- 11.11.1: Give an example for each type of intermolecular force. (a) dipole-d...
- 11.11.2: Explain the term polarizability. What kind of molecules tend to hav...
- 11.11.3: Explain the difference between a temporary dipole moment and the pe...
- 11.11.4: Give some evidence that all atoms and molecules exert attractive fo...
- 11.11.5: What physical properties should you consider in comparing the stren...
- 11.11.6: Which elements can take part in hydrogen bonding? Why is hydrogen u...
- 11.11.7: The compounds Br2 and ICl have the same number of electrons, yet Br...
- 11.11.8: If you lived in Alaska, which of the following natural gases would ...
- 11.11.9: The binary hydrogen compounds of the Group 4A elements and their bo...
- 11.11.1b: List the types of intermolecular forces that exist between molecule...
- 11.11.11: Ammonia is both a donor and an acceptor of hydrogen in hydrogen-bon...
- 11.11.12: Which of the following species are capable of hydrogen-bonding amon...
- 11.11.13: Arrange the following in order of increasing boiling point: RbF, CO...
- 11.11.14: Diethyl ether has a boiling point of 34.5C, and 1-butanol has a boi...
- 11.11.15: Which member of each of the following pairs of substances would you...
- 11.11.16: Which substance in each of the following pairs would you expect to ...
- 11.11.17: Explain in terms of intermolecular forces why (a) NH3 has a higher ...
- 11.11.18: What kind of attractive forces must be overcome in order to (a) mel...
- 11.11.19: The following compounds have the same molecular formulas (C4H10). W...
- 11.11.2b: Explain the difference in the melting points of the following compo...
- 11.11.21: Explain why liquids, unlike gases, are virtually incompressible
- 11.11.22: What is surface tension? What is the relationship between intermole...
- 11.11.23: Despite the fact that stainless steel is much denser than water, a ...
- 11.11.24: Use water and mercury as examples to explain adhesion and cohesion.
- 11.11.25: A glass can be filled slightly above the rim with water. Explain wh...
- 11.11.26: Draw diagrams showing the capillary action of (a) water and (b) mer...
- 11.11.27: What is viscosity? What is the relationship between intermolecular ...
- 11.11.28: Why does the viscosity of a liquid decrease with increasing tempera...
- 11.11.29: Why is ice less dense than water?
- 11.11.3b: Outdoor water pipes have to be drained or insulated in winter in a ...
- 11.11.31: Predict which of the following liquids has greater surface tension:...
- 11.11.32: Predict the viscosity of ethylene glycol relative to that of ethano...
- 11.11.33: Define the following terms: crystalline solid, lattice point, unit ...
- 11.11.34: Describe the geometries of the following cubic cells: simple cubic,...
- 11.11.35: Classify the solid states in terms of crystal types of the elements...
- 11.11.36: The melting points of the oxides of the third-period elements are g...
- 11.11.37: What is the coordination number of each sphere in (a) a simple cubi...
- 11.11.38: Calculate the number of spheres that would be found within a simple...
- 11.11.39: Metallic iron crystallizes in a cubic lattice. The unit cell edge l...
- 11.11.4b: Barium metal crystallizes in a body-centered cubic lattice (the Ba ...
- 11.11.41: Vanadium crystallizes in a body-centered cubic lattice (the V atoms...
- 11.11.42: Europium crystallizes in a body-centered cubic lattice (the Eu atom...
- 11.11.43: Crystalline silicon has a cubic structure. The unit cell edge lengt...
- 11.11.44: A face-centered cubic cell contains 8 X atoms at the corners of the...
- 11.11.45: Define X-ray diffraction. What are the typical wavelengths (in nano...
- 11.11.46: Write the Bragg equation. Define every term and describe how this e...
- 11.11.47: When X rays of wavelength 0.090 nm are diffracted by a metallic cry...
- 11.11.48: The distance between layers in a NaCl crystal is 282 pm. X rays are...
- 11.11.49: Describe and give examples of the following types of crystals: (a) ...
