Classification of Elements and Periodicity in Properties
89727
The atomic numbers of elements $A, B, C$ and $D$ are $Z-1, Z, Z+1$ and $Z+2$, respectively. If ' $B$ ' is a noble gas, choose the correct answers from the following statements
1 (1) and (2)
2 (2) and (3)
3 (1) and (3)
4 (1), (2) and (3)
Explanation:
Given that, Atomic no. of element $A=Z-1$, i.e, halogen Atomic no. of element $B=Z$, i.e, noble gas Atomic no. of element $C=Z+1$, i.e, group IA Atomic no. of element $\mathrm{D}=\mathrm{Z}+2$, i.e, group IIA $\therefore$ Element A must be halogen i.e, have the highest electron affinity. - Element B is Noble gas. - Element $\mathrm{C}$ must be an alkali metal exist as +1 oxidation state. - Element D must be alkaline earth metal.
A.P.EAMCET 2008
Classification of Elements and Periodicity in Properties
89731
Which of the following has lowest electron affinity?
1 $\mathrm{Cl}$
2 I
3 $\mathrm{F}$
4 $\mathrm{Br}$
Explanation:
When we moving on a group, electron affinity decrease due to the size of atom increase. | Halogen | $F$ | $Cl$ | $Br$ | $I$ | |---|---|---|---|---| |$()$ | -3.6 | -3.8 | -3.5 | -3 | | Hence, the electron affinity is highest in $\mathrm{Cl}$ and lowest in Iodine(I).
J and K CET-(2005)
Classification of Elements and Periodicity in Properties
89700
The correct order of electron affinity is
1 B $<\mathrm{C}<\mathrm{O}>\mathrm{N}$
2 B $>$ C $>\mathrm{N}>\mathrm{O}$
3 O $>$ C $>$ B $>\mathrm{N}$
4 O $<$ C $<$ B $<\mathrm{N}$
Explanation:
When on going from left to right in the periodic table, electron affinity increases, because the distance between the nucleus and outermost shell decreases. So the attraction of the nucleus and electrons of the outermost shell increases hence the added electron get stabilization. Nitrogen has a half-filled electronic configuration, so, it tendency to accept electron is very less than carbon and boron. Hence, the electron affinity order is- $$ \mathrm{O}>\mathrm{C}>\mathrm{B}>\mathrm{N} $$
J and K CET-(2005) Assam CEE-2014
Classification of Elements and Periodicity in Properties
89698
Maximum electron affinity is shown by the following:
1 $\mathrm{Cl}$
2 $\mathrm{Br}$
3 $\mathrm{N}$
4 $\mathrm{Na}$
Explanation:
Electron affinity:- The amount of energy liberated when an electron is added to a neutral atom to form a negatively charged ion. Electron affinity : $\mathrm{Cl}>\mathrm{F}>\mathrm{Br}>\mathrm{I}$. Electron affinity $\propto \frac{1}{\text { Atomicsize }}$.
Classification of Elements and Periodicity in Properties
89727
The atomic numbers of elements $A, B, C$ and $D$ are $Z-1, Z, Z+1$ and $Z+2$, respectively. If ' $B$ ' is a noble gas, choose the correct answers from the following statements
1 (1) and (2)
2 (2) and (3)
3 (1) and (3)
4 (1), (2) and (3)
Explanation:
Given that, Atomic no. of element $A=Z-1$, i.e, halogen Atomic no. of element $B=Z$, i.e, noble gas Atomic no. of element $C=Z+1$, i.e, group IA Atomic no. of element $\mathrm{D}=\mathrm{Z}+2$, i.e, group IIA $\therefore$ Element A must be halogen i.e, have the highest electron affinity. - Element B is Noble gas. - Element $\mathrm{C}$ must be an alkali metal exist as +1 oxidation state. - Element D must be alkaline earth metal.
A.P.EAMCET 2008
Classification of Elements and Periodicity in Properties
89731
Which of the following has lowest electron affinity?
