[SOLVED] Ionic solids do not conduct electricity in

> Which of the substances in each of the following sets would be expected to have the highest boiling point? Explain why. a. Ga, KBr, O2 b. Hg, NaCl, He c. H2, O2, H2O

> Given the densities and conditions of ice, liquid water, and steam listed in Table 14.1, calculate the volume of 1.0 g of water under each of these circumstances. From table 14.1 Density (g/cm) State solid (0 °C, 1 atm) liquid (25 °C, 1 atm) gas (10

> For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor pressure f. intermolecular g. intramolecular h. io

> Sketch a heating/cooling curve for water, starting out at -20 °C and going up to 120 °C, applying heat to the sample at a constant rate. Mark on your sketch the portions of the curve that represent the melting of the solid and the boiling of the liquid.

> What is a dipole moment? Give four examples of molecules that possess dipole moments, and draw the direction of the dipole as shown in Section 12.3.

> For Exercises 51–60 choose one of the following terms to match the definition or description given. a. alloy b. specific heat c. crystalline solid d. dipole–dipole attraction e. equilibrium vapor pressure f. intermolecular g. intramolecular h. io

> The “Chemistry in Focus” segment Metal with a Memory discusses Nitinol, an alloy that “remembers” a shape originally impressed in it. Which elements comprise Nitinol, and why is it classified as an alloy?

> For each of the following sets of pressure/volume data, calculate the missing quantity. Assume that the temperature and the amount of gas remain constant. a. V = 53.2 mL at 785 mm Hg; V = ? mL at 700. mm Hg b. V = 2.25 L at 1.67 atm; V = 2.00 L at ? at

> How are the three states of matter similar, and how do they differ?

> What types of forces exist between the individual particles in an ionic solid? Are these forces relatively strong or relatively weak?

> The enthalpy (∆H) of vaporization of water is about seven times larger than water’s enthalpy of fusion (41 kJ/mol vs. 6 kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?

> What are crystalline solids? What kind of microscopic structure do such solids have? How is this microscopic structure reflected in the macroscopic appearance of such solids?

> Although water and ammonia differ in molar mass by only one unit, the boiling point of water is over 100 °C higher than that of ammonia. What forces in liquid water that do not exist in liquid ammonia could account for this observation?

> What is evaporation? What is condensation? Which of these processes is endothermic and which is exothermic?

> The heats of fusion of three substances are listed below. Explain the trend this list reflects. HI…………………2.87 kJ/mol HBr………………2.41 kJ/mol HCl………………1.99 kJ/mol

> Discuss the types of intermolecular forces acting in the liquid state of each of the following substances. a. Xe b. NH3 c. F2 d. ICl

> What type of intermolecular forces is active in the liquid state of each of the following substances? a. Ne b. CO c. CH3OH d. Cl2

> are relatively weak forces that exist among noble gas atoms and nonpolar molecules that involve an accidental dipole that induces a momentary dipole in a neighbor.

> Which bond in each of the following pairs has the greater ionic character? a. Na-F or Na-I b. Ca-S or Ca-O c. Li-Cl or Cs-Cl d. Mg-N or Mg-P

> The text implies that hydrogen bonding is a special case of very strong dipole–dipole interactions possible among only certain atoms. What atoms in addition to hydrogen are necessary for hydrogen bonding? How does the small size of the hydrogen atom cont

> Dipole–dipole forces become as the distance between the dipoles decreases (gets closer together).

> Liquids and solids are (more/less) compressible than are gases.

> Consider the iodine monochloride molecule, ICl. Because chlorine is more electronegative than iodine, this molecule is a dipole. How would you expect iodine monochloride molecules in the gaseous state to orient themselves with respect to each other as th

> It requires 113 J to melt 1.00 g of sodium metal at its normal melting point of 98 °C. Calculate the molar heat of fusion of sodium.

> The molar heats of fusion and vaporization for silver are 11.3 kJ/mol and 250. kJ/mol, respectively. Silver’s normal melting point is 962 °C, and its normal boiling point is 2212 °C. What quantity of heat is required to melt 12.5 g of silver at 962 °C? W

> The molar heat of fusion of aluminum metal is 10.79 kJ/mol, whereas its heat of vaporization is 293.4 kJ/mol. a. Why is the heat of fusion of aluminum so much smaller than the heat of vaporization? b. What quantity of heat would be required to vaporize

> The following data have been collected for substance X. Construct a heating curve for substance X. (The drawing does not need to be absolutely to scale, but it should clearly show relative differences.) normal melting point…………………………...-15 °C molar heat

> The energy required to melt 1 mole of a solid is called the .

