Classification of Elements and Periodicity in Properties
89608
The second ionisation energy of the following elements follows the order
1 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
2 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
3 $\mathrm{Cd}>\mathrm{Hg}<\mathrm{Zn}$
4 $\mathrm{Zn}<\mathrm{Cd}<\mathrm{Hg}$
Explanation:
From moving top to bottom in a group ionisation energy decrease due to nuclear charge increases, atomic size increase and the number of shells increases. Thus the electron are loosely held with the nucleus. The order of ionisation energy is- $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89618
The second ionisation enthalpy of which of the following alkaline earth metals is the highest?
1 $\mathrm{Ba}$
2 $\mathrm{Mg}$
3 $\mathrm{Ca}$
4 $\mathrm{Sr}$
5 $\mathrm{Be}$
Explanation:
Ionization energy increase on decreasing the size of atom. Ionisation energy $\propto \frac{1}{\text { size }}$ The second ionisation energy of $\mathrm{Be}$ is the enthalpy change when 1 mole of gaseous ion of an element each with a single positive charge each lose an electron to form gaseous ion each with a double positive charge ie. $\mathrm{Be}^{+2}$ due to less size and high ionisation potential.
Kerala-CEE-2016
Classification of Elements and Periodicity in Properties
89627
The correct order of ionization energies is
1 $\mathrm{Cu}>\mathrm{Ag}>\mathrm{Au}$
2 $\mathrm{Cu}>\mathrm{Au}>\mathrm{Ag}$
3 $\mathrm{Au}>\mathrm{Cu}>\mathrm{Ag}$
4 $\mathrm{Ag}>\mathrm{Au}>\mathrm{Cu}$
Explanation:
These element belong to the 11 group of Periodic tables. As we move down the group, ionization energy decreases, but due to f-electrons and its ionization energy becomes high so, the order of ionization energies is- $$ \mathrm{Au}>\mathrm{Cu}>\mathrm{Ag} $$
UPTU/UPSEE-2013
Classification of Elements and Periodicity in Properties
89629
Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se and Ar?
Ionisation energy of element increases across a period in the periodic table because the electrons are held tightly by the higher effective nuclear charge. The ionisation energy of the elements decreases on moving down the group because the electrons are held in lower energy orbitals away from the nucleus. Ar is higher ionisation energy because it is a noble gas and $\mathrm{Ba}$ has the lowest ionization energy as it in six period of element. So, the increasing order of first ionisation energy are- $$ \mathrm{Ba}<\mathrm{Ca}<\mathrm{Se}<\mathrm{S}<\mathrm{Ar} $$
(JEE Main 2013)
Classification of Elements and Periodicity in Properties
89635
Which one of the following does not correctly represent the correct order of the property indicated against it?
1 $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$; increasing number of oxidation states
2 $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$; magnetic moment
The increasing order of second ionisation energy is $\mathrm{Cr}>\mathrm{Mn}>\mathrm{V}>\mathrm{Ti}$ (A) $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$ has increasing oxidation state (B) $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$ has magnetic moment increases (C) $\mathrm{Ti}<\mathrm{V}<\mathrm{Mn}<\mathrm{Cr}$ has increasing $2^{\text {nd }}$ ionisation enthalpy
Classification of Elements and Periodicity in Properties
89608
The second ionisation energy of the following elements follows the order
1 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
2 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
3 $\mathrm{Cd}>\mathrm{Hg}<\mathrm{Zn}$
4 $\mathrm{Zn}<\mathrm{Cd}<\mathrm{Hg}$
Explanation:
From moving top to bottom in a group ionisation energy decrease due to nuclear charge increases, atomic size increase and the number of shells increases. Thus the electron are loosely held with the nucleus. The order of ionisation energy is- $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89618
The second ionisation enthalpy of which of the following alkaline earth metals is the highest?
1 $\mathrm{Ba}$
2 $\mathrm{Mg}$
3 $\mathrm{Ca}$
4 $\mathrm{Sr}$
5 $\mathrm{Be}$
Explanation:
Ionization energy increase on decreasing the size of atom. Ionisation energy $\propto \frac{1}{\text { size }}$ The second ionisation energy of $\mathrm{Be}$ is the enthalpy change when 1 mole of gaseous ion of an element each with a single positive charge each lose an electron to form gaseous ion each with a double positive charge ie. $\mathrm{Be}^{+2}$ due to less size and high ionisation potential.
