Final answer:
Larger molecules with greater surface areas have stronger dispersion forces. The provided hydrocarbons are ranked from the most dispersion forces (largest molecule) to the least (smallest molecule), with CH3CH(CH3)C(CH3)2CH2CH3 having the most and CH4 having the least.
Step-by-step explanation:
To rank the compounds from the most to the least dispersion forces, we need to consider their molecular sizes and shapes, as these determine the strength of London dispersion forces. In general, larger molecules with greater surface areas have stronger dispersion forces. Based on this, here's the ranking:
- CH3CH(CH3)C(CH3)2CH2CH3 (Most)
- CH3CH2(CH2)4CH2CH3
- CH3CH2CH2CHCH3
- CH3C(CH3)2CH3
- CH3CH2CH3
- CH4 (Least)
For the compounds provided in the question, CH3CH(CH3)C(CH3)2CH2CH3, being the largest molecule, has the most dispersion force. The smallest molecule, CH4 (methane), will have the least dispersion force.