?Sulfur dioxide is a reducing agent. When it is bubbled through an aqueous solution

Explain why solid \(\mathrm{CO}_{2}\) is referred to as dry ice. Text Transcription: CO_2

Silicon bonds to oxygen to form a tetrahedral shape in both the network covalent silica compound, \(\mathrm{SiO}_{2}\), and in ionic silicate compounds. What is the oxidation state of Si in each of these structures? a. silica compound, \(\mathrm{SiO}_{2}\) b. orthosilicates, \(\mathrm{SiO}_{4}^{4-}\) c. pyrosilicates, \(\mathrm{Si}_{2} \mathrm{O}_{7}^{6-}\) Text Transcription: SiO2 SiO4 4- Si2O7 6-

What is the oxidation state of Si in each of these structures? a. pyroxenes, \(\mathrm{SiO}_{3}^{2-}\) b. amphiboles, \(\mathrm{Si}_{4} \mathrm{O}_{11}^{6-}\) c. phyllosilicates, \(\mathrm{Si}_{2} \mathrm{O}_{5}^{2-}\) Text Transcription: SiO3 2- Si4O11 6- Si2O5 2-

In the orthosilicate garnet, the formula unit has three \(\mathrm{SiO}_{4}{ }^{4-}\) units and is balanced by \(\mathrm{Ca}^{2+}\) and \(\mathrm{Al}^{3+}\) cations. Determine the formula unit of garnet. Text Transcription: SiO4 4- Ca2+ Al 3+

In the pyroxene kanoite, the formula unit has two \(\mathrm{SiO}_{3}^{2-}\) units and is balanced by manganese and magnesium ions. Determine the formula unit of kanoite. Assume that the oxidation state of Mn is +2. Text Transcription: SiO_3^2-

Kaolin is a clay material that is a phyllosilicate. Use charge balancing to determine how many hydroxide ions are in the formula for kaolin, \(\mathrm{Al}_{2} \mathrm{Si}_{2} \mathrm{O}_{5}(\mathrm{OH})_{x}\). Text Transcription: Al_2Si_2O_5(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, \(\mathrm{Ca}_{2} \mathrm{Mg}_{5} \mathrm{Si}_{8} \mathrm{O}_{22}(\mathrm{OH})_{x}\). Text Transcription: Ca_2Mg_5Si_8O_22(OH)x

How are the silica tetrahedrons linked for \(\mathrm{ZrSiO}_{4}\) ? Which class of silicates does this compound belong to? Text Transcription: ZrSiO_4

How are the silica tetrahedrons linked for \(\mathrm{CaSiO}_{3}\) ? Which class of silicates does this compound belong to? Text Transcription: CaSiO_3

Predict the structure and give the charges on the cations in one of the minerals in the hornblende family, \(\mathrm{Ca}_{2} \mathrm{Mg}_{4} \mathrm{FeSi}_{7} \mathrm{AlO}_{22}(\mathrm{OH})_{2}\). Text Transcription: Ca_2Mg_4FeSi_7AlO_22(OH)_2

Predict the structure and label the charges on the cations in the mineral hedenbergite, \(\mathrm{CaFeSi}_{2} \mathrm{O}_{6}\). Text Transcription: CaFeSi_2O_6

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. Text Transcription: Na_2[B_4O_5(OH)_4] dot 3H_2O 1.0 x 10^3 kg

An uncommon mineral of boron is ulexite, \(\mathrm{NaCaB}_{5} \mathrm{O}_{9} \cdot 8 \mathrm{H}_{2} \mathrm{O}\). How many grams of boron can be produced from \(5.00 \times 10^{2} \mathrm{~kg}\) of ulexite-bearing ore if the ore contains 0.032 % ulexite by mass and the process has an 88 % yield? Text Transcription: NaCaB_5O_9 dot 8H_2O 5.00 x 10^2 kg

Explain why the bond angles in \(\mathrm{BCl}_{3}\) and \(\mathrm{NCl}_{3}\) are different. Text Transcription: BCl_3 NCl_3

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. Text Transcription: BCl_3

Predict the number of vertices and faces on each closo-borane. a. \(\mathrm{B}_{6} \mathrm{H}_{6}^{2-}\) b. \(\mathrm{B}_{12} \mathrm{H}_{12}^{2-}\) Text Transcription: B_6H_6 2- B_12H_12 2-

