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Statement-1: Metallic character of first...

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.

A

Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-15

B

Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-15

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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The periodicity is related to the electronic configuration. That is, all chemical and physical properties are a manifestation of the electronic configuratio of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence, the ionization enthalpes generally increase and electron gain enthalpies become more negative across a period. In order words, the ionization enthalpy of the extreme left element in a period is the least and the electron gain enthalpy of the element on the extreme right is the highest negative. This results into high chemical reactivity at the two extremes and the lowest in the centre. Similary, down the group, the increase in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducing and oxidising behaviour, and also with metallic and non-metallic character respectively of the elements. The correct order of the metallic character is:

The periodicity is related to the electronic configuration. That is, all chemical and physical properties are a manifestation of the electronic configuratio of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence, the ionization enthalpes generally increase and electron gain enthalpies become more negative across a period. In order words, the ionization enthalpy of the extreme left element in a period is the least and the electron gain enthalpy of the element on the extreme right is the highest negative. This results into high chemical reactivity at the two extremes and the lowest in the centre. Similary, down the group, the increase in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducing and oxidising behaviour, and also with metallic and non-metallic character respectively of the elements. The correct order of the non-metallic character is:

The periodicity is related to the electronic configuration. That is, all chemical and physical properties are a manifestation of the electronic configuration of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence, the ionization enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words, the ionization enthalpy of the exterme left element in a period is the least and teh electron gain enthalpy of the element on the exterme right is the highest negative. This results into high chemical reactivity at the two extermes and the lowest in he centre. Similarly down the group, the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducting and oxidising behaviour, and also with metallic and non-metallic character respectively, of the elements. The correct order of the metallic character is:

The periodicity is related to the electronic configuration. That is, all chemical and physical properties are a manifestation of the electronic configuratio of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence, the ionization enthalpes generally increase and electron gain enthalpies become more negative across a period. In order words, the ionization enthalpy of the extreme left element in a period is the least and the electron gain enthalpy of the element on the extreme right is the highest negative. This results into high chemical reactivity at the two extremes and the lowest in the centre. Similary, down the group, the increase in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducing and oxidising behaviour, and also with metallic and non-metallic character respectively of the elements. Which of the following statements is incorrect?

The periodicity is related to the electronic configuration. That is, all chemical and physical properties are a manifestation of the electronic configuration of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence, the ionization enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words, the ionization enthalpy of the exterme left element in a period is the least and teh electron gain enthalpy of the element on the exterme right is the highest negative. This results into high chemical reactivity at the two extermes and the lowest in he centre. Similarly down the group, the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducting and oxidising behaviour, and also with metallic and non-metallic character respectively, of the elements. Which of the following statements is correct?

"Solubility of alkali metal fluorices increases down the group " Select correct explanation for given statement :

Assertion :- Metallic character increases on going down the group Reason :- I.E. decreases on going down the group

The periodicity is related to the electronic configuration. That is, all chemical and physical properties are a manifestation of the electronic configuration of the elements. The atomic and ionic radii generally decrease in a period from left to right. As a consequence, the ionization enthalpies generally increase and electron gain enthalpies become more negative across a period. In other words, the ionization enthalpy of the exterme left element in a period is the least and teh electron gain enthalpy of the element on the exterme right is the highest negative. This results into high chemical reactivity at the two extermes and the lowest in he centre. Similarly down the group, the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements) in electron gain enthalpies in the case of main group elements. The loss and gain of electrons can be co-related with the reducting and oxidising behaviour, and also with metallic and non-metallic character respectively, of the elements. Considering the elements B, C, N, F and Si , the correct order of their non-metallic character is:

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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