Classification of Elements and Periodicity in Properties
89577
A sudden large jump between the values of second and third ionization energies of elements would be associated with which of the following electronic configurations?
The sudden large jump between the value of second and third ionisaiton energies of an element. Because after losing two electron it has acquired stable configuration. Thus, in order to remove third electron much higher energy is needed. Therefore, the electronic configuration is $1 \mathrm{~s}^2 2 \mathrm{~s}^2 2 \mathrm{p}^6 3 \mathrm{~s}^2$.
J and K CET-(2004)
Classification of Elements and Periodicity in Properties
89578
First ionisation potential of $B e$ and $B$ will be
1 8.8 and 8.8
2 6.6 and 6.6
3 6.6 and 8.8
4 8.8 and 6.6
Explanation:
Ionization potential increase from left to right in a period but in case of $\mathrm{Be}$ and $\mathrm{B}$. Beryllium is having more ionization potential than boron to completely filled s-orbital in beryllium. So, the first ionization potential of $\mathrm{Be}$ and $\mathrm{B}$ will be 8.8 and 6.6 respectively.
NEET-1998
Classification of Elements and Periodicity in Properties
89580
Which one of the following order is correct for the first ionization energies of the elements?
1 B $<$ Be $<\mathrm{N}<\mathrm{O}$
2 $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$
3 B $<$ Be $<\mathrm{O}<\mathrm{N}$
4 $\mathrm{B}<\mathrm{O}<\mathrm{Be}<\mathrm{N}$
Explanation:
Along a period first ionization energy increases. Thus, the first IE of the elements in second period should follow the order $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$ The first IE of these elements follows the order $\mathrm{B}<\mathrm{Be}$ $<\mathrm{O}<\mathrm{N}$ The lower IE of $\mathrm{B}$ than that of $\mathrm{Be}$ is because in $\mathrm{B}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2 2 \mathrm{p}^1\right)$, electron is to be removed from $2 \mathrm{p}$ which is easy while in $\operatorname{Be}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2\right)$, electron is to be removed from $2 \mathrm{~s}$ which is difficult. The low IE of $\mathrm{O}$ than that of $\mathrm{N}$ is because of the half-filled $2 \mathrm{p}$ orbitals in $\mathrm{N}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2 2 \mathrm{p}^3\right)$.
JIPMER-2004
Classification of Elements and Periodicity in Properties
89584
The third ionisation enthalpy is highest in
1 Alkali metals
2 Alkaline earth metals
3 Chalcogens
4 Pnictogens
Explanation:
Alkaline earth metals acquired the outer two electron in s-orbital. After removing of two electron from alkaline earth's metal, they get the stable configuration. So more energy required for the removing of electron. Hence, alkaline earth metals have the highest third ionization enthalphy.
Classification of Elements and Periodicity in Properties
89577
A sudden large jump between the values of second and third ionization energies of elements would be associated with which of the following electronic configurations?
The sudden large jump between the value of second and third ionisaiton energies of an element. Because after losing two electron it has acquired stable configuration. Thus, in order to remove third electron much higher energy is needed. Therefore, the electronic configuration is $1 \mathrm{~s}^2 2 \mathrm{~s}^2 2 \mathrm{p}^6 3 \mathrm{~s}^2$.
J and K CET-(2004)
Classification of Elements and Periodicity in Properties
89578
First ionisation potential of $B e$ and $B$ will be
1 8.8 and 8.8
2 6.6 and 6.6
3 6.6 and 8.8
4 8.8 and 6.6
Explanation:
Ionization potential increase from left to right in a period but in case of $\mathrm{Be}$ and $\mathrm{B}$. Beryllium is having more ionization potential than boron to completely filled s-orbital in beryllium. So, the first ionization potential of $\mathrm{Be}$ and $\mathrm{B}$ will be 8.8 and 6.6 respectively.
NEET-1998
Classification of Elements and Periodicity in Properties
89580
Which one of the following order is correct for the first ionization energies of the elements?
1 B $<$ Be $<\mathrm{N}<\mathrm{O}$
2 $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$
3 B $<$ Be $<\mathrm{O}<\mathrm{N}$
4 $\mathrm{B}<\mathrm{O}<\mathrm{Be}<\mathrm{N}$
Explanation:
Along a period first ionization energy increases. Thus, the first IE of the elements in second period should follow the order $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$ The first IE of these elements follows the order $\mathrm{B}<\mathrm{Be}$ $<\mathrm{O}<\mathrm{N}$ The lower IE of $\mathrm{B}$ than that of $\mathrm{Be}$ is because in $\mathrm{B}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2 2 \mathrm{p}^1\right)$, electron is to be removed from $2 \mathrm{p}$ which is easy while in $\operatorname{Be}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2\right)$, electron is to be removed from $2 \mathrm{~s}$ which is difficult. The low IE of $\mathrm{O}$ than that of $\mathrm{N}$ is because of the half-filled $2 \mathrm{p}$ orbitals in $\mathrm{N}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2 2 \mathrm{p}^3\right)$.
JIPMER-2004
Classification of Elements and Periodicity in Properties
89584
The third ionisation enthalpy is highest in
1 Alkali metals
2 Alkaline earth metals
3 Chalcogens
4 Pnictogens
Explanation:
Alkaline earth metals acquired the outer two electron in s-orbital. After removing of two electron from alkaline earth's metal, they get the stable configuration. So more energy required for the removing of electron. Hence, alkaline earth metals have the highest third ionization enthalphy.