Predict the number of vertices and faces on each closo-borane. a. \(\mathrm{B}_{4} \mathrm{H}_{4}^{2-}\) b. \(\mathrm{B}_{9} \mathrm{H}_{9}^{2-}\) Text Transcription: B_4H_4 2- B_9H_9 2-

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. Text Transcription: [(CH_3)_2Si]_8

Referring to the phase diagram in Section 12.8, describe what happens to the phase of \(\mathrm{CO}_{2}\) during each process. a. reducing the pressure on solid \(\mathrm{CO}_{2}\) that is at \(-80^{\circ} \mathrm{C}\) b. decreasing the temperature on \(\mathrm{CO}_{2}\) gas that is held at a pressure of 20 atm c. increasing the temperature on solid \(\mathrm{CO}_{2}\) that is held at a pressure of 0.8 atm Text Transcription: CO_2 -80^circ C

Referring to the phase diagram in Section 12.8, describe what happens to the phase of \(\mathrm{CO}_{2}\) during each process: a. reducing the temperature from the critical point b. increasing the pressure on \(\mathrm{CO}_{2}\) gas that is held at a temperature of \(-50^{\circ} \mathrm{C}\) c. increasing the temperature on solid \(\mathrm{CO}_{2}\) that is held at a pressure of 20 atm Text Transcription: CO_2 -50^circ C

Predict the products for each reaction and write a balanced equation. a. CO( g) + CuO(s) b. \(\mathrm{SiO}_{2}(s)+\mathrm{C}(s)\) c. S(s) + CO( g) Text Transcription: SiO_2(s) + C(s)

Predict the products for each reaction and write a balanced equation. a. \(\mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\) b. \(\mathrm{CO}_{2}(g)+\mathrm{Mg}(s)\) c. S(s) + C(s) Text Transcription: CO( g) + Cl_2( g) CO_2( g) + Mg(s)

Give the oxidation state for carbon in: a. CO b. \(\mathrm{CO}_{2}\) c. \(\mathrm{C}_{3} \mathrm{O}_{2}\) Text Transcription: CO_2 C_3O_2

Write a balanced reaction for the gas release reaction of AlkaSeltzer, sodium bicarbonate with citric acid, \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\). (The acid is a triprotic acid and consists of a chain of three carbon atoms, each with a carboxylic acid group, COOH.) Text Transcription: C_6H_8O_7

Referring to the tables in Appendix IIB, determine whether or not hydrogen azide is stable at room temperature compared to its elements, \(\mathrm{H}_{2}\) and \(\mathrm{N}_{2}\). Is hydrogen azide stable at any temperature? Text Transcription: H_2 N_2

Referring to the tables in Appendix IIB, determine if dinitrogen monoxide is stable at room temperature compared to its elements, \(\mathrm{O}_{2}\) and \(\mathrm{N}_{2}\). Is dinitrogen monoxide stable at any temperature? Text Transcription: O_2 N_2

Predict the products for each reaction and write a balanced equation. a. \(\mathrm{NH}_{4} \mathrm{NO}_{3}(a q)+\) heat b. \(\mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) c. \(\mathrm{PCl}_{3}(l)+\mathrm{O}_{2}(g)\) Text Transcription: NH_4NO_3(aq) + NO_2( g) + H_2O(l) PCl_3(l) + O_2( g)

Predict the products for each reaction and write a balanced equation. a. NO(g) + NO2(g) b. heating \(\mathrm{PH}_{3}\) c. \(\mathrm{P}_{4}(s)+5 \mathrm{O}_{2}(g)\) Text Transcription: PH_3 P_4(s) + 5 O_2( g)

Rank the nitrogen ions from the one with N in the highest oxidation state to the one with N in the lowest. \(\mathrm{N}_{3}{ }^{-}, \mathrm{N}_{2} \mathrm{H}_{5}{ }^{+}, \mathrm{NO}_{3}{ }^{-}, \mathrm{NH}_{4}^{+}, \mathrm{NO}_{2}^{-}\) Text Transcription: N_3 -, N_2H_5 +, NO_3 -, NH_4 +, NO_2 -

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. \(3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{HNO}_{3}(l)+\mathrm{NO}(g)\) Text Transcription: 3 NO_2( g) + H_2O(l) longrightarrow 2 HNO_3(l) + NO( g)

Draw the Lewis structures for the phosphorus halides \(\mathrm{PCl}_{3}\) and \(\mathrm{PCl}_{5}\). Describe their VSEPR shape. Text Transcription: PCl_3 PCl_5

