Solved: Identify each compound as an oxide, peroxide, or

Problem 1E Why does BN form compounds similar to those formed by elemental carbon?

Problem 2E What is the main characteristic that determines whether or not an element is a main-group element?

Use charge balance to determine x in the formula for the sorosilicate bertrandite, Be4Si2O7(OH)x. a) 1 b) 2 c) 3 d) 4

Problem 3SAQ Which element is important in the manufacturing of glassware intended for heating? a) carbon b) nitrogen c) phosphorus d) boron

Problem 4E Why does silicon form only single bonds with oxygen but carbon, which is in the same family as silicon, form double bonds with oxygen in many compounds?

Problem 4SAQ Fertilizers commonly contain compounds of which element? a) nitrogen b) aluminum c) fluorine d) boron

What is the oxidation state of bromine in the compound NaBrO3? a) +2 b) -3 c) -4 d) +5

Problem 6E What is the difference between a rock and a mineral?

Problem 7E Briefly define each term. a. orthosilicate b. amphibole c. pyroxene d. pyrosilicate e. feldspar

Which element is oxidized in the reaction? a) Ca b) O c) S d) None of the above (no element is oxidized in the reaction)

Problem 8E Why is boron oxide often added to silica glass?

Problem 9E Why does boron form electron-deficient bonds? Provide an example.

Which carbon oxide does not exist? a) CO b) CO2 c) CO32- d) CO4

Problem 10E List three allotropes of crystalline carbon.

Problem 12E Nitric acid and phosphoric acid are two major chemical products of the chemical industry. Describe some of their uses.

Explain why solid CO2 is referred to as dry ice.

Which substance forms when carbon dioxide dissolves in water? a) CO b) H2CO c) CH4 d) H2CO3

Calculate the standard enthalpy of reaction for reducing the different forms of iron oxide to iron metal and CO2 from the reaction of the oxide with CO. Identify which reaction is the most exothermic per mole of iron and explain why. a. Fe3O4 b. FeO c. Fe2O3

Balance the equation for the production of acetylene (C2H2) from the reaction of calcium carbide with water. If the acetylene is burned to form water and carbon dioxide, how many kilojoules of energy are produced from the complete reaction of 18 g of calcium carbide?

Use the data in Appendix II , Table B to calculate for the formation of a 1 M solution of H2SO4 from SO3(g).

Carbon suboxide, C3O2, is a linear molecule with the two oxygen atoms at the end and double bonds between each carbon and oxygen atom. a. Draw the Lewis structure for C3O2. b. State the type of hybridization of each carbon atom. c. Calculate the heat of reaction for the reaction of carbon suboxide with water to form malonic acid (HO2CCH2CO2H). Hint: Each end of malonic acid has a carbon double bonded to an oxygen and bonded to a hydroxide.

List two chemical and two physical properties that distinguish a metal from a nonmetal

Make a list of physical and chemical properties of chlorine (Cl2) and magnesium. Comment on their differences with reference to the fact that one is a metal and the other is a nonmetal

Carbon is usually classified as a nonmetal. However, the graphite used in lead pencils conducts electricity. Look at a pencil and list two nonmetallic properties of graphite

Describe two laboratory and two industrial preparations for hydrogen.

Hydrogen exhibits three types of bonding in its compounds. Describe each type of bonding with an example.

What are interstitial hydrides?

Give the name of (a) an ionic hydride and (b) a covalent hydride. In each case describe the preparation and give the structure of the compound.

Describe what is meant by the hydrogen economy.

Elements number 17 and 20 form compounds with hydrogen. Write the formulas for these two compounds and compare their chemical behavior in water

Give an example of hydrogen as (a) an oxidizing agent and (b) a reducing agent.

Compare the physical and chemical properties of the hydrides of each of the following elements: Na, Ca, C, N, O, Cl

Suggest a physical method that would enable you to separate hydrogen gas from neon gas.

Write a balanced equation to show the reaction between CaH2 and H2O. How many grams of CaH2 are needed to produce 26.4 L of H2 gas at 20C and 746 mmHg?

How many kilograms of water must be processed to obtain 2.0 L of D2 at 25C and 0.90 atm pressure? Assume that deuterium abundance is 0.015 percent and that recovery is 80 percent.

