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5. explain the relative volatilities for a) iodine, b) graphite, c) sodium chloride in terms of the particles they contain and the forces of attraction between them.
Accepted Answer
Here's an explanation of the volatilities based on their bonding and intermolecular forces:
a) Iodine (I2)
Particles: Diatomic molecules held together by strong covalent bonds.
Forces: Weak London Dispersion forces between molecules due to temporary dipoles.
Volatility: Iodine is relatively volatile. The weak intermolecular forces allow molecules to break free easily and transition to the gas phase at moderate temperatures.
b) Graphite
Particles: A giant covalent structure composed of layers of carbon atoms in hexagonal rings.
Forces: Strong covalent bonds within the layers and weak London Dispersion forces between layers.
Volatility: Graphite is not volatile. The strong covalent bonds within the layers make it very difficult to break apart the structure, requiring very high temperatures for vaporization.
c) Sodium chloride (NaCl)
Particles: Ionic compound made of Na+ and Cl- ions.
Forces: Strong electrostatic attractions between oppositely charged ions, forming a giant ionic lattice.
Volatility: Sodium chloride is not volatile. The strong electrostatic attractions require very high temperatures to overcome, preventing easy transition to the gas phase.
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