Classification of Elements and Periodicity in Properties
89605
The element having greater difference between its first and second ionization energies, is:
1 $\mathrm{Ca}$
2 $\mathrm{Sc}$
3 $\mathrm{Ba}$
4 $\mathrm{K}$
Explanation:
Alkali metal have high difference in the first and second ionization energy and they achieve stable noble gas configuration offer first ionization. First ionization energy is the energy required to remove an electron from an atom in the gaseous state. The second ionization energy is defined as the energy needed to remove one mole of $1^{+}$ions in the gaseous state to form one mole of $2^{+}$ions in the gaseous state. The value of $2^{\text {nd }}$ I.E. are- For $\quad \mathrm{Ca}, \mathrm{I} \cdot \mathrm{E}_2=1145.4 \mathrm{~kJ} / \mathrm{mole}$ Sc, I. $E_2=1235.0 \mathrm{~kJ} / \mathrm{mole}$ $\mathrm{K}, \mathrm{I} . \mathrm{E}_2=3052.0 \mathrm{~kJ} / \mathrm{mole}$ $\mathrm{Ba}, \mathrm{I}_2 \mathrm{E}_2=965.2 \mathrm{~kJ} / \mathrm{mole}$ Hence, potassium $(\mathrm{K})$ has highest ionization energy.
(JEE Main 2019
Classification of Elements and Periodicity in Properties
89612
What will be ionization energy of Be atom? Consider the first ionization energy of $H$ atom as $13.6 \mathrm{eV}$.
1 $-217.6 \mathrm{eV}$
2 $54.4 \mathrm{eV}$
3 $108.8 \mathrm{eV}$
4 $4 \mathrm{eV}$
Explanation:
According to Bohr's model of energy $E=-13.6 \times \frac{z^2}{n^2}$ Where, $\mathrm{E}=$ Energy of electron $\mathrm{n}=$ Shell $\mathrm{Z}=$ Atomic number Ionisation energy of $1^{\text {st }}$ orbit of $\mathrm{Be}=\frac{-13.6 \times 4^2}{1^2}$ $=-13.6 \times 16$ $=-217.6 \mathrm{eV}$ So, Ionisation energy $=217.6 \mathrm{eV}$
J and K CET-(2018)
Classification of Elements and Periodicity in Properties
89613
The ionisation energy of nitrogen is larger than that of oxygen because :
1 the size of nitrogen atom is smaller
2 there is greater attraction of electrons towards the nucleus
3 half-filled p-orbitals of nitrogen have extra stability
4 None of the above
Explanation:
The electronic configuration of nitrogen and oxygen are- $\begin{aligned} & { }_7 \mathrm{~N}-1 \mathrm{~s}^2, 2 \mathrm{~s}^2, 2 \mathrm{p}^3 \\ & { }_8 \mathrm{O}-1 \mathrm{~s}^2, 2 \mathrm{~s}^2, 2 \mathrm{p}^4 \end{aligned}$ Thus, the ionisation energy of nitrogen is larger than that of oxygen because of half-filled p-orbitals of nitrogen have extra stability.
Manipal-2017
Classification of Elements and Periodicity in Properties
89604
Assertion: $\mathrm{Li}$ has high ionisation enthalpy, while $\mathrm{Li}$ is the strongest reducing agent in aqueous medium. Reason : $\mathrm{Li}$ has high oxidation potential.
1 If both Assertion and Reason are correct and Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
Li has high ionization energy, while $\mathrm{Li}$ is the strongest reducing agent in aqueous medium because of large amount of hydration energy is realized and on account of large amount of hydration energy molecules it strongest reducing agent and $\mathrm{Li}$ has high oxidation potential.
Classification of Elements and Periodicity in Properties
89605
The element having greater difference between its first and second ionization energies, is:
1 $\mathrm{Ca}$
2 $\mathrm{Sc}$
3 $\mathrm{Ba}$
4 $\mathrm{K}$
Explanation:
Alkali metal have high difference in the first and second ionization energy and they achieve stable noble gas configuration offer first ionization. First ionization energy is the energy required to remove an electron from an atom in the gaseous state. The second ionization energy is defined as the energy needed to remove one mole of $1^{+}$ions in the gaseous state to form one mole of $2^{+}$ions in the gaseous state. The value of $2^{\text {nd }}$ I.E. are- For $\quad \mathrm{Ca}, \mathrm{I} \cdot \mathrm{E}_2=1145.4 \mathrm{~kJ} / \mathrm{mole}$ Sc, I. $E_2=1235.0 \mathrm{~kJ} / \mathrm{mole}$ $\mathrm{K}, \mathrm{I} . \mathrm{E}_2=3052.0 \mathrm{~kJ} / \mathrm{mole}$ $\mathrm{Ba}, \mathrm{I}_2 \mathrm{E}_2=965.2 \mathrm{~kJ} / \mathrm{mole}$ Hence, potassium $(\mathrm{K})$ has highest ionization energy.