> The forces that connect two hydrogen atoms to an oxygen atom in a water molecule are (intermo lecular/intramolecular), but the forces that hold water molecules close together in an ice cube are (intermolecular/intramolecular).

> On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. a. O-Cl or O-Br b. N-O or N-F c. P-S or P-O d. H-O or H-N From fig 12.3: 21 F Be 3.5 4.0 1.5 20 Ti V Cr Mn L6

> Gases have (higher/lower) densities than liquids or solids.

> Consider the following chemical equation: N2(g) + 3H2(g) ( 2NH3(g) What minimum total volume of reactant gases is needed to produce 4.00 g of ammonia if the volume of each gas is measured at 11 °C and 0.998 atm?

> A sample of helium gas occupies a volume of 25.2 mL at 95 °C and a pressure of 892 mm Hg. Calculate the volume of the gas at STP.

> What volume does a mixture of 14.2 g of He and 21.6 g of H2 occupy at 28 °C and 0.985 atm?

> Many transition metal salts are hydrates: they contain a fixed number of water molecules bound per formula unit of the salt. For example, copper(II) sulfate most commonly exists as the pentahydrate, CuSO4.5H2O. If 5.00 g of CuSO4.5H2O is heated strongly

> Make the indicated pressure conversions. a. 699 mm Hg to atmospheres b. 18.2 psi to mm Hg c. 862 mm Hg to torr d. 795 mm Hg to psi

> Consider the following reaction: C(s) + O2(g) CO2(g) What volume of oxygen gas at 25 °C and 1.02 atm would be required to react completely with 1.25 g of carbon?

> What is the molar volume of a gas? Do all gases that behave ideally have the same molar volume?

> The kinetic molecular theory of gases suggests that gas particles exert attractive or repulsive forces on each other.

> Collisions of the molecules in a sample of gas with the walls of the container are responsible for the gas’s observed .

> On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. a. H-F or H-Cl b. H-Cl or H-I c. H-Br or H-Cl d. H-I or H-Br From fig 12.3: 21 F Be 3.5 4.0 1.5 20 Ti V Cr Mn

> When is a scientific theory considered to be successful? Are all theories successful? Will a theory that has been successful in the past necessarily be successful in the future?

> What is a scientific law? What is a theory? How do these concepts differ? Does a law explain a theory, or does a theory attempt to explain a law?

> A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2O2, in the presence of a small amount of manganese catalyst by the reaction 2H2O2 (aq) 2H2O(g) + O2(g) The oxygen thus pr

> A sample of oxygen gas is saturated with water vapor at 27 °C. The total pressure of the mixture is 772 torr, and the vapor pressure of water is 26.7 torr at 27 °C. What is the partial pressure of the oxygen gas?

> Make the indicated pressure conversions. a. 45.2 kPa to atmospheres b. 755 mm Hg to atmospheres c. 802 torr to kilopascals d. 1.04 atm to millimeters of mercury

> The “Chemistry in Focus” segment Snacks Need Chemistry, Too! discusses why popcorn “pops.” You can estimate the pressure inside a kernel of popcorn at the time of popping by using the ideal gas law. Basically, you determine the mass of water released whe

> What will the volume of the sample become if 459 mL of an ideal gas at 27 °C and 1.05 atm is cooled to 15 °C and 0.997 atm?

> Suppose that 1.29 g of argon gas is confined to a volume of 2.41 L at 29 °C. What would be the pressure in the container? What would the pressure become if the temperature were raised to 42 °C without a change in volume?

> Suppose that a 1.25-g sample of neon gas is confined in a 10.1-L container at 25 °C. What will be the pressure in the container? Suppose the temperature is then raised to 50 °C. What will the new pressure be after the temperature is increased?

> At what temperature (in °C) will a 5.00-g sample of neon gas exert a pressure of 1.10 atm in a 7.00-L container?