Predict the outcome of the following reactions: (a) CuO(s) 1 H2(g) (b) Na2O(s) 1 H2(g)

Starting with H2, describe how you would prepare (a) HCl, (b) NH3, (c) LiOH.

Give an example of a carbide and a cyanide

How are cyanide ions used in metallurgy?

Briefly discuss the preparation and properties of carbon monoxide and carbon dioxide.

What is coal?

Explain what is meant by coal gasification

Describe two chemical differences between CO and CO2.

Describe the reaction between CO2 and OH2 in terms of a Lewis acid-base reaction such as that shown on p. 705.

Draw a Lewis structure for the C2 22 ion.

Balance the following equations: (a) Be2C(s) 1 H2O(l) (b) CaC2(s) 1 H2O(l)

Unlike CaCO3, Na2CO3 does not readily yield CO2 when heated. On the other hand, NaHCO3 undergoes thermal decomposition to produce CO2 and Na2CO3. (a) Write a balanced equation for the reaction. (b) How would you test for the CO2 evolved? [Hint: Treat the gas with limewater, an aqueous solution of Ca(OH)2.]

Two solutions are labeled A and B. Solution A contains Na2CO3 and solution B contains NaHCO3. Describe how you would distinguish between the two solutions if you were provided with a MgCl2 solution. (Hint: You need to know the solubilities of MgCO3 and MgHCO3.)

Magnesium chloride is dissolved in a solution containing sodium bicarbonate. On heating, a white precipitate is formed. Explain what causes the precipitation

A few drops of concentrated ammonia solution added to a calcium bicarbonate solution cause a white precipitate to form. Write a balanced equation for the reaction.

Sodium hydroxide is hygroscopicthat is, it absorbs moisture when exposed to the atmosphere. A student placed a pellet of NaOH on a watch glass. A few days later, she noticed that the pellet was covered with a white solid. What is the identity of this solid? (Hint: Air contains CO2.)

A piece of red-hot magnesium ribbon will continue to burn in an atmosphere of CO2 even though CO2 does not support combustion. Explain.

Is carbon monoxide isoelectronic with nitrogen (N2)?

Describe a laboratory and an industrial preparation of nitrogen gas.

What is meant by nitrogen fixation? Describe a process for fixation of nitrogen on an industrial scale.

Describe an industrial preparation of phosphorus.

Why is the P4 molecule unstable?

Nitrogen can be obtained by (a) passing ammonia over red-hot copper(II) oxide and (b) heating ammonium dichromate [one of the products is Cr(III) oxide]. Write a balanced equation for each preparation.

Write balanced equations for the preparation of sodium nitrite by (a) heating sodium nitrate and (b) heating sodium nitrate with carbon

Sodium amide (NaNH2) reacts with water to produce sodium hydroxide and ammonia. Describe this reaction as a Brnsted acid-base reaction.

Write a balanced equation for the formation of urea, (NH2)2CO, from carbon dioxide and ammonia. Should the reaction be run at a high or low pressure to maximize the yield?

Some farmers feel that lightning helps produce a better crop. What is the scientific basis for this belief?

At 620 K the vapor density of ammonium chloride relative to hydrogen (H2) under the same conditions of temperature and pressure is 14.5, although, according to its formula mass, it should have a vapor density of 26.8. How would you account for this discrepancy?

Explain, giving one example in each case, why nitrous acid can act both as a reducing agent and as an oxidizing agent.

Explain why nitric acid can be reduced but not oxidized.

Write a balanced equation for each of the following processes: (a) On heating, ammonium nitrate produces nitrous oxide. (b) On heating, potassium nitrate produces potassium nitrite and oxygen gas. (c) On heating, lead nitrate produces lead(II) oxide, nitrogen dioxide (NO2), and oxygen gas.

Explain why, under normal conditions, the reaction of zinc with nitric acid does not produce hydrogen

Potassium nitrite can be produced by heating a mixture of potassium nitrate and carbon. Write a balanced equation for this reaction. Calculate the theoretical yield of KNO2 produced by heating 57.0 g of KNO3 with an excess of carbon

Predict the geometry of nitrous oxide, N2O, by the VSEPR method and draw resonance structures for the molecule. (Hint: The atoms are arranged as NNO.)

Consider the reaction N2(g) 1 O2(g) 2NO(g) Given that the G for the reaction at 298 K is 173.4 kJ/mol, calculate (a) the standard free energy of formation of NO, (b) KP for the reaction, and (c) Kc for the reaction.

