13. Liquids, Solids & Intermolecular Forces

Which of the following will have the lowest boiling point?

Which molecules would most likely cause a liquid to have the lowest viscosity?

(i) CH₃−CH₂−CH₂−CH₃

(ii)CH₃−CH₂−O−CH₂−CH₃

(iii) CH₃−CH₂−CH₂−CH₂−OH

Ammonia and hydrogen fluoride both have unusually high boiling points due to _____.

Which compound has the highest melting point: Al₂(CO₃)₃, C₁₂H₂₂O₁₁, C₈H₁₈, or H₂O?

A liquid with high viscosity _____ flow easily and _____ effective in wetting a surface.

Which would have a higher vapor pressure: ethanol (C₂H₅OH) or dimethyl ether (CH₃OCH₃)?

Choose the correct description of viscosity. Under what conditions does magma have high viscosity?

Which of the following properties of water is responsible for the formation of raindrops?

Which of the following properties of water is responsible for the formation of raindrops?

Which would have a higher vapor pressure: ethanol (C₂H₅OH) or dimethyl ether (CH₃OCH₃)?

Water readily sticks to many other substances, a property called ______.

Which of the following straight-chain hydrocarbons will have the highest viscosity at 298 K?

Solid ice will change to liquid water and then to gaseous steam when you add

Rank the following based on increasing intermolecular forces? C₂H₆, C₄H₁₀, C₆H₁₄, C₈H₁₈.

Which of the following is most likely to have the highest viscosity at 25°C?

What are the properties and common uses of water in each of its states?

Which of the following should have the highest surface tension at a given temperature?

The ionic liquid (bmim+)(PF6−) has a melting point of 10°C and a surface tension of approximately 4.5×10−2 J/m2 at room temperature. By comparison, the melting point of H2O is 0°C and its surface tension is 7.3×10−2 J/m2 at room temperature. What is the most plausible explanation for the higher surface tension of water?

i. hydrogen bonding interactions are stronger than ion–ion interactions.

ii. Surface tension increases as molecules become smaller and more symmetric because the number of neighboring molecules in the liquid state increases.

iii. As the molecules become smaller, they can escape into the gas phases more easily, leading to an increase in surface tension.