Question

1. organic chemists identified four different liquids of varying volatilities that they want to test further. they want to compare the overall volatility and intermolecular forces of these liquids. look at the picture. for closed beaker, the circles indicate the amount of liquid volatility. a beaker with a large number of circles would have more liquid volatility than a beaker with only a few circles. which option correctly ranks the liquids in the order of increasing intermolecular forces? a. iv<iii<ii<i b. i<iii<ii<iv c. ii<iii<i<iv d. iii<ii<i<iv 24. which of the molecules has the highest boiling point? a. liquid 1: ch₄ b. liquid 2: ch₃ch₃ c. liquid 3: ch₃ch₂ch₃ d. liquid 4: ch₃ch₂ch₂ch₃

Explanation:

Step1: Analyze volatility and intermolecular forces relationship

Volatility is inversely related to intermolecular forces. Higher volatility means weaker intermolecular forces. From the beakers, the number of circles (representing volatility) is \(I < II < III < IV\). So, the order of increasing intermolecular forces (since intermolecular forces are inversely related to volatility) is \(I < II < III < IV\).

Step2: Analyze boiling - point and intermolecular forces relationship

For non - polar hydrocarbons (\(CH_4\), \(CH_3CH_3\), \(CH_3CH_2CH_3\), \(CH_3CH_2CH_2CH_3\)), the boiling point increases with the increase in molecular weight (or the number of carbon atoms). As the molecular weight increases, the London dispersion forces (a type of intermolecular force) increase. The number of carbon atoms: \(CH_4\) (\(n = 1\)), \(CH_3CH_3\) (\(n=2\)), \(CH_3CH_2CH_3\) (\(n = 3\)), \(CH_3CH_2CH_2CH_3\) (\(n=4\)).

Answer:

1. B. \(I
2. D. Liquid 4: \(CH_3CH_2CH_2CH_3\)