Dinitrogen pentoxide is an ionic compound formed from the ions \(\mathrm{NO}_{2}{ }^{+}\) and \(\mathrm{NO}_{3}{ }^{-}\). Give the oxidation state of N in each ion and the VSEPR shape for each of the ions. Text Transcription: NO2 + NO3 -

Ammonium carbonate is produced from the reaction of urea, \(\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2}\) with water. Write a balanced equation for this reaction and determine how much urea is needed to produce 23 g of ammonium carbonate. Text Transcription: CO(NH_2)_2

Explain why phosphine, \(\mathrm{PH}_{3}\), is less polar than ammonia. Text Transcription: PH_3

Reacting oxygen with white phosphorus can form either \(\mathrm{P}_{4} \mathrm{O}_{6}\) or \(\mathrm{P}_{4} \mathrm{O}_{10}\). State the conditions that determine which product forms. Text Transcription: P_4O_6 P_4O_10

\(\mathrm{P}_{4} \mathrm{O}_{10}\) 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 \(\mathrm{SO}_{3}\) Text Transcription: P_4O_10 HNO_3 N_2O_5 H_2SO_4 SO_3

Identify each compound as an oxide, peroxide, or superoxide. a. \(\mathrm{LiO}_{2}\) b. CaO c. \(\mathrm{K}_{2} \mathrm{O}_{2}\) Text Transcription: LiO_2 K_2O_2

Identify each compound as an oxide, peroxide, or superoxide. a. MgO b. \(\mathrm{Na}_{2} \mathrm{O}_{2}\) c. \(\mathrm{CsO}_{2}\) Text Transcription: Na_2O_2 CsO_2

Sulfur dioxide is a toxic sulfur compound. List one natural source and one industrial source that produce \(\mathrm{SO}_{2}\). Text Transcription: SO_2

Calculate the maximum mass (in grams) of each metal sulfide that will dissolve in 1.0 L of a solution that is \(5.00 \times 10^{-5} \mathrm{M}\) in \(\mathrm{Na}_{2} \mathrm{~S}\). a. PbS b. ZnS Text Transcription: 5.00 x 10 - 5 M Na_2S

A coal source contains 1.1% sulfur by mass. If \(2.0 \times 10^{4} \mathrm{~kg}\) of coal is burned and forms oxides, calculate the mass of \(\mathrm{CaSO}_{4}(s)\) that is produced from "scrubbing" the \(\mathrm{SO}_{2}\) pollutant out of the exhaust gas. Assume that all of the sulfur in the coal is converted to calcium sulfate. Text Transcription: 2.0 x 10^4 kg CaSO_4(s) SO_2

Write the equation for roasting iron pyrite in the absence of air to form elemental sulfur. Calculate the volume of \(S_{2}\) 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 \(S_{2}\) gas. (Assume STP to calculate the gas volume.) Text Transcription: S_2

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.) Text Transcription: H_2S

Determine the oxidation state of Xe and give the VSEPR structure for each compound. a. \(\mathrm{XeF}_{2}\) b. \(\mathrm{XeF}_{6}\) c. \(\mathrm{XeOF}_{4}\) Text Transcription: XeF_2 XeF_6 XeOF_4

Describe the shape of each halogen compound. a. \(\mathrm{BrF}_{4}{ }^{-}\) b. \(\mathrm{IF}_{3}\) c. \(\mathrm{BrO}_{2}{ }^{-}\) d. \(\mathrm{ClO}_{4}{ }^{-}\) Text Transcription: BrF4 - IF3 BrO2 - ClO4 -

Carbon tetrachloride is produced by passing chlorine gas over carbon disulfide in the presence of a catalyst. The reaction also produces \(\mathrm{S}_{2} \mathrm{Cl}_{2}\). Write the balanced reaction and identify which element is oxidized and which element is reduced. Text Transcription: S_2Cl_2

If 55 g of \(\mathrm{SiO}_{2}(s)\) 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. Text Transcription: SiO_2(s)

Describe the difference in the types of bonds (single, double, triple) and the shapes of the following two iodine ions: \(\mathrm{ICl}_{4}{ }^{-}\) and \(\mathrm{IO}_{4}{ }^{-}\). Text Transcription: ICl4 - IO4 -

From the compositions of lignite and bituminous coal, calculate the mass of sulfuric acid that could potentially form as acid rain from burning \(1.00 \times 10^{2} \mathrm{~kg}\) of each type of coal. Text Transcription: 1.00 x 10^2 kg

