Hydrogen bonding
The electronegative atoms O or N have a stronger pull on the electrons in the covalent bond with hydrogen, causing the bond to become polarised
Ammonia can form a maximum of one hydrogen bond per molecule Water can form a maximum of two hydrogen bonds per molecule Properties of water
High melting & boiling points
Hydrogen bonds are strong intermolecular forces which are difficult to break causing water to have high melting and boiling points
The high enthalpy change of evaporation of water suggests that instantaneous dipole-induced dipole forces are not the only forces present in the molecule – there are also those of the strong hydrogen bonds, which cause the high boiling points High surface tension
The surface molecules are pulled downwards due to the hydrogen bonds with other molecules, whereas the inner water molecules are pulled in all directions Density
The ‘more open’ structure of molecules in ice causes it to have a lower density than liquid water
Ice floats on water because of ice's lower density. Page 2The nuclear charge, atomic radius and shielding are all linked to each other.As nuclear charge increases, the nucleus has a greater attractive force on the electrons in shells given that the shielding doesn’t increase.As a result of this, the atomic radius decreases. Page 3
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