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BF(3) and NF(3) both molecules, are cova...

`BF_(3) and NF_(3)` both molecules, are covalent, but `BF_(3)` is non - polar and `NF_(3)` is polar.Its reason is

A

Boron is a solid and nitrogen is a gas in free state

B

`BF_(3)` is planner but `NF_(3)` is pyramidal in shap

C

Boron is a metalloid while nitrogen is a non-metal

D

Atomic size of boron is smaller than that of nitrogen

Text Solution

Verified by Experts

The correct Answer is:
b
`BF_(3)` is planar, hence the dipole moment of the molecule is zero `NF_(3)` is pyramidal, thus it posses dipole moment Hence `NF_(3)` is a pole compounds
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Knowledge Check

  • BF_(1) and NF_(3) both molecules, are covalent, but BF_(3) is non - polar and NF_(3) pole. Its reason is

    A
    In uncombined state botom is metal and nitrogen is gas
    B
    `B - F` bond has no dipole moment whereas `N - F` bond has dipole moment
    C
    The size of boron atom is smaller than nitrogen
    D
    `BF_(3)` is planar whereas `NF_(3)` is pyramidal

  • The molecule BF_3 and NF_3 both are covalent compounds, but BF_3 is non-polar and NF_3 is polar. The reason is that

    A
    boron is a metal and nitrogen is a gas in uncombined state.
    B
    `BF_3`bonds no dipole moment whereas `NF_3` bond have dipole moment.
    C
    atomic size of boron is smaller than that of nitrogen
    D
    `BF_3` is symmetrical molecule whereas `NF_3` is unsymmetrical.

  • The molecules BF_(3) and NF_(3) are both covalent compounds, but BF_(3) is non polar whereas NF_(3) is polar. The reason for this is

    A
    atomic size of boron is larger than nitrogen
    B
    Boron is metal while nitrogen is gas
    C
    B-F bonds are non-polar while N-F bonds are polar
    D
    `BF_(3)` is planar but `NF_(3)` is pyramidal

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    The molecules BF_(3)&NF_(3) both are covalent. But BF_(3) is non-polar & NF_(3) is polar. The reason is that:-

    BF_(3) and NF_(3) both are covalent compounds but NF_(3) is polar whereas BF_(3) is non-polar. This is because :

    A polar covalent bond with positive and negative charge centres at its ends is called a dipole. The polarity of a dipole is measured by its dipole moment. Mathematically it is expressed as dipole moment, mu=q xx d where q and d are the net charge and the distance between the two charges respectively. Dipole moment is a vector quantity. The net dipole moment of a polyatomic molecule is the resultant of the various bond moments present in the molecule. The values of dipole moment are expressed in Debye (D) or in SI units in terms of coulomb- metre (Cm). One of the most important applications of dipole moment is in the determination of geometry and shape of molecules besides prediction of a number of properties of the molecules. The molecules BF_3 and NH_3 both are covalent compounds but BF_3 is non-polar while NF_3 is polar . The reason is that

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