307312
Which one of the following statements in relation to the hydrogen atom is correct?
1 \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\)-orbitals all have the same energy
2 \(3 \mathrm{~s}\) and \(3 \mathrm{p}\)-orbitals are of lower energy than \(3 \mathrm{~d}\)-orbital
3 \(3 \mathrm{p}\)-orbital is lower in energy than \(3 \mathrm{~d}\)- orbital
4 \(3 \mathrm{~s}\)-orbital is lower in energy than \(3 \mathrm{p}\)- orbital
Explanation:
The hydrogen atom has the configuration \(1 \mathrm{~s}^{1}\) and \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\) -orbitals will have same energy with respect to \(1 \mathrm{~s}\)-orbital.
CHXI02:STRUCTURE OF ATOM
307313
Read the Statement - A and Statement - B carefully to mark the correct options given below Statement A : The orbitals having same energy are called as degenerate orbitals. Statement B : In hydrogen atom, 3 p and 3 d orbitals are not degenerate orbitals.
1 Statement A is incorrect but Statement B is correct.
2 Both statements are correct.
3 Statement A is correct but Statement B is incorrect.
4 Both Statements are incorrect.
Explanation:
In hydrogen atom, orbitals having same principal quantum number ( n ) are degenerate orbitals, i.e., energy of \({\mathrm{3 s=3 p=3 d}}\). So, the correct option is (3).
JEE Main - 2024
CHXI02:STRUCTURE OF ATOM
307314
For the electrons of oxygen atom, which of the following statements is correct?
1 \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \(\mathrm{2 p}\) orbital
2 An electron in the \(\mathrm{2 \mathrm{~s}}\) orbital has the same energy as an electron in the \(\mathrm{2p}\) orbital
3 \(\mathrm{Z_{\text {eff }}}\) for an electron in \({\text{1s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital
4 The two electrons present in the \({\text{2s}}\) orbital have spin quantum numbers \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) but of opposite sign
Explanation:
(a) Electrons in \(\mathrm{2 s}\) and \(\mathrm{2 p}\) orbitals have different screening effect. Hence, their \(\mathrm{Z_{\text {eff }}}\) is different \(\mathrm{\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{~s}}\) orbital \(\mathrm{>\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{p}}\) orbital. (b) Energy of 2s orbital \(\mathrm{ < }\) eneryg of \(\mathrm{2 p}\) orbital. (c) \(\mathrm{Z_{\text {eff }}}\) of \(\mathrm{1 \mathrm{~s}}\) orbital \(\mathrm{\neq Z_{\text {eff }}}\) of \(\mathrm{2 s}\) orbital (d) For the two electrons of \(\mathrm{2 \mathrm{~s}}\) orbital, the value of \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) is \(\mathrm{+\dfrac{1}{2}}\) and \(\mathrm{-\dfrac{1}{2}}\) i.e., is two electrons have same magnitude but have opposite sign (+ and -). Hence, option (4) is correct.
CHXI02:STRUCTURE OF ATOM
307315
Arrange in decreasing order, the energy of \(2 \mathrm{~s}\) orbitals in the following atoms \(\mathrm{H}, \mathrm{Li}, \mathrm{Na}, \mathrm{K}\)
Energy of the similar orbitals of different atoms decreases with increase in nuclear charge. Nuclear charge increases with number of nucleons present in nucleus. So, order of nuclear charge decreases as \(\mathrm{K}>\mathrm{Na}>\mathrm{Li}>\mathrm{H}\). Thus energy in decreasing order given as \({{\rm{E}}_{{\rm{2s(H)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Li)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Na)}}}}\,{\rm{ > }}{{\rm{E}}_{{\rm{2s(\;K)}}}}{\rm{.}}\)
CHXI02:STRUCTURE OF ATOM
307316
Arrange the orbitals of H-atom in the increasing order of their energies. \({\rm{3}}{{\rm{p}}_{\rm{x}}}{\rm{,2s,4}}{{\rm{d}}_{{\rm{xy}}}}{\rm{,3s,4}}{{\rm{p}}_{\rm{z}}}{\rm{,3}}{{\rm{p}}_{\rm{y}}}{\rm{,4s}}\)
307312
Which one of the following statements in relation to the hydrogen atom is correct?
