307449
What is the maximum number of electrons that can be associated with a following set of quantum numbers? \({\rm{(n = 3,l = 1}}\,\,{\rm{and}}\,\,{\rm{m = - 1)}}\)
1 \({\rm{2}}\)
2 \({\rm{4}}\)
3 \({\rm{6}}\)
4 \({\rm{10}}\)
Explanation:
\({\rm{(n = 3,l = 1}}\) is 3p sub-shell and thus 2 electrons can exist in one of the 3p-orbital \(\left( {{\rm{m = - 1}}} \right)\) \({\rm{n = 5,l = 0,m = 0,s = + }}\frac{{\rm{1}}}{{\rm{2}}}\) or \({\rm{ - }}\frac{{\rm{1}}}{{\rm{2}}}\)
CHXI02:STRUCTURE OF ATOM
307450
The maximum number of electrons with clockwise spin that can be accommodated in a f-subshell is
1 \({\rm{14}}\)
2 \({\rm{7}}\)
3 \({\rm{5}}\)
4 \({\rm{10}}\)
Explanation:
In a f–subshell, maximum 14 electrons can be accommodated, out of which 7 will have clockwise spin.
CHXI02:STRUCTURE OF ATOM
307468
Which one of the following set of quantum numbers is not possible for 4p electron?
307451
What is the correct orbital designation of an electron with the quantum number, \({\rm{n = 4,l = 3,m = - 2,s = 1/2}}\)?
1 \({\rm{3s}}\)
2 \({\rm{4f}}\)
3 \({\rm{5p}}\)
4 \({\rm{6s}}\)
Explanation:
\({\rm{n = 4}}\) represents \({{\rm{4}}^{{\rm{th}}}}\) orbit \({\rm{l = 3}}\) represents f subshell \({\rm{m = - 2}}\) represents orientation of f-orbital \({\rm{s = 1/2}}\) represents direction of spin of electron. \(\therefore \) The orbital is \({\rm{4f}}{\rm{.}}\)
307449
What is the maximum number of electrons that can be associated with a following set of quantum numbers? \({\rm{(n = 3,l = 1}}\,\,{\rm{and}}\,\,{\rm{m = - 1)}}\)
1 \({\rm{2}}\)
2 \({\rm{4}}\)
3 \({\rm{6}}\)
4 \({\rm{10}}\)
Explanation:
\({\rm{(n = 3,l = 1}}\) is 3p sub-shell and thus 2 electrons can exist in one of the 3p-orbital \(\left( {{\rm{m = - 1}}} \right)\) \({\rm{n = 5,l = 0,m = 0,s = + }}\frac{{\rm{1}}}{{\rm{2}}}\) or \({\rm{ - }}\frac{{\rm{1}}}{{\rm{2}}}\)
CHXI02:STRUCTURE OF ATOM
307450
The maximum number of electrons with clockwise spin that can be accommodated in a f-subshell is
1 \({\rm{14}}\)
2 \({\rm{7}}\)
3 \({\rm{5}}\)
4 \({\rm{10}}\)
Explanation:
In a f–subshell, maximum 14 electrons can be accommodated, out of which 7 will have clockwise spin.
CHXI02:STRUCTURE OF ATOM
307468
Which one of the following set of quantum numbers is not possible for 4p electron?
307451
What is the correct orbital designation of an electron with the quantum number, \({\rm{n = 4,l = 3,m = - 2,s = 1/2}}\)?
