Question

Three compounds that are fairly typical of pure liquid substances include bromine (Br2), hexane (C6H14), and diethyl ether (C4H10O). Make an overall statement about the type of bonding present in these liquid substances.

Answer 1

Br2 is a diatomic molecule where the two Bromins forms covalent
bond by sharing a pair of electron.Thus octet will be satisfied
.Each bromine atom has 7 valance electron.Hence by sharing 1pair
of electron each get 8 electrons in their valance shell. The molecule
is non polar ,thus there is no dipole-dipole inter molecular
force between molecules.Only london force is present in Br2

Hexane molecule has single covalent bonds between carbon atoms and
between C and H atoms.Hexane is a non polar molecule.So only
inter molecular force present is weak london dispersion force

Di ethyl ether molecule has C,H and O atoms.Between atoms in the
molecule there is single covalent bond is present. SO ether also
a covalent compound. When we consider intermolecular forces:
the molecule has a more elecletro negative oxygen atom makes it
polar .SO ether has dipole moment.Thus there is dipole-dipole interaction
between positive end and negative end of different ether molecules.
Thus ether has inter molecular forces 1) dipole-dipole 2) london dispersion
forces.

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