> Which of the following molecules contain polar covalent bonds? a. phosphorus, P4 b. oxygen, O2 c. ozone, O3 d. hydrogen fluoride, HF

> What volume will 2.04 g of helium gas occupy at 100. °C and 785 mm Hg pressure?

> Determine the pressure in a 125-L tank containing 56.2 kg of oxygen gas at 21 °C.

> Which of the following statements is(are) true? a. If the number of moles of a gas is doubled, the volume will double, assuming the pressure and temperature of the gas remain constant. b. If the temperature of a gas increases from 25 °C to 50 °C, the vol

> Consider the unbalanced chemical equation: CaSiO3(s) + HF(g) / CaF2(aq) + SiF4(g) + H2O(l) Suppose a 32.9-g sample of CaSiO3 is reacted with 31.8 L of HF at 27.0 °C and 1.00 atm. Assuming the reaction goes to completion, calculate the mass of SiF4 and H

> A 20.0-L nickel container was charged with 0.859 atm of xenon gas and 1.37 atm of fluorine gas at 400 °C. The xenon and fluorine react to form xenon tetrafluoride. What mass of xenon tetrafluoride can be produced, assuming 100% yield?

> A large flask with a volume of 936 mL is evacuated and found to have a mass of 134.66 g. It is then filled to a pressure of 0.967 atm at 31 °C with a gas of unknown molar mass and then reweighed to give a new mass of 135.87 g. What is the molar mass of t

> A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25 °C and the barometric pressure is 730 torr. The balloon then rises to an altitude of 6000 ft, where the pressu

> A steel cylinder contains 150.0 moles of argon gas at a temperature of 25 °C and a pressure of 8.93 MPa. After some argon has been used, the pressure is 2.00 MPa at a temperature of 19 °C. What mass of argon remains in the cylinder?

> A glass vessel contains 28 g of nitrogen gas. Assuming ideal behavior, which of the processes listed below would double the pressure exerted on the walls of the vessel? a. Adding 28 g of oxygen gas b. Raising the temperature of the container from 273 °

> Complete the following table for an ideal gas. P(atm) V(L) n (mol) 6.74 2.00 155 °C 0.300 1.74 155 K 4.47 25.0 2.19 °C 2.25 10.5 93 °C

> Which of the following molecules contain polar covalent bonds? a. water, H2O b. carbon monoxide, CO c. fluorine, F2 d. nitrogen, N2

> The “Chemistry in Focus” segment Breath Fingerprinting discusses using breath analysis to diagnose diseases. The volume of the average human breath is approximately 500 mL, and carbon dioxide (CO2) makes up 4% of what we exhale. Determine the mass of car

> The “Chemistry in Focus” segment The Chemistry of Air Bags discusses how the decomposition of sodium azide inflates the air bag. Use the balanced chemical equation in the segment to determine the mass of sodium azide required to inflate an air bag to 70.

> Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H2O2(aq) 2H2O(l) + O2(g) What volume of pure O2(g), collected at 27 °C and 764 torr, would be generated

> What volume of CO2 measured at STP is produced when 27.5 g of CaCO3 is decomposed? CaCO3(s) / CaO(s) + CO2(g)

> Consider the flasks in the following diagrams. a. Which is greater, the initial pressure of helium or the initial pressure of neon? How much greater? b. Assuming the connecting tube has negligible volume, draw what each diagram will look like after th

> A sample of oxygen gas has a volume of 125 L at 25 °C and a pressure of 0.987 atm. Calculate the volume of this oxygen sample at STP.

> What volume does 35 moles of N2 occupy at STP?

> When sodium bicarbonate, NaHCO3(s), is heated, sodium carbonate is produced, with the evolution of water vapor and carbon dioxide gas. 2NaHCO3(s) / Na2CO3(s) + H2O(g) + CO2(g) What total volume of gas, measured at 29 °C and 769 torr, is produced when 1.

> Consider the following unbalanced chemical equation: Cu2S(s) + O2(g) Cu2O(s) + SO2(g) What volume of oxygen gas, measured at 27.5 °C and 0.998 atm, is required to react with 25 g of copper(I) sulfide? What volume of sulfur diox

> The following demonstration takes place in a two-step process: First, solid calcium carbide (CaC2) reacts with liquid water to produce acetylene gas (C2H2) and aqueous calcium hydroxide. Second, the acetylene gas produced is then ignited with a match, ca

> Discuss the similarities and differences between the arrangements of molecules and the forces between molecules in liquid water versus steam, and in liquid water versus ice.