- 11.11.5b: Why are metals good conductors of heat and electricity? Why does th...
- 11.11.51: A solid is hard, brittle, and electrically nonconducting. Its melt ...
- 11.11.52: A solid is soft and has a low melting point (below 100C). The solid...
- 11.11.53: A solid is very hard and has a high melting point. Neither the soli...
- 11.11.54: Which of the following are molecular solids and which are covalent ...
- 11.11.55: Classify the solid state of the following substances as ionic cryst...
- 11.11.56: Explain why diamond is harder than graphite. Why is graphite an ele...
- 11.11.57: What is an amorphous solid? How does it differ from crystalline solid?
- 11.11.58: Define glass. What is the chief component of glass? Name three type...
- 11.11.59: What is a phase change? Name all possible changes that can occur am...
- 11.11.6b: What is the equilibrium vapor pressure of a liquid? How is it measu...
- 11.11.61: Use any one of the phase changes to explain what is meant by dynami...
- 11.11.62: Define the following terms: (a) molar heat of vaporization, (b) mol...
- 11.11.63: How is the molar heat of sublimation related to the molar heats of ...
- 11.11.64: What can we learn about the intermolecular forces in a liquid from ...
- 11.11.65: The greater the molar heat of vaporization of a liquid, the greater...
- 11.11.66: Define boiling point. How does the boiling point of a liquid depend...
- 11.11.67: As a liquid is heated at constant pressure, its temperature rises. ...
- 11.11.68: What is critical temperature? What is the significance of critical ...
- 11.11.69: What is the relationship between intermolecular forces in a liquid ...
- 11.11.7b: How do the boiling points and melting points of water and carbon te...
- 11.11.71: Why is solid carbon dioxide called dry ice?
- 11.11.72: Wet clothes dry more quickly on a hot, dry day than on a hot, humid...
- 11.11.73: Which of the following phase transitions gives off more heat? (a) 1...
- 11.11.74: A beaker of water is heated to boiling by a Bunsen burner. Would ad...
- 11.11.75: Calculate the amount of heat (in kJ) required to convert 74.6 g of ...
- 11.11.76: How much heat (in kJ) is needed to convert 866 g of ice at 210C to ...
- 11.11.77: How is the rate of evaporation of a liquid affected by (a) temperat...
- 11.11.78: The molar heats of fusion and sublimation of molecular iodine are 1...
- 11.11.79: The following compounds, listed with their boiling points, are liqu...
- 11.11.8b: Freeze-dried coffee is prepared by freezing brewed coffee and then ...
- 11.11.81: A student hangs wet clothes outdoors on a winter day when the tempe...
- 11.11.82: Steam at 100C causes more serious burns than water at 100C. Why?
- 11.11.83: Vapor pressure measurements at several different temperatures are s...
- 11.11.84: The vapor pressure of benzene, C6H6, is 40.1 mmHg at 7.6C. What is ...
- 11.11.85: The vapor pressure of liquid X is lower than that of liquid Y at 20...
- 11.11.86: Explain why splashing a small amount of liquid nitrogen (b.p. 77 K)...
- 11.11.87: What is a phase diagram? What useful information can be obtained fr...
- 11.11.88: Explain how waters phase diagram differs from those of most substan...
- 11.11.89: The phase diagram of sulfur is shown here. (a) How many triple poin...
- 11.11.9b: A length of wire is placed on top of a block of ice. The ends of th...
- 11.11.91: The boiling point and freezing point of sulfur dioxide are 210C and...
- 11.11.92: A phase diagram of water is shown at the end of this problem. Label...
- 11.11.93: Name the kinds of attractive forces that must be overcome in order ...
- 11.11.94: Which of the following properties indicates very strong intermolecu...
- 11.11.95: At 235C, liquid HI has a higher vapor pressure than liquid HF. Expl...
- 11.11.96: Based on the following properties of elemental boron, classify it a...
- 11.11.97: Referring to Figure 11.41, determine the stable phase of CO2 at (a)...
- 11.11.98: Classify the unit cell of molecular iodine
- 11.11.99: A CO2 fire extinguisher is located on the outside of a building in ...