Calculate the volume of \(\mathrm{CO}_{2}\) released from heating and decomposing 88 g of sodium bicarbonate. (Assume standard pressure and temperature.) Text Transcription: CO_2

All of the halogens form oxoacids. The perhalic acids have the general formula of \(\mathrm{HXO}_{4}\). Explain why \(\mathrm{HClO}_{4}\) is a much stronger acid than \(\mathrm{HIO}_{4}\). Text Transcription: HXO_4 HClO_4 HIO_4

The halogens form oxoacids with different amounts of oxygen. Explain why \(\mathrm{HClO}_{4}\) is a stronger acid than \(\mathrm{HClO}_{2}\). Text Transcription: HClO_4 HClO_2

Determine the ratio of effusion rates of HCl compared to each gas. a. \(\mathrm{Cl}_{2}\) b. HF c. HI Text Transcription: CI_2

Calculate the ratio of effusion rates for each pair of gases. a. \({ }^{238} \mathrm{UF}_{6}\) and ClF b. \({ }^{238} \mathrm{UF}_{6}\) and \({ }^{235} \mathrm{UF}_{6}\) Text Transcription: 238UF_6 238UF_6 235UF_6

Sodium peroxide is a very powerful oxidizing agent. Balance the reaction of sodium peroxide with elemental iron to give sodium oxide and \(\mathrm{Fe}_{3} \mathrm{O}_{4}\). Text Transcription: Fe_3O_4

Sulfur dioxide is a reducing agent. When it is bubbled through an aqueous solution containing \(\mathrm{Br}_{2}\), 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. Text Transcription: Br_2

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 \(\mathrm{B}_{6} \mathrm{H}_{6}{ }^{2-}\) 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. \(\mathrm{B}_{4} \mathrm{H}_{4}{ }^{2-}\) b. \(\mathrm{B}_{12} \mathrm{H}_{12}{ }^{2-}\) Text Transcription: B_6H_6 2- B_4H_4 2- B_12H_12 2-

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 \(\Delta H\) of sublimation of diamond from the data in Appendix II, Table B. Then do the calculation using the C-C bond energy in Table 10.3. Suggest a reason for the difference between the two values. Text Transcription: Delta H

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 (\(\mathrm{C}_{8} \mathrm{H}_{18}\), 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 \(40 \mathrm{~m}^{3}\) at 298 K and 1.0 atm. Text Transcription: C_8H_18 40 m^3

Given that the \(\Delta H_{\mathrm{f}}^{\circ}\) of \(1 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{3}\) is -633 kJ, use the data in Appendix II, Table B to calculate the \(\Delta H^{\circ}\) for the formation of a 1 M solution of \(\mathrm{SO}_{2}\) in water from \(\mathrm{SO}_{2}(\mathrm{~g})\). Text Transcription: Delta H_f^circ 1 M H_2SO_3 Delta H^circ SO_2 SO_2( g)

Use the data in Appendix II, Table B to calculate \(\Delta H^{\circ}\) for the formation of a 1 M solution of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from \(\mathrm{SO}_{3}(g)\). Text Transcription: Delta H^circ H_2SO_4 SO_3( g)

Calculate the standard enthalpy of reaction for reducing the different forms of iron oxide to iron metal and \(\mathrm{CO}_{2}\) from the reaction of the oxide with CO. Identify which reaction is the most exothermic per mole of iron and explain why. a. \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) b. FeO c. \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) Text Transcription: CO_2 Fe_3O_4 Fe_2O_3

Balance the equation for the production of acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) 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? Text Transcription: (C_2H_2)

Carbon suboxide, \(\mathrm{C}_{3} \mathrm{O}_{2}\), 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 \(\mathrm{C}_{3} \mathrm{O}_{2}\). 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 \(\left(\mathrm{HO}_{2} \mathrm{CCH}_{2} \mathrm{CO}_{2} \mathrm{H}\right)\). Hint: Each end of malonic acid has a carbon double bonded to an oxygen and to a hydroxide. Text Transcription: C_3O_2 (HO_2CCH_2CO_2H)

