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STATEMENT-1: Half-filled and fully-fille...

STATEMENT-1: Half-filled and fully-filled degenerate orbitals are more stable.
STATEMEHNT-2: Extra stabillity is due to the symmetrical distribution of electrons and exchange energy.

A

If both the statement are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1

B

If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1

C

If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE

D

If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

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Half-filled and fully-filled orbital orbitals are more stable

We know that fully filled and half filled orbitals are more stable. Can you write the electronic configuration of Cr(Z=24)?

Knowledge Check

  • STATEMENT-1 : Principal Quantum number of outermost electron in Fe is 4. and STATEMENT-2 : Last electron is filled in 3d.

    A
    Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
    B
    Statement-1 is True, Statement-2 isTrue, Statement-2 is NOT a correct explanation for Statement-1
    C
    Statement-1 is True, Statement-2 is False
    D
    Statement-1 is False , Statement-2 isTrue

  • STATEMENT-1 : The 19^(th) electron in potassium atom enters into 4s-orbital than in 3d-orbital. and STATEMENT-2 : (n+1l) rule is followed for determining the orbital of lowest energy state.

    A
    Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
    B
    Statement-1 is True, Statement-2 isTrue, Statement-2 is NOT a correct explanation for Statement-1
    C
    Statement-1 is True, Statement-2 is False
    D
    Statement-1 is False , Statement-2 isTrue

  • The extra stability of half-filled and completely-filled subshell is due to

    A
    relatively small shielding
    B
    smaller coulombic repulsion enegry
    C
    larger exchange enegry
    D
    all of these

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    Statement 1. 4s orbital has lower energy than 3d orbital. Statement 2. s-orbital is spherically symmetrical and remains closer to the nucleus and has lower energy than d-orbital.

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    The minimum amount of energy required to remove the most loosely bound electron form an isolated atom in the gaseous state is known as ionization energy or first ionization energy or inonization enthalpy (IE_(1)) of the element. The energy required to remove the second electron from the monovalent cation is called second ionization enthalpy (IE_(2)). Simllarly, we have third, fourth .................... fonization enthalpies. The values of ionization energy depends on a number of factors such as (i) size of the atom (ii) screening effect (iii) nuclear charge (iv) half filled and fuly filled orbitals (v) shape of orbital. In a group, the ionization energy decreases from top to bottom. In a period, the valup of ionisation energy increases from left to right with breaks where atoms have somewhat stable configurations. Compared to the second ionization energy (IE_(2)) of an atom the third ionization energy (IE_(2)) is

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