Q:

What kind of bond is in NH3?

A:

Quick Answer

NH3, commonly referred to as ammonia, has a polar covalent bond. This means that the valence electrons in the bond are shared between the elements but are attracted unequally between them.

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Full Answer

The electronegativity of nitrogen (3.0) is higher than that of hydrogen (2.2). Therefore, when the two elements form a molecule by sharing electron pairs, the electrons tend to be attracted more strongly toward the nitrogen side than to the hydrogen side. The overall effect is an electric dipole in the molecule formed, with a slight positive charge in the hydrogen and a slight negative charge in the nitrogen. Hence, the molecule has a polar covalent bond.

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Related Questions

  • Q:

    What is the chemical name for Nh3?

    A:

    The chemical that is designated with the chemical notation of Nh3 is ammonia. Ammonia is a colorless gas at room temperature that has a strong, suffocating odor. In its liquid form, which is commonly used in refrigerants, ammonia is colorless or clear and does not contain any visible impurities.

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  • Q:

    What is the compound NH4CH3CO2 commonly known as?

    A:

    NH4CH3CO2, or C2H7NO2, is the chemical formula of ammonium acetate, the ammonium salt of the acetic acid CH3COOH. The molar mass of this chemical compound is 77.08 grams per mole. It exists as white solid crystals, and its density is 1.17 grams per cubic centimeter at 20 degrees Celsius.

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  • Q:

    What is the Lewis dot structure of NH3?

    A:

    NH3, commonly known as ammonia, is arranged as a T-shaped molecule with nitrogen at its center and three hydrogen atoms at its extremities. Each hydrogen atom is covalently bonded to the nitrogen via an electron pair, and another pair of electrons is attached to the nitrogen atom's outer shell.

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  • Q:

    What types of intermolecular forces are present in NH3?

    A:

    The types of intermolecular forces present in ammonia, or NH3, are hydrogen bonds. The hydrogen bonds are many magnitudes stronger than other intermolecular forces in NH3; therefore, when examining intermolecular bonding in this molecule, other forces can be safely ignored.

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