From the data in Appendix 3, calculate H for the synthesis of NO (which is the first step in the manufacture of nitric acid) at 25C: 4NH3(g) 1 5O2(g) 4NO(g) 1 6H2O(l)

Explain why two N atoms can form a double bond or a triple bond, whereas two P atoms normally can form only a single bond.

When 1.645 g of white phosphorus are dissolved in 75.5 g of CS2, the solution boils at 46.709C, whereas pure CS2 boils at 46.300C. The molal boiling-point elevation constant for CS2 is 2.34C/m. Calculate the molar mass of white phosphorus and give the molecular formula

Starting with elemental phosphorus, P4, show how you would prepare phosphoric acid.

Dinitrogen pentoxide is a product of the reaction between P4O10 and HNO3. Write a balanced equation for this reaction. Calculate the theoretical yield of N2O5 if 79.4 g of P4O10 are reacted with an excess of HNO3. (Hint: One of the products is HPO3.)

Explain why (a) NH3 is more basic than PH3, (b) NH3 has a higher boiling point than PH3, (c) PCl5 exists but NCl5 does not, (d) N2 is more inert than P4.

What is the hybridization of phosphorus in the phosphonium ion, PH4 1?

Describe one industrial and one laboratory preparation of O2.

Give an account of the various kinds of oxides that exist and illustrate each type by two examples.

Hydrogen peroxide can be prepared by treating barium peroxide with sulfuric acid. Write a balanced equation for this reaction.

Describe the Frasch process for obtaining sulfur

Describe the contact process for the production of sulfuric acid.

How is hydrogen sulfide generated in the laboratory?

Draw molecular orbital energy level diagrams for O2, O2 2, and O2 22

One of the steps involved in the depletion of ozone in the stratosphere by nitric oxide may be represented as NO(g) 1 O3(g) NO2(g) 1 O2(g) From the data in Appendix 3 calculate G, KP, and Kc for the reaction at 25C.

Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) 2H2O(l) 1 O2(g) This reaction is accelerated by light, heat, or a catalyst. (a) Explain why hydrogen peroxide sold in drugstores comes in dark bottles. (b) The concentrations of aqueous hydrogen peroxide solutions are normally expressed as percent by mass. In the decomposition of hydrogen peroxide, how many liters of oxygen gas can be produced at STP from 15.0 g of a 7.50 percent hydrogen peroxide solution?

What are the oxidation numbers of O and F in HFO?

Oxygen forms double bonds in O2, but sulfur forms single bonds in S8. Explain.

In 2008, about 48 million tons of sulfuric acid were produced in the United States. Calculate the amount of sulfur (in grams and moles) used to produce that amount of sulfuric acid.

Sulfuric acid is a dehydrating agent. Write balanced equations for the reactions between sulfuric acid and the following substances: (a) HCOOH, (b) H3PO4, (c) HNO3, (d) HClO3. (Hint: Sulfuric acid is not decomposed by the dehydrating action.)

Calculate the amount of CaCO3 (in grams) that would be required to react with 50.6 g of SO2 emitted by a power plant.

SF6 exists but OF6 does not. Explain

Explain why SCl6, SBr6, and SI6 cannot be prepared.

Compare the physical and chemical properties of H2O and H2S.

The bad smell of water containing hydrogen sulfide can be removed by the action of chlorine. The reaction is H2S(aq) 1 Cl2(aq) 2HCl(aq) 1 S(s) If the hydrogen sulfide content of contaminated water is 22 ppm by mass, calculate the amount of Cl2 (in grams) required to remove all the H2S from 2.0 3 102 gallons of water. (1 gallon 5 3.785 L.)

Describe two reactions in which sulfuric acid acts as an oxidizing agent

Concentrated sulfuric acid reacts with sodium iodide to produce molecular iodine, hydrogen sulfide, and sodium hydrogen sulfate. Write a balanced equation for the reaction.

Describe an industrial method for preparing each of the halogens.

Name the major uses of the halogens.

