Math

QuestionClassify each of the characteristics as a property of butane or 1-propanol.
Butane, CH3CH2CH2CH3\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3} 1-Propanol, CH3CH2CH2OH\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH} \square \square
Answer Bank stronger intermolecular forces less soluble in H2O\mathrm{H}_{2} \mathrm{O} less polar higher boiling point

Studdy Solution

STEP 1

What is this asking? We need to figure out which of the properties belong to butane and which belong to 1-propanol, comparing their intermolecular forces, solubility, polarity, and boiling points. Watch out! Don't mix up the effects of polarity and hydrogen bonding on intermolecular forces and physical properties.

STEP 2

1. Analyze the structures
2. Compare intermolecular forces
3. Determine properties

STEP 3

Let's look at butane: CH3CH2CH2CH3\mathrm{CH}_{3}\mathrm{CH}_{2}\mathrm{CH}_{2}\mathrm{CH}_{3}.
It's a **nonpolar hydrocarbon**, meaning it only has carbon and hydrogen atoms connected by nonpolar covalent bonds.

STEP 4

Now, consider 1-propanol: CH3CH2CH2OH\mathrm{CH}_{3}\mathrm{CH}_{2}\mathrm{CH}_{2}\mathrm{OH}.
It has an **oxygen atom** bonded to a hydrogen atom, forming an **O-H group**.
This is important because it allows for **hydrogen bonding**, a strong type of intermolecular force.

STEP 5

Butane, being nonpolar, only has **weak London Dispersion Forces**.
These forces arise from temporary fluctuations in electron distribution.

STEP 6

1-Propanol, on the other hand, has **hydrogen bonding** in addition to London Dispersion Forces.
Hydrogen bonding is significantly **stronger** than London Dispersion Forces.

STEP 7

Since 1-propanol has stronger intermolecular forces (hydrogen bonding), it will have a **higher boiling point**.
It takes more energy to overcome those stronger attractions and make 1-propanol boil.
So, **1-propanol** gets the "stronger intermolecular forces" and "higher boiling point" properties.

STEP 8

Water (H2O\mathrm{H}_{2}\mathrm{O}) is a polar molecule and readily dissolves other polar molecules ("like dissolves like").
Butane, being nonpolar, won't dissolve well in water.
Therefore, **butane** is "less soluble in H2O\mathrm{H}_{2}\mathrm{O}".

STEP 9

Again, butane is a nonpolar hydrocarbon, while 1-propanol has a polar O-H bond.
Thus, **butane** is "less polar".

STEP 10

Butane: less soluble in H2O\mathrm{H}_{2}\mathrm{O}, less polar 1-Propanol: stronger intermolecular forces, higher boiling point

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