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General Chemistry Principles And Modern Applications 11th Edition Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette - Solutions

The melting points of NaF, NaCl, NaBr, and NaI are 988, 801, 755, and 651 °C, respectively. Are these data consistent with ideas developed? Explain.
Are the fullerenes network covalent solids? What makes them different from diamond and graphite? It has been shown that carbon can form chains in which every other carbon atom is bonded to the next carbon atom by a triple bond. Is this allotrope of carbon a network covalent solid? Explain.
Use Coulomb’s law to verify the conclusion concerning the relative strengths of the attractive forces in the ion pairs Na+Cl- and Mg2+O2- presented in Figure 12-36.Figure 12-36 Attractive force Radius sum= distance between center of ions: Radius: Nat 280 pm CI Na+ = 99 pm CF = 181 pm Attractive
Will the mineral villaumite (NaF) or periclase (MgO) have a higher Mohs hardness value (see Exercise 67)?Exercise 67The hardness of crystals is rated based on Mohs hardness values. The higher the Mohs value, the harder the material is to scratch. Which crystal will have the highest Mohs value: NaF,
The hardness of crystals is rated based on Mohs hardness values. The higher the Mohs value, the harder the material is to scratch. Which crystal will have the highest Mohs value: NaF, NaCl, or KCl?
Explain why there are two arrangements for the closest packing of spheres rather than a single one.
Argon, copper, sodium chloride, and carbon dioxide all crystallize in the fcc structure. How can this be when their physical properties are so different?
Stacking spheres always leaves open space. Consider the corresponding situation in two dimensions: Squares can be arranged to cover all the area, but circles cannot. For the arrangement of circles pictured here, what percentage of the area remains uncovered?
Magnesium crystallizes in the hcp arrangement shown in Figure 12-41. The dimensions of the unit cell are height, 520 pm; length on an edge, 320 pm. Calculate the density of Mg(s), and compare with the measured value of 1.738 g/cm3.Figure 12-41 60° (a) (b) 120°
Tungsten has a body-centered cubic crystal structure. Using a metallic radius of 139 pm for the W atom, calculate the density of tungsten.
Polonium (Po) is the only element known to take on the simple cubic crystal system. The distance between nearest neighbor Po atoms in this structure is 335 pm.(a) What is the diameter of a Po atom?(b) What is the density of Po metal?(c) At what angle (in degrees) to the parallel faces of the Po
Show that the unit cells for CaF2 and TiO2 in Figure 12-50 are consistent with their formulas.Figure 12-50 = Zn²+ (a) Unit cell of ZnS, the zinc blende structure = $²- = Ti4+ = Ca²+ = 0²- (c) Unit cell of TiO2, the rutile structure =F- (b) Unit cell of CaF2, the fluorite structure
Germanium has a cubic unit cell with a side edge of 565 pm. The density of germanium is 5.36 g/cm3. What is the crystal system adopted by germanium?
The crystal structure of magnesium oxide, MgO, is of the NaCl type (Fig. 12-48). Use this fact, together with ionic radii from Figure 9-11, to establish the following.(a) The coordination numbers of Mg2+ and O2-;(b) The number of formula units in the unit cell;(c) The length and volume of a unit
Silicon tetrafluoride molecules are arranged in a body-centered cubic unit cell. How many silicon atoms are in the unit cell?
Two views, a top and side view, for the unit cell for rutile (TiO2) are shown here. (a) How many titanium atoms (blue) are in this unit cell? (b) How many oxygen atoms (red) are in this unit cell?