- 11.11.1c: What is the vapor pressure of mercury at its normal boiling point (...
- 11.11.101: A flask of water is connected to a powerful vacuum pump. When the p...
- 11.11.102: The liquid-vapor boundary line in the phase diagram of any substanc...
- 11.11.103: The interionic distance of several alkali halide crystals are: NaCl...
- 11.11.104: Which has a greater density, crystalline SiO2 or amorphous SiO2? Why?
- 11.11.105: In 2009, thousands of babies in China became ill from drinking cont...
- 11.11.106: The vapor pressure of a liquid in a closed container depends on whi...
- 11.11.107: A student is given four solid samples labeled W, X, Y, and Z. All e...
- 11.11.108: Which of the following statements are false? (a) Dipole-dipole inte...
- 11.11.109: The diagram below shows a kettle of boiling water on a stove. Ident...
- 11.11.11c: The south pole of Mars is covered with dry ice, which partly sublim...
- 11.11.111: The properties of gases, liquids, and solids differ in a number of ...
- 11.11.112: Select the substance in each pair that should have the higher boili...
- 11.11.113: A small drop of oil in water assumes a spherical shape. Explain. (H...
- 11.11.114: Under the same conditions of temperature and density, which of the ...
- 11.11.115: The fluorides of the second-period elements and their melting point...
- 11.11.116: The standard enthalpy of formation of gaseous molecular iodine is 6...
- 11.11.117: The following graph shows approximate plots of ln P versus 1/T for ...
- 11.11.118: Determine the final state and its temperature when 150.0 kJ of heat...
- 11.11.119: The distance between Li1 and Cl2 is 257 pm in solid LiCl and 203 pm...
- 11.11.12c: Heat of hydration, that is, the heat change that occurs when ions b...
- 11.11.121: If water were a linear molecule, (a) would it still be polar, and (...
- 11.11.122: Calculate the H for the following processes at 25C: (a) Br2(l) Br2(...
- 11.11.123: Gaseous or highly volatile liquid anesthetics are often preferred i...
- 11.11.124: A beaker of water is placed in a closed container. Predict the effe...
- 11.11.125: The phase diagram of helium is shown here. Helium is the only known...
- 11.11.126: Referring to Figure 11.26, determine the number of each type of ion...
- 11.11.127: Ozone (O3) is a strong oxidizing agent that can oxidize all the com...
- 11.11.128: A sample of limestone (CaCO3) is heated in a closed vessel until it...
- 11.11.129: Silicon used in computer chips must have an impurity level below 10...
- 11.11.13c: Carbon and silicon belong to Group 4A of the periodic table and hav...
- 11.11.131: A pressure cooker is a sealed container that allows steam to escape...
- 11.11.132: A 1.20-g sample of water is injected into an evacuated 5.00-L flask...
- 11.11.133: What are the advantages of cooking the vegetable broccoli with stea...
- 11.11.134: A quantitative measure of how efficiently spheres pack into unit ce...
- 11.11.135: Provide an explanation for each of the following phenomena: (a) Sol...
- 11.11.136: Argon crystallizes in the face-centered cubic arrangement at 40 K. ...
- 11.11.137: A chemistry instructor performed the following mystery demonstratio...
- 11.11.138: Given the phase diagram of carbon shown, answer the following quest...
- 11.11.139: Swimming coaches sometimes suggest that a drop of alcohol (ethanol)...
- 11.11.14c: Use the concept of intermolecular forces to explain why the far end...
- 11.11.141: Why do citrus growers spray their trees with water to protect them ...
- 11.11.142: What is the origin of dark spots on the inner glass walls of an old...
- 11.11.143: The compound dichlorodifluoromethane (CCl2F2) has a normal boiling ...
- 11.11.144: A student heated a beaker of cold water (on a tripod) with a Bunsen...
- 11.11.145: Sketch the cooling curves of water from about 110C to about 210C. H...
- 11.11.146: Iron crystallizes in a body-centered cubic lattice. The cell length...