1 \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\)-orbitals all have the same energy
2 \(3 \mathrm{~s}\) and \(3 \mathrm{p}\)-orbitals are of lower energy than \(3 \mathrm{~d}\)-orbital
3 \(3 \mathrm{p}\)-orbital is lower in energy than \(3 \mathrm{~d}\)- orbital
4 \(3 \mathrm{~s}\)-orbital is lower in energy than \(3 \mathrm{p}\)- orbital
Explanation:
The hydrogen atom has the configuration \(1 \mathrm{~s}^{1}\) and \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\) -orbitals will have same energy with respect to \(1 \mathrm{~s}\)-orbital.
CHXI02:STRUCTURE OF ATOM
307313
Read the Statement - A and Statement - B carefully to mark the correct options given below Statement A : The orbitals having same energy are called as degenerate orbitals. Statement B : In hydrogen atom, 3 p and 3 d orbitals are not degenerate orbitals.
1 Statement A is incorrect but Statement B is correct.
2 Both statements are correct.
3 Statement A is correct but Statement B is incorrect.
4 Both Statements are incorrect.
Explanation:
In hydrogen atom, orbitals having same principal quantum number ( n ) are degenerate orbitals, i.e., energy of \({\mathrm{3 s=3 p=3 d}}\). So, the correct option is (3).
JEE Main - 2024
CHXI02:STRUCTURE OF ATOM
307314
For the electrons of oxygen atom, which of the following statements is correct?
1 \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \(\mathrm{2 p}\) orbital
2 An electron in the \(\mathrm{2 \mathrm{~s}}\) orbital has the same energy as an electron in the \(\mathrm{2p}\) orbital
3 \(\mathrm{Z_{\text {eff }}}\) for an electron in \({\text{1s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital
4 The two electrons present in the \({\text{2s}}\) orbital have spin quantum numbers \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) but of opposite sign
Explanation:
(a) Electrons in \(\mathrm{2 s}\) and \(\mathrm{2 p}\) orbitals have different screening effect. Hence, their \(\mathrm{Z_{\text {eff }}}\) is different \(\mathrm{\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{~s}}\) orbital \(\mathrm{>\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{p}}\) orbital. (b) Energy of 2s orbital \(\mathrm{ < }\) eneryg of \(\mathrm{2 p}\) orbital. (c) \(\mathrm{Z_{\text {eff }}}\) of \(\mathrm{1 \mathrm{~s}}\) orbital \(\mathrm{\neq Z_{\text {eff }}}\) of \(\mathrm{2 s}\) orbital (d) For the two electrons of \(\mathrm{2 \mathrm{~s}}\) orbital, the value of \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) is \(\mathrm{+\dfrac{1}{2}}\) and \(\mathrm{-\dfrac{1}{2}}\) i.e., is two electrons have same magnitude but have opposite sign (+ and -). Hence, option (4) is correct.
CHXI02:STRUCTURE OF ATOM
307315
Arrange in decreasing order, the energy of \(2 \mathrm{~s}\) orbitals in the following atoms \(\mathrm{H}, \mathrm{Li}, \mathrm{Na}, \mathrm{K}\)
Energy of the similar orbitals of different atoms decreases with increase in nuclear charge. Nuclear charge increases with number of nucleons present in nucleus. So, order of nuclear charge decreases as \(\mathrm{K}>\mathrm{Na}>\mathrm{Li}>\mathrm{H}\). Thus energy in decreasing order given as \({{\rm{E}}_{{\rm{2s(H)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Li)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Na)}}}}\,{\rm{ > }}{{\rm{E}}_{{\rm{2s(\;K)}}}}{\rm{.}}\)
CHXI02:STRUCTURE OF ATOM
307316
Arrange the orbitals of H-atom in the increasing order of their energies. \({\rm{3}}{{\rm{p}}_{\rm{x}}}{\rm{,2s,4}}{{\rm{d}}_{{\rm{xy}}}}{\rm{,3s,4}}{{\rm{p}}_{\rm{z}}}{\rm{,3}}{{\rm{p}}_{\rm{y}}}{\rm{,4s}}\)
307312
Which one of the following statements in relation to the hydrogen atom is correct?