Use data from Figure 9-11 to predict the type of cubic unit cell adopted by (a) CaO; (b) CuCl; (c) LiO2 (the radius of the O2- ion is 128 pm).Figure 9-11 155 59 Li+ Be²+ 102 K Na Mg 190 160 Na Mg2+ 235 Be 112 138 27 152 72 K+ Ca²+ Sc³+ Ca Sc Ti 197 162 147 100 Rb 248 215 Rb
Use data from Figure 9-9 to predict the type of cubic unit cell adopted by (a) BaO; (b) CuI; (c) LiS2.(The radii of Ba2+ and S2- ions are 135 and 198 pm, respectively.)Figure 9-9 Tne/ao 9 8 7 6 5 Li 3 2 1 He Na Ne K Ar 20 Rb Kr Csa Xe 40 60 Atomic number 80 Rn 100
Potassium chloride has the same crystal structure as NaCl. Careful measurement of the internuclear distance between K+ and Cl- ions gave a value of 314.54 pm. The density of KCl is 1.9893 g/cm3. Use these data to evaluate the Avogadro constant, NA.
Without doing calculations, indicate how you would expect the lattice energies of LiCl(s), KCl(s), RbCl(s), and CsCl(s) to compare with the value of -787 kJ mol-1 determined for NaCl(s).
In ionic compounds with certain metals, hydrogen exists as the hydride ion, H-. Determine the electron affinity of hydrogen; that is, ΔrH for the process H(g) + e- : H-(g). The bond energy of H2(g) from Table 10.3; -812 kJ mol-1 for the lattice energy of NaH(s); and -57 kJ mol-1 NaH for the
Determine the lattice energy of KF(s) from the following data: ΔfH°[KF(s)] = -567.3 kJ mol-1; enthalpy of sublimation of K(s), 89.24 kJ mol-1; enthalpy of dissociation of F2(g), 159 kJ mol-1 F2; Ei for K(g), 418.9 kJ mol-1; Eea for F(g), -328kJ mol-1.
Refer to Example 12-12. Together with data given there, use the data here to calculate ΔfH° for 1 mol MgCl2(s). Explain why you would expect MgCl2 to be a much more stable compound than MgCl. (The second ionization energy of Mg is 1451 kJ mol-1; the lattice energy of MgCl2(s) is -2526 kJ mol-1
The normal boiling point of water is 100.00 °C and the enthalpy of vaporization at this temperature is ΔvapH = 40.657 kJ mol-1. What would be the boiling point of water if it were based on a pressure of 1 bar instead of the standard atm?
When a wax candle is burned, the fuel consists of gaseous hydrocarbons appearing at the end of the candle wick. Describe the phase changes and processes by which the solid wax is ultimately consumed.
Estimate how much heat is absorbed when 1.00 g of Instant Car Kooler vaporizes. Comment on the effectiveness of this spray in cooling the interior of a car. Assume the spray is 10% C2H5OH(aq) by mass, the temperature is 55 °C, the heat capacity of air is 29 J mol-1 K-1, and use ΔvapH data from
A supplier of cylinder gases warns customers to determine how much gas remains in a cylinder by weighing the cylinder and comparing this mass to the original mass of the full cylinder. In particular, the customer is told not to try to estimate the mass of gas available from the measured gas
To vaporize 1.000 g water at 20 °C requires 2447 J of heat. At 100 °C, 10.00kJ of heat will convert 4.430 g H2O(l) to H2O(g). Do these observations conform to your expectations? Explain.
