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chemistry principles and practice

Chemistry Principles And Practice 3rd Edition Daniel L. Reger, Scott R. Goode, David W. Ball - Solutions

Explain why the viscosity of a liquid may not be consistent with the enthalpy of vaporization and the boiling point as a measure of the strength of intermolecular forces.
Explain why the effect of hydrogen bonding on the boiling point is considerably greater for water than for ammonia and hydrogen fluoride.
For a typical substance, arrange the enthalpies of sublimation, fusion, and vaporization in order of increasing value.
Determine the number of sodium ions and chloride ions present in the face-centered cubic unit cell of sodium chloride.StrategyUse Figure 11.27 to count the atoms of each type. Remember that an atom in a corner contributes one eighth of an atom to that unit cell, an atom on a face contributes only
Use the data in Example 11.8 to calculate the atomic radius (in pm) of the molybdenum atom. In a body-centered cubic structure, the atoms along the cube diagonal are in contact, and the length of the cube diagonal isExample 11.8Molybdenum crystallizes in a body-centered cubic array of atoms. The
Cesium chloride crystallizes in a simple cubic array of Cs ions, with one Cl- at the center of the unit cell. How many ions of each type are present in the unit cell?
Nickel crystallizes in a face-centered cubic array of atoms, and the length of the unit cell edge is 351 pm . What is the radius of the nickel atom?StrategyOn one face of this cell there are five nickel atoms—one at each corner and one in the center of the face. Since we assume that each atom is
Trouton’s rule states that the enthalpy of vaporization for a substance divided by its normal boiling point on the Kelvin scale is approximately 88 J/K. Is this in agreement with the expected behavior of these properties as intermolecular forces change? Explain.
Molybdenum crystallizes in a body-centered cubic array of atoms. The edge of the unit cell is 0.314 nm long. Calculate the density of this metal.StrategyFirst, determine the net number of atoms per unit cell; then determine the mass using the atomic mass of molybdenum. Divide this mass by the
Copper crystallizes in a face-centered cubic array of atoms in which the edge of the unit cell is 0.362 nm. Calculate the density of copper.
A crystal is found to diffract 154 pm x rays at an angle of 19.3 degrees . Assuming that n = 1 in the Bragg equation, calculate the distance (in pm) between the layers of atoms that give rise to this diffraction.StrategyUse Equation 11.1 to solve for d.Equation 11.1 n = 2d sin 0
How does humidity affect the efficiency of cooling by perspiration? Explain.
Identify the intermolecular forces of attraction, and predict which substance of each pair has the stronger forces of attraction.StrategyAll of the molecules will have London dispersion forces. We must determine whether a molecule is polar to determine whether dipole-dipole forces exist. If a
Calculate the energy necessary to boil 100.0 g carbon disulfide, CS2, at its normal boiling point.StrategyDetermine the number of moles of carbon disulfide; then use the enthalpy of vaporization from Table 11.3 as a conversion factor to determine the energy needed.Table 11.3 TABLE 11.3 Boiling
Aspartame is a compound that is 200 times sweeter than sugar and is used extensively (under the trade name NutraSweet) in diet soft drinks. The skeleton structure of the atoms in aspartame is H-0. . H H C H HC HC T H_N-C-C-N-C-C-0-CH,
The molecular orbital diagram of NO shown in Figure 10.47 also applies to CO. Draw the complete molecular orbital diagram for CO. What is the C–O bond order?Figure 10.47 Energy Atomic orbitals 12p 111 -10 Natom Molecular orbitals 11 1L 1L 11 12p 02p 12p 02S 025 1L NO molecule Atomic orbitals 111
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron confi guration of each, indicating the bond order and the number of unpaired electrons.(a) LiBe+(b) CO+(c) CN-(d) OFFigure 10.47 Energy Atomic orbitals 12p 111 12s
Assuming that the molecular orbital diagram shown in Figure 10.40 is correct for heteronuclear diatomic molecules containing elements that are close to each other in the periodic table, write a homonuclear diatomic molecule and a heteronuclear diatomic molecule (remember that molecules are neutral)
Use the VSEPR model to predict the bond angles around each central atom in the following Lewis structures. Note that the drawings do not necessarily depict the bond angles correctly. (a) H :0: H | || | H-C-C-C-H H T H (b) H H-C-C=N: H
Use the VSEPR model to predict the shape of the following species.(a) BeF2(b) SF6(c) SiH4(d) FCN(e) BeF−3
Describe the bonding in molecular orbital terms for the delocalized bond in O3.
Draw two types of bonding molecular orbitals that can form from the overlap of 2p orbitals.