When hydrazine is dissolved in water, it acts like a base. \(\mathrm{N}_{2} \mathrm{H}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{N}_{2} \mathrm{H}_{5}^{+}(a q)+\mathrm{OH}^{-}(a q) \\ K_{\mathrm{b}_{1}}=8.5 \times 10^{-7}\) \(\mathrm{N}_{2} \mathrm{H}_{5}^{+}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{N}_{2} \mathrm{H}_{6}^{2+}(a q)+\mathrm{OH}^{-}(a q) \\ K_{\mathrm{b}_{2}}=8.9 \times 10^{-16}\) a. Calculate the \(K_{\mathrm{b}}\) for the overall reaction of hydrazine forming \(\mathrm{N}_{2} \mathrm{H}_{6}{ }^{2+}\). b. Calculate \(K_{\mathrm{a}_{1}}\) for \(\mathrm{N}_{2} \mathrm{H}_{5}{ }^{+}\). 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. Text Transcription: N_2H_4(aq) + H_2O(l) rightleftharpoons N_2H_5 +(aq) + OH-(aq) Kb_1 = 8.5 x 10-7 N_2H_5 +(aq) + H_2O(l) rightleftharpoons N_2H_6 2+(aq) + OH-(aq) Kb_2 = 8.9 * 10-16 K_b N_2H_6 2+ K_a1 N_2H_5 +.

Solid fuel in the booster rockets for spacecraft consists of aluminum powder as the fuel and ammonium perchlorate as the oxidizing agent. \(3 \mathrm{NH}_{4} \mathrm{ClO}_{4}(s)+3 \mathrm{Al}(s) \longrightarrow \\ \mathrm{Al}_{2} \mathrm{O}_{3}(s)+\mathrm{AlCl}_{3}(s)+6 \mathrm{H}_{2} \mathrm{O}(g)+3 \mathrm{NO}(g)\) If a rocket launch burns \(2.200 \times 10^{3} \mathrm{~kg}\) 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. Text Transcription: 3 NH_4ClO_4(s) + 3 Al(s) longrightarrow Al_2O_3(s) + AlCl_3(s) + 6 H_2O( g) + 3 NO( g) 2.200 x 10^3 kg

Two known compounds have the formula \(\mathrm{H}_{2} \mathrm{~N}_{2} \mathrm{O}_{2}\). 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. Text Transcription: H_2N_2O_2

Explain why \(\mathrm{H}_{2} \mathrm{~S}\) has a different bond angle and is much more reactive than \(\mathrm{H}_{2} \mathrm{O}\). Text Transcription: H_2S H_2O

Explain why \(\mathrm{SO}_{2}\) is used as a reducing agent but \(\mathrm{SO}_{3}\) is not. Text Transcription: SO_2 SO_3

Explain why the interhalogen molecule \(\mathrm{BrCl}_{3}\) exists but \(\mathrm{ClBr}_{3}\) does not. Text Transcription: BrCl_3 ClBr_3

As a group, create a single schematic drawing of a factory that uses the Haber-Bosch process and the Ostwald process to make \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) fertilizer. The factory may only take in \(\mathrm{N}_{2}(g), \mathrm{H}_{2}(g)\), and \(\mathrm{O}_{2}(g)\). Pass your diagram around the group and have each group member add one step in the process. Where might the factory obtain \(\mathrm{H}_{2}\) ? Text Transcription: NH_4NO_3 N2( g), H2( g) O2( g) H_2