A 1.05 mol sample of H2O(g) is compressed into a 2.61 L flask at 30.0 °C. Describe the point(s) in Figure 12-30 representing the final condition.Figure 12-30 Pressure (not to scale) 1 atm Ice II Ice I Ice V Ice III/ D P Ice VII Ice VI Liquid water Gaseous water Temperature (not to scale) C --R
Because solid p-dichlorobenzene, C6H4Cl2 sublimes rather easily, it has been used as a moth repellent. From the data given, estimate the sublimation pressure of C6H4Cl2(s) at 25 °C For C6H4Cl2; mp = 53.1°C; vapor pressure of C6H4Cl2(l) at 54.8 °C is 10.0 mmHg; ΔfusH = 17.88 kJ mol-1 ; ΔvapH =
By the method used to graph Figure 12-20, plot ln P versus 1/T for liquid white phosphorus, and estimate (a) Its normal boiling point and (b) Its enthalpy of vaporization, ΔvapH, in kJ mol-1. Vapor pressure data: 76.6 °C, 1 mmHg; 128.0 °C, 10 mmHg; 166.7 °C, 40 mmHg; 197.3 °C, 100 mmHg;
One handbook lists the sublimation pressure of solid benzene as a function of Kelvin temperature, T, as log P (mmHg) = 9.846 - 2309/T. Another handbook lists the vapor pressure of liquid benzene as a function of Celsius temperature, t, as log P (mmHg) = 6.90565 - 1211.033/(220.790 + t). Use these
Assume that a skater has a mass of 80 kg and that his skates make contact with 2.5 cm2 of ice. (a) Calculate the pressure in atm exerted by the skates on the ice.(b) If the melting point of ice decreases by 1.0 °C for every 125 atm of pressure, what would be the melting point of the ice under the
Inspection of the straight-line graphs in Figure 12-20 suggests that the graphs for benzene and water intersect at a point that falls off the page. At this point, the two liquids have the same vapor pressure. Estimate the temperature and the vapor pressure at this point by a calculation based on
Estimate the boiling point of water in Leadville, Colorado, elevation 3170 m. To do this, use the barometric formula relating pressure and altitude: P = P0 x 10-Mgh/2.303 RT (where P = pressure in atm; P0 = 1 atm; acceleration due to gravity, g = 9.81 m s-2; molar mass of air, M = 0.02896 kg mol-1
A cylinder containing 151 lb Cl2 has an inside diameter of 10 in. and a height of 45 in. The gas pressure is 100 psi (1 atm = 14.7 psi) at 20 °C. Cl2 melts at -103 °C, boils at -35 °C, and has its critical point at 144 °C and 76 atm. In what state(s) of matter does the Cl2 exist in the cylinder?
At room temperature, iron crystallizes in a bcc structure. By X-ray diffraction, the edge of the cubic cell corresponding to Figure 12-45 is found to be 287 pm. What is the radius of an iron atom?Figure 12-45 13 1 = 287 pm W21 YB 1 = 287 pm IN2
Water molecules will form small, stable clusters. Draw one possible water cluster by using six water molecules and maximizing the number of hydrogen bonds for each water molecule.
(A) Use the result of Practice Example 12-9A, the molar mass of K, and the Avogadro constant to calculate the density of potassium.(B) Use the result of Practice Example 12-9B, the molar mass of Al, and its density (2.6984 g cm-3) to evaluate the Avogadro constant, NA.Example 12-9A(A) Potassium
Use data from Example 12-9, together with the molar mass of Fe and the Avogadro constant, to calculate the density of iron.Example 12-9At room temperature, iron crystallizes in a bcc structure. By X-ray diffraction, the edge of the cubic cell corresponding to Figure 12-45 is found to be 287 pm.
The ionic radii of Na+ and Cl- in NaCl are 99 and 181 pm, respectively. What is the edge length of the unit cell?
Silicone oils, such as H3C[SiO(CH3)2]n Si(CH3), are used in water repellents for treating tents, hiking boots, and similar items. Explain how silicone oils function.
(A) The ionic radius of Cs+ is 167 pm. Use Figure 12-49 and information in Examples 12-9 and 12-11 to determine the edge length of the unit cell of CsCl.(B) Use the length of the unit cell of NaCl obtained in Example 12-11, together with the molar mass of NaCl and the Avogadro constant, to estimate
With the following data, calculate ΔfH° of MgCl(s): Enthalpy of sublimation of Mg(s): +146 kJ mol-1; enthalpy of dissociation of Cl2(g): +244 kJ mol-1 ; first ionization energy of Mg(g): +738 kJ mol-1; electron affinity of Cl(g): -349 kJ mol-1; lattice energy of MgCl(s): -676 kJ mol-1.
Surface tension, viscosity, and vapor pressure are all related to intermolecular forces. Why do surface tension and viscosity decrease with temperature, whereas vapor pressure increases with temperature?