In the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of CO2 was dissolved in the lake at the time.(a) What volume of gas is this at standard temperature and pressure?(b) Assuming that this dissolved gas was in equilibrium with the normal partial pressure
Rank the following in order of increasing strength of intermolecular forces in the pure substances. Which are gases at 25 °C and 1 atm?(a) CH3CH2CH2CH3 (butane)(b) CH3OH (methanol)(c) He
At -30 °C, hydrogen sulfide (H2S) is a gas, hydrogen telluride (H2Te) is a liquid, and water (H2O) is a solid. Arrange these compounds in order of increasing strength of intermolecular attractions.
Sketch what you think an edge-centered cubic unit cell looks like. How many atoms are there per unit cell for this type of crystal?
An amorphous solid can sometimes be converted to a crystalline solid by a process called annealing. Annealing consists of heating the substance to a temperature just below the melting point of the crystalline form and then cooling it slowly. Explain why this process helps produce a crystalline
The compounds ethanol (C2H5OH) and dimethyl ether (CH3–O–CH3) have the same molecular formula. Which is expected to have the higher surface tension? Why?
How does an amorphous solid differ from a crystalline solid?
Explain why the surface of the HCl(aq) liquid in a buret is curved rather than flat.
Water forms beads on the surface of a newly painted car. After the car is exposed to the weather for a long time, water spreads out into a thin film on its surface. What has happened to the paint to cause this change? 000
The nitrosyl ion, NO+, has an interesting chemistry.(a) Is NO+ diamagnetic or paramagnetic? If paramagnetic, how many unpaired electrons does it have?(b) Assume the molecular orbital diagram for a homonuclear diatomic molecule applies to NO+. What is the highest-energy molecular orbital occupied
State how each of the following properties changes with increasing strength of intermolecular forces.(a) Enthalpy of fusion(b) Melting point(c) Surface tension(d) Viscosity(e) Enthalpy of vaporization(f) Boiling point
From the graph in Figure 11.11, is there any evidence that hydrogen bonding occurs for any elements other than nitrogen, oxygen, and fluorine? Explain.Figure 11.11 Boiling point (C) 100 -100 -200- HO HF NH3 CH4 HCI PH3 SiH4 HS 3 HSe AsHg. HBr. Period GeH4 H Te SbH3 HI 5 SnH4
Explain why high pressures are needed in the industrial process that makes diamond (d = 3.5 g/cm3) from graphite (d = 2.2 g/cm3).
Even when the atmospheric temperature is above normal body temperature, sweating is effective in cooling a person. Explain how this happens, since heat flows from a warmer object to a cooler one.
Each of two glasses contains 200 g of an ice-water mixture. In one glass, 10 g is ice, and in the other glass, 90 g is ice. Assuming both samples are at equilibrium, which is colder?
The enthalpy of vaporization of water (boiling point = 100 °C) is greater than that of diethyl ether (boiling point = 35 °C). Despite its smaller enthalpy of vaporization, liquid diethyl ether feels colder than water does when it evaporates from a person’s skin. Explain.
Phosgene, COCl2, is a highly toxic gas that was used in combat during World WarI. $3It is an important intermediate in the preparation of a number of organic compounds but must be handled with extreme care. Given that carbon is the central atom in phosgene, determine the Lewis structure, the
Histidine is an essential amino acid that the body uses to form proteins. The Lewis structure of histidine follows. What are the approximate values for bond angles 1 through 5 (indicated on the structure by blue numbers)? H :N C H-N: H H C. H C N: C. H H C4 :O: -H
Draw the molecular orbital diagrams for NO- and NO+. Compare the bond orders in these two ions.
Write one important resonance structure for each of the following species, and use the VSEPR model to predict the bond angles around each central atom. Also indicate the hybrid orbitals on each central atom and whether the molecule is polar or nonpolar. (a) H H N-N O (b) H-N-N-N
Write all important resonance structures for each of the following species, and use the VSEPR model to determine the bond angles around each central atom. Also indicate the hybrid orbitals on each central atom. Does each resonance structure use the same hybrid orbitals? (a) [0- C-N] (b) 0 _O-N-O_
Vitamin A is converted by the body to retinal, a compound that is critical to human sight. The skeleton structure of vitamin A follows. Write the Lewis structure. How many sp2 and sp3 hybridized carbon atoms are in vitamin A? H-C H-C, AR CH, CH, -CH3 CH3 CH, | H . T -0-H
A compound is analyzed and found to contain 54.53% carbon, 9.15% hydrogen, and 36.32% oxygen by mass. A mass spectrometry experiment shows that the molar mass is 44 g/mol. What is the molecular formula? There are two reasonable ways to draw noncyclic skeleton structures of this molecule. Draw the
At room temperature, chlorine is a gas, bromine is a liquid, and iodine is a solid. Arrange these substances in order of increasing strength of intermolecular attractions.StrategyThe lower the intermolecular attractions between molecules, the more likely a substance will exist as a liquid or, in
Why does water have a lower vapor pressure at 25 °C than dimethyl ether (CH3OCH3)? Which of these two liquids has the greater enthalpy of vaporization?