Metal chlorides can be prepared in a number of ways: (a) direct combination of metal and molecular chlorine, (b) reaction between metal and hydrochloric acid, (c) acid-base neutralization, (d) metal carbonate treated with hydrochloric acid, (e) precipitation reaction. Give an example for each type of preparation

Sulfuric acid is a weaker acid than hydrochloric acid. Yet hydrogen chloride is evolved when concentrated sulfuric acid is added to sodium chloride. Explain

Show that chlorine, bromine, and iodine are very much alike by giving an account of their behavior (a) with hydrogen, (b) in producing silver salts, (c) as oxidizing agents, and (d) with sodium hydroxide. (e) In what respects is fluorine not a typical halogen element?

A 375-gallon tank is filled with water containing 167 g of bromine in the form of Br2 ions. How many liters of Cl2 gas at 1.00 atm and 20C will be required to oxidize all the bromide to molecular bromine?

Draw structures for (a) (HF)2 and (b) HF2 2

Hydrogen fluoride can be prepared by the action of sulfuric acid on sodium fluoride. Explain why hydrogen bromide cannot be prepared by the action of the same acid on sodium bromide

Aqueous copper(II) sulfate solution is blue. When aqueous potassium fluoride is added to the CuSO4 solution, a green precipitate is formed. If aqueous potassium chloride is added instead, a bright-green solution is formed. Explain what happens in each case.

What volume of bromine (Br2) vapor measured at 100C and 700 mmHg pressure would be obtained if 2.00 L of dry chlorine (Cl2), measured at 15C and 760 mmHg, were absorbed by a potassium bromide solution?

Use the VSEPR method to predict the geometries of the following species: (a) I3 2, (b) SiCl4, (c) PF5, (d) SF4.

Iodine pentoxide, I2O5, is sometimes used to remove carbon monoxide from the air by forming carbon dioxide and iodine. Write a balanced equation for this reaction and identify species that are oxidized and reduced.

Write a balanced equation for each of the following reactions: (a) Heating phosphorous acid yields phosphoric acid and phosphine (PH3). (b) Lithium carbide reacts with hydrochloric acid to give lithium chloride and methane. (c) Bubbling HI gas through an aqueous solution of HNO2 yields molecular iodine and nitric oxide. (d) Hydrogen sulfide is oxidized by chlorine to give HCl and SCl2

(a) Which of the following compounds has the great est ionic character? PCl5, SiCl4, CCl4, BCl3 (b) Which of the following ions has the smallest ionic radius? F2, C42, N32, O22 (c) Which of the following atoms has the highest ionization energy? F, Cl, Br, I (d) Which of the following oxides is most acidic? H2O, SiO2, CO2

Both N2O and O2 support combustion. Suggest one physical and one chemical test to distinguish between the two gases.

What is the change in oxidation number for the following reaction? 3O2 2O3

Describe the bonding in the C2 22 ion in terms of the molecular orbital theory.

Starting with deuterium oxide (D2O), describe how you would prepare (a) NaOD, (b) DCl, (c) ND3, (d) C2D2, (e) CD4, (f) D2SO4.

Solid PCl5 exists as [PCl 4 1][PCl6 2]. Draw Lewis structures for these ions. Describe the hybridization state of the P atoms.

Consider the Frasch process. (a) How is it possible to heat water well above 100C without turning it into steam? (b) Why is water sent down the outermost pipe? (c) Why would excavating a mine and digging for sulfur be a dangerous procedure for obtaining the element?

Predict the physical and chemical properties of astatine, a radioactive element and the last member of Group 7A.

Lubricants used in watches usually consist of longchain hydrocarbons. Oxidation by air forms solid polymers that eventually destroy the effectiveness of the lubricants. It is believed that one of the initial steps in the oxidation is removal of a hydrogen atom (hydrogen abstraction). By replacing the hydrogen atoms at reactive sites with deuterium atoms, it is possible to substantially slow down the overall oxidation rate. Why? (Hint: Consider the kinetic isotope effect.)

How are lightbulbs frosted? (Hint: Consider the action of hydrofluoric acid on glass, which is made of silicon dioxide.)

Life evolves to adapt to its environment. In this respect, explain why life most frequently needs oxygen for survival, rather than the more abundant nitrogen

As mentioned in Chapter 3, ammonium nitrate is the most important nitrogen-containing fertilizer in the world. Given only air and water as starting materials and any equipment and catalyst at your disposal, describe how you would prepare ammonium nitrate. State conditions under which you can increase the yield in each step.

