The ionization enthalpy of B is lower than that of Be. This is because electronic configuration of $\left(1 \mathrm{~s}^2\right.$, $\left.2 \mathrm{~s}^2, 2 \mathrm{p}^1\right)$ is less stable than that of $\operatorname{Be}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2\right)$ which has completely filled orbitals. The $2 \mathrm{p}$ orbital of B is not strongly attracted by the nucleus as the $2 \mathrm{~s}$ electron of $\mathrm{Be}$. Thus, the increasing order of first ionization enthalpies of element is- $\mathrm{F}>\mathrm{N}>\mathrm{C}>\mathrm{Be}>\mathrm{B}$
AIIMS-2016
Classification of Elements and Periodicity in Properties
89619
Which of the following atoms has the highest first ionisation energy?
1 $\mathrm{Na}$
2 $\mathrm{K}$
3 $\mathrm{Sc}$
4 $\mathrm{Rb}$
Explanation:
Order of ionisation energy is $\mathrm{Sc}>\mathrm{Na}>\mathrm{K}>$ $\mathrm{Rb}$. It is poor shielding effect and removal of one electron from $4 \mathrm{~s}$ orbital is difficult as compared to $3 \mathrm{~s}-$ orbital.
(JEE Main 2016)
Classification of Elements and Periodicity in Properties
89620
The ionization energy of hydrogen atom in the ground state is
1 $13.6 \mathrm{MeV}$
2 $13.6 \mathrm{eV}$
3 13.6 Joule
4 Zero
Explanation:
Ionization energy is the amount of energy required to remove an electron from an isolated atom or molecule. The ionization energy of hydrogen atom in the ground state is $13.6 \mathrm{eV}$.
The ionization enthalpy of B is lower than that of Be. This is because electronic configuration of $\left(1 \mathrm{~s}^2\right.$, $\left.2 \mathrm{~s}^2, 2 \mathrm{p}^1\right)$ is less stable than that of $\operatorname{Be}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2\right)$ which has completely filled orbitals. The $2 \mathrm{p}$ orbital of B is not strongly attracted by the nucleus as the $2 \mathrm{~s}$ electron of $\mathrm{Be}$. Thus, the increasing order of first ionization enthalpies of element is- $\mathrm{F}>\mathrm{N}>\mathrm{C}>\mathrm{Be}>\mathrm{B}$
AIIMS-2016
Classification of Elements and Periodicity in Properties
89619
Which of the following atoms has the highest first ionisation energy?
1 $\mathrm{Na}$
2 $\mathrm{K}$
3 $\mathrm{Sc}$
4 $\mathrm{Rb}$
Explanation:
Order of ionisation energy is $\mathrm{Sc}>\mathrm{Na}>\mathrm{K}>$ $\mathrm{Rb}$. It is poor shielding effect and removal of one electron from $4 \mathrm{~s}$ orbital is difficult as compared to $3 \mathrm{~s}-$ orbital.
(JEE Main 2016)
Classification of Elements and Periodicity in Properties
89620
The ionization energy of hydrogen atom in the ground state is
1 $13.6 \mathrm{MeV}$
2 $13.6 \mathrm{eV}$
3 13.6 Joule
4 Zero
Explanation:
Ionization energy is the amount of energy required to remove an electron from an isolated atom or molecule. The ionization energy of hydrogen atom in the ground state is $13.6 \mathrm{eV}$.
The ionization enthalpy of B is lower than that of Be. This is because electronic configuration of $\left(1 \mathrm{~s}^2\right.$, $\left.2 \mathrm{~s}^2, 2 \mathrm{p}^1\right)$ is less stable than that of $\operatorname{Be}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2\right)$ which has completely filled orbitals. The $2 \mathrm{p}$ orbital of B is not strongly attracted by the nucleus as the $2 \mathrm{~s}$ electron of $\mathrm{Be}$. Thus, the increasing order of first ionization enthalpies of element is- $\mathrm{F}>\mathrm{N}>\mathrm{C}>\mathrm{Be}>\mathrm{B}$
AIIMS-2016
Classification of Elements and Periodicity in Properties
89619
Which of the following atoms has the highest first ionisation energy?
1 $\mathrm{Na}$
2 $\mathrm{K}$
3 $\mathrm{Sc}$
4 $\mathrm{Rb}$
Explanation:
Order of ionisation energy is $\mathrm{Sc}>\mathrm{Na}>\mathrm{K}>$ $\mathrm{Rb}$. It is poor shielding effect and removal of one electron from $4 \mathrm{~s}$ orbital is difficult as compared to $3 \mathrm{~s}-$ orbital.
(JEE Main 2016)
Classification of Elements and Periodicity in Properties
89620
The ionization energy of hydrogen atom in the ground state is
1 $13.6 \mathrm{MeV}$
2 $13.6 \mathrm{eV}$
3 13.6 Joule
4 Zero
Explanation:
Ionization energy is the amount of energy required to remove an electron from an isolated atom or molecule. The ionization energy of hydrogen atom in the ground state is $13.6 \mathrm{eV}$.
The ionization enthalpy of B is lower than that of Be. This is because electronic configuration of $\left(1 \mathrm{~s}^2\right.$, $\left.2 \mathrm{~s}^2, 2 \mathrm{p}^1\right)$ is less stable than that of $\operatorname{Be}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2\right)$ which has completely filled orbitals. The $2 \mathrm{p}$ orbital of B is not strongly attracted by the nucleus as the $2 \mathrm{~s}$ electron of $\mathrm{Be}$. Thus, the increasing order of first ionization enthalpies of element is- $\mathrm{F}>\mathrm{N}>\mathrm{C}>\mathrm{Be}>\mathrm{B}$
AIIMS-2016
Classification of Elements and Periodicity in Properties
89619
Which of the following atoms has the highest first ionisation energy?
1 $\mathrm{Na}$
2 $\mathrm{K}$
3 $\mathrm{Sc}$
4 $\mathrm{Rb}$
Explanation:
Order of ionisation energy is $\mathrm{Sc}>\mathrm{Na}>\mathrm{K}>$ $\mathrm{Rb}$. It is poor shielding effect and removal of one electron from $4 \mathrm{~s}$ orbital is difficult as compared to $3 \mathrm{~s}-$ orbital.
(JEE Main 2016)
Classification of Elements and Periodicity in Properties
89620
The ionization energy of hydrogen atom in the ground state is
1 $13.6 \mathrm{MeV}$
2 $13.6 \mathrm{eV}$
3 13.6 Joule
4 Zero
Explanation:
Ionization energy is the amount of energy required to remove an electron from an isolated atom or molecule. The ionization energy of hydrogen atom in the ground state is $13.6 \mathrm{eV}$.