Kerala-CEE-2016
Classification of Elements and Periodicity in Properties
89627
The correct order of ionization energies is
1 $\mathrm{Cu}>\mathrm{Ag}>\mathrm{Au}$
2 $\mathrm{Cu}>\mathrm{Au}>\mathrm{Ag}$
3 $\mathrm{Au}>\mathrm{Cu}>\mathrm{Ag}$
4 $\mathrm{Ag}>\mathrm{Au}>\mathrm{Cu}$
Explanation:
These element belong to the 11 group of Periodic tables. As we move down the group, ionization energy decreases, but due to f-electrons and its ionization energy becomes high so, the order of ionization energies is- $$ \mathrm{Au}>\mathrm{Cu}>\mathrm{Ag} $$
UPTU/UPSEE-2013
Classification of Elements and Periodicity in Properties
89629
Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se and Ar?
Ionisation energy of element increases across a period in the periodic table because the electrons are held tightly by the higher effective nuclear charge. The ionisation energy of the elements decreases on moving down the group because the electrons are held in lower energy orbitals away from the nucleus. Ar is higher ionisation energy because it is a noble gas and $\mathrm{Ba}$ has the lowest ionization energy as it in six period of element. So, the increasing order of first ionisation energy are- $$ \mathrm{Ba}<\mathrm{Ca}<\mathrm{Se}<\mathrm{S}<\mathrm{Ar} $$
(JEE Main 2013)
Classification of Elements and Periodicity in Properties
89635
Which one of the following does not correctly represent the correct order of the property indicated against it?
1 $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$; increasing number of oxidation states
2 $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$; magnetic moment
The increasing order of second ionisation energy is $\mathrm{Cr}>\mathrm{Mn}>\mathrm{V}>\mathrm{Ti}$ (A) $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$ has increasing oxidation state (B) $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$ has magnetic moment increases (C) $\mathrm{Ti}<\mathrm{V}<\mathrm{Mn}<\mathrm{Cr}$ has increasing $2^{\text {nd }}$ ionisation enthalpy
Classification of Elements and Periodicity in Properties
89608
The second ionisation energy of the following elements follows the order
1 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
2 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
3 $\mathrm{Cd}>\mathrm{Hg}<\mathrm{Zn}$
4 $\mathrm{Zn}<\mathrm{Cd}<\mathrm{Hg}$
Explanation:
From moving top to bottom in a group ionisation energy decrease due to nuclear charge increases, atomic size increase and the number of shells increases. Thus the electron are loosely held with the nucleus. The order of ionisation energy is- $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89618
The second ionisation enthalpy of which of the following alkaline earth metals is the highest?
1 $\mathrm{Ba}$
2 $\mathrm{Mg}$
3 $\mathrm{Ca}$
4 $\mathrm{Sr}$
5 $\mathrm{Be}$
Explanation:
Ionization energy increase on decreasing the size of atom. Ionisation energy $\propto \frac{1}{\text { size }}$ The second ionisation energy of $\mathrm{Be}$ is the enthalpy change when 1 mole of gaseous ion of an element each with a single positive charge each lose an electron to form gaseous ion each with a double positive charge ie. $\mathrm{Be}^{+2}$ due to less size and high ionisation potential.
Kerala-CEE-2016
Classification of Elements and Periodicity in Properties
89627
The correct order of ionization energies is
1 $\mathrm{Cu}>\mathrm{Ag}>\mathrm{Au}$
2 $\mathrm{Cu}>\mathrm{Au}>\mathrm{Ag}$
3 $\mathrm{Au}>\mathrm{Cu}>\mathrm{Ag}$
4 $\mathrm{Ag}>\mathrm{Au}>\mathrm{Cu}$
Explanation:
These element belong to the 11 group of Periodic tables. As we move down the group, ionization energy decreases, but due to f-electrons and its ionization energy becomes high so, the order of ionization energies is- $$ \mathrm{Au}>\mathrm{Cu}>\mathrm{Ag} $$
UPTU/UPSEE-2013
Classification of Elements and Periodicity in Properties
89629
Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se and Ar?