As we saw in Section 21.2, the reduction of iron oxides is accomplished by using carbon monoxide as a reducing agent. Starting with coke in a blast furnace, the following equilibrium plays a key role in the extraction of iron: C(s) 1 CO2(g) 2CO(g) Use the data in Appendix 3 to calculate the equilibrium constant at 25C and 1000C. Assume H and S to be independent of temperature.

Assuming ideal behavior, calculate the density of gaseous HF at its normal boiling point (19.5C). The experimentally measured density under the same conditions is 3.10 g/L. Account for the discrepancy between your calculated value and the experimental result

A 10.0-g sample of white phosphorus was burned in an excess of oxygen. The product was dissolved in enough water to make 500 mL of solution. Calculate the pH of the solution at 25C.

An aluminosilicate is composed of a crystal in which Al atoms substitute for three-fourths of the Si atoms in the silica structure. The negative charge of the AlO2- groups is balanced by Na+ ions. What is the formula of the aluminosilicate? a) Na(AlSi3O8) b) Na2(Al2Si2O8) c) Na3(Al3SiO8) d) NaSiO2

Problem 3E Does the metallic characteristic of a main-group element increase or decrease as we move down a family? Explain why.

What is the difference between SiO2 that is cooled slowly and SiO2 that is cooled quickly?

What is the molecular geometry of ICl4-? a) tetrahedral b) square planar c) octahedral d) seesaw

Problem 9SAQ Which element is extracted from the ground primarily in its elemental form? a) boron b) phosphorus c) sulfur d) fluorine

Problem 13E What is the typical concentration of oxygen in dry air?

Problem 14E Describe how nitrogen can be separated from the other components of air.

Problem 15E Earth's atmosphere originally did not contain oxygen. Explain how the atmosphere gained oxygen.

Problem 16E Name a benefit, a hazard, and a useful commercial application of ozone.

Silicon bonds to oxygen to form a tetrahedral shape in both the network covalent silica compound, SiO2, and in ionic silicate compounds. What is the oxidation state of Si in each of these structures? a. silica compound, SiO2 b. orthosilicates, SiO44- c. pyrosilicates, Si2O76-

What is the oxidation state of \(\mathrm{Si}\) in each of these structures? a. pyroxenes, \(\mathrm{SiO}_3{ }^{2-}\) b. amphiboles, \(\mathrm{Si}_4 \mathrm{O}_{11}^{6-}\) c. phyllosilicates, \(\mathrm{Si}_2 \mathrm{O}_5{ }^{2-}\)

In the orthosilicate garnet, the formula unit has three SiO44- units and is balanced by Ca2+ and Al3+ cations. Determine the formula unit of garnet.

In the pyroxene kanoite, the formula unit has two SiO32- units and is balanced by manganese and magnesium ions. Determine the formula unit of kanoite. Assume that the oxidation state of Mn is +2.

Kaolin is a clay material that is a phyllosilicate. Use charge balancing to determine how many hydroxide ions are in the formula for kaolin, Al2Si2O5(OH)x.

Tremolite is a double-chain silicate in the amphibole class. Use charge balancing to determine how many hydroxide ions are in the formula for tremolite, Ca2Mg5Si8O22(OH)x.

How are the silica tetrahedrons linked for ZrSiO4? Which class of silicates does this compound belong to?

How are the silica tetrahedrons linked for CaSiO3? Which class of silicates does this compound belong to?

Predict the structure and label the charges on the cations in the mineral hedenbergite, CaFeSi2O6.

Predict the structure and give the charges on the cations in one of the minerals in the hornblende family, \(\mathrm{Ca}_{2} \mathrm{Mg}_{4} \mathrm{FeSi}_{7} \mathrm{AlO}_{22}(\mathrm{OH})_{2}\).

A major source of boron is the mineral kernite, \(\mathrm{Na}_2\left[\mathrm{~B}_4 \mathrm{O}_5(\mathrm{OH})_4\right] \cdot 3 \mathrm{H}_2 \mathrm{O}\). Calculate how many grams of boron can be produced from \(1.0 \times 10^3 \mathrm{~kg}\) of a kernite-bearing ore if the ore contains 0.98% kernite by mass and the process has a 65% yield.

