The dipole moment of a molecule is a measure of its polarity, which is the separation of charge within the molecule. It is calculated using the formula:Dipole moment = Charge Q Distance d For ammonia NH3 , the molecule has a trigonal pyramidal shape with the nitrogen atom at the apex and the three hydrogen atoms surrounding it. The nitrogen atom is more electronegative than the hydrogen atoms, which leads to a separation of charge within the molecule.The bond dipole moment for each N-H bond can be calculated using the bond length d and the partial charges on the nitrogen and hydrogen atoms. The bond length for N-H in ammonia is approximately 1.012 1.012 10^-10 m . The partial charges on nitrogen and hydrogen are approximately -0.82e and +0.27e, respectively, where e is the elementary charge 1.6 10^-19 C .Bond dipole moment _NH = Charge Q Distance d _NH = -0.82e 1.012 10^-10 m To find the total dipole moment of ammonia, we need to consider the vector sum of the three bond dipole moments. Due to the trigonal pyramidal geometry of ammonia, the bond angle between the N-H bonds is approximately 107.5. Using vector addition and trigonometry, we can find the total dipole moment:_total = _NH 1 + 2 cos 107.5 Plugging in the values and solving for _total:_total 1.47 DebyeThe dipole moment of ammonia NH3 is approximately 1.47 Debye.