(A) The enthalpy of sublimation of cesium is 78.2 kJ mol-1, and ΔfH°[CsCl(s)] = -442.8 kJ mol-1. Use these values, together with other data from the text, to calculate the lattice energy of CsCl(s).(B) Given the following data, together with data included in Example 12-12, calculate ΔfH° of
Is there any scientific basis for the colloquial expression “slower than molasses in January”? Explain.
In acetic acid vapor, some molecules exist as monomers and some as dimers (see Figure 12-9). If the density of the vapor at 350 K and 1 atm is 3.23 g/L, what percentage of the molecules must exist as dimers? Would you expect this percent to increase or decrease with temperature?Figure 12-9
A 685 mL sample of Hg(l) at 20 °C is added to a large quantity of liquid N2 kept at its boiling point in a thermally insulated container. What mass of N2(l) is vaporized as the Hg is brought to the temperature of the liquid N2? For the specific heat of Hg(l) from 20 to -39 °C use 0.138 J g-1
Sketched here are two hypothetical phase diagrams for a substance, but neither of these diagrams is possible. Indicate what is wrong with each of them. P Solid Liquid T Vapor P Solid Liquid T Vapor
A chemistry handbook lists the following equation for the vapor pressure of NH3(l) as a function of temperature. What is the normal boiling point of NH3(l)? log10 P(mmHg) = 9.95028 0.003863T 1473.17 T
The triple point temperature of bismuth is 544.5 K and the normal boiling point is 1832 K. Imagine that a 1.00 mol sample of bismuth is heated at a constant rate of 1.00 kJ min-1 in an apparatus in which the sample is maintained under a constant pressure of 1 atm. In the manner shown in Figure
The crystal structure of lithium sulfide (Li2S), is pictured here. The length of the unit cell is 5.88 x 102 pm. For this structure, determine(a) The coordination numbers of Li+ and S2-;(b) The number of formula units in the unit cell;(c) The density of Li2S. = S²- = Lit
Refer to Figure 12-44 and Figure 12-48. Suppose that the two planes of ions pictured in Figure 12-44 correspond to the top and middle planes of ions in the NaCl unit cell in Figure 12-48. If the X-rays used have a wavelength of 154.1 pm, at what angle θ would the diffracted beam have its greatest
Use the analyses of a bcc structure and the fcc structure in Exercise 146 to determine the percent voids in the packing-of-spheres arrangement found in the fcc crystal structure.Exercise 146The fcc unit cell is a cube with atoms at each of the corners and in the center of each face, as shown here.
One way to describe ionic crystal structures is in terms of cations filling voids among closely packed anions. Show that in order for cations to fill the tetrahedral voids in a close packed arrangement of anions, the radius ratio of cation, rc, to anion, ra, must fall between the following limits
Use the unit cell of diamond in Figure 12-32(b) and a carbon-to-carbon bond length of 154.45 pm, together with other relevant data from the text, to calculate the density of diamond.Figure 12-32(b) (b)
The enthalpy of formation of NaI(s) is -288 kJ mol-1. Use this value, together with other data in the text, to calculate the lattice energy of NaI(s).
Show that the formation of NaCl2(s) is very unfavorable; that is, ΔfH°[NaCl2(s)] is a large positive quantity. Assume that the lattice energy for NaCl2 would be about the same as that of MgCl2, -2.5 x 103 kJ mol-1.