Ionisation energy of element increases across a period in the periodic table because the electrons are held tightly by the higher effective nuclear charge. The ionisation energy of the elements decreases on moving down the group because the electrons are held in lower energy orbitals away from the nucleus. Ar is higher ionisation energy because it is a noble gas and $\mathrm{Ba}$ has the lowest ionization energy as it in six period of element. So, the increasing order of first ionisation energy are- $$ \mathrm{Ba}<\mathrm{Ca}<\mathrm{Se}<\mathrm{S}<\mathrm{Ar} $$
(JEE Main 2013)
Classification of Elements and Periodicity in Properties
89635
Which one of the following does not correctly represent the correct order of the property indicated against it?
1 $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$; increasing number of oxidation states
2 $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$; magnetic moment
The increasing order of second ionisation energy is $\mathrm{Cr}>\mathrm{Mn}>\mathrm{V}>\mathrm{Ti}$ (A) $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$ has increasing oxidation state (B) $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$ has magnetic moment increases (C) $\mathrm{Ti}<\mathrm{V}<\mathrm{Mn}<\mathrm{Cr}$ has increasing $2^{\text {nd }}$ ionisation enthalpy
Classification of Elements and Periodicity in Properties
89608
The second ionisation energy of the following elements follows the order
1 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
2 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
3 $\mathrm{Cd}>\mathrm{Hg}<\mathrm{Zn}$
4 $\mathrm{Zn}<\mathrm{Cd}<\mathrm{Hg}$
Explanation:
From moving top to bottom in a group ionisation energy decrease due to nuclear charge increases, atomic size increase and the number of shells increases. Thus the electron are loosely held with the nucleus. The order of ionisation energy is- $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89618
The second ionisation enthalpy of which of the following alkaline earth metals is the highest?
1 $\mathrm{Ba}$
2 $\mathrm{Mg}$
3 $\mathrm{Ca}$
4 $\mathrm{Sr}$
5 $\mathrm{Be}$
Explanation:
Ionization energy increase on decreasing the size of atom. Ionisation energy $\propto \frac{1}{\text { size }}$ The second ionisation energy of $\mathrm{Be}$ is the enthalpy change when 1 mole of gaseous ion of an element each with a single positive charge each lose an electron to form gaseous ion each with a double positive charge ie. $\mathrm{Be}^{+2}$ due to less size and high ionisation potential.
Kerala-CEE-2016
Classification of Elements and Periodicity in Properties
89627
The correct order of ionization energies is
1 $\mathrm{Cu}>\mathrm{Ag}>\mathrm{Au}$
2 $\mathrm{Cu}>\mathrm{Au}>\mathrm{Ag}$
3 $\mathrm{Au}>\mathrm{Cu}>\mathrm{Ag}$
4 $\mathrm{Ag}>\mathrm{Au}>\mathrm{Cu}$
Explanation:
These element belong to the 11 group of Periodic tables. As we move down the group, ionization energy decreases, but due to f-electrons and its ionization energy becomes high so, the order of ionization energies is- $$ \mathrm{Au}>\mathrm{Cu}>\mathrm{Ag} $$
UPTU/UPSEE-2013
Classification of Elements and Periodicity in Properties
89629
Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se and Ar?
Ionisation energy of element increases across a period in the periodic table because the electrons are held tightly by the higher effective nuclear charge. The ionisation energy of the elements decreases on moving down the group because the electrons are held in lower energy orbitals away from the nucleus. Ar is higher ionisation energy because it is a noble gas and $\mathrm{Ba}$ has the lowest ionization energy as it in six period of element. So, the increasing order of first ionisation energy are- $$ \mathrm{Ba}<\mathrm{Ca}<\mathrm{Se}<\mathrm{S}<\mathrm{Ar} $$
(JEE Main 2013)
Classification of Elements and Periodicity in Properties
89635
Which one of the following does not correctly represent the correct order of the property indicated against it?
