Thus ,as the distance increases from nucleus ionization potential decreases.
P(15)→ 1s2 2s2 2p6 3s2 3p3.
As(33 )–> 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3 .
Thus, As outer most electrons are farther away since principal quantum number increases n=4.hence ionization potential should drop
But moving to As from P, nuclear charge also increases so ionization energy should leap up! but distance influences more and more (1/r²) and P has greater ionization energy.
Thus ,as the distance increases from nucleus ionization potential decreases.
P(15)→ 1s2 2s2 2p6 3s2 3p3.
As(33 )–> 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3 .
Thus, As outer most electrons are farther away since principal quantum number increases n=4.hence ionization potential should drop
But moving to As from P, nuclear charge also increases so ionization energy should leap up! but distance influences more and more (1/r²) and P has greater ionization energy.
because phosphorus has extra stable electronic configuration of 3p³ (half filled sub shell) which makes removal of electron more difficult than sulphur (which has 3p⁴ configuration).
because phosphorus has extra stable electronic configuration of 3p³ (half filled sub shell) which makes removal of electron more difficult than sulphur (which has 3p⁴ configuration).
Ionization energy decreases in moving down in a group, since both P & As belongs to same group , As has lower Ionization energy due to increase in size in comparison to P.
Ionization energy decreases in moving down in a group, since both P & As belongs to same group , As has lower Ionization energy due to increase in size in comparison to P.
Sulfurs 3p subshell has a pair of electrons in one of its orbitals, whereas in the 3p subshell of phosphorus, there are no electron pairs in any of its orbitals, therefore it is easier to remove the electron from sulfurs 3p since the presence of an electron pair in one of its orbitals leads to increased repulsion, making it easier to remove and thus giving it a lower ionization energy.
Sulfurs 3p subshell has a pair of electrons in one of its orbitals, whereas in the 3p subshell of phosphorus, there are no electron pairs in any of its orbitals, therefore it is easier to remove the electron from sulfurs 3p since the presence of an electron pair in one of its orbitals leads to increased repulsion, making it easier to remove and thus giving it a lower ionization energy.
Roughly speaking ionization potential, I= constant×Zeff/r².
Thus ,as the distance increases from nucleus ionization potential decreases.
P(15)→ 1s2 2s2 2p6 3s2 3p3.
As(33 )–> 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3 .
Thus, As outer most electrons are farther away since principal quantum number increases n=4.hence ionization potential should drop
But moving to As from P, nuclear charge also increases so ionization energy should leap up! but distance influences more and more (1/r²) and P has greater ionization energy.
Roughly speaking ionization potential, I= constant×Zeff/r².
Thus ,as the distance increases from nucleus ionization potential decreases.
P(15)→ 1s2 2s2 2p6 3s2 3p3.
As(33 )–> 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3 .
Thus, As outer most electrons are farther away since principal quantum number increases n=4.hence ionization potential should drop
But moving to As from P, nuclear charge also increases so ionization energy should leap up! but distance influences more and more (1/r²) and P has greater ionization energy.
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because phosphorus has extra stable electronic configuration of 3p³ (half filled sub shell) which makes removal of electron more difficult than sulphur (which has 3p⁴ configuration).
because phosphorus has extra stable electronic configuration of 3p³ (half filled sub shell) which makes removal of electron more difficult than sulphur (which has 3p⁴ configuration).
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Ionization energy decreases in moving down in a group, since both P & As belongs to same group , As has lower Ionization energy due to increase in size in comparison to P.
Ionization energy decreases in moving down in a group, since both P & As belongs to same group , As has lower Ionization energy due to increase in size in comparison to P.
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Sulfurs 3p subshell has a pair of electrons in one of its orbitals, whereas in the 3p subshell of phosphorus, there are no electron pairs in any of its orbitals, therefore it is easier to remove the electron from sulfurs 3p since the presence of an electron pair in one of its orbitals leads to increased repulsion, making it easier to remove and thus giving it a lower ionization energy.
Sulfurs 3p subshell has a pair of electrons in one of its orbitals, whereas in the 3p subshell of phosphorus, there are no electron pairs in any of its orbitals, therefore it is easier to remove the electron from sulfurs 3p since the presence of an electron pair in one of its orbitals leads to increased repulsion, making it easier to remove and thus giving it a lower ionization energy.
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