1 \({\rm{3s}}\)
2 \({\rm{4f}}\)
3 \({\rm{5p}}\)
4 \({\rm{6s}}\)
Explanation:
\({\rm{n = 4}}\) represents \({{\rm{4}}^{{\rm{th}}}}\) orbit \({\rm{l = 3}}\) represents f subshell \({\rm{m = - 2}}\) represents orientation of f-orbital \({\rm{s = 1/2}}\) represents direction of spin of electron. \(\therefore \) The orbital is \({\rm{4f}}{\rm{.}}\)
307449
What is the maximum number of electrons that can be associated with a following set of quantum numbers? \({\rm{(n = 3,l = 1}}\,\,{\rm{and}}\,\,{\rm{m = - 1)}}\)
1 \({\rm{2}}\)
2 \({\rm{4}}\)
3 \({\rm{6}}\)
4 \({\rm{10}}\)
Explanation:
\({\rm{(n = 3,l = 1}}\) is 3p sub-shell and thus 2 electrons can exist in one of the 3p-orbital \(\left( {{\rm{m = - 1}}} \right)\) \({\rm{n = 5,l = 0,m = 0,s = + }}\frac{{\rm{1}}}{{\rm{2}}}\) or \({\rm{ - }}\frac{{\rm{1}}}{{\rm{2}}}\)
CHXI02:STRUCTURE OF ATOM
307450
The maximum number of electrons with clockwise spin that can be accommodated in a f-subshell is
1 \({\rm{14}}\)
2 \({\rm{7}}\)
3 \({\rm{5}}\)
4 \({\rm{10}}\)
Explanation:
In a f–subshell, maximum 14 electrons can be accommodated, out of which 7 will have clockwise spin.
CHXI02:STRUCTURE OF ATOM
307468
Which one of the following set of quantum numbers is not possible for 4p electron?
307451
What is the correct orbital designation of an electron with the quantum number, \({\rm{n = 4,l = 3,m = - 2,s = 1/2}}\)?
1 \({\rm{3s}}\)
2 \({\rm{4f}}\)
3 \({\rm{5p}}\)
4 \({\rm{6s}}\)
Explanation:
\({\rm{n = 4}}\) represents \({{\rm{4}}^{{\rm{th}}}}\) orbit \({\rm{l = 3}}\) represents f subshell \({\rm{m = - 2}}\) represents orientation of f-orbital \({\rm{s = 1/2}}\) represents direction of spin of electron. \(\therefore \) The orbital is \({\rm{4f}}{\rm{.}}\)
307449
What is the maximum number of electrons that can be associated with a following set of quantum numbers? \({\rm{(n = 3,l = 1}}\,\,{\rm{and}}\,\,{\rm{m = - 1)}}\)
1 \({\rm{2}}\)
2 \({\rm{4}}\)
3 \({\rm{6}}\)
4 \({\rm{10}}\)
Explanation:
\({\rm{(n = 3,l = 1}}\) is 3p sub-shell and thus 2 electrons can exist in one of the 3p-orbital \(\left( {{\rm{m = - 1}}} \right)\) \({\rm{n = 5,l = 0,m = 0,s = + }}\frac{{\rm{1}}}{{\rm{2}}}\) or \({\rm{ - }}\frac{{\rm{1}}}{{\rm{2}}}\)
CHXI02:STRUCTURE OF ATOM
307450
The maximum number of electrons with clockwise spin that can be accommodated in a f-subshell is
1 \({\rm{14}}\)
2 \({\rm{7}}\)
3 \({\rm{5}}\)
4 \({\rm{10}}\)
Explanation:
In a f–subshell, maximum 14 electrons can be accommodated, out of which 7 will have clockwise spin.
CHXI02:STRUCTURE OF ATOM
307468
Which one of the following set of quantum numbers is not possible for 4p electron?
307451
What is the correct orbital designation of an electron with the quantum number, \({\rm{n = 4,l = 3,m = - 2,s = 1/2}}\)?
1 \({\rm{3s}}\)
2 \({\rm{4f}}\)
3 \({\rm{5p}}\)
4 \({\rm{6s}}\)
Explanation:
\({\rm{n = 4}}\) represents \({{\rm{4}}^{{\rm{th}}}}\) orbit \({\rm{l = 3}}\) represents f subshell \({\rm{m = - 2}}\) represents orientation of f-orbital \({\rm{s = 1/2}}\) represents direction of spin of electron. \(\therefore \) The orbital is \({\rm{4f}}{\rm{.}}\)
