Start typing, then use the up and down arrows to select an option from the list.

General Chemistry

Learn the toughest concepts covered in Chemistry with step-by-step video tutorials and practice problems by world-class tutors

13. Liquids, Solids & Intermolecular Forces

Molecular Polarity

10 videos30 questions

VIDEOS 10

Previous videos for

Next videos for

PRACTICE 30

Multiple Choice
Determine if the compound of BCl₂F is polar or nonpolar.
884views
1
2
Multiple Choice
Determine if phosphorus trihydride, PH₃, is polar or nonpolar.
617views
1
Multiple Choice
Which of the following compounds is/are nonpolar?
I. COF₂ II. ICl₂^– III. XeF₄ IV. C₈H₁₈
380views
Multiple Choice
Determine if disulfur dichloride, S₂Cl₂, is polar or nonpolar.
602views
1
Textbook Question
(a) Consider the following two molecules: PCl3 and BCl3. Which molecule has a nonzero dipole moment?
123views
Textbook Question
Dichloroethylene 1C2H2Cl22 has three forms (isomers), each of which is a different substance. (b) Which of these isomers has a zero dipole moment?
59views
Textbook Question
Fluorine is more electronegative than chlorine, yet fluoromethane 1CH3F; m = 1.86 D2 has a smaller dipole moment than chloromethane 1CH3Cl; m = 1.90 D2. Explain.
97views
Textbook Question
Draw three-dimensional structures of PCl3 and PCl5, and then explain why one of the molecules has a dipole moment and one does not.
99views
Textbook Question
Ethyl acetate, CH3CO2CH2CH3, is commonly used as a solvent and nail-polish remover. Look at the following electrostatic potential map of ethyl acetate, and explain the observed polarity.
13views
Textbook Question
Just as individual bonds in a molecule are often polar, molecules as a whole are also often polar because of the net sum of individual bond polarities. There are three possible structures for substances with the formula C2H2Cl2, two of which are polar overall and one of which is not. (b) Which of the three structures is nonpolar, and which two are polar? Explain.
96views
Textbook Question
Which of the following substances would you expect to have a nonzero dipole moment? Explain, and show the direction of each. (a) Cl2O (b) XeF4 (c) Chloroethane, CH3CH2Cl (d) BF3
66views
Textbook Question
Which molecule has polar bonds but is nonpolar? (LO 8.6) (a) SF6 (b) SF2 (c) F2 (d) NF3
174views
Textbook Question
The dipole moment of methanol is m = 1.70 D. Use arrows to indicate the direction in which electrons are displaced.
15views
Textbook Question
Of the two compounds SiF4 and SF4, which is polar and which is nonpolar?
171views
Textbook Question
The molecules
have the same molecular formula (C3H8O) but different chemical structures. (b) Which molecule do you expect to have a larger dipole moment? [Sections 11.2 and 11.5]
13views
Textbook Question
The molecule shown here is difluoromethane 1CH2F22, which is used as a refrigerant called R-32. (c) If the molecule is polar, which of the following describes the direction of the overall dipole moment vector in the molecule: (i) from the carbon atom toward a fluorine atom, (ii) from the carbon atom to a point midway between the fluorine atoms, (iii) from the carbon atom to a point midway between the hydrogen atoms, or (iv) from the carbon atom toward a hydrogen atom?
15views
Textbook Question
Dihydroxybenzene, C6H6O2, exists in three forms (isomers) called ortho, meta, and para:
Which of these has a nonzero dipole moment?
18views
Textbook Question
Fill in the blank spaces in the following chart. If the molecule column is blank, find an example that fulfills the conditions of the rest of the row. Molecule Electron-Domain Hybridization Dipole Geometry of Central Atom Moment? Yes or No CO2 sp3 Yes sp3 No Trigonal planar No SF4 Octahedral No sp2 Yes Trigonal bipyramidal No XeF2 Complete the first row of the table.
131views
Textbook Question
Predict whether each of the following molecules is polar or nonpolar: (a) CCl4, (b) NH3, (c) SF4, (d) XeF4, (e) CH3Br, (f) GaH3.
217views
Textbook Question
Predict whether each of the following molecules is polar or nonpolar: (a) IF, (b) CS2, (c) SO3, (d) PCl3, (e) SF6, (f) IF5.
559views
Textbook Question
Determine whether each molecule is polar or nonpolar. a. SiCl4 b. CF2Cl2 c. SeF6 d. IF5
237views
Textbook Question
Determine whether each molecule is polar or nonpolar. c. BrCl5
193views
Textbook Question
Determine whether each molecule is polar or nonpolar. b. SCl4
380views
Textbook Question
Draw the structure of a molecule with the formula C4H6Cl2 that has a dipole moment of 0.
254views
Textbook Question
Most vitamins can be classified as either fat soluble, which results in their tendency to accumulate in the body (so that taking too much can be harmful), or water soluble, which results in their tendency to be quickly eliminated from the body in urine. Examine the structural formulas and space-filling models of these vitamins and determine whether each one is fat soluble (mostly nonpolar) or water soluble (mostly polar). (c) niacin (vitamin B3)
16views
Textbook Question
Most vitamins can be classified as either fat soluble, which results in their tendency to accumulate in the body (so that taking too much can be harmful), or water soluble, which results in their tendency to be quickly eliminated from the body in urine. Examine the structural formulas and space-filling models of these vitamins and determine whether each one is fat soluble (mostly nonpolar) or water soluble (mostly polar). (a) vitamin C
14views
Textbook Question
CH3F is a polar molecule, even though the tetrahedral geometry often leads to nonpolar molecules. Explain.
1575views
Textbook Question
Explain why CO2 and CCl4 are both nonpolar even though they contain polar bonds.
352views
Textbook Question
Determine whether each molecule in Exercise 58 is polar or nonpolar. a. CF4 b. NF3 c. OF2 d. H2S
548views
Textbook Question
Determine whether each molecule in Exercise 57 is polar or nonpolar. a. PF3 b. SBr2 c. CHCl3 d. CS2
105views