Why does a perspiring body achieve greater cooling when the wind is blowing than in calm air?
Using the phase diagram in Example 11.4, sketch the heating curves expected at pressures of(a) 1 atm and(b) 0.2 atm.StrategyFollow the proper horizontal line in the phase diagram to determine what phases occur as heat is added to the sample.Example 11.4Using the phase diagram to the left,
Identify the intermolecular forces and their relative strengths in SF4 and SeF4.
“A liquid stops evaporating when the equilibrium vapor pressure is reached.” What is wrong with this statement?
What phase or phases are present in equilibrium at points B, D, and F on the phase diagram?
Using the phase diagram to the left, identify the phase or phases present at each of the lettered points A, C, and E.StrategyDetermine which phase exists in each region of the phase diagram. If a point falls on a line between two phases, both of those phases exist in equilibrium. If a point lies at
The accompanying graph shows the heating curves for one mole each of substances A and B, at one atmosphere pressure.(a) Give the melting and boiling points for each substance.(b) Which substance has the greater enthalpy of vaporization?(c) Which substance has a greater molar heat capacity in the
For most substances, the liquid state is less dense than the solid state. How does density affect the energy of the intermolecular attractions?
What is the enthalpy change when 75.0 g carbon dioxide condenses at its boiling point?
For any particular substance, the types of intermolecular forces in the solid, liquid, and gas phases are the same. What determines which of these phases is stable at a given temperature?
Hydrogen sulfide, H2S, is a gas at room temperature, and water is a liquid. Which compound has the stronger intermolecular attractions?
The density of liquid sulfur dioxide is 1.43 g/mL, and that of the gas is 0.00293 g/mL at standard temperature and pressure. Account for the large diff erence between these two densities.
The compound cubane, C8H8, has an unusual structure with each carbon atom at the corner of a cube, bonded to three other carbon atoms, and a single hydrogen atom is bonded to each carbon.(a) Draw the Lewis structure of cubane, and indicate the hybridization of the carbon atoms.(b) Given the
A 1.30-g sample of C2H2 reacts with exactly 1.22 L H2 gas at 27 °C and 1.01 atm of pressure to yield a compound with the formula C2Hx. What is the value of x, and what are the orbitals on the carbon atoms that form the C–C bond(s)?
Recently, the compound CF3SF5 was discovered in the atmosphere and identified as a potential greenhouse gas. Assume the carbon and sulfur atoms are both central atoms, and draw the Lewis structure for this compound. What is the hybridization of each central atom and the bond angles with the
Two compounds have the formula S2F2. Disulfur difluoride has the skeleton structure F–S–S–F, whereas thiothionyl fluoride has the skeletal structureDetermine Lewis structures for each compound. S-S F F
The reaction of sulfur, S8, with fluorine, F2, yields a product with the general formula SFx. If 4.01 g S8 reacts with 4.76 g F2 to yield only SFx, what is the value of x? Draw the Lewis structure of this compound, indicating the F–S–F bond angles and the hybrid orbitals on sulfur.
The reaction of calcium carbide with water is used to generate acetylene: CaC2 + 2H2O → H–CC–H + Ca(OH)2. Calcium carbide, CaC2, contains the carbide ion, C2−2 . Sketch the molecular orbital energy level diagram for the ion. How many π and bonds does the ion have? What is the
More than 5 billion pounds of ethylene oxide, C2H4O, is produced annually. Ethylene oxide is used in the production of ethylene glycol, HOCH2CH2OH, the main component of antifreeze, and acrylonitrile, CH2CHCN, used in the production of synthetic fibers and other chemicals. Ethylene oxide has an
Write all important resonance structures for each of the following species, and use the VSEPR model to predict the bond angles around each central atom. Also indicate the hybrid orbitals on each central atom and whether the molecule is polar or nonpolar. Does each resonance structure use the same
Ionization energies can be determined for molecules and atoms. Draw the molecular orbital diagrams for NO and CO, and predict which compound has the lower ionization energy.
Formamide, HC(O)NH2, is prepared at high pressures from carbon monoxide and ammonia, and serves as an industrial solvent (the parentheses around the O indicate that it is bonded only to the carbon atom and that the carbon atom is also bonded to the H and the N atoms). Two resonance forms (one with
Calcium cyanamide, CaNCN, is used both to kill weeds and as a fertilizer. Give the Lewis structure of the NCN2- ion and the bonded-atom lone-pair arrangement and hybridization of the carbon atom. H H H-N: H H N: H H O-H C4 H:0:
Recently, the structure of an amine compound, NR3 (R = large organic group), has been determined to have C–N–C bond angles of 119.2 degrees. It is believed that the bond angles of about 109 degrees expected from the VSEPR model are not observed because of the large substituents bonded to the
Aspirin, or acetylsalicylic acid, has the formula C9H8O4 and the skeleton structure . H C-O-H 0 TT 0-C-C-H
The ions ClF-2 and ClF+2 have both been observed. Use the VSEPR model to predict the F–Cl–F bond angle in each.
