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Chemistry The Central Science 12th edition Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward - Solutions

Write a balanced equation for each of the following reactions: (a) Sulfur dioxide reacts with water. (b) Solid zinc sulfide reacts with hydrochloric acid. (c) Elemental sulfur reacts with sulfite ion to form thiosulfate. (d) Sulfur trioxide is dissolved in sulfuric acid.
Write the molecular formula and Lewis structure for each of the following oxides of nitrogen:
Write a balanced equation for each of the following reactions. (You may have to guess at one or more of the reaction products, but you should be able to make a reasonable guess, based on your study of this chapter.)
Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) Sodium nitrite (b) Ammonia (c) Nitrous oxide (d) Sodium cyanide (e) Nitric acid (f) Nitrogen dioxide (g) Nitrogen (h) Boron nitride.
Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) Nitric oxide (b) Hydrazine (c) Potassium cyanide (d) Sodium nitrite (e) Ammonium chloride (f) Lithium nitride.
Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: (a) HNO2 (b) N3- (c) N2H5+ (d) NO3-
Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: (a) NH4+ (b) NO2- (c) N2O (d) NO2.
Complete and balance the following equations: (a) Mg3N2(s) + H2O(l) → (b) NO(g) + O2(g) → (c) N2O5(g) + H2O(l) → (d) NH3(aq) + H+ (aq) → (e) N2H4(l) + O2(g) → Which ones of these are redox reactions?
Write a balanced net ionic equation for each of the following reactions: (a) Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. (b) Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. (c) Concentrated nitric acid oxidizes sulfur dioxide with
Write complete balanced half-reactions for (a) oxidation of nitrous acid to nitrate ion in acidic solution, (b) oxidation of N2 to N2O in acidic solution.
Write a molecular formula for each compound, and indicate the oxidation state of the group 5A element in each formula: (a) Phosphorous acid (b) Pyrophosphoric acid (c) Antimony trichloride (d) Magnesium arsenide (e) Diphosphorus pentoxide (f) Sodium phosphate.
Which property of the group 6A elements might be the one depicted in the graph shown here:(a) Electronegativity(b) First ionization energy(c) Density(d) X-X single-bond enthalpy(e) Electron affinity? Explain your answer.
Write a chemical formula for each compound or ion, and indicate the oxidation state of the group 5A element in each formula: (a) Phosphate ion (b) Arsenous acid (c) Antimony(III) sulfide (d) Calcium dihydrogen phosphate (e) Potassium phosphide (f) Gallium arsenide.
Account for the following observations: (a) Phosphorus forms a pentachloride, but nitrogen does not. (b) H3PO2 is a monoprotic acid.
Account for the following observations: (a) H3PO3 is a diprotic acid. (b) Nitric acid is a strong acid, whereas phosphoric acid is weak. (c) Phosphate rock is ineffective as a phosphate fertilizer. (d) Phosphorus does not exist at room temperature as diatomic molecules, but nitrogen does.
Write a balanced equation for each of the following reactions:(a) Preparation of white phosphorus from calcium phosphate,(b) Hydrolysis of PBr3(c) Reduction of PBr3 to P4 in the gas phase, using H2.
Write a balanced equation for each of the following reactions:(a) Hydrolysis of PCl5(b) Dehydration of phosphoric acid (also called orthophosphoric acid) to form pyrophosphoric acid,(c) Reaction of P4O10 with water.
Give the chemical formula for (a) Hydrocyanic acid (b) Nickel tetracarbonyl (c) Barium bicarbonate (d) Calcium acetylide (e) Potassium carbonate.
Give the chemical formula for (a) Carbonic acid (b) Sodium cyanide (c) Potassium hydrogen carbonate (d) Acetylene (e) Iron pentacarbonyl.
