Why are intermolecular forces generally much weaker than bonding forces? What is

Question

Why are intermolecular forces generally much weaker than bonding forces?

What is capillary action? How does it depend on the relative strengths of adhesive and cohesive forces?

Water (a) “wets” some surfaces and beads up on others. Mercury (b), in contrast, beads up on almost all surfaces, Explain this difference?

When a thin glass tube is put into water, the water rises 1.4 cm. When the same tube is put into hexane, the hexane rises only 0.4 cm, explain the difference?

Why is vaporization endothermic? Why is condensation exothermic?

Is fusion exothermic or endothermic? Why?

Calculate the amount of heat required to completely sublime 91.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.

Why is the heat of vaporization of water greater at room temperature than it is at its boiling point?

Explanation / Answer

The bonding forces involves overlaping of orbitals, while the Intermolecular forces do not involve formal orbital overlap, Generally the intermolecular forces invole dipole and ion interactions - attraction.

It can be well understand by the fact that we need less than 800C of temperature to boil it ( as it involves the breaking of intermolecular interactions), however we can not separate the Carbon and hydrogen and oxygen from ethanol at such a low temeperature as these are bonded by bonding forces.

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