1 \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\)-orbitals all have the same energy
2 \(3 \mathrm{~s}\) and \(3 \mathrm{p}\)-orbitals are of lower energy than \(3 \mathrm{~d}\)-orbital
3 \(3 \mathrm{p}\)-orbital is lower in energy than \(3 \mathrm{~d}\)- orbital
4 \(3 \mathrm{~s}\)-orbital is lower in energy than \(3 \mathrm{p}\)- orbital
Explanation:
The hydrogen atom has the configuration \(1 \mathrm{~s}^{1}\) and \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\) -orbitals will have same energy with respect to \(1 \mathrm{~s}\)-orbital.
CHXI02:STRUCTURE OF ATOM
307313
Read the Statement - A and Statement - B carefully to mark the correct options given below Statement A : The orbitals having same energy are called as degenerate orbitals. Statement B : In hydrogen atom, 3 p and 3 d orbitals are not degenerate orbitals.
1 Statement A is incorrect but Statement B is correct.
2 Both statements are correct.
3 Statement A is correct but Statement B is incorrect.
4 Both Statements are incorrect.
Explanation:
In hydrogen atom, orbitals having same principal quantum number ( n ) are degenerate orbitals, i.e., energy of \({\mathrm{3 s=3 p=3 d}}\). So, the correct option is (3).
JEE Main - 2024
CHXI02:STRUCTURE OF ATOM
307314
For the electrons of oxygen atom, which of the following statements is correct?
1 \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \(\mathrm{2 p}\) orbital
2 An electron in the \(\mathrm{2 \mathrm{~s}}\) orbital has the same energy as an electron in the \(\mathrm{2p}\) orbital
3 \(\mathrm{Z_{\text {eff }}}\) for an electron in \({\text{1s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital
4 The two electrons present in the \({\text{2s}}\) orbital have spin quantum numbers \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) but of opposite sign
Explanation:
(a) Electrons in \(\mathrm{2 s}\) and \(\mathrm{2 p}\) orbitals have different screening effect. Hence, their \(\mathrm{Z_{\text {eff }}}\) is different \(\mathrm{\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{~s}}\) orbital \(\mathrm{>\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{p}}\) orbital. (b) Energy of 2s orbital \(\mathrm{ < }\) eneryg of \(\mathrm{2 p}\) orbital. (c) \(\mathrm{Z_{\text {eff }}}\) of \(\mathrm{1 \mathrm{~s}}\) orbital \(\mathrm{\neq Z_{\text {eff }}}\) of \(\mathrm{2 s}\) orbital (d) For the two electrons of \(\mathrm{2 \mathrm{~s}}\) orbital, the value of \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) is \(\mathrm{+\dfrac{1}{2}}\) and \(\mathrm{-\dfrac{1}{2}}\) i.e., is two electrons have same magnitude but have opposite sign (+ and -). Hence, option (4) is correct.
CHXI02:STRUCTURE OF ATOM
307315
Arrange in decreasing order, the energy of \(2 \mathrm{~s}\) orbitals in the following atoms \(\mathrm{H}, \mathrm{Li}, \mathrm{Na}, \mathrm{K}\)
Energy of the similar orbitals of different atoms decreases with increase in nuclear charge. Nuclear charge increases with number of nucleons present in nucleus. So, order of nuclear charge decreases as \(\mathrm{K}>\mathrm{Na}>\mathrm{Li}>\mathrm{H}\). Thus energy in decreasing order given as \({{\rm{E}}_{{\rm{2s(H)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Li)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Na)}}}}\,{\rm{ > }}{{\rm{E}}_{{\rm{2s(\;K)}}}}{\rm{.}}\)
CHXI02:STRUCTURE OF ATOM
307316
Arrange the orbitals of H-atom in the increasing order of their energies. \({\rm{3}}{{\rm{p}}_{\rm{x}}}{\rm{,2s,4}}{{\rm{d}}_{{\rm{xy}}}}{\rm{,3s,4}}{{\rm{p}}_{\rm{z}}}{\rm{,3}}{{\rm{p}}_{\rm{y}}}{\rm{,4s}}\)
NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXI02:STRUCTURE OF ATOM
307312
Which one of the following statements in relation to the hydrogen atom is correct?