(JEE Main 2019
Classification of Elements and Periodicity in Properties
89612
What will be ionization energy of Be atom? Consider the first ionization energy of $H$ atom as $13.6 \mathrm{eV}$.
1 $-217.6 \mathrm{eV}$
2 $54.4 \mathrm{eV}$
3 $108.8 \mathrm{eV}$
4 $4 \mathrm{eV}$
Explanation:
According to Bohr's model of energy $E=-13.6 \times \frac{z^2}{n^2}$ Where, $\mathrm{E}=$ Energy of electron $\mathrm{n}=$ Shell $\mathrm{Z}=$ Atomic number Ionisation energy of $1^{\text {st }}$ orbit of $\mathrm{Be}=\frac{-13.6 \times 4^2}{1^2}$ $=-13.6 \times 16$ $=-217.6 \mathrm{eV}$ So, Ionisation energy $=217.6 \mathrm{eV}$
J and K CET-(2018)
Classification of Elements and Periodicity in Properties
89613
The ionisation energy of nitrogen is larger than that of oxygen because :
1 the size of nitrogen atom is smaller
2 there is greater attraction of electrons towards the nucleus
3 half-filled p-orbitals of nitrogen have extra stability
4 None of the above
Explanation:
The electronic configuration of nitrogen and oxygen are- $\begin{aligned} & { }_7 \mathrm{~N}-1 \mathrm{~s}^2, 2 \mathrm{~s}^2, 2 \mathrm{p}^3 \\ & { }_8 \mathrm{O}-1 \mathrm{~s}^2, 2 \mathrm{~s}^2, 2 \mathrm{p}^4 \end{aligned}$ Thus, the ionisation energy of nitrogen is larger than that of oxygen because of half-filled p-orbitals of nitrogen have extra stability.
Manipal-2017
Classification of Elements and Periodicity in Properties
89604
Assertion: $\mathrm{Li}$ has high ionisation enthalpy, while $\mathrm{Li}$ is the strongest reducing agent in aqueous medium. Reason : $\mathrm{Li}$ has high oxidation potential.
1 If both Assertion and Reason are correct and Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
Li has high ionization energy, while $\mathrm{Li}$ is the strongest reducing agent in aqueous medium because of large amount of hydration energy is realized and on account of large amount of hydration energy molecules it strongest reducing agent and $\mathrm{Li}$ has high oxidation potential.
Classification of Elements and Periodicity in Properties
89605
The element having greater difference between its first and second ionization energies, is:
1 $\mathrm{Ca}$
2 $\mathrm{Sc}$
3 $\mathrm{Ba}$
4 $\mathrm{K}$
Explanation:
Alkali metal have high difference in the first and second ionization energy and they achieve stable noble gas configuration offer first ionization. First ionization energy is the energy required to remove an electron from an atom in the gaseous state. The second ionization energy is defined as the energy needed to remove one mole of $1^{+}$ions in the gaseous state to form one mole of $2^{+}$ions in the gaseous state. The value of $2^{\text {nd }}$ I.E. are- For $\quad \mathrm{Ca}, \mathrm{I} \cdot \mathrm{E}_2=1145.4 \mathrm{~kJ} / \mathrm{mole}$ Sc, I. $E_2=1235.0 \mathrm{~kJ} / \mathrm{mole}$ $\mathrm{K}, \mathrm{I} . \mathrm{E}_2=3052.0 \mathrm{~kJ} / \mathrm{mole}$ $\mathrm{Ba}, \mathrm{I}_2 \mathrm{E}_2=965.2 \mathrm{~kJ} / \mathrm{mole}$ Hence, potassium $(\mathrm{K})$ has highest ionization energy.
(JEE Main 2019
Classification of Elements and Periodicity in Properties
89612
What will be ionization energy of Be atom? Consider the first ionization energy of $H$ atom as $13.6 \mathrm{eV}$.
1 $-217.6 \mathrm{eV}$
2 $54.4 \mathrm{eV}$
3 $108.8 \mathrm{eV}$
4 $4 \mathrm{eV}$
Explanation:
According to Bohr's model of energy $E=-13.6 \times \frac{z^2}{n^2}$ Where, $\mathrm{E}=$ Energy of electron $\mathrm{n}=$ Shell $\mathrm{Z}=$ Atomic number Ionisation energy of $1^{\text {st }}$ orbit of $\mathrm{Be}=\frac{-13.6 \times 4^2}{1^2}$ $=-13.6 \times 16$ $=-217.6 \mathrm{eV}$ So, Ionisation energy $=217.6 \mathrm{eV}$
J and K CET-(2018)
Classification of Elements and Periodicity in Properties
89613
The ionisation energy of nitrogen is larger than that of oxygen because :
1 the size of nitrogen atom is smaller
2 there is greater attraction of electrons towards the nucleus
3 half-filled p-orbitals of nitrogen have extra stability
4 None of the above
Explanation:
The electronic configuration of nitrogen and oxygen are- $\begin{aligned} & { }_7 \mathrm{~N}-1 \mathrm{~s}^2, 2 \mathrm{~s}^2, 2 \mathrm{p}^3 \\ & { }_8 \mathrm{O}-1 \mathrm{~s}^2, 2 \mathrm{~s}^2, 2 \mathrm{p}^4 \end{aligned}$ Thus, the ionisation energy of nitrogen is larger than that of oxygen because of half-filled p-orbitals of nitrogen have extra stability.
