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The correct statement regarding the following physical properties is
- a)Bond order follows Li2 < C2 < B2 < N2 order.
- b)Melting point follows NH3 < PH3 < AsH3 < SbH3 order.
- c)Pauling electronegativity follows Al < Si < S < P order.
- d)First ionization energy follows Li < B < Be < C order.
Correct answer is option 'D'. Can you explain this answer?
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The correct statement regarding the following physical properties isa)...
Bond order of given molecules can be calculate by
- Molecular orbital configuration of C2 = (6+6) = 12
- Molecular orbital configuration of B2 = (5+5) = 10
- Molecular orbital configuration of N2 = (7+7) = 14
- Molecular orbital configuration of Li2 = (3+3) = 6.
Therefore correct sequence of bond order is B2 < Li2 < C2 < N2.
2. Melting point increased down the group as size and mass of the molecule increases down the group due to which Vander Waal force for also increase. NH3 shows drastically high melting point due to the presence of strong intermolecular hydrogen bonding.
So the correct order of melting point is
PH3 < AsH3 < SbH3 < NH3 .
3. Pauling electronegativity increase across the period moving from left to right because of the increase in nuclear charge of atom.
The correct order for electronegativity is
Al < Si < P< S.
4. As we know that ionization energy increase across the period moving from left to right due to increase in nuclear charge of atom. But Be and B show exception in this case. Be has 1s2, 2s2 electronic configuration and B has 1s2, 2s2,2p1 electronic configuration. It is easy to remove electron from p orbital compared to fully fill s orbital. So the ionization energy of Be is greater than B.
The correct order for first ionization energy is
Li < B < Be < C.
Therefore, the correct statement regarding physical properties is first ionization energy follows Li < B < Be < C order.
2. Melting point increased down the group as size and mass of the molecule increases down the group due to which Vander Waal force for also increase. NH3 shows drastically high melting point due to the presence of strong intermolecular hydrogen bonding.
So the correct order of melting point is
PH3 < AsH3 < SbH3 < NH3 .
3. Pauling electronegativity increase across the period moving from left to right because of the increase in nuclear charge of atom.
The correct order for electronegativity is
Al < Si < P< S.
4. As we know that ionization energy increase across the period moving from left to right due to increase in nuclear charge of atom. But Be and B show exception in this case. Be has 1s2, 2s2 electronic configuration and B has 1s2, 2s2,2p1 electronic configuration. It is easy to remove electron from p orbital compared to fully fill s orbital. So the ionization energy of Be is greater than B.
The correct order for first ionization energy is
Li < B < Be < C.
Therefore, the correct statement regarding physical properties is first ionization energy follows Li < B < Be < C order.
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The correct statement regarding the following physical properties isa)...
First Ionization Energy Trend
- The first ionization energy is the energy required to remove the most loosely bound electron from an atom.
- The trend in first ionization energy generally increases across a period and decreases down a group in the periodic table.
- In this case, the correct order of first ionization energy follows Li < b="" />< be="" />< />
- This order is based on the atomic structure and effective nuclear charge of the elements.
Explanation of the Trend
- Lithium (Li) has the lowest first ionization energy in the given options because it has one electron in its outermost shell, which is relatively easy to remove compared to the other elements.
- Boron (B) has a higher first ionization energy than lithium because it has one more proton in its nucleus, leading to a stronger attraction to its electrons.
- Beryllium (Be) has a lower first ionization energy compared to boron because it has a filled 2s subshell, making it more stable and easier to remove an electron.
- Carbon (C) has the highest first ionization energy in the given options due to its half-filled p orbital, which provides extra stability and makes it harder to remove an electron compared to the other elements.
Conclusion
- The trend in first ionization energy among Li, B, Be, and C follows a logical pattern based on the atomic structure and electron configuration of the elements.
- Understanding these trends can help predict the behavior of elements in chemical reactions and their physical properties.
- The first ionization energy is the energy required to remove the most loosely bound electron from an atom.
- The trend in first ionization energy generally increases across a period and decreases down a group in the periodic table.
- In this case, the correct order of first ionization energy follows Li < b="" />< be="" />< />
- This order is based on the atomic structure and effective nuclear charge of the elements.
Explanation of the Trend
- Lithium (Li) has the lowest first ionization energy in the given options because it has one electron in its outermost shell, which is relatively easy to remove compared to the other elements.
- Boron (B) has a higher first ionization energy than lithium because it has one more proton in its nucleus, leading to a stronger attraction to its electrons.
- Beryllium (Be) has a lower first ionization energy compared to boron because it has a filled 2s subshell, making it more stable and easier to remove an electron.
- Carbon (C) has the highest first ionization energy in the given options due to its half-filled p orbital, which provides extra stability and makes it harder to remove an electron compared to the other elements.
Conclusion
- The trend in first ionization energy among Li, B, Be, and C follows a logical pattern based on the atomic structure and electron configuration of the elements.
- Understanding these trends can help predict the behavior of elements in chemical reactions and their physical properties.
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The correct statement regarding the following physical properties isa)Bond order follows Li2< C2< B2< N2order.b)Melting point follows NH3< PH3< AsH3< SbH3order.c)Pauling electronegativity follows Al < Si < S < P order.d)First ionization energy follows Li < B < Be < C order.Correct answer is option 'D'. Can you explain this answer?
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The correct statement regarding the following physical properties isa)Bond order follows Li2< C2< B2< N2order.b)Melting point follows NH3< PH3< AsH3< SbH3order.c)Pauling electronegativity follows Al < Si < S < P order.d)First ionization energy follows Li < B < Be < C order.Correct answer is option 'D'. Can you explain this answer? for UGC NET 2024 is part of UGC NET preparation. The Question and answers have been prepared according to the UGC NET exam syllabus. Information about The correct statement regarding the following physical properties isa)Bond order follows Li2< C2< B2< N2order.b)Melting point follows NH3< PH3< AsH3< SbH3order.c)Pauling electronegativity follows Al < Si < S < P order.d)First ionization energy follows Li < B < Be < C order.Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for UGC NET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The correct statement regarding the following physical properties isa)Bond order follows Li2< C2< B2< N2order.b)Melting point follows NH3< PH3< AsH3< SbH3order.c)Pauling electronegativity follows Al < Si < S < P order.d)First ionization energy follows Li < B < Be < C order.Correct answer is option 'D'. Can you explain this answer?.
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