- 11.11.147: The boiling point of methanol is 65.0C and the standard enthalpy of...
- 11.11.148: An alkali metal in the form of a cube of edge length 0.171 cm is va...
- 11.11.149: A closed vessel of volume 9.6 L contains 2.0 g of water. Calculate ...
- 11.11.15c: A sample of water shows the following behavior as it is heated at a...
- 11.11.151: The electrical conductance of copper metal decreases with temperatu...
- 11.11.152: Assuming ideal behavior, calculate the density of gaseous HF at its...
- 11.11.153: Both calcium and strontium crystallize in face-centered cubic unit ...
- 11.11.154: Is the vapor pressure of a liquid more sensitive to changes in temp...
- 11.11.155: Estimate the molar heat of vaporization of a liquid whose vapor pre...
- 11.11.156: On a summer day the temperature and (relative) humidity were 95F an...
- 11.11.157: Without the aid of instruments, give two examples of evidence that ...
Solutions for Chapter 11: Intermolecular Forces and Liquids and Solids
Full solutions for Chemistry | 12th Edition
ISBN: 9780078021510
Chapter 11: Intermolecular Forces and Liquids and Solids includes 157 full step-by-step solutions. Since 157 problems in chapter 11: Intermolecular Forces and Liquids and Solids have been answered, more than 235530 students have viewed full step-by-step solutions from this chapter. This expansive textbook survival guide covers the following chapters and their solutions. Chemistry was written by and is associated to the ISBN: 9780078021510. This textbook survival guide was created for the textbook: Chemistry, edition: 12.
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actinide series.
Elements that have incompletely filled 5f subshells or readily give rise to cations that have incompletely filled 5f subshells. (7.9)
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Allylic carbocation
A carbocation in which an allylic carbon bears the positive charge.
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battery.
A galvanic cell, or a series of combined galvanic cells, that can be used as a source of direct electric current at a constant voltage. (18.6)
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bimolecular reaction
An elementary reaction that involves two molecules. (Section 14.6)
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chemical kinetics.
The area of chemistry concerned with the speeds, or rates, at which chemical reactions occur. (13.1)
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Conjugate addition
Addition of a nucleophile to the b-carbon of an a,b-unsaturated carbonyl compound. (Section 20.2A) Addition to carbons 1 and 4 of a conjugated diene.
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cycloalkane
An alkane whose structure contains a ring.
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Diamagnetic current in NMR
The circulation of electron density in a molecule in an applied magnetic fi eld.
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diatomic molecule.
A molecule that consists of two atoms. (2.5)
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endo
In Diels-Alder reactions that produce bicyclic structures, the positions that are syn to the larger bridge.
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Fischer esterifi cation
The process of forming an ester by refl uxing a carboxylic acid and an alcohol in the presence of an acid catalyst, commonly H2SO4, ArSO3H, or HCl
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gas constant (R)
The constant of proportionality in the ideal-gas equation. (Section 10.4)
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ketose
A carbohydrate that contains a ketone group.
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molal boiling-point-elevation constant (Kb)
A constant characteristic of a particular solvent that gives the increase in boiling point as a function of solution molality: ?Tb = Kbm. (Section 13.5)
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n+1 rule
In NMR spectroscopy, if n is the number of neighboring protons, then the multiplicity will be n+1.
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natural gas
A naturally occurring mixture of gaseous hydrocarbon compounds composed of hydrogen and carbon. (Section 5.8)
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Nucleic acid
A biopolymer containing three types of monomer units: heterocyclic aromatic amine bases derived from purine and pyrimidine, the monosaccharides d-ribose or 2-deoxy-d-ribose, and phosphoric acid
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particle accelerator
A device that uses strong magnetic and electrostatic fields to accelerate charged particles. (Section 21.3)
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saponification
Hydrolysis of an ester in the presence of a base. (Section 24.4)
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specific rotation
For a chiral compound that is subjected to plane-polarized light, the observed rotation when a standard concentration (1 g/mL) and a standard path length (1 dm) are used.