Intermolecular Forces

14 videos45 questions

VIDEOS 14

Previous videos for

Next videos for

PRACTICE 45

Textbook Question

Ethanol 1CH CH OH 2 dissolves in hexane 1C H 2. Give the strongest type of intermolecular force between two sol- ute molecules, between two solvent molecules, and between a solute and solvent molecule. (LO 13.1) (a)

Textbook Question

Intermolecular forces are important in creating ordered arrangements in liquid crystals. What types of intermolecu- lar forces exist in a sample of the following compound?

Textbook Question

What types of intermolecular forces exist in a sample of acetone? (LO 8.8)

(a) Dispersion forces (b) Dispersion forces and dipole–dipole forces (c) Dipole–dipole forces (d) Dispersion forces, dipole–dipole forces, and hydrogen bonding

Textbook Question

When ethyl alcohol, CH3CH2OH, dissolves in water, how many hydrogen bonds are formed between one ethyl alcohol molecule and surrounding water molecules? Sketch the hydro- gen bonding interactions. (Hint: Add lone pairs of electrons to the structure before drawing hydrogen bonds.)

Textbook Question

List the three states of matter in order of (b) increasing intermolecular attrac- tion.

Textbook Question

List the three states of matter in order of (a) increasing molecular disorder

Textbook Question

Which member in each pair has the greater dispersion forces?(c) SiH4 or GeH4.

Textbook Question

Which member in each pair has the greater dispersion forces? (a) H2O or H2S,

Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. d. I2

Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. d. HF

Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. a. Kr

Textbook Question

A number of salts containing the tetrahedral polyatomic anion, BF4-, are ionic liquids, whereas salts containing the somewhat larger tetrahedral ion SO42 - do not form ionic liquids. Explain this observation.

Textbook Question

(a) How does the average kinetic energy of molecules com- pare with the average energy of attraction between mole- cules in solids, liquids, and gases?

Textbook Question

At room temperature, Si is a solid,CCl4 is a liquid, and Ar is a gas. List these substances in order of (a) increasing intermo- lecular energy of attraction and

Textbook Question

(a) Which kind of intermolecular attractive force is shown in each case here? (b) Predict which of the four interactions is the weakest. [Section 11.2] (i)

Textbook Question

True or false: (b) For the noble gases the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table.

Textbook Question

The table below shows the normal boiling points of benzene and benzene derivatives.

(a) How many of these compounds exhibit dispersion in- teractions?

Textbook Question

Two isomers of the planar compound 1,2-dichloroethylene are shown here.

(a) Which of the two isomers will have the stronger dipole– dipole forces?

Textbook Question

The critical temperatures and pressures of a series of haloge- nated methanes are as follows:

(a) List the intermolecular forces that occur for each compound.

Textbook Question

Describe the intermolecular forces that must be overcome to convert these substances from a liquid to a gas: (b) CH3COOH,

Textbook Question

Which member in each pair has the stronger intermolecular dispersion forces? (c) CH3CH2CH2Cl or (CH3)2CHCl

Textbook Question

True or false: (e) The larger the atom, the more polarizable it is.

Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. c. CH3OH

Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. d. He

Textbook Question

Determine the kinds of intermolecular forces that are present in each element or compound. b. NCl3

Textbook Question

Would you expect that an anion would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?

Intermolecular Forces and Physical Properties

10 videos44 questions

Previous videos for

Next videos for

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

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.

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?

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.

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.

Textbook Question

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

Textbook Question

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

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

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?

Textbook Question

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

Textbook Question

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

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.

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.

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?

Textbook Question

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

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?

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.

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?

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.

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.

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?

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.

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)

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.

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).

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.

Textbook Question

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

Textbook Question

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

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.

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

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

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.

Textbook Question

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

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

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

Textbook Question

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

Textbook Question

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

Clausius-Clapeyron Equation

11 videos15 questions

Previous videos for

Next videos for

Phase Diagrams

12 videos36 questions

Previous videos for

Next videos for

Heating and Cooling Curves

10 videos22 questions

Previous videos for

Next videos for

Atomic, Ionic, and Molecular Solids

9 videos67 questions

Previous videos for

Next videos for

Crystalline Solids

8 videos53 questions

Previous videos for

Next videos for

Simple Cubic Unit Cell

7 videos18 questions

Previous videos for

Next videos for

Body Centered Cubic Unit Cell

7 videos22 questions

Previous videos for

Next videos for

Face Centered Cubic Unit Cell

7 videos41 questions

Previous videos for

Next videos for

Divider

Download the Mobile app

© 1996–2023 Pearson All rights reserved.