1 $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$; increasing number of oxidation states
2 $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$; magnetic moment
The increasing order of second ionisation energy is $\mathrm{Cr}>\mathrm{Mn}>\mathrm{V}>\mathrm{Ti}$ (A) $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$ has increasing oxidation state (B) $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$ has magnetic moment increases (C) $\mathrm{Ti}<\mathrm{V}<\mathrm{Mn}<\mathrm{Cr}$ has increasing $2^{\text {nd }}$ ionisation enthalpy
Classification of Elements and Periodicity in Properties
89608
The second ionisation energy of the following elements follows the order
1 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
2 $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
3 $\mathrm{Cd}>\mathrm{Hg}<\mathrm{Zn}$
4 $\mathrm{Zn}<\mathrm{Cd}<\mathrm{Hg}$
Explanation:
From moving top to bottom in a group ionisation energy decrease due to nuclear charge increases, atomic size increase and the number of shells increases. Thus the electron are loosely held with the nucleus. The order of ionisation energy is- $\mathrm{Zn}>\mathrm{Cd}>\mathrm{Hg}$
WB-JEE-2019
Classification of Elements and Periodicity in Properties
89618
The second ionisation enthalpy of which of the following alkaline earth metals is the highest?
1 $\mathrm{Ba}$
2 $\mathrm{Mg}$
3 $\mathrm{Ca}$
4 $\mathrm{Sr}$
5 $\mathrm{Be}$
Explanation:
Ionization energy increase on decreasing the size of atom. Ionisation energy $\propto \frac{1}{\text { size }}$ The second ionisation energy of $\mathrm{Be}$ is the enthalpy change when 1 mole of gaseous ion of an element each with a single positive charge each lose an electron to form gaseous ion each with a double positive charge ie. $\mathrm{Be}^{+2}$ due to less size and high ionisation potential.
Kerala-CEE-2016
Classification of Elements and Periodicity in Properties
89627
The correct order of ionization energies is
1 $\mathrm{Cu}>\mathrm{Ag}>\mathrm{Au}$
2 $\mathrm{Cu}>\mathrm{Au}>\mathrm{Ag}$
3 $\mathrm{Au}>\mathrm{Cu}>\mathrm{Ag}$
4 $\mathrm{Ag}>\mathrm{Au}>\mathrm{Cu}$
Explanation:
These element belong to the 11 group of Periodic tables. As we move down the group, ionization energy decreases, but due to f-electrons and its ionization energy becomes high so, the order of ionization energies is- $$ \mathrm{Au}>\mathrm{Cu}>\mathrm{Ag} $$
UPTU/UPSEE-2013
Classification of Elements and Periodicity in Properties
89629
Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se and Ar?
Ionisation energy of element increases across a period in the periodic table because the electrons are held tightly by the higher effective nuclear charge. The ionisation energy of the elements decreases on moving down the group because the electrons are held in lower energy orbitals away from the nucleus. Ar is higher ionisation energy because it is a noble gas and $\mathrm{Ba}$ has the lowest ionization energy as it in six period of element. So, the increasing order of first ionisation energy are- $$ \mathrm{Ba}<\mathrm{Ca}<\mathrm{Se}<\mathrm{S}<\mathrm{Ar} $$
(JEE Main 2013)
Classification of Elements and Periodicity in Properties
89635
Which one of the following does not correctly represent the correct order of the property indicated against it?
1 $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$; increasing number of oxidation states
2 $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$; magnetic moment
The increasing order of second ionisation energy is $\mathrm{Cr}>\mathrm{Mn}>\mathrm{V}>\mathrm{Ti}$ (A) $\mathrm{Ti}<\mathrm{V}<\mathrm{Cr}<\mathrm{Mn}$ has increasing oxidation state (B) $\mathrm{Ti}^{3+}<\mathrm{V}^{3+}<\mathrm{Cr}^{3+}<\mathrm{Mn}^{3+}$ has magnetic moment increases (C) $\mathrm{Ti}<\mathrm{V}<\mathrm{Mn}<\mathrm{Cr}$ has increasing $2^{\text {nd }}$ ionisation enthalpy