Hydrogen sulfide \(\left(\mathrm{H}_{2} \mathrm{~S}\right)\) smells like rotten eggs; its smell can be detected at concentrations as low as 0.02 ppm. Well water, which is drawn from underground depths of 30-250 meters (100-800 feet), is sometimes contaminated with hydrogen sulfide. The contamination arises from bacterial decomposition of sulfur-containing organic and inorganic matter present in the oxygen-deficient underground environment. Some \(\mathrm{H}_{2} \mathrm{~S}\) gas dissolves in the water that is pumped for drinking supplies, where it is detected by taste at concentrations as low as 0.05 ppm. Municipalities remove \(\mathrm{H}_{2} \mathrm{~S}\) to improve water taste and to prevent the accumulation of toxic \(\mathrm{H}_{2} \mathrm{~S}\) gas within the system. The first table that follows lists hydrogen sulfide solubility in water when the partial pressure of hydrogen sulfide is 1.00 atm. The second table lists solubility product constant data for common metal sulfides. Use the information provided in the tables to answer the following questions: a. What can you conclude about the temperature dependence of \(\mathrm{H}_{2} \mathrm{~S}\) solubility in water? b. Suppose that water analysis indicates that your well's water contains \(1.8 \mathrm{mg} \ \mathrm{H}_{2} \mathrm{~S}\) per liter of well water. Using Henry's law (Chapter 14) and the data in the first table, calculate the partial pressure of \(\mathrm{H}_{2} \mathrm{~S}\), in atm, that exists above your well water at \(25{ }^{\circ} \mathrm{C}\). (Assume the well water is in a closed container). c. Air containing \(\mathrm{H}_{2} \mathrm{~S}\) at 20 ppm (by volume) and below is considered safe to breathe. Is the air above the solution in part b safe to breathe? (The total pressure is 1.00 atm.) d. A water technician recommends that you treat your well water with hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\), in order to convert \(\mathrm{H}_{2} \mathrm{~S}\) to sulfate (which does not have an offensive odor or taste), according to the following unbalanced reaction: \(\mathrm{H}_{2} \mathrm{O}_{2}(a q)+\mathrm{H}_{2} \mathrm{~S}(a q) \longrightarrow \mathrm{SO}_{4}{ }^{2-}(a q)+\mathrm{H}^{+}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) What volume of a 3.0% by mass solution of hydrogen peroxide is required to treat 955 liters of your well water? (Assume that no other species are present to react with the \(\mathrm{H}_{2} \mathrm{O}_{2}\) and that the density of the hydrogen peroxide solution is 1.0 g/mL.) e. Hydrogen sulfide is a weak diprotic acid that ionizes in water to form hydrogen sulfide \(\left(\mathrm{HS}^{-}\right)\) and sulfide \(\left(\mathrm{S}^{2-}\right)\). Sulfide dissolved in water can be precipitated as an insoluble metal sulfide, according to the following reaction: \(\mathrm{M}^{2+}(a q)+\mathrm{S}^{2-}(a q) \longrightarrow \mathrm{MS}(s)\) Which metal in the second table most effectively removes hydrogen sulfide from water? f. What volume, in mL, of a 0.500 M solution of the metal ion you chose in part e is required to remove the hydrogen sulfide present in 955 liters of your well water (from part b)? g. What mass, in grams, of the metal sulfide (from part f) precipitates? (Assume 100\% yield.) Text Transcription: (H_2S) H_2S 25^circ C H_2O_2 H_2O_2(aq) + H_2S(aq) longrightarrow SO_4 2-(aq) + H+ (aq) + H_2O(l) (HS - ) (S2-) M2 + (aq) + S2-(aq) longrightarrow MS(s)

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

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

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

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

What is the difference between a rock and a mineral?

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

Why is boron oxide often added to silica glass?

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

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

What is the typical concentration of oxygen in dry air?

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

Earth’s atmosphere originally did not contain oxygen. Explain how the atmosphere gained oxygen.

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

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

Describe how boron is used in the nuclear industry.

Describe the difference between regular charcoal and activated charcoal.

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

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

Explain the process of fixing nitrogen.

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

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

Describe how red and black phosphorus are made from white phosphorus.

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

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

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

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

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

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.

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?

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

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.

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

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.

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

Have each group member select a different element from this list: B, C, N, O, and F. Have all group members look up the following values for their elements: valence electron configuration, covalent atomic radius, effective nuclear charge, first ionization energy, and Pauling electronegativity. All members should compare the values for their elements with those of the group. Repeat with O, S, Se, Te, and Po. Account for the trends you see by referring to quantum-mechanical shells. Note and provide a tentative explanation for any exceptions to trends you observe.

Provide a detailed chemical description of your birthstone or favorite gem. If two members of the group share a birthstone, have one select another gem, so that no two group members work with the same gem. Is your gem a silicate? What type? Share your findings with your group. Does your group agree on which gem has the most interesting structure?

Ask each group member to work individually to write out two or three reactions from one section of the chapter. Replace the symbol for the element that is the topic of that section with a blank or an X. Take turns playing “identify the mystery element” as follows. One person shares his or her reactions (with the blanks) with the group. The person to the right of the person sharing tries to identify the missing element. If that person can’t, the group member to the right tries. Continue until either the element has been identified or all group members have had a chance. The next round starts with the person who was first to guess the element sharing reactions with the group. Continue until all have shared reactions and all reactions have been correctly identified.

Working individually, find a sentence in the chapter that uniquely describes a particular main-group compound. As in the previous question, take turns reading your sentences to the group saying “blank” in place of the name of the compound and giving group members a chance to identify the compound.