolute zero.
J and K CET-(2014)
Classification of Elements and Periodicity in Properties
89626
The incorrect statements among the following is
1 the first ionization potential of $\mathrm{Al}$ is less than the first ionization potential of $\mathrm{Mg}$
2 the second ionization potential of $\mathrm{Mg}$ is lower than the second ionization potential of $\mathrm{Na}$
3 the first ionization potential of $\mathrm{Na}$ is less than the first ionization potential of $\mathrm{Mg}$
4 the third ionization potential of $\mathrm{Mg}$ is greater than the third ionisation potential of $\mathrm{Al}$
Explanation:
Ionisation energy is the energy required to remove one electron from the atom. The second ionization potential indicates the energy required to remove another electron after the first ionization. Hence, the second ionization potential of $\mathrm{Mg}$ is higher than the second ionization potential of $\mathrm{Na}$.
The electronic configuration $1 \mathrm{~s}^2 \quad 2 \mathrm{~s}^2 \quad 2 \mathrm{p}^3$ having a half-filled electronic configuration which is stable. If one electron is removed then the high amount of energy is required.
JIPMER-2016
Classification of Elements and Periodicity in Properties
89623
The correct order of first ionization enthalpies of the following elements is
1 Be $>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ra}>\mathrm{Ba}$
2 Ra $>$ Ba $>$ Sr $>\mathrm{Ca}>\mathrm{Mg}>\mathrm{Be}$
3 Be $>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}>\mathrm{Ra}$
On moving from up to down in a group ionization energy decrease due to effective nuclear charge increase. So, the correct order of first ionization enthalpies of the element is- $\mathrm{Be}>\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ra}>\mathrm{Ba}$
Kerala-CEE-2015
Classification of Elements and Periodicity in Properties
89625
Ionization energy and electron affinity are defined at
1 enthalpy
2 spontaneity
3 equilibrium
4 absolute zero.
Explanation:
The electron affinity of an atom or molecule is defined as the amount of energy released when an electron is attached to a neutral atom or molecule in the gaseous state to form a negative ion. The ionisation enthalpy is defined as the change of electron as negative sign when energy released overall say that electron affinity and ionisation energy are defined at absolute zero.
J and K CET-(2014)
Classification of Elements and Periodicity in Properties
89626
The incorrect statements among the following is
1 the first ionization potential of $\mathrm{Al}$ is less than the first ionization potential of $\mathrm{Mg}$
2 the second ionization potential of $\mathrm{Mg}$ is lower than the second ionization potential of $\mathrm{Na}$
3 the first ionization potential of $\mathrm{Na}$ is less than the first ionization potential of $\mathrm{Mg}$
4 the third ionization potential of $\mathrm{Mg}$ is greater than the third ionisation potential of $\mathrm{Al}$
Explanation:
Ionisation energy is the energy required to remove one electron from the atom. The second ionization potential indicates the energy required to remove another electron after the first ionization. Hence, the second ionization potential of $\mathrm{Mg}$ is higher than the second ionization potential of $\mathrm{Na}$.