1 $\mathrm{Cl}$
2 I
3 $\mathrm{F}$
4 $\mathrm{Br}$
Explanation:
When we moving on a group, electron affinity decrease due to the size of atom increase. | Halogen | $F$ | $Cl$ | $Br$ | $I$ | |---|---|---|---|---| |$()$ | -3.6 | -3.8 | -3.5 | -3 | | Hence, the electron affinity is highest in $\mathrm{Cl}$ and lowest in Iodine(I).
J and K CET-(2005)
Classification of Elements and Periodicity in Properties
89700
The correct order of electron affinity is
1 B $<\mathrm{C}<\mathrm{O}>\mathrm{N}$
2 B $>$ C $>\mathrm{N}>\mathrm{O}$
3 O $>$ C $>$ B $>\mathrm{N}$
4 O $<$ C $<$ B $<\mathrm{N}$
Explanation:
When on going from left to right in the periodic table, electron affinity increases, because the distance between the nucleus and outermost shell decreases. So the attraction of the nucleus and electrons of the outermost shell increases hence the added electron get stabilization. Nitrogen has a half-filled electronic configuration, so, it tendency to accept electron is very less than carbon and boron. Hence, the electron affinity order is- $$ \mathrm{O}>\mathrm{C}>\mathrm{B}>\mathrm{N} $$
J and K CET-(2005) Assam CEE-2014
Classification of Elements and Periodicity in Properties
89698
Maximum electron affinity is shown by the following:
1 $\mathrm{Cl}$
2 $\mathrm{Br}$
3 $\mathrm{N}$
4 $\mathrm{Na}$
Explanation:
Electron affinity:- The amount of energy liberated when an electron is added to a neutral atom to form a negatively charged ion. Electron affinity : $\mathrm{Cl}>\mathrm{F}>\mathrm{Br}>\mathrm{I}$. Electron affinity $\propto \frac{1}{\text { Atomicsize }}$.
Classification of Elements and Periodicity in Properties
89727
The atomic numbers of elements $A, B, C$ and $D$ are $Z-1, Z, Z+1$ and $Z+2$, respectively. If ' $B$ ' is a noble gas, choose the correct answers from the following statements
1 (1) and (2)
2 (2) and (3)
3 (1) and (3)
4 (1), (2) and (3)
Explanation:
Given that, Atomic no. of element $A=Z-1$, i.e, halogen Atomic no. of element $B=Z$, i.e, noble gas Atomic no. of element $C=Z+1$, i.e, group IA Atomic no. of element $\mathrm{D}=\mathrm{Z}+2$, i.e, group IIA $\therefore$ Element A must be halogen i.e, have the highest electron affinity. - Element B is Noble gas. - Element $\mathrm{C}$ must be an alkali metal exist as +1 oxidation state. - Element D must be alkaline earth metal.
A.P.EAMCET 2008
Classification of Elements and Periodicity in Properties
89731
Which of the following has lowest electron affinity?
1 $\mathrm{Cl}$
2 I
3 $\mathrm{F}$
4 $\mathrm{Br}$
Explanation:
When we moving on a group, electron affinity decrease due to the size of atom increase. | Halogen | $F$ | $Cl$ | $Br$ | $I$ | |---|---|---|---|---| |$()$ | -3.6 | -3.8 | -3.5 | -3 | | Hence, the electron affinity is highest in $\mathrm{Cl}$ and lowest in Iodine(I).
