Assertion(A) - Silicon tetrafluoride. `SiF_4` is non polar even though fluorine is much more electronegative than silicon.
Reason(R)-The four bond dipoles cancel one another in `SiF_4`.

(A): SiF_4 is non polar even though fluorine is much more electronegative than silicon (B) : The four bond dipoles cancel one another in SiF_4 molecule

This question has statement I and Statement II. Of the four choices given after the statements, choose the one that best describes the two Statements. (1) Statement-I is true, Statement-II is true, Statement-II is a correct explanation of Statement-I (2) Statement-I is true, Statement-II is true,Statement-II is not a correct explanation of Statement-I (3)Statement-I is a true , Statement-II is false (4) Statement-I is false, Statement-II is true Statement 1 : Silicon tetrafluoride, SiF_4 is non polar even though fluorine is much more electronegative than silicon. Statement 2: The four bond dipoles cancel one another in SiF_4 .

Assertion (A): Though fluorine is more electronegative than silicon, SiF_(4) is non-polar Reason (R): The four fluorine atoms have the same force of attraction on silicon.

The dipole moment of fluorobenzene is lower than that of iodobenzene, even though fluorine is more electronegative than iodine - explain.

Assertion (A): F, has lower bond dissociation energy than Cl_(2) . Reason (R): Flourine is more electronegative than chlorine.

Assertion BF_(3) has greater dipole momnet than H_(2)S Reasoning Fluorine is more electronegative than sulphur .

Assertion BF_(3) has greater dipole momnet than H_(2)S Reasoning Fluorine is more electronegative than sulphur .

Assertion : Dipole moment of NH_(3) is greater than that of NF_(3) . Reason : Nitrogen is more electronegative than fluorine.