Following are the structures of three isomers of difluoro benzene, C6H4F2. Are any of them nonpolar? H H F H H H H F H H H F F H H
Write one Lewis structure of N2O5 (O2NONO2 skeleton structure). What are the bond angles around the central oxygen atom and the two nitrogen atoms? What is the hybridization of each?
The delocalized bonding that describes O3 also applies to NO−2. Draw the delocalized molecular orbital for NO−2.
The molecular orbital diagram of NO shown in Figure 10.47 also applies to OF-. Draw the complete molecular orbital diagram for OF-. What is the OF bond order?Figure 10.47 Energy Atomic orbitals 12p 111 12s Natom Molecular orbitals 11 1L 1L 11 p 02p 2p 02S 025 11 NO molecule Atomic orbitals 111
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly. (a) (b) IT H=C=C= H IT H-C-0-C-C-H (c) F - Xe-F
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly. (a) H T H-C-S H H (b) H-N-N-H
Indicate which of the following molecules are polar. Draw the molecular structure of each polar molecule, including the arrows that indicate the bond dipoles and the molecular dipole moment.(a) NF3 (b) CBr4 (c) BeI2
Identify the set of hybrid orbitals of a central atom that forms bonds with the following angles.(a) 120 degrees(b) 90 degrees(c) 180 degrees
Identify the hybridization of the central atom that has the bonded-atom lone-pair arrangement of(a) A tetrahedron.(b) A trigonal bipyramid.(c) An octahedron.
Identify two homonuclear diatomic molecules or ions with each of the following molecular orbital electron configurations. Are these species stable? (a) (02)(02)(2)(02) (b) (02)(0)(12)4 (c) (0)(0)
Identify two homonuclear diatomic molecules or ions with each of the following molecular orbital electron configurations. Are these species stable? (a) (0)(0)(2)(2p) (p) (0)(o)(2) 4 (02) (c) (0)(0) (b)
Use the molecular orbital diagram in Figure 10.40 to predict which species in each pair has the stronger bond.(a) F2 or F−2 (b) O−2 or O+2 (c) C2+2 or C2Figure 10.40 Energy Atomic orbitals 12p 2s Molecular orbitals + Tp 02p 2p 02s Atomic orbitals 12p
Use the molecular orbital diagram in Figure 10.40 to predict which species in each pair has the stronger bond.(a) B2 or B−2 (b) C−2 or C+2(c) O2+2 or O2Figure 10.40 Energy Atomic orbitals 12p 2s Molecular orbitals + Tp 02p 2p 02s Atomic orbitals 12p
Which species, O2 or O−2, has the higher bond order? Explain your answer.
Which species, N2 or N−2, has the higher bond order? Explain your answer.
Draw the molecular orbital diagram, including the electrons, and write the electron configuration of C2. Give the bond order and the number of unpaired electrons, if any. Is this a stable species?
Draw the molecular orbital diagram, including the electrons, and write the electron configuration of Li2. Give the bond order and the number of unpaired electrons, if any. Is this a stable species?
Draw the molecular orbital diagram, including the electrons, and write the electron configuration of H−2 . Give the bond order and the number of unpaired electrons, if any. Is this a stable species?
Draw the molecular orbital diagram, including the electrons, and write the electron configuration of He2+2 . Give the bond order and the number of unpaired electrons, if any. Is this a stable species?
Tetrafluoroethylene, C2F4, is used to produce Teflon. Draw the Lewis structure of tetrafluoroethylene, and indicate the hybridization of each carbon atom.
Orlon is produced from acrylonitrile, H2CCHCN. Draw the Lewis structure of acrylonitrile, and indicate the hybridization of each central atom.
Predict the hybridization at each central atom in the following molecules. (a) H :S: | || H-C-C-H I H (b) H H 1 H-C-0-C-H H H
Predict the hybridization at each central atom in the following molecules. (a) | H-C-N: | | (b) H H=C=C=C-H H
Two resonance structures can be written for NO−2. Indicate the hybridization on the central atom for each resonance form.
Three resonance structures can be written for N−3. Indicate the hybridization on the central atom for each resonance form.
Give the hybridization of each central atom in the following molecules.(a) CO2(b) H3CCCH(c) H3CC(O)H, which has the Lewis structure H :O: H-C-C-H H
Give the hybridization of each central atom in the following molecules.(a) Cyclohexene(b) Phosgene, Cl2CO (c) Glycine, H2NC(1)H2C(2)OOH H C. H-C || H-C, C C- - C-H H

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