A crystalline solid contains three types of ions, Na+, O2-, and Cl-. The solid is made up of cubic unit cells that have O2- ions at each corner, Na+ ions at the center of each face, and Cl- ions at the center of the cells. What is the chemical formula of the compound? What are the coordination
A certain mineral has a cubic unit cell with calcium at each corner, oxygen at the center of each face, and titanium at its body center. What is the formula of the mineral? An alternate way of drawing the unit cell has calcium at the center of each cubic unit cell. What are the positions of
Calculate the radius ratio (r+/r-) for CaF2. Suggest an alternative structure to that shown in Figure 12-50(b) that better conforms to the radius ratio you compute.Figure 12-50(b) = Ca²+ =F-
In some barbecue grills the electric lighter consists of a small hammer-like device striking a small crystal, which generates voltage and causes a spark between wires that are attached to opposite surfaces of the crystal. The phenomenon of causing an electric potential through mechanical stress is
Intermolecular forces play vital and varied roles in nature. For example, these forces enable gecko lizards to climb walls and hang upside down from ceilings, seemingly defying gravity. Intermolecular forces—more specifically, hydrogen bonds—are the reason that DNA molecules, carriers of the
In an ionic crystal lattice each cation will be attracted by anions next to it and repulsed by cations near it. Consequently the coulomb potential leading to the lattice energy depends on the type of crystal. To get the total lattice energy you must sum all of the electrostatic interactions on a
Plot the following data first as boiling point versus polarizability, and then as boiling point versus molecular mass. What conclusions can you draw from these plots? Compound H₂ N₂ Cl₂ HF HCI HBr HI N₂O CO SO₂ H₂S CS₂ NH3 HCN CH4 C₂H6 Polarizability, 10-25
In a 1999 study of cobalt nanocrystals, D. P. Dinega and M. G. Bawendi discovered that cobalt forms an interesting cubic structure unlike any of the cubic structures described in this chapter. They called this new form -cobalt to distinguish it from the more commonly encountered hcp and fcc forms
We have learned that the enthalpy of vaporization of a liquid is generally a function of temperature. If we wish to take this temperature variation into account, we cannot use the Clausius–Clapeyron equation in the form given in the text (that is, equation 12.2). Instead, we must go back to the
In a capillary rise experiment, the height (h) to which a liquid rises depends on the density (d) and surface tension (ɣ) of the liquid and the radius of the capillary (r). The equation relating these quantities and the acceleration due to gravity (g) is h = 2ɣ/dgr. The sketch provides data
The Born–Fajans–Haber cycle uses thermodynamic cycles to determine lattice energy. An alternative to the Born–Fajans–Haber method is one based on fundamental principles. Because the dominant interactions in an ionic crystal are Coulomb interactions, we can use the theory of electrostatics
Explain the important distinctions between each pair of terms: (a) Adhesive and cohesive forces;(b) Vaporization and condensation; c) Triple point and critical point; (d) Face-centered and body-centered cubic unit cell; (e) Tetrahedral and octahedral hole.
In your own words, define or explain the following terms or symbols: (a) ΔvapH;(b) Tc;(c) Instantaneous dipole; (d) Coordination number; (e) Unit cell.
Briefly describe each of the following phenomena or methods: (a) Capillary action; (b) Polymorphism;(c) Sublimation; (d) Supercooling; (e) Determining the freezing point of a liquid from a cooling curve.
The magnitude of one of the following properties must always increase with temperature; that one is (a) Surface tension; (b) Density; (c) Vapor pressure; (d) ΔvapH.
A metal that crystallizes in the body-centered cubic (bcc) structure has a crystal coordination number of (a) 6; (b) 8; (c) 12; (d) Any even number between 4 and 12.
Which of the following liquid properties depends on the strength of intermolecular attractions? (a) Surface tension; (b) Boiling point; (c) Vapor pressure; (d) Heat of vaporization; (e) All of these.
A liquid is in equilibrium with its vapor in a closed container. The lid of the container is removed briefly, allowing some of the vapor to escape, and then replaced. What is the immediate result of the vapor escaping? (a) Vaporization rate decreases; (b) Condensation rate decreases;(c)
A unit cell of an ionic crystal (a) Shares some ions with other unit cells; (b) Is the same as the formula unit; (c) Is any portion of the crystal that has a cubic shape; (d) Must contain the same number of cations and anions.
In the responses below, the vapor pressure of trichloroethene is listed for a given temperature. In which response does the given temperature correspond to the normal boiling point? (a) 40 Torr at 40.1 °C; (b) 100 Torr at 61.3 °C; (c) 400 Torr at 100.0 °C;(d) 760 Torr at 120.8 °C; (e) None
The normal boiling point of acetone is 56.2 °C, and the molar heat of vaporization is 32.0 kJ mol–1. What is the boiling temperature of acetone under a pressure of 50.0 mmHg?
