Home
Class 11
CHEMISTRY
Assertion: Boron has a smaller first ion...

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.

A

If both assertion and reason are true and reason is the correct explanation of assertion

B

If the assertion and reason are true but reason is not the correct explanation of assertion.

C

If assertion is true but reason is false.

D

If assertion is false but reason is true.

Text Solution

Verified by Experts

The correct Answer is:
A
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY OF PROPERTIES

    A2Z|Exercise AIPMT/ NEET Questions|13 Videos

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY OF PROPERTIES

    A2Z|Exercise AIIMS Questions|24 Videos

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY OF PROPERTIES

    A2Z|Exercise Electronegativity And Nature Of Oxides|42 Videos

  • CHEMICAL THERMODYNAMICS

    A2Z|Exercise Section D - Chapter End Test|30 Videos

  • CLASSIFICTION, PURIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    A2Z|Exercise Section D - Chapter End Test|30 Videos

Similar Questions

Explore conceptually related problems

Al has a smaller first ionization enthalpy than Mg. Consider the following statements : I. It is easier to remove 3p electron than 3s electron . II . 3p electron of Al is more shielded from the nucleus by the inner coreof electron than the 3s electrons of Mg III. 3s electron hasmore penetration power than 3p electron IV. Atomic radius of Al is more than Mg ( atomic number Al=13, Mg = 12 ) The correct statements are :

The first ionisation energy of beryllium is more than that of boron because

Knowledge Check

  • 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 .

    A
    Assertion and reason both are correct statement but reason is not correct explanation for assertion
    B
    Assertion is correct statement but reason is wrong statement.
    C
    Assertion and reason both are correct statement and reason is correct explanation for assertion
    D
    Assertion is reason both are wrong statements.

  • 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.

    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

  • B has a smaller first ionization enthalpy than Be. Consider the following statements (i) it is easier to remove 2p electron than 2s electron (ii) 2p electron of B is more shielded from the nucleus by the inner core of electrons than the 2s electrons of Be (iii) 2s electron has more penetration power than 2p electron (iv) atomic radius of B is more than Be (atomic number B= 5, Be = 4) The correct statements are

    A
    (i),(ii) and (iv)
    B
    (i),(iii) and (iv)
    C
    (i),(ii) and (iii)
    D
    (ii),(iii) and (iv)

    • Similar Questions

    Explore conceptually related problems

    The inner electrons are shielded to a "______" extent than the outer electrons.

    Which of the following has more electrons than neutrons?

    Assertion (A): The first ionisation energy of B is less than that of Be Assertion (R): The penetration ability of s-electron is higher than that of p-electrons the correct answer is

    Which of the following has more electrons than neutrons?

    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.

    Home
    Profile