Question

considering the following list of compounds, which statement is most likely to be true? pentane (c₅h₁₂), decane (c₁₀h₂₂), trichloromethane (chcl₃), carbon tetrachloride (ccl₄) carbon tetrachloride (ccl₄) has a higher boiling point than pentane (c₅h₁₂) because carbon tetrachloride (ccl₄) has the greatest intermolecular dipole - dipole forces. decane (c₁₀h₂₂) is more viscous than pentane (c₅h₁₂) because decane (c₁₀h₂₂) has the greatest intermolecular dispersion forces they should all have the same surface tension because they contain a group iv element (carbon). trichloromethane (chcl₃) is more viscous than carbon tetrachloride (ccl₄) because trichloromethane (chcl₃) has greater intermolecular hydrogen bonding. pentane (c₅h₁₂) has a higher boiling point than decane

Explanation:

1. For the first option: Carbon - tetrachloride ($CCl_4$) is non - polar, so it has only London dispersion forces, not dipole - dipole forces.
2. For the second option: Viscosity is related to the strength of intermolecular forces. Larger molecules like decane ($C_{10}H_{22}$) have more electrons and larger surface areas, resulting in greater London dispersion forces compared to smaller pentane ($C_5H_{12}$), so decane is more viscous.
3. For the third option: Surface tension depends on the strength of intermolecular forces, not just the presence of a Group IV element. Different substances have different intermolecular forces and thus different surface tensions.
4. For the fourth option: Trichloromethane ($CHCl_3$) does not have hydrogen bonding as hydrogen must be bonded to a highly electronegative element like N, O, or F for hydrogen bonding to occur.
5. For the fifth option: Decane has a higher boiling point than pentane because decane has stronger London dispersion forces due to its larger size and more electrons.

Answer:

Decane ($C_{10}H_{22}$) is more viscous than pentane ($C_5H_{12}$) because decane ($C_{10}H_{22}$) has the greatest intermolecular dispersion forces.