1 \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\)-orbitals all have the same energy
2 \(3 \mathrm{~s}\) and \(3 \mathrm{p}\)-orbitals are of lower energy than \(3 \mathrm{~d}\)-orbital
3 \(3 \mathrm{p}\)-orbital is lower in energy than \(3 \mathrm{~d}\)- orbital
4 \(3 \mathrm{~s}\)-orbital is lower in energy than \(3 \mathrm{p}\)- orbital
Explanation:
The hydrogen atom has the configuration \(1 \mathrm{~s}^{1}\) and \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\) -orbitals will have same energy with respect to \(1 \mathrm{~s}\)-orbital.
CHXI02:STRUCTURE OF ATOM
307313
Read the Statement - A and Statement - B carefully to mark the correct options given below Statement A : The orbitals having same energy are called as degenerate orbitals. Statement B : In hydrogen atom, 3 p and 3 d orbitals are not degenerate orbitals.
1 Statement A is incorrect but Statement B is correct.
2 Both statements are correct.
3 Statement A is correct but Statement B is incorrect.
4 Both Statements are incorrect.
Explanation:
In hydrogen atom, orbitals having same principal quantum number ( n ) are degenerate orbitals, i.e., energy of \({\mathrm{3 s=3 p=3 d}}\). So, the correct option is (3).
JEE Main - 2024
CHXI02:STRUCTURE OF ATOM
307314
For the electrons of oxygen atom, which of the following statements is correct?
1 \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \(\mathrm{2 p}\) orbital
2 An electron in the \(\mathrm{2 \mathrm{~s}}\) orbital has the same energy as an electron in the \(\mathrm{2p}\) orbital
3 \(\mathrm{Z_{\text {eff }}}\) for an electron in \({\text{1s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital
4 The two electrons present in the \({\text{2s}}\) orbital have spin quantum numbers \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) but of opposite sign
Explanation:
(a) Electrons in \(\mathrm{2 s}\) and \(\mathrm{2 p}\) orbitals have different screening effect. Hence, their \(\mathrm{Z_{\text {eff }}}\) is different \(\mathrm{\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{~s}}\) orbital \(\mathrm{>\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{p}}\) orbital. (b) Energy of 2s orbital \(\mathrm{ < }\) eneryg of \(\mathrm{2 p}\) orbital. (c) \(\mathrm{Z_{\text {eff }}}\) of \(\mathrm{1 \mathrm{~s}}\) orbital \(\mathrm{\neq Z_{\text {eff }}}\) of \(\mathrm{2 s}\) orbital (d) For the two electrons of \(\mathrm{2 \mathrm{~s}}\) orbital, the value of \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) is \(\mathrm{+\dfrac{1}{2}}\) and \(\mathrm{-\dfrac{1}{2}}\) i.e., is two electrons have same magnitude but have opposite sign (+ and -). Hence, option (4) is correct.
CHXI02:STRUCTURE OF ATOM
307315
Arrange in decreasing order, the energy of \(2 \mathrm{~s}\) orbitals in the following atoms \(\mathrm{H}, \mathrm{Li}, \mathrm{Na}, \mathrm{K}\)
Energy of the similar orbitals of different atoms decreases with increase in nuclear charge. Nuclear charge increases with number of nucleons present in nucleus. So, order of nuclear charge decreases as \(\mathrm{K}>\mathrm{Na}>\mathrm{Li}>\mathrm{H}\). Thus energy in decreasing order given as \({{\rm{E}}_{{\rm{2s(H)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Li)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Na)}}}}\,{\rm{ > }}{{\rm{E}}_{{\rm{2s(\;K)}}}}{\rm{.}}\)
CHXI02:STRUCTURE OF ATOM
307316
Arrange the orbitals of H-atom in the increasing order of their energies. \({\rm{3}}{{\rm{p}}_{\rm{x}}}{\rm{,2s,4}}{{\rm{d}}_{{\rm{xy}}}}{\rm{,3s,4}}{{\rm{p}}_{\rm{z}}}{\rm{,3}}{{\rm{p}}_{\rm{y}}}{\rm{,4s}}\)
307312
Which one of the following statements in relation to the hydrogen atom is correct?