An uncommon mineral of boron is ulexite, NaCaB5O9 8 H2O. How many grams of boron can be produced from 5.00 x 102 kg of ulexite-bearing ore if the ore contains 0.032% ulexite by mass and the process has an 88% yield?

Explain why the bond angles in BCl3 and NCl3 are different.

Explain why the bond between B and Cl in the molecule \(\mathrm{BCl}_{3}\) is shorter than would be expected for a single B—Cl bond.

Predict the number of vertices and faces on each closo-borane. a. B6H62- b. B12H122-

Predict the number of vertices and faces on each closo -borane. a. B4H42- b. B9H92-

Problem 33E Describe the differences among a closo -borane, a nido -borane, and an arachno -borane.

Problem 34E Describe how boron is used in the nuclear industry.

Problem 35E Explain why the graphite structure of carbon allows graphite to be used as a lubricant, but the diamond structure of carbon does not.

Problem 36E Explain why graphite can conduct electricity, but diamond does not.

Problem 37E Describe the difference between regular charcoal and activated charcoal.

Problem 38E Explain why the structure of charcoal allows carbon to act as a good filter while the diamond structure does not.

Problem 39E Describe the difference between an ionic carbide and a covalent carbide. Which types of atoms will form these carbides with carbon?

Silicon carbide is produced by heating silicone polymers, forming methane gas, hydrogen gas, and silicon carbide. Balance the reaction of heating \(\left[\left(\mathrm{CH}_3\right)_2 \mathrm{Si}\right]_8\) to form silicon carbide.

Referring to the phase diagram in Section 11.8 , describe what happens to the phase of CO2 during each process. a. reducing the pressure on solid CO2 that is at -80 oC b. decreasing the temperature on CO2 gas that is held at a pressure of 20 atm c. increasing the temperature on solid CO2 that is held at a pressure of 0.8 atm

Referring to the phase diagram in Section 11.8 , describe what happens to the phase of CO2 during each process. a. reducing the temperature from the critical point b. increasing the pressure on CO2 gas that is held at a temperature of -50 oC c. increasing the temperature on solid CO2 that is held at a pressure of 20 atm

Predict the products for each reaction and write a balanced equation. a. CO(g) + CuO(s) b. SiO2(s) + C(s) c. S(s) + CO(g)

Give the oxidation state for carbon in: a. CO b. \(\mathrm{CO}_{2}\) c. \(\mathrm{C}_{3} \mathrm{O}_{2}\)

Predict the products for each reaction and write a balanced equation. a. CO(g) + Cl2(g) b. CO2(g) + Mg(s) c. S(s) + C(s)

Write a balanced reaction for the gas release reaction of Alka-Seltzer, sodium bicarbonate with citric acid, C6H8O7. (The acid is a triprotic acid and consists of a chain of three carbon atoms, each with a carboxylic acid group, COOH.)

Explain the process of fixing nitrogen.

Problem 48E Explain why the diatomic nitrogen atom is unusable by most plants. Where do plants get nitrogen?

Problem 49E Describe the differences in the allotropes of white and red phosphorus. Explain why red phosphorus is more stable.

Problem 50E Describe how red and black phosphorus are made from white phosphorus.

Problem 51E Saltpeter and Chile saltpeter are two important mineral sources for nitrogen. Calculate the mass percent of nitrogen in each mineral.

Problem 52E Apatite is a main mineral source for the production of phosphorus. Calculate the atomic and mass percent of P in the mineral apatite.

Referring to the tables in Appendix IIB , determine whether or not hydrogen azide is stable at room temperature compared to its elements, H2 and N2. Is hydrogen azide stable at any temperature?

Referring to the tables in Appendix IIB , determine if dinitrogen monoxide is stable at room temperature compared to its elements, O2 and N2. Is dinitrogen monoxide stable at any temperature?

Predict the products for each reaction and write a balanced equation. a. NH4NO3(aq) + heat b. NO2(g) + H2O(l) c. PCl3(l) + O2(g)

Predict the products for each reaction and write a balanced equation. a. NO(g) + NO2(g) b. heating PH3 c. P4(s) + 5 O2(g)

Rank the nitrogen ions from the one with N in the highest oxidation state to the one with N in the lowest.

Draw the Lewis structures for the phosphorus halides PCl3 and PCl5. Describe their VSEPR shape.

Determine the oxidation state of N in the compounds in the reaction for the formation of nitric acid. Identify the oxidizing agent and the reducing agent.

