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13. Liquids, Solids & Intermolecular Forces

Intermolecular Forces and Physical Properties

13. Liquids, Solids & Intermolecular Forces

Intermolecular Forces and Physical Properties

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Intermolecular Forces & Physical Properties Concept 1

Intermolecular Forces & Physical Properties Concept 1

Intermolecular Forces & Physical Properties Example 1

Intermolecular Forces & Physical Properties Example 1

Intermolecular Forces & Physical Properties Concept 2

Intermolecular Forces & Physical Properties Concept 2

Intermolecular Forces & Physical Properties Example 2

Intermolecular Forces & Physical Properties Example 2

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Intermolecular Forces - Hydrogen Bonding, Dipole Dipole Interactions - Boiling Point & Solubility

Intermolecular Forces - Hydrogen Bonding, Dipole Dipole Interactions - Boiling Point & Solubility

The Organic Chemistry Tutor

Liquids: Crash Course Chemistry #26

Liquids: Crash Course Chemistry #26

Viscosity, Cohesive and Adhesive Forces, Surface Tension, and Capillary Action

Viscosity, Cohesive and Adhesive Forces, Surface Tension, and Capillary Action

Professor Dave Explains

Intermolecular forces and physical properties

Intermolecular forces and physical properties

Benjamin Shepler

What are Intermolecular Forces?

What are Intermolecular Forces?

Intermolecular Forces and Boiling Points

Intermolecular Forces and Boiling Points

Professor Dave Explains

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Practice this topic

Multiple Choice

Which of the following will have the lowest boiling point?

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Multiple Choice

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

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Multiple Choice

Which of the following is a false statement about dispersion forces?

Multiple Choice

Which of the following statements is false about the changes occurring when ice is heated in an open beaker from −10.0℃ to water vapor at 110.0℃?

Multiple Choice

In order for a molecule to exhibit dipole-dipole forces, __________ must be present in the molecule.

Multiple Choice

Which of the following molecules will have the highest melting point?

(i) CH₃−CH₂−CH₂−CH₃

(ii)CH₃−CH₂−O−CH₂−CH₃

(iii) CH₃−CH₂−CH₂−CH₂−OH

Multiple Choice

Which of the following statements about viscosity is true?

Textbook Question

Three identical tubes are filled with different liquids; water, ethylene glycol, and olive oil. A small steel sphere was dropped into the tube, and the time it took to fall to the bottom was recorded. Which property of liquids is responsible for the differences in time for the sphere to fall through the liquid? (LO 11.1) (a) Surface tension (b) Boiling point (c) Viscosity (d) Vapor pressure

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Textbook Question

Which organic compound has the lowest viscosity? (LO 11.2)

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Textbook Question

Arrange the following molecules from lowest to highest boiling point. (LO 8.9) (I)

(a) I 6 II 6 III 6 IV (b) II 6 III 6 I 6 IV (c) IV 6 II 6 III 6 I (d) IV 6 I 6 II 6 III

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Textbook Question

Which type of intermolecular force accounts for each of these differences? (d) Acetone boils at 56 °C, whereas 2-methylpropane boils at -12 °C.

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Textbook Question

(a) List the following molecules in order of increasing polar- izability: GeCl4, CH4, SiCl4, SiH4, and GeBr4. (b) Predict the order of boiling points of the substances in part (a).

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Textbook Question

Water flows quickly through the narrow neck of a bottle, but maple syrup flows sluggishly. Is this different behavior due to a difference in viscosity or in surface tension for the liquids?

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Textbook Question

Predict which substance in each pair has the highest surface tension. (a) CCl4 or CH2Br2

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Textbook Question

Predict which substance in each pair has the highest viscosity. (b) Pentane or neopentane

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Textbook Question

Predict which substance in each pair has the highest viscosity. (a) Hexane 1CH3CH2CH2CH2CH2CH32 or 1-hexanol 1CH3CH2CH2CH2CH2CH2OH2

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Textbook Question

The chemical structure for oleic acid, the primary component of olive oil, is shown. Explain why olive oil has a higher vis- cosity than water.

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Textbook Question

The viscosity of water at 20 °C is 1.00 * 10-3 1N • s>m2 2 higher than dimethyl sulfide 31CH322 S4 2.8 * 10-4 1N • s>m2 2. Explain the difference in viscosity based on chemical structure.

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Textbook Question

Ethylene glycol (HOCH2CH2OH), the major substance in antifreeze, has a normal boiling point of 198 °C. By comparison, ethyl alcohol (CH3CH2OH) boils at 78 °C at atmospheric pressure. Ethylene glycol dimethyl ether (CH3OCH2CH2OCH3) has a normal boiling point of 83 °C, and ethyl methyl ether (CH3CH2OCH3) has a nomral boiling point of 11 °C. (a) Explain why replacement of a hydrogen on the oxygen by a CH3 group generally results in a lower boiling point.

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Textbook Question

Based on the type or types of intermolecular forces, predict the substance in each pair that has the higher boiling point: (d) phosgene (Cl2CO) or formaldehyde (H2CO)

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Textbook Question

The following diagram shows a close-up view of part of the vapor-pressure curves for a solvent (red curve) and a solution of the solvent with a second liquid (green curve). Is the second liquid more volatile or less volatile than the solvent?

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Textbook Question

The generic structural formula for a 1-alkyl-3-methylimid- azolium cation is where R is a -CH2(CH2)nCH3 alkyl group. The melting points of the salts that form between 1-alkyl-3-methylimidazolium cation and the PF6- anion are as follows: R = CH2CH3 (m.p. = 60 °C), R = CH2CH2CH3 (m.p. = 40 °C), r = CH2CH2CH2CH3 (m.p. = 10 °C), and R = CH2CH2CH2CH2CH2CH3 (m.p. = -61 °C). Why does the melting point decrease as the length of alkyl group increases?