1 \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\)-orbitals all have the same energy
2 \(3 \mathrm{~s}\) and \(3 \mathrm{p}\)-orbitals are of lower energy than \(3 \mathrm{~d}\)-orbital
3 \(3 \mathrm{p}\)-orbital is lower in energy than \(3 \mathrm{~d}\)- orbital
4 \(3 \mathrm{~s}\)-orbital is lower in energy than \(3 \mathrm{p}\)- orbital
Explanation:
The hydrogen atom has the configuration \(1 \mathrm{~s}^{1}\) and \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\) -orbitals will have same energy with respect to \(1 \mathrm{~s}\)-orbital.
CHXI02:STRUCTURE OF ATOM
307313
Read the Statement - A and Statement - B carefully to mark the correct options given below Statement A : The orbitals having same energy are called as degenerate orbitals. Statement B : In hydrogen atom, 3 p and 3 d orbitals are not degenerate orbitals.
1 Statement A is incorrect but Statement B is correct.
2 Both statements are correct.
3 Statement A is correct but Statement B is incorrect.
4 Both Statements are incorrect.
Explanation:
In hydrogen atom, orbitals having same principal quantum number ( n ) are degenerate orbitals, i.e., energy of \({\mathrm{3 s=3 p=3 d}}\). So, the correct option is (3).
JEE Main - 2024
CHXI02:STRUCTURE OF ATOM
307314
For the electrons of oxygen atom, which of the following statements is correct?
1 \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \(\mathrm{2 p}\) orbital
2 An electron in the \(\mathrm{2 \mathrm{~s}}\) orbital has the same energy as an electron in the \(\mathrm{2p}\) orbital
3 \(\mathrm{Z_{\text {eff }}}\) for an electron in \({\text{1s}}\) orbital is the same as \(\mathrm{Z_{\text {eff }}}\) for an electron in a \({\text{2s}}\) orbital
4 The two electrons present in the \({\text{2s}}\) orbital have spin quantum numbers \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) but of opposite sign
Explanation:
(a) Electrons in \(\mathrm{2 s}\) and \(\mathrm{2 p}\) orbitals have different screening effect. Hence, their \(\mathrm{Z_{\text {eff }}}\) is different \(\mathrm{\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{~s}}\) orbital \(\mathrm{>\mathrm{Z}_{\text {eff }}}\) of \(\mathrm{2 \mathrm{p}}\) orbital. (b) Energy of 2s orbital \(\mathrm{ < }\) eneryg of \(\mathrm{2 p}\) orbital. (c) \(\mathrm{Z_{\text {eff }}}\) of \(\mathrm{1 \mathrm{~s}}\) orbital \(\mathrm{\neq Z_{\text {eff }}}\) of \(\mathrm{2 s}\) orbital (d) For the two electrons of \(\mathrm{2 \mathrm{~s}}\) orbital, the value of \(\mathrm{\mathrm{m}_{\mathrm{s}}}\) is \(\mathrm{+\dfrac{1}{2}}\) and \(\mathrm{-\dfrac{1}{2}}\) i.e., is two electrons have same magnitude but have opposite sign (+ and -). Hence, option (4) is correct.
CHXI02:STRUCTURE OF ATOM
307315
Arrange in decreasing order, the energy of \(2 \mathrm{~s}\) orbitals in the following atoms \(\mathrm{H}, \mathrm{Li}, \mathrm{Na}, \mathrm{K}\)
Energy of the similar orbitals of different atoms decreases with increase in nuclear charge. Nuclear charge increases with number of nucleons present in nucleus. So, order of nuclear charge decreases as \(\mathrm{K}>\mathrm{Na}>\mathrm{Li}>\mathrm{H}\). Thus energy in decreasing order given as \({{\rm{E}}_{{\rm{2s(H)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Li)}}}}\,{\rm{ > }}\,{{\rm{E}}_{{\rm{2s(Na)}}}}\,{\rm{ > }}{{\rm{E}}_{{\rm{2s(\;K)}}}}{\rm{.}}\)
CHXI02:STRUCTURE OF ATOM
307316
Arrange the orbitals of H-atom in the increasing order of their energies. \({\rm{3}}{{\rm{p}}_{\rm{x}}}{\rm{,2s,4}}{{\rm{d}}_{{\rm{xy}}}}{\rm{,3s,4}}{{\rm{p}}_{\rm{z}}}{\rm{,3}}{{\rm{p}}_{\rm{y}}}{\rm{,4s}}\)