Dinitrogen pentoxide is an ionic compound formed from the ions NO2+ and NO3-. Give the oxidation state of N in each ion and the VSEPR shape for each of the ions.

Ammonium carbonate is produced from the reaction of urea, CO(NH2)2 with water. Write a balanced equation for this reaction and determine how much urea is needed to produce 23 g of ammonium carbonate.

Explain why phosphine, PH3, is less polar than ammonia.

Reacting oxygen with white phosphorus can form either P4O6 or P4O10. State the conditions that determine which product forms.

\(\mathrm{P}_{4} \mathrm{O}_{10}\) is one of the most effective drying agents, having the ability to extract water from other molecules. The \(\mathrm{P}_{4} \mathrm{O}_{10}\) forms phosphoric acid. Write balanced reactions for the reaction of \(\mathrm{P}_{4} \mathrm{O}_{10}\) with: a. \(\mathrm{HNO}_{3}\), forming \(\mathrm{N}_{2} \mathrm{O}_{5}\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}\), forming \(\mathrm{SO}_{3}\)

Problem 65E Name the major source of the element oxygen and describe how it is produced.

Problem 66E Explain why either greatly decreasing or increasing the percentage of oxygen in the atmosphere is dangerous.

Identify each compound as an oxide, peroxide, or superoxide. a. LiO2 b. CaO c. K2O2

Identify each compound as an oxide, peroxide, or superoxide. a. MgO b. Na2O2 c. CsO2

Problem 69E Explain why the viscosity of liquid sulfur increases with increasing temperature initially, but then decreases upon further increases in temperature.

Calculate the maximum mass (in grams) of each metal sulfide that will dissolve in 1.0 L of a solution that is 5.00 x 10-5 M in Na2S. a. PbS b. ZnS

Sulfur dioxide is a toxic sulfur compound. List one natural source and one industrial source that produces \(\mathrm{SO}_{2}\).

A coal source contains 1.1% sulfur by mass. If 2.0 x 104 kg of coal is burned and forms oxides, calculate the mass of CaSO4(s) that is produced from “scrubbing” the SO2 pollutant out of the exhaust gas. Assume that all of the sulfur in the coal is converted to calcium sulfate.

Write the equation for roasting iron pyrite in the absence of air to form elemental sulfur. Calculate the volume of S2 gas that can be produced from roasting 5.5 kg of iron pyrite. Assume that all of the sulfur in the iron pyrite is converted to S2 gas. (Assume STP to calculate the gas volume.)

Write an overall reaction from the two steps in the Claus process. Calculate the volume of \(\mathrm{H}_{2} \mathrm{S}\) gas needed to produce 1.0 kg of S(s). (Assume STP to calculate the gas volume.)

Describe the shape of each halogen compound. a. BrF4= b. IF3 c. BrO2- d. ClO4-

Determine the oxidation state of Xe and give the VSEPR structure for each compound. a. XeF2 b. XeF6 c. XeOF4

Problem 77E When chlorine is bubbled through a colorless aqueous solution containing bromide ions, the solution turns red and the chlorine is reduced. Write a balanced equation for this reaction and identify the oxidizing and reducing agent.

Carbon tetrachloride is produced by passing chlorine gas over carbon disulfide in the presence of a catalyst. The reaction also produces S2Cl2. Write the balanced reaction and identify which element is oxidized and which element is reduced.

If 55 g of SiO2(s) glass is placed into 111 L of 0.032 M HF, is there enough HF to dissolve all of the glass? Determine which substance is the limiting reagent and calculate how much of the other reagent is left if the reaction proceeds to completion.

From the compositions of lignite and bituminous coal, calculate the mass of sulfuric acid that could potentially form as acid rain from burning \(1.00\times10^2\mathrm{\ kg}\) of each type of coal.

Describe the difference in the types of bonds (single, double, triple) and the shapes of the following two iodine ions: \(\mathrm{ICl}_4^{\ -}\) and \(\mathrm{IO}_4^{\ -}\)

Calculate the volume of CO2 released from heating and decomposing 88 g of sodium bicarbonate. (Assume standard pressure and temperature.)

All of the halogens form oxoacids. The perhalic acids have the general formula of HXO4. Explain why HClO4 is a much stronger acid than HIO4.

