Classification of Elements and Periodicity in Properties
89556
The ionisation potential of which element is highest?
1 $\mathrm{H}$
2 $\mathrm{He}$
3 $\mathrm{Ar}$
4 $\mathrm{F}$
Explanation:
The ionization potential of $\mathrm{He}$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period. So, inert gas has highest ionization potential.
CG PET-22.05.2022
Classification of Elements and Periodicity in Properties
89560
The first ionization potential of $\mathrm{Na}, \mathrm{Mg}$ and $\mathrm{Si}$ are respectively 496,737 and $786 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$. The ionization potential of $\mathrm{Al}$ will be closer to
1 $760 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $575 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $801 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $419 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Explanation:
The ionization energy of $\mathrm{Mg}$ will be larger than that of $\mathrm{Na}$ due to fully filled configuration. The ionization energy of $\mathrm{Al}$ will be smaller than that of $\mathrm{Mg}$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $\mathrm{Al}$ will be $760 \mathrm{~kJ} / \mathrm{mole}$.
AMU-2014
Classification of Elements and Periodicity in Properties
89561
The decreasing order of the ionization potential of the following elements is
On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $\mathrm{Ne}>$ $\mathrm{Cl}>\mathrm{P}>\mathrm{S}>\mathrm{Mg}>\mathrm{Al}$.
CG PET -2005
Classification of Elements and Periodicity in Properties
89562
In which of the following arrangements, the order is NOT according to the property indicated against It
When we move from $\mathrm{B}$ to $\mathrm{O}$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $\mathrm{B}<\mathrm{C}<\mathrm{N}<\mathrm{O}$ : increasing first ionization enthalpy.
AIIMS-2015
Classification of Elements and Periodicity in Properties
89563
In the following, the element with the highest ionization energy is
The given electronic configuration [Ne] $3 \mathrm{~s}^2$ $3 \mathrm{p}^3$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.
Classification of Elements and Periodicity in Properties
89556
The ionisation potential of which element is highest?
1 $\mathrm{H}$
2 $\mathrm{He}$
3 $\mathrm{Ar}$
4 $\mathrm{F}$
Explanation:
The ionization potential of $\mathrm{He}$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period. So, inert gas has highest ionization potential.
CG PET-22.05.2022
Classification of Elements and Periodicity in Properties
89560
The first ionization potential of $\mathrm{Na}, \mathrm{Mg}$ and $\mathrm{Si}$ are respectively 496,737 and $786 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$. The ionization potential of $\mathrm{Al}$ will be closer to
1 $760 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $575 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $801 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $419 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Explanation:
The ionization energy of $\mathrm{Mg}$ will be larger than that of $\mathrm{Na}$ due to fully filled configuration. The ionization energy of $\mathrm{Al}$ will be smaller than that of $\mathrm{Mg}$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $\mathrm{Al}$ will be $760 \mathrm{~kJ} / \mathrm{mole}$.
AMU-2014
Classification of Elements and Periodicity in Properties
89561
The decreasing order of the ionization potential of the following elements is
On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $\mathrm{Ne}>$ $\mathrm{Cl}>\mathrm{P}>\mathrm{S}>\mathrm{Mg}>\mathrm{Al}$.
CG PET -2005
Classification of Elements and Periodicity in Properties
89562
In which of the following arrangements, the order is NOT according to the property indicated against It
When we move from $\mathrm{B}$ to $\mathrm{O}$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $\mathrm{B}<\mathrm{C}<\mathrm{N}<\mathrm{O}$ : increasing first ionization enthalpy.
AIIMS-2015
Classification of Elements and Periodicity in Properties
89563
In the following, the element with the highest ionization energy is
The given electronic configuration [Ne] $3 \mathrm{~s}^2$ $3 \mathrm{p}^3$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.
Classification of Elements and Periodicity in Properties
89556
The ionisation potential of which element is highest?
1 $\mathrm{H}$
2 $\mathrm{He}$
3 $\mathrm{Ar}$
4 $\mathrm{F}$
Explanation:
The ionization potential of $\mathrm{He}$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period. So, inert gas has highest ionization potential.
CG PET-22.05.2022
Classification of Elements and Periodicity in Properties
89560
The first ionization potential of $\mathrm{Na}, \mathrm{Mg}$ and $\mathrm{Si}$ are respectively 496,737 and $786 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$. The ionization potential of $\mathrm{Al}$ will be closer to
1 $760 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $575 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $801 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $419 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Explanation:
The ionization energy of $\mathrm{Mg}$ will be larger than that of $\mathrm{Na}$ due to fully filled configuration. The ionization energy of $\mathrm{Al}$ will be smaller than that of $\mathrm{Mg}$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $\mathrm{Al}$ will be $760 \mathrm{~kJ} / \mathrm{mole}$.
