Question

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1. Indicate which is the strongest intermolecular force between each of the two molecules below: a. H2S and H2O b. C4H10 (butane) and (CH3)2CO (acetone) 2. Considering properties of liquids: a. Surface tension is proportional to the magnitude of intermolecular forces and/or attractive forces among the molecules in the liquid. With this perspective in mind, which in the following pair of liquids would have the highest surface tension: H2O or CHCl3 (chloroform) b. Indicate if each of the following liquids would be expected to form a concave or convex meniscus in a glass graduated cylinder: H20; Hg c. Indicate which of the following pairs of liquids would have the highest viscosity: CH3COOH (acetic acid) or CH 4 (hexane) d. Indicate which of the following pairs of liquids would have the highest vapour pressure: CH3OH (methanol) or C2H4O2 (ethyelene glycol) 3. Indicate the types of attractive forces could each type of solid has within its structure: a. Molecular solid b. Metallic solid c. Network solid d. Ionic solid 4. Identify the type of solid ionic, metallic, molecular, or network solid) for each of the following compound compounds: a. H2Os) (ice) b. BN (boron nitride) C. KCIE d. Au

Answer 1

1. a. Hydrogen bonding interaction shall occur with h of h2s and o of h2o.

b. Here vanderWaal type interaction shall predominate between C=C bonds and C=O bonds.

2. a.As H2O is a hydrogen bonded solid, it shall have greater surface tension due to greater intermolecular force of attraction.

b. Water wets the glass surface, ie adhesive force exist between water and glass, a concave meniscus would form. For mercury, adhesive force is minimal. Hence it forms concave meniscus.

c. Acetic acid undergoes intermolecular hydrogen bonding and hence would have higher viscosity.

d. Methanol has one OH group whereas ethylene glycol has two. Therefore hydrogen bonding sites are less in methanol, which memakes it more volatile. Hence methanol would have higher vapour pressure.

3. In molecular solids, vanderwaals interaction are present.

In metallic solids, expensive metal bonds present.

In network solids, covalent bonds provide attractive force

In ionic solids, ionic bonding between cation and anion imparts stability.

4. a. Ice is a hydrogen bonded network solid.

b. Boron nitride is a molecular solid.

c. KCl is an ionic solid.

d. Au(s) is a metallic solid