Complete and balance the following equations:(b) BaC2(s) + H2O(l) †’(c) C2H2(g) + O2(g) †’(d) CS2(g) + O2(g) †’(e) Ca(CN)2(s) + HBr(aq) †’
Complete and balance the following equations:(a) CO2(g) + OH- (aq) †’(b) NaHCO3(s) + H+(aq) †’(e) CuO(s) + CO(g) †’
Write a balanced equation for each of the following reactions:(a) Hydrogen cyanide is formed commercially by passing a mixture of methane, ammonia, and air over a catalyst at 800°C.Water is a by-product of the reaction.(b) Baking soda reacts with acids to produce carbon dioxide gas.(c) When barium
The atomic and ionic radii of the first three group 6A elements are(a) Explain why the atomic radius increases in moving downward in the group. (b) Explain why the ionic radii are larger than the atomic radii. (c) Which of the three anions would you expect to be the strongest base in water? Explain.
Write a balanced equation for each of the following reactions:(a) Burning magnesium metal in a carbon dioxide atmosphere reduces the CO2 to carbon.(b) In photosynthesis, solar energy is used to produce glucose (C6H12O6) and O2 from carbon dioxide and water.(c) When carbonate salts dissolve in
Write the formulas for the following compounds, and indicate the oxidation state of the group 4A element or of boron in each: (a) Boric acid (b) Silicon tetrabromide (c) Lead(II) chloride (d) Sodium tetraborate decahydrate (borax) (e) Boric oxide (f) Germanium dioxide.
Write the formulas for the following compounds, and indicate the oxidation state of the group 4A element or of boron in each: (a) Silicon dioxide (b) Germanium tetrachloride (c) Sodium borohydride (d) Stannous chloride (e) Diborane (f) Boron trichloride.
Select the member of group 4A that best fits each description: (a) Has the lowest first ionization energy (b) Is found in oxidation states ranging from -4 to +4 (c) Is most abundant in Earth's crust.
(a) What is the characteristic geometry about silicon in all silicate minerals? (b) Metasilicic acid has the empirical formula H2SiO3.Which of the structures shown in Figure 22.34 would you expect metasilicic acid to have?
Speculate as to why carbon forms carbonate rather than silicate analogs.
(a) How does the structure of diborane (B2H6) differ from that of ethane (C2H6)? (b) Explain why diborane adopts the geometry that it does. (c) What is the significance of the statement that the hydrogen atoms in diborane are described as "hydridic"?
Write a balanced equation for each of the following reactions:(a) Diborane reacts with water to form boric acid and molecular hydrogen.(b) Upon heating, boric acid undergoes a condensation reaction to form tetraboric acid.
In your own words, define the following terms: (a) Allotrope (b) Disproportionation (c) Interhalogen (d) Acidic anhydride (e) Condensation reaction (f) Protium.
Which property of the third-row nonmetallic elements might be the one depicted in the graph on the next page:(a) First ionization energy(b) Atomic radius(c) Electronegativity(d) Melting point(e) X-X single-bond enthalpy? Explain both your choice and why the other choices would not be correct.
Although the CIO4- and IO4- ions have been known for a long time, BrO4- was not synthesized until 1965. The ion was synthesized by oxidizing the bromate ion with xenon difluoride, producing xenon, hydrofluoric acid, and the perbromate ion. (a) Write the balanced equation for this reaction. (b) What
Write a balanced equation for the reaction of each of the following compounds with water: (a) SO2(g) (b) Cl2O7(g) (c) Na2O2(s) (d) BaC2(s) (e) RbO2(s) (f) Mg3N2(s) (g) NaH(s).
What is the anhydride for each of the following acids: (a) H2SO4 (b) HClO3 (c) HNO2 (d) H2CO3 (e) H3PO4?
Explain why SO2 can be used as a reducing agent but SO3 cannot.
A sulfuric acid plant produces a considerable amount of heat. This heat is used to generate electricity, which helps reduce operating costs. The synthesis of H2SO4 consists of three main chemical processes: (1) Oxidation of S to SO2 (2) Oxidation of SO2 to SO3 (3) The dissolving of SO3 in H2SO4 and
(a) What is the oxidation state of P in PO43- and of N in NO3-? (b) Why doesn't N form a stable NO43- ion analogous to P?
