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Statement-1: Generally, ionisation entha...

Statement-1: Generally, ionisation enthalpy increases from left to right in a period.
Statement-2: When successive electrons are added to the orbitals in the same principal quantum level, the shielding effect of inner core of electrons does not increase very much to compensate for the increased attraction of the electron to the nucleus.

A

Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-2

B

Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-2

C

Statement-1 is True, Statement-2 is False

D

Statement-1 is False, Statement-2 is True

Text Solution

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The correct Answer is:
B
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Assertion: (A) Generally, ionsiation enthalpy increases from left to right in a period. Reason ( R) When successive electrons are added to the orbitals in the same principle quantum level, the shielding effect of inner core of electrons does not increase very much to compensate for the increased attraction of the electrons to the nucleus.

Assertion: Generally, ionisation enthalpy than beryllium. Reason: When successive electrons are added to the orbitals in the same principle quantum level, the shiielding effect of inner core of electrons does not increase very much to compensate for the increased attraction of the electron to the nucleus.

Statement 1: Metallic character decreases from left to right. Statement 2: Ionization enthalpy increase and electronegativity decreases.

Statement-1: Boron has a smaller first ionisation enthalpy than beryllium. Statement-2: The penetration of a 2s electron to the nucleus is more than the 2p electron hence 2p electron is more shielded by the inner core of electrons than the 2s electrons.

Statement-1 : First electron gain enthalpy is alway -ve for an element. Statement-2 : Magnitude of electron gain enthalpy irregularly increases from left to right in a period.

Statement-1: Metallic character of first group metals increases down the group with the decreasing ionisation energy. Statement-2: The loss and gain of electron(s) can be used in explaining the reducing and oxidising behaviour of the element respectively.

GRB PUBLICATION-PERIODIC TABLE-Reasoning Type
  1. Statement-1: First ionisation energy of O^(+)(g) is greater than that ...

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  2. Statement-1: Down the group, electronegativity decreases from B to TI....

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  3. Statement-1: Sc(Z = 21) is placed as d-block element. Statement-2: L...

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  4. Statement-1: Na^(+) and AI^(3+) are isoelectronic but the magnitude of...

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  5. Statement-1: The atomic radii of the elements of the oxygen family are...

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  6. Statement-1: Metallic character of first group metals increases down t...

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  7. Statement-1: Fluorine has a less negative electron gain enthalpy than ...

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  8. Statement-1: Fluorine forms only one oxoacid, HOF, Statement-2: Fluo...

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  9. Statement-1: Li and Mg shows diagonal relationship. Statement-2: Li...

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  10. Statement-1: The decreasing order of acidi character of CO(2),N(2)O(5)...

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  11. Statement-1: Oxidising property of F(2) is greater than Cl(2). State...

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  12. Statement-1: Generally, ionisation enthalpy increases from left to rig...

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  13. Statement-1: Boron has a smaller first ionisation enthalpy than beryll...

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  14. Assertion: Electron gain enthalpy always becomes less negative as we g...

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  15. Assertion: The first ionisation energy of Be is greater than that of B...

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  16. Statement-1: The acidic strength order of hydra acids is HF lt HCI lt ...

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  17. Statement-1: The decreasing order of acidic character of CO(2),N(2)O(5...

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  18. Statement-1: The ionisation potential of Sn is greater than Pb. Stat...

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  19. Statement-1: (I.E.)(n) of an atom is always greater than (I.E)(n-1) (n...

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  20. Statement-1: Nitrogen atom has higher ionization energy than fluorine ...

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