The halogens form oxoacids with different amounts of oxygen. Explain why HClO4 is a stronger acid than HClO2.

Determine the ratio of effusion rates of HCl compared to each gas a. \(\mathrm{Cl}_{2}\) b. HF c. HI

Calculate the ratio of effusion rates for each pair of gases. a. 238UF6 and ClF b. 238UF6 and 235UF6

Sodium peroxide is a very powerful oxidizing agent. Balance the reaction of sodium peroxide with elemental iron to give sodium oxide and Fe3O4.

Sulfur dioxide is a reducing agent. When it is bubbled through an aqueous solution containing Br2, a red-colored solution, it reduces the bromine to colorless bromide ions and forms sulfuric acid. Write a balanced equation for this reaction and identify the oxidizing and reducing agent.

Using the molecular orbital model for a diatomic molecule, explain the different bond lengths for the ions of oxygen. Also state which ion is diamagnetic.

The closo -borane with the formula B6H62- has the six B atoms at vertices, forming an octahedron structure with eight faces. The formula for the number of sides is 2n - 4, where n is the number of boron atoms. Determine the number of vertices and faces for each closo-borane. a. B4H42- b. B12H122-

Find the amount (in moles) of C—C bonds that must be broken when 1.0 mole of C( g ) is formed from C(diamond). Calculate the of sublimation of diamond from the data in Appendix II , Table B. Then do the calculation using the C—C bond energy in Table 9.3 . Suggest a reason for the difference between the two values.

Breathing air that contains 0.13% CO by volume for 30 minutes will cause death. CO can form by incomplete combustion of carbon-containing compounds. Calculate the minimum volume of octane (C8H18, a component of gasoline, which has a density of 0.70 g/mL) that must burn to produce this composition of CO in a garage of volume 40 m3 at 298 K and 1.0 atm.

Given that the of 1 M H2SO3 is -633 kJ, use the data in Appendix II , Table B to calculate the for the formation of a 1 M solution of SO2 in water from SO2(g).

Problem 98E Calcium carbonate is insoluble in water. Yet, it dissolves in an acidic solution. Calculate the standard enthalpy, entropy, and Gibbs free energy change for the reaction between solid calcium carbonate and hydrochloric acid. What drives the reaction, the enthalpy change, or the entropy change?

When hydrazine is dissolved in water it acts like a base. a. Calculate the Kb for the overall reaction of hydrazine forming N2H62+. b. Calculate Ka1 for N2H5+. c. Calculate the concentration of hydrazine and both cations in a solution buffered at a pH of 8.5 for a solution that was made by dissolving 0.012 mol of hydrazine in 1 L of water.

Solid fuel in the booster rockets for spacecraft consists of aluminum powder as the fuel and ammonium perchlorate as the oxidizing agent. If a rocket launch burns 2.200 x 103 kg of aluminum, calculate the energy produced in joules. Calculate the volume of the gas produced assuming it was cooled back to 298 K at 1 atm. The standard enthalpy of formation of solid ammonium perchlorate is -295.3 kJ/mol.

Two known compounds have the formula H2N2O2. One of them is a weak acid and one is a weak base. The acid, called hyponitrous acid, has two O—H bonds. The base, called nitramide, has no O—H bonds. Draw Lewis structures for these compounds. Predict whether the acid is stronger or weaker than nitrous acid and whether the base is stronger or weaker than ammonia.

Explain why fine particles of activated charcoal can absorb more (as a filter) than large briquettes of charcoal.

Problem 103E The two major components of the atmosphere are the diatomic molecules of nitrogen and oxygen. Explain why pure nitrogen is used as a protective atmosphere in the laboratory and pure oxygen is much more reactive.

Problem 104E Explain why nitrogen can form compounds with many different oxidation numbers.

Explain why H2S has a different bond angle and is much more reactive than H2O.

Describe how sodium dihydrogen phosphate can be used as a pH buffering agent.

Explain why fluorine is found only with the oxidation state of -1 or 0, while the other halogens are found in compounds with other oxidation states.

Problem 108E Why do some substances burn in fluorine gas even if they do not burn in oxygen gas?

Explain why SO2 is used as a reducing agent but SO3 is not.

Explain why the interhalogen molecule \(\mathrm{BrCl}_{3}\) exists but \(\mathrm{ClBr}_{3}\) does not.