Manipal-2017
Classification of Elements and Periodicity in Properties
89604
Assertion: $\mathrm{Li}$ has high ionisation enthalpy, while $\mathrm{Li}$ is the strongest reducing agent in aqueous medium. Reason : $\mathrm{Li}$ has high oxidation potential.
1 If both Assertion and Reason are correct and Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
Li has high ionization energy, while $\mathrm{Li}$ is the strongest reducing agent in aqueous medium because of large amount of hydration energy is realized and on account of large amount of hydration energy molecules it strongest reducing agent and $\mathrm{Li}$ has high oxidation potential.
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Classification of Elements and Periodicity in Properties
89605
The element having greater difference between its first and second ionization energies, is:
1 $\mathrm{Ca}$
2 $\mathrm{Sc}$
3 $\mathrm{Ba}$
4 $\mathrm{K}$
Explanation:
Alkali metal have high difference in the first and second ionization energy and they achieve stable noble gas configuration offer first ionization. First ionization energy is the energy required to remove an electron from an atom in the gaseous state. The second ionization energy is defined as the energy needed to remove one mole of $1^{+}$ions in the gaseous state to form one mole of $2^{+}$ions in the gaseous state. The value of $2^{\text {nd }}$ I.E. are- For $\quad \mathrm{Ca}, \mathrm{I} \cdot \mathrm{E}_2=1145.4 \mathrm{~kJ} / \mathrm{mole}$ Sc, I. $E_2=1235.0 \mathrm{~kJ} / \mathrm{mole}$ $\mathrm{K}, \mathrm{I} . \mathrm{E}_2=3052.0 \mathrm{~kJ} / \mathrm{mole}$ $\mathrm{Ba}, \mathrm{I}_2 \mathrm{E}_2=965.2 \mathrm{~kJ} / \mathrm{mole}$ Hence, potassium $(\mathrm{K})$ has highest ionization energy.
(JEE Main 2019
Classification of Elements and Periodicity in Properties
89612
What will be ionization energy of Be atom? Consider the first ionization energy of $H$ atom as $13.6 \mathrm{eV}$.
1 $-217.6 \mathrm{eV}$
2 $54.4 \mathrm{eV}$
3 $108.8 \mathrm{eV}$
4 $4 \mathrm{eV}$
Explanation:
According to Bohr's model of energy $E=-13.6 \times \frac{z^2}{n^2}$ Where, $\mathrm{E}=$ Energy of electron $\mathrm{n}=$ Shell $\mathrm{Z}=$ Atomic number Ionisation energy of $1^{\text {st }}$ orbit of $\mathrm{Be}=\frac{-13.6 \times 4^2}{1^2}$ $=-13.6 \times 16$ $=-217.6 \mathrm{eV}$ So, Ionisation energy $=217.6 \mathrm{eV}$
J and K CET-(2018)
Classification of Elements and Periodicity in Properties
89613
The ionisation energy of nitrogen is larger than that of oxygen because :
1 the size of nitrogen atom is smaller
2 there is greater attraction of electrons towards the nucleus
3 half-filled p-orbitals of nitrogen have extra stability
4 None of the above
Explanation:
The electronic configuration of nitrogen and oxygen are- $\begin{aligned} & { }_7 \mathrm{~N}-1 \mathrm{~s}^2, 2 \mathrm{~s}^2, 2 \mathrm{p}^3 \\ & { }_8 \mathrm{O}-1 \mathrm{~s}^2, 2 \mathrm{~s}^2, 2 \mathrm{p}^4 \end{aligned}$ Thus, the ionisation energy of nitrogen is larger than that of oxygen because of half-filled p-orbitals of nitrogen have extra stability.
Manipal-2017
Classification of Elements and Periodicity in Properties
89604
Assertion: $\mathrm{Li}$ has high ionisation enthalpy, while $\mathrm{Li}$ is the strongest reducing agent in aqueous medium. Reason : $\mathrm{Li}$ has high oxidation potential.
1 If both Assertion and Reason are correct and Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
Li has high ionization energy, while $\mathrm{Li}$ is the strongest reducing agent in aqueous medium because of large amount of hydration energy is realized and on account of large amount of hydration energy molecules it strongest reducing agent and $\mathrm{Li}$ has high oxidation potential.
