Answer:
The answer to the question is;
The inter-molecular forces of water are stronger than those of hydrogen.
Explanation:
Ammonia is a compressible gas at room temperature with molecules free to move about and so fill up the volume of the container in which it is placed due to the weaker inter-molecular Van der Waals forces such as Keesom, Debye and London dispersion forces holding the particles of ammonia together in a given volume of the compound.
The inter-molecular forces between water molecules is hydrogen binding and dipole moments due to the strongly electronegative oxygen and hydrogen which tends to move the electrons towards the oxygen creating a charge imbalance that causes the hydrogen surrounding the water molecule to aggregate to neutralize the the charge imbalance forming the bases for the strong hydrogen bonds.
Therefore water is a liquid at room temperature while ammonia is a gas due to the difference in strength of their inter-molecular forces.
The intermolecular forces in water are stronger than the intermolecular forces in ammonia.
The intermolecular forces hold substances together in a particular state of matter. There are three states of matter;
The strongest degree of intermolecular interaction occurs between matter in the solid state. weaker intermolecular interactions occur in the liquid state and the weakest intermolecular interaction occurs in the gaseous state.
Since ammonia is a gas at room temperature, it has weaker intermolecular interaction between its molecules compared to molecules of water at room temperature:
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