1.1 Explain why ethanol is soluble in water. Refer to the...

1.1 Explain why ethanol is soluble in water. Refer to the relative strength of the intermolecular forces in ethanol and water. 1.2 Explain why the boiling point of iodine is higher than that of bromine. Refer to the intermolecular forces present in EACH substance in the explanation. 1.3 Explain why phosphine will evaporate faster than ammonia by referring to the types of intermolecular forces present in EACH substance. 1.4 Water, ethanol and bromine are all liquids at room temperature. Which ONE will have the highest vapour pressure? 1.5 Give a reason for the answer to QUESTION 1.4 by referring to the relative strength of the intermolecular forces and boiling points. 2. The boiling point of compounds A to E are given in the table below.

Transcript

00:01 All right, so we've got a couple questions to answer here.

00:03 Firstly, explaining why ethanol is soluble in water.

00:08 Refer to relative strengths of the intermolecular forces.

00:11 Okay, so if ethanol was by itself, it would be capable of some vanderwals interactions.

00:17 If carbon, i mean, this was perplexing to me that every single one of these, whether they have dipole, dipole, or h bonding, any of these intermolecular forces, they will also have vanderwals.

00:27 But if it is soluble in water, it means if any compound is soluble in a solvent, it means that it is bonding stronger to the solvent than it was to itself.

00:41 So the power of h bonding at this hydroxyl group with water must be sexier to a methanol than its interactions with itself.

00:51 Next, explain why the boiling point of iodide is higher than bromine.

00:55 Okay, both diatomic molecules.

00:59 So they both are only experiencing vanderwals forces, but because iodide is so much larger than bromine, its electron cloud is more polarizable.

01:13 So if another iodide little group came over, it would warp that cloud more significantly.

01:21 So these electrons would be like, oh, get out of the way.

01:24 This other guys are repulsive.

01:26 And they would collect over here, creating this induced dipole more intensely than something that is not of as large an atomic radius.

01:37 All right.

01:38 Next, why phosphine is evaporating faster than ammonia.

01:43 Well, phosphine, though there is a dipole right here because of the electronegativity differences of phosphorus and hydrogen, it is not one of those atoms.

01:55 There's a magic combo of atoms that have to happen to create h bonding.

02:01 You have to have an n to an h, o to an h, or f to an h, and then another electromagnetic atom on a neighboring molecule.

02:09 So as you see, there is also a dipole here from this n to h on the ammonium, but it's in the h bonding category, which is stronger than dipole dipole...

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