> Consider the following chemical equation: N2(g) + 3H2(g) 2NH3(g) What volumes of nitrogen gas and hydrogen gas, each measured at 11 °C and 0.998 atm, are needed to produce 5.00 g of ammonia?

> You have two rigid gas cylinders. Gas cylinder A has a volume of 48.2 L and contains N2(g) at 8.35 atm at 25 °C. Gas cylinder B has a volume of 22.0 L and contains He(g) at 25 °C. When the two cylinders are connected with a valve of negligible volume and

> A mixture at 33 °C contains H2 at 325 torr, N2 at 475 torr, and O2 at 650. torr. a. What is the total pressure of the gases in the system? b. Which gas contains the greatest number of moles?

> An aluminum can contain a small amount of water and is boiled with the lid removed. The heat is then turned off, and the can is sealed. Over time, the can crumples. a. Why doesnât the can explode or crumple when the water is heated

> If 3.20 g of nitrogen gas occupies a volume of 1.71 L at 0 °C and a pressure of 1.50 atm, what would the volume become if 8.80 g of nitrogen gas were added at constant conditions of temperature and pressure?

> A 22-g sample of neon gas exerts a pressure of 2.0 atm at a certain temperature and volume. What pressure does a 44-g sample of argon gas exert at these conditions of temperature and volume?

> Which of the following statements is(are) true? a. LiF will have a higher vapor pressure at 25 °C than H2S. b. HF will have a lower vapor pressure at 250 °C than HBr. c. Cl2 will have a higher boiling point than Ar. d. HCl is more soluble in water th

> Which of the following statements about intermolecular forces is(are) true? a. London dispersion forces are the only type of intermolecular force that nonpolar molecules exhibit. b. Molecules that have only London dispersion forces will always be gases

> Describe, on a microscopic basis, the processes of evaporation and condensation. Which process requires an input of energy? Why?

> Given each of the following sets of values for three of the gas variables, calculate the unknown quantity. a. P = 1.034 atm; V = 21.2 mL; n = 0.00432 mol; T =? K b. P =? atm; V = 1.73 mL; n = 0.000115 mol; T = 182 K c. P = 1.23 mm Hg; V =? L; n = 0.77

> Make the indicated pressure conversions. a. 1.54 * 105 Pa to atmospheres b. 1.21 atm to pascals c. 97,345 Pa to mm Hg d. 1.32 kPa to pascals

> Given each of the following sets of values for three of the gas variables, calculate the unknown quantity. a. P = 21.2 atm; V = 142 mL; n = 0.432 mol; T =? K b. P =? atm; V = 1.23 mL; n = 0.000115 mol; T = 293 K c. P = 755 mm Hg; V =? mL; n = 0.473 mo

> You have a gas in a container fitted with a piston, and you change one of the conditions of the gas such that a change takes place, as shown below: State three distinct changes you can make to accomplish this, and explain why each would work. volum

> Although the noble gas elements are monatomic and could not give rise to dipole–dipole forces or hydrogen bonding, these elements still can be liquefied and solidified. Explain.

> For each of the following sets of volume/temperature data, calculate the missing quantity. Assume that the pressure and the amount of gas remain constant. a. V = 22.4 L at 0 °C; V = 44.4 L at? K b. V = 1.0 3 1023 mL at 2272 °C; V =? at 25 °C c. V = 32

> Arrange the atoms and/or ions in the following groups in order of decreasing size. a. O, O+, O2- b. Fe2+, Ni2+, Zn2+ c. Ca2+, K+, Cl-

> Describe in detail the microscopic processes that take place when a liquid boils. What kind of forces must be overcome? Are any chemical bonds broken during these processes?

> What are London dispersion forces and how do they arise in a nonpolar molecule? Are London forces typically stronger or weaker than dipole–dipole attractions between polar molecules? Are London forces stronger or weaker than covalent bonds? Explain.

Question: Ionic solids do not conduct electricity in

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