Classification of Elements and Periodicity in Properties
89577
A sudden large jump between the values of second and third ionization energies of elements would be associated with which of the following electronic configurations?
The sudden large jump between the value of second and third ionisaiton energies of an element. Because after losing two electron it has acquired stable configuration. Thus, in order to remove third electron much higher energy is needed. Therefore, the electronic configuration is $1 \mathrm{~s}^2 2 \mathrm{~s}^2 2 \mathrm{p}^6 3 \mathrm{~s}^2$.
J and K CET-(2004)
Classification of Elements and Periodicity in Properties
89578
First ionisation potential of $B e$ and $B$ will be
1 8.8 and 8.8
2 6.6 and 6.6
3 6.6 and 8.8
4 8.8 and 6.6
Explanation:
Ionization potential increase from left to right in a period but in case of $\mathrm{Be}$ and $\mathrm{B}$. Beryllium is having more ionization potential than boron to completely filled s-orbital in beryllium. So, the first ionization potential of $\mathrm{Be}$ and $\mathrm{B}$ will be 8.8 and 6.6 respectively.
NEET-1998
Classification of Elements and Periodicity in Properties
89580
Which one of the following order is correct for the first ionization energies of the elements?
1 B $<$ Be $<\mathrm{N}<\mathrm{O}$
2 $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$
3 B $<$ Be $<\mathrm{O}<\mathrm{N}$
4 $\mathrm{B}<\mathrm{O}<\mathrm{Be}<\mathrm{N}$
Explanation:
Along a period first ionization energy increases. Thus, the first IE of the elements in second period should follow the order $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$ The first IE of these elements follows the order $\mathrm{B}<\mathrm{Be}$ $<\mathrm{O}<\mathrm{N}$ The lower IE of $\mathrm{B}$ than that of $\mathrm{Be}$ is because in $\mathrm{B}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2 2 \mathrm{p}^1\right)$, electron is to be removed from $2 \mathrm{p}$ which is easy while in $\operatorname{Be}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2\right)$, electron is to be removed from $2 \mathrm{~s}$ which is difficult. The low IE of $\mathrm{O}$ than that of $\mathrm{N}$ is because of the half-filled $2 \mathrm{p}$ orbitals in $\mathrm{N}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2 2 \mathrm{p}^3\right)$.
JIPMER-2004
Classification of Elements and Periodicity in Properties
89584
The third ionisation enthalpy is highest in
1 Alkali metals
2 Alkaline earth metals
3 Chalcogens
4 Pnictogens
Explanation:
Alkaline earth metals acquired the outer two electron in s-orbital. After removing of two electron from alkaline earth's metal, they get the stable configuration. So more energy required for the removing of electron. Hence, alkaline earth metals have the highest third ionization enthalphy.
Classification of Elements and Periodicity in Properties
89577
A sudden large jump between the values of second and third ionization energies of elements would be associated with which of the following electronic configurations?
The sudden large jump between the value of second and third ionisaiton energies of an element. Because after losing two electron it has acquired stable configuration. Thus, in order to remove third electron much higher energy is needed. Therefore, the electronic configuration is $1 \mathrm{~s}^2 2 \mathrm{~s}^2 2 \mathrm{p}^6 3 \mathrm{~s}^2$.
J and K CET-(2004)
Classification of Elements and Periodicity in Properties
89578
First ionisation potential of $B e$ and $B$ will be
1 8.8 and 8.8
2 6.6 and 6.6
3 6.6 and 8.8
4 8.8 and 6.6
Explanation:
Ionization potential increase from left to right in a period but in case of $\mathrm{Be}$ and $\mathrm{B}$. Beryllium is having more ionization potential than boron to completely filled s-orbital in beryllium. So, the first ionization potential of $\mathrm{Be}$ and $\mathrm{B}$ will be 8.8 and 6.6 respectively.
NEET-1998
Classification of Elements and Periodicity in Properties
89580
Which one of the following order is correct for the first ionization energies of the elements?
1 B $<$ Be $<\mathrm{N}<\mathrm{O}$
2 $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$
3 B $<$ Be $<\mathrm{O}<\mathrm{N}$
4 $\mathrm{B}<\mathrm{O}<\mathrm{Be}<\mathrm{N}$
Explanation:
Along a period first ionization energy increases. Thus, the first IE of the elements in second period should follow the order $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$ The first IE of these elements follows the order $\mathrm{B}<\mathrm{Be}$ $<\mathrm{O}<\mathrm{N}$ The lower IE of $\mathrm{B}$ than that of $\mathrm{Be}$ is because in $\mathrm{B}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2 2 \mathrm{p}^1\right)$, electron is to be removed from $2 \mathrm{p}$ which is easy while in $\operatorname{Be}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2\right)$, electron is to be removed from $2 \mathrm{~s}$ which is difficult. The low IE of $\mathrm{O}$ than that of $\mathrm{N}$ is because of the half-filled $2 \mathrm{p}$ orbitals in $\mathrm{N}\left(1 \mathrm{~s}^2, 2 \mathrm{~s}^2 2 \mathrm{p}^3\right)$.
JIPMER-2004
Classification of Elements and Periodicity in Properties
89584
The third ionisation enthalpy is highest in
1 Alkali metals
2 Alkaline earth metals
3 Chalcogens
4 Pnictogens
Explanation:
Alkaline earth metals acquired the outer two electron in s-orbital. After removing of two electron from alkaline earth's metal, they get the stable configuration. So more energy required for the removing of electron. Hence, alkaline earth metals have the highest third ionization enthalphy.