Arrange the following substances in the expected order of increasing melting point: KI, Ne, K2SO4, C3H8, CH3CH2OH,MgO, CH2OHCHOHCH2OH.
If the triple point pressure of a substance is greater than 1 atm, which two of the following conclusions are valid?(a) The solid and liquid states of the substance cannot coexist at equilibrium.(b) The melting point and boiling point of the substance are identical.(c) The liquid state of the
In each of the following pairs, which would you expect to have the higher boiling point? (a) C7H16 or C10H22(b) C3H8 or (CH3)2O; (c) CH3CH2SH or CH3CH2OH.
The fcc unit cell is a cube with atoms at each of the corners and in the center of each face, as shown here. Copper has the fcc crystal structure. Assume an atomic radius of 128 pm for a Cu atom.(a) What is the length of the unit cell of Cu?(b) What is the volume of the unit cell?(c) How many atoms
The following data are given for CCl4. Normal melting point, -23 °C; normal boiling point, 77 °C; density of liquid 1.59 g/mL; ΔfusH = 3.28 kJ mol-1; vapor pressure at 25 °C, 110 Torr.(a) What phases—solid, liquid, and/or gas—are present if 3.50 g CCl4 is placed in a closed 8.21 L container
One of the substances is out of order in the following list based on increasing boiling point. Identify it, and put it in its proper place: N2, O3, F2, Ar, Cl2. Explain your reasoning.
Is it possible to obtain a sample of ice from liquid water without ever putting the water in a freezer or other enclosure at a temperature below 0 °C? If so, how might this be done?
Of the following liquids at 20 °C, which has the smallest surface tension? (a) CH3OH;(b) CH3CH2OH;(c) CH3CH2CH2OH;(d) CH3CH2CH2CH2OH.
Of the following liquids at 20 °C, which has the smallest viscosity? (a) Dodecane, C12H26; (b) n-nonane, C9H20;(c) n-heptane, C7H16; (d) n-pentane, C5H12.
Consider the following ions: Na+, K+, Ca2+, Mg2+, F–, Br–, O2–, and S2–. Which cation and which anion do you expect to combine to form the highest melting compound? Carefully explain your choice.
Would you expect an ionic solid or a network covalent solid to have the higher melting point?
In the lithium iodide crystal, the Li–I distance is 3.02 Å. Calculate the iodide radius, assuming that the iodide ions are in contact.
Which of the following phase transitions is most likely to occur when the pressure on a metallic solid increases? (a) bcc to sc; (b) fcc to sc; (c) bcc to fcc;(d) fcc to sc.
Construct a concept map representing the different types of intermolecular forces and their origin.
Construct a concept map using the ideas of packing of spheres and the structure of metal and ionic crystals.
Construct a concept map showing the ideas contained in a phase diagram.
The ionization energies of Li, Be+, B2+, and C3+ are, respectively, 520, 1757, 3659, and 6221 kJ mol–1. The ionization energies Na, Mg+, Al2+, and Si3+ are (from Table 9.4) 495.8, 1451, 2745, and 4356 kJ mol–1. Plot a graph of the square roots of the ionization energies versus the nuclear
Elements 114–116 have recently been reported to be synthesized. Using data given below and the periodic law, fill in the missing data for these elements.The entries for each element are organized as follows: Sn 50 5s²5p²
The work functions for a number of metals are given in the following table. How do the work functions vary (a) Down a group?(b) Across a period?(c) Estimate the work function for potassium and compare it with a published value.(d) What periodic property is the work function most like?
The following are a few elements and their characteristic X-ray wavelengths:Use these data to determine the constants A and b in Moseley’s relationship. Compare your value of A with the value obtained from Bohr’s theory for the frequencies emitted by one-electron atoms. Suggest a reasonable

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