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i guess,its hydrogen bond..
An ammonia molecule has covalent bonds in it.
106
There is only one bond. It is on the N atom.
When each molecule is considered, only three covalent bonds are there. When liquid ammonia is considered, there are hydrogen bonds between the molecules.
i guess,its hydrogen bond..
An ammonia molecule has covalent bonds in it.
Luzzy
106
There are a infinitely growing number of bond pairs between atoms.
There is only one bond. It is on the N atom.
The lone pair of electrons in the ammonia molecule is located in the outermost electron shell of the ammonia molecule. This will enable it to easily form a bond with any compound that it is mixed with.
Bond angles in various molecules tend to be as big as possible and therefore we would expect a bond angle of 120°. Ammonia, however, is a permanent dipole and therefore acts like it owns a 4th hydrogen atom. Ammonia more or less acts like a tetrahedral molecule. This phenomena occurs in water as well. The theoretical bond angle for a tetrahedral molecule would be 109.5°, but in ammonia it's a little lower, the experimental bond angle of ammonia is 107°. This is because of the additional repulsive force of the electron pair occupying the "fourth" spot of the tetrahedron.
When each molecule is considered, only three covalent bonds are there. When liquid ammonia is considered, there are hydrogen bonds between the molecules.
The bond angles between two N-H bonds in ammonia are close to the bond angles characteristic of a tetrahedron, but the molecule as a whole is not a tetrahedron because one of the four bonds to a central atom found in an actual tetrahedral molecule is missing; there are only three hydrogen atoms bound to a central nitrogen atom in ammonia. In an ammonium ion, however, the tetrahedron is complete.
use the prefix trans-
NH3 is the molecular formula for ammonia, and each N-H bond is polar, and the 3-D structure of the molecule makes the molecule polar. NH3 molecules will form hydrogen bonds with other molecules. Refer to the related links for an illustration of the ammonia molecule.