Home
Class 11
CHEMISTRY
Assertion: (A) Generally, ionsiation ent...

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.

A

Assertion is correct statement and reason is wrong statement.

B

Assertion and reason both are correct statements and reason is correct explanation of Assertion.

C

Assertion and reason both are wrong statements.

D

Assertion and wrong statements and reason is correct statements.

Text Solution

Verified by Experts

The correct Answer is:
A
Assertion and reason both are correct statements and reason is correct explanation of assertion. Ionisation enthalpy increases along a period because effective nuclear charge increases and atomic size decreases.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES.

    NCERT EXEMPLAR|Exercise Long answer types question|7 Videos

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES.

    NCERT EXEMPLAR|Exercise Matching the Columns|3 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    NCERT EXEMPLAR|Exercise Long Answer type questions|9 Videos

  • ENVIRONMENTAL CHEMISTRY

    NCERT EXEMPLAR|Exercise Long Answer Type|5 Videos

Similar Questions

Explore conceptually related problems

Along a period atomic volume of the elements gradually increases from left to right due to an incerase in the number of valence electrons

With increase in atomic number, the Electron affinity........from left to right in a period.

Knowledge Check

  • Assertion (A) , Generally ionisation enthalpy increases from left to right in a period. Reason ( R ) : 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 fore the increased attraction of the electron of the nucleus.

    A
    Assertion is correct statement and reason is wrong statement.
    B
    Assertion and reson both are correct statement and reason is correct explanation of assertion
    C
    Assertion and reason both are wrong statement .
    D
    Assertion is wrong statement and reason is correct statement.

  • This section contains Assertion and Reason type questions each question has 4 choices (1)(2)(3)(4) out of which only one is correct Assertion(A): Genrally ionisation 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 electron to the nucleus

    A
    Both Assertion and Reason are correct and Reason ias the correct explanation of Assertion
    B
    Both Assertion and Reason are corect but Reason is not the correct explanation of Assertion
    C
    Assertion is correct but Reason is incorrect
    D
    Both Assertion and Reason are incorrcet

  • 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

    • Similar Questions

    Explore conceptually related problems

    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.

    Assertion (A): The atomic and ionic radii generally decrease towards right in a period. Reason (R): The ionisation enthalpy increases on moving towards left in a period.

    Assertion (A) : Boron has smaller first ionisation enthalpy than beryllium Reason ( R ) : 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 2s electrons .

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

    Assertion: Number of valence electrons increases down a group. Reason: More electrons are added in valence shell as we move from right to left in a period.

    Home
    Profile