J and K CET-(2005)
Classification of Elements and Periodicity in Properties
89700
The correct order of electron affinity is
1 B $<\mathrm{C}<\mathrm{O}>\mathrm{N}$
2 B $>$ C $>\mathrm{N}>\mathrm{O}$
3 O $>$ C $>$ B $>\mathrm{N}$
4 O $<$ C $<$ B $<\mathrm{N}$
Explanation:
When on going from left to right in the periodic table, electron affinity increases, because the distance between the nucleus and outermost shell decreases. So the attraction of the nucleus and electrons of the outermost shell increases hence the added electron get stabilization. Nitrogen has a half-filled electronic configuration, so, it tendency to accept electron is very less than carbon and boron. Hence, the electron affinity order is- $$ \mathrm{O}>\mathrm{C}>\mathrm{B}>\mathrm{N} $$
J and K CET-(2005) Assam CEE-2014
Classification of Elements and Periodicity in Properties
89698
Maximum electron affinity is shown by the following:
1 $\mathrm{Cl}$
2 $\mathrm{Br}$
3 $\mathrm{N}$
4 $\mathrm{Na}$
Explanation:
Electron affinity:- The amount of energy liberated when an electron is added to a neutral atom to form a negatively charged ion. Electron affinity : $\mathrm{Cl}>\mathrm{F}>\mathrm{Br}>\mathrm{I}$. Electron affinity $\propto \frac{1}{\text { Atomicsize }}$.
Classification of Elements and Periodicity in Properties
89727
The atomic numbers of elements $A, B, C$ and $D$ are $Z-1, Z, Z+1$ and $Z+2$, respectively. If ' $B$ ' is a noble gas, choose the correct answers from the following statements
1 (1) and (2)
2 (2) and (3)
3 (1) and (3)
4 (1), (2) and (3)
Explanation:
Given that, Atomic no. of element $A=Z-1$, i.e, halogen Atomic no. of element $B=Z$, i.e, noble gas Atomic no. of element $C=Z+1$, i.e, group IA Atomic no. of element $\mathrm{D}=\mathrm{Z}+2$, i.e, group IIA $\therefore$ Element A must be halogen i.e, have the highest electron affinity. - Element B is Noble gas. - Element $\mathrm{C}$ must be an alkali metal exist as +1 oxidation state. - Element D must be alkaline earth metal.
A.P.EAMCET 2008
Classification of Elements and Periodicity in Properties
89731
Which of the following has lowest electron affinity?
1 $\mathrm{Cl}$
2 I
3 $\mathrm{F}$
4 $\mathrm{Br}$
Explanation:
When we moving on a group, electron affinity decrease due to the size of atom increase. | Halogen | $F$ | $Cl$ | $Br$ | $I$ | |---|---|---|---|---| |$()$ | -3.6 | -3.8 | -3.5 | -3 | | Hence, the electron affinity is highest in $\mathrm{Cl}$ and lowest in Iodine(I).
J and K CET-(2005)
Classification of Elements and Periodicity in Properties
89700
The correct order of electron affinity is
1 B $<\mathrm{C}<\mathrm{O}>\mathrm{N}$
2 B $>$ C $>\mathrm{N}>\mathrm{O}$
3 O $>$ C $>$ B $>\mathrm{N}$
4 O $<$ C $<$ B $<\mathrm{N}$
Explanation:
When on going from left to right in the periodic table, electron affinity increases, because the distance between the nucleus and outermost shell decreases. So the attraction of the nucleus and electrons of the outermost shell increases hence the added electron get stabilization. Nitrogen has a half-filled electronic configuration, so, it tendency to accept electron is very less than carbon and boron. Hence, the electron affinity order is- $$ \mathrm{O}>\mathrm{C}>\mathrm{B}>\mathrm{N} $$
J and K CET-(2005) Assam CEE-2014
Classification of Elements and Periodicity in Properties
89698
Maximum electron affinity is shown by the following:
1 $\mathrm{Cl}$
2 $\mathrm{Br}$
3 $\mathrm{N}$
4 $\mathrm{Na}$
Explanation:
Electron affinity:- The amount of energy liberated when an electron is added to a neutral atom to form a negatively charged ion. Electron affinity : $\mathrm{Cl}>\mathrm{F}>\mathrm{Br}>\mathrm{I}$. Electron affinity $\propto \frac{1}{\text { Atomicsize }}$.