AMU-2014
Classification of Elements and Periodicity in Properties
89561
The decreasing order of the ionization potential of the following elements is
On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $\mathrm{Ne}>$ $\mathrm{Cl}>\mathrm{P}>\mathrm{S}>\mathrm{Mg}>\mathrm{Al}$.
CG PET -2005
Classification of Elements and Periodicity in Properties
89562
In which of the following arrangements, the order is NOT according to the property indicated against It
When we move from $\mathrm{B}$ to $\mathrm{O}$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $\mathrm{B}<\mathrm{C}<\mathrm{N}<\mathrm{O}$ : increasing first ionization enthalpy.
AIIMS-2015
Classification of Elements and Periodicity in Properties
89563
In the following, the element with the highest ionization energy is
The given electronic configuration [Ne] $3 \mathrm{~s}^2$ $3 \mathrm{p}^3$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.
Classification of Elements and Periodicity in Properties
89556
The ionisation potential of which element is highest?
1 $\mathrm{H}$
2 $\mathrm{He}$
3 $\mathrm{Ar}$
4 $\mathrm{F}$
Explanation:
The ionization potential of $\mathrm{He}$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period. So, inert gas has highest ionization potential.
CG PET-22.05.2022
Classification of Elements and Periodicity in Properties
89560
The first ionization potential of $\mathrm{Na}, \mathrm{Mg}$ and $\mathrm{Si}$ are respectively 496,737 and $786 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$. The ionization potential of $\mathrm{Al}$ will be closer to
1 $760 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $575 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $801 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $419 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Explanation:
The ionization energy of $\mathrm{Mg}$ will be larger than that of $\mathrm{Na}$ due to fully filled configuration. The ionization energy of $\mathrm{Al}$ will be smaller than that of $\mathrm{Mg}$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $\mathrm{Al}$ will be $760 \mathrm{~kJ} / \mathrm{mole}$.
AMU-2014
Classification of Elements and Periodicity in Properties
89561
The decreasing order of the ionization potential of the following elements is
On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $\mathrm{Ne}>$ $\mathrm{Cl}>\mathrm{P}>\mathrm{S}>\mathrm{Mg}>\mathrm{Al}$.
CG PET -2005
Classification of Elements and Periodicity in Properties
89562
In which of the following arrangements, the order is NOT according to the property indicated against It
When we move from $\mathrm{B}$ to $\mathrm{O}$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $\mathrm{B}<\mathrm{C}<\mathrm{N}<\mathrm{O}$ : increasing first ionization enthalpy.
AIIMS-2015
Classification of Elements and Periodicity in Properties
89563
In the following, the element with the highest ionization energy is
The given electronic configuration [Ne] $3 \mathrm{~s}^2$ $3 \mathrm{p}^3$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.
Classification of Elements and Periodicity in Properties
89556
The ionisation potential of which element is highest?
1 $\mathrm{H}$
2 $\mathrm{He}$
3 $\mathrm{Ar}$
4 $\mathrm{F}$
Explanation:
The ionization potential of $\mathrm{He}$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period. So, inert gas has highest ionization potential.
CG PET-22.05.2022
Classification of Elements and Periodicity in Properties
89560
The first ionization potential of $\mathrm{Na}, \mathrm{Mg}$ and $\mathrm{Si}$ are respectively 496,737 and $786 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}$. The ionization potential of $\mathrm{Al}$ will be closer to
1 $760 \mathrm{~kJ} \mathrm{~mol}^{-1}$
2 $575 \mathrm{~kJ} \mathrm{~mol}^{-1}$
3 $801 \mathrm{~kJ} \mathrm{~mol}^{-1}$
4 $419 \mathrm{~kJ} \mathrm{~mol}^{-1}$
Explanation:
The ionization energy of $\mathrm{Mg}$ will be larger than that of $\mathrm{Na}$ due to fully filled configuration. The ionization energy of $\mathrm{Al}$ will be smaller than that of $\mathrm{Mg}$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $\mathrm{Al}$ will be $760 \mathrm{~kJ} / \mathrm{mole}$.
AMU-2014
Classification of Elements and Periodicity in Properties
89561
The decreasing order of the ionization potential of the following elements is
On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $\mathrm{Ne}>$ $\mathrm{Cl}>\mathrm{P}>\mathrm{S}>\mathrm{Mg}>\mathrm{Al}$.
CG PET -2005
Classification of Elements and Periodicity in Properties
89562
In which of the following arrangements, the order is NOT according to the property indicated against It
When we move from $\mathrm{B}$ to $\mathrm{O}$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $\mathrm{B}<\mathrm{C}<\mathrm{N}<\mathrm{O}$ : increasing first ionization enthalpy.
AIIMS-2015
Classification of Elements and Periodicity in Properties
89563
In the following, the element with the highest ionization energy is
The given electronic configuration [Ne] $3 \mathrm{~s}^2$ $3 \mathrm{p}^3$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.