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Textbook Question

(b) What is the relationship between viscos- ity and temperature?

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Textbook Question

Based on their composition and structure, list CH2Cl2, CH3CH2CH3, and CH3CH2OH in order of (c) increasing surface tension

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Textbook Question

Liquids can interact with flat surfaces just as they can with capillary tubes; the cohesive forces within the liquid can be stronger or weaker than the adhesive forces between liquid and surface: (i)

(b) Which of these diagrams, i or ii, rep- resents what happens when water is on a nonpolar surface?

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Textbook Question

Two dichloroethylene molecules with the same chemical formula 1C2H2Cl22, but different arrangements of atoms are shown.

(c) Which form of dichloroethylene has the highest boiling point?

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Textbook Question

The boiling points, surface tensions, and viscosities of water and several alcohols are as shown below: (b) How do you explain the fact that propanol and ethylene glycol have similar molecular weights (60 versus 62 amu), yet the viscosity of ethylene glycol is more than 10 times larger than propa- nol?

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Textbook Question

In each pair of compounds, pick the one with the higher boiling point. Explain your reasoning. c. CH4 or CH3CH3

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Textbook Question

In each pair of compounds, pick the one with the higher boiling point. Explain your reasoning. b. CS2 or CO2

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Textbook Question

In each pair of compounds, pick the one with the higher vapor pressure at a given temperature. Explain your reasoning. c. CH3OH or H2CO

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Textbook Question

In each pair of compounds, pick the one with the higher vapor pressure at a given temperature. Explain your reasoning. b. CH3CH2CH2OH or CH3OH

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Textbook Question

Which compound would you expect to have greater surface tension: acetone [(CH3)2CO] or water (H2O)? Explain.

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Textbook Question

The critical temperatures and pressures of a series of haloge- nated methanes are as follows: (c) Predict the critical temperature and pres- sure for CCl4 based on the trends in this table. Look up the experimentally determined critical temperatures and pressures for CCl4, using a source such as the CRC Hand- book of Chemistry and Physics, and suggest a reason for any discrepancies.

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Textbook Question

The structures of two isomers of heptane are shown. Which of these two compounds would you expect to have the greater viscosity?

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Textbook Question

Explain why the viscosity of multigrade motor oils is less temperature- dependent than that of single-grade motor oils.

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Textbook Question

(a) Place the following substances in order of increasing volatility: CH4, CBr4, CH2Cl2, CH3Cl, CHBr3, and CH2Br2. (b) How do the boiling points vary through this series? (c) Explain your answer to part (b) in terms of intermolec- ular forces.

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Textbook Question

When a thin glass tube is put into water, the water rises 1.4 cm. When the same tube is put into hexane, the hexane rises only 0.4 cm. Explain.

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Textbook Question

Which evaporates more quickly: 55 mL of water (H2O) in a beaker or 55 mL of acetone [(CH3)2CO] in an identical beaker under identical conditions? Is the vapor pressure of the two substances different? Explain.

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Textbook Question

As the intermolecular attractive forces between molecules increase in magnitude, do you expect each of the following to increase or decrease in magnitude? (g) critical temperature.

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Textbook Question

Suppose you have two colorless molecular liquids, one boil- ing at - 84 °C, the other at 34 °C, and both at atmospheric 6 pressure. Which of the following statements is correct? For each statement that is not correct, modify the statement so that it is correct. (e) At - 84 °C both liquids have vapor pressures of 760 mm Hg.

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Textbook Question

Suppose you have two colorless molecular liquids, one boil- ing at - 84 °C, the other at 34 °C, and both at atmospheric 6 pressure. Which of the following statements is correct? For each statement that is not correct, modify the statement so that it is correct. (d) The two liquids have iden- tical vapor pressures at their normal boiling points.

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Textbook Question

The table below shows the normal boiling points of benzene and benzene derivatives. (e) Why is the boiling point of phenol the highest of all?

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Textbook Question

(a) When you exercise vigorously, you sweat. How does this help your body cool?

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Textbook Question

(b) A flask of water is connected to a vacuum pump. A few moments after the pump is turned on, the water begins to boil. After a few minutes, the water begins to freeze. Explain why these processes occur.

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Textbook Question

Explain the observed trend in the melting points of the hydrogen halides. HI -50.8 °C HBr -88.5 °C HCl -114.8 °C HF -83.1 °C

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Textbook Question

Explain the observed trend in the boiling points of these compounds. H2Te -2 °C H2Se -41.5 °C H2S -60.7 °C H2O 100 °C

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Textbook Question

In Table 11.3, we saw that the viscosity of a series of hydro- carbons increased with molecular weight, doubling from the six-carbon molecule to the ten-carbon molecule.

(a) The eight-carbon hydrocarbon, octane, has an isomer, isooctane. Would you predict that isooctane would have a larger or smaller viscosity than octane? Why?

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Textbook Question

For each of the following substances, identify the intermolecular force or forces that predominate. Using your knowledge of the relative strengths of the various forces, rank the substances in order of their normal boiling points: Al2O3, F2, H2O, Br2, ICl, NaCl.

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

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Ionic compounds are formed from ionic bonds, whereby an electron is transferred from the metal cation to the nonmetal anion. ions form solid lattices of ions. covalent compounds form solids through the attraction of two covalent molecules. since the attraction between two covalent molecules is weak compared to the ionic bonds holding an ionic compound together, ionic compounds tend to have higher melting points. which of the following compounds has the highest boiling point?

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

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

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

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

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

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

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

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

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

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

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

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

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

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