(a) The P4, P4O6, and P4O10 molecules have a common structural feature of four P atoms arranged in a tetrahedron (Figures 22.27 and 22.28). Does this mean that the bonding between the P atoms is the same in all these cases? Explain. (b) Sodium trimetaphosphate (Na3P3O9) and sodium
Ultrapure germanium, like silicon, is used in semiconductors. Germanium of "ordinary" purity is prepared by the hightemperature reduction of GeO2 with carbon. The Ge is converted to GeCl4 by treatment with Cl2 and then purified by distillation; GeCl4 is then hydrolyzed in water to GeO2 and reduced
Hydrogen peroxide is capable of oxidizing (a) Hydrazine to N2 and H2O (b) SO2 to SO42- (c) NO2- to NO3- (d) H2S(g) to S(s) (e) Fe2+ to Fe3+. Write a balanced net ionic equation for each of these redox reactions.
(a) How many grams of H2 can be stored in 100.0 kg of the alloy FeTi if the hydride FeTiH2 is formed? (b) What volume does this quantity of H2 occupy at STP? (c) If this quantity of hydrogen was combusted in air to produce liquid water, how much energy could be produced?
Which of the following compounds would you expect to be the most generally reactive, and why?
Using the thermochemical data in Table 22.1 and Appendix C, calculate the average Xe-F bond enthalpies in XeF2, XeF4, and XeF6, respectively. What is the significance of the trend in these quantities?
Hydrogen gas has a higher fuel value than natural gas on a mass basis but not on a volume basis. Thus, hydrogen is not competitive with natural gas as a fuel transported long distances through pipelines. Calculate the heats of combustion of H2 and CH4 (the principal component of natural gas) (a)
The solubility of Cl2 in 100 g of water at STP is 310 cm3. Assume that this quantity of Cl2 is dissolved and equilibrated as follows:(a) If the equilibrium constant for this reaction is 4.7 Ã— 10-4, calculate the equilibrium concentration of HClO formed.
When ammonium perchlorate decomposes thermally, the products of the reaction are N2(g),O2(g),H2O(g), and HCl(g).(a) Write a balanced equation for the reaction.(b) Calculate the enthalpy change in the reaction per mole of NH4ClO4. The standard enthalpy of formation of NH4ClO4(s) is -295.8 kJ.(c)
The dissolved oxygen present in any highly pressurized, hightemperature steam boiler can be extremely corrosive to its metal parts. Hydrazine, which is completely miscible with water, can be added to remove oxygen by reacting with it to form nitrogen and water. (a) Write the balanced equation for
One method proposed for removing SO2 from the flue gases of power plants involves reaction with aqueous H2S. Elemental sulfur is the product. (a) Write a balanced chemical equation for the reaction. (b) What volume of H2S at and 760 torr would be required to remove the SO2 formed by burning 2.0
The maximum allowable concentration of H2S(g) in air is 20 mg per kilogram of air (20 ppm by mass). How many grams of FeS would be required to react with hydrochloric acid to produce this concentration at 1.00 atm and in an average room measuring 12 ft × 20 ft × 8 ft? (Under these conditions, the
The standard heats of formation of H2O(g), H2S(g), H2Se(g), and H2Te(g) are -241.8, -20.17, +29.7, and +99.6 kJ/mol, respectively. The enthalpies necessary to convert the elements in their standard states to one mole of gaseous atoms are 248, 277, 227, and 197 kJ/mol of atoms for O, S, Se, and Te,
Manganese silicide has the empirical formula MnSi and melts at 1280°C. It is insoluble in water but does dissolve in aqueous HF. (a) What type of compound do you expect MnSi to be: metallic, molecular, covalent-network, or ionic? (b) Write a likely balanced chemical equation for the reaction of
Chemists tried for a long time to make molecular compounds containing silicon-silicon double bonds; they finally succeed in 1981. The trick is having large, bulky R groups on the silicon atoms to make R2Si = SiR2 compounds. What experiments could you do to prove that a new compound has a
This chart shows the variation in an important property of the metals from K through Ge. Is the property atomic radius, electronegativity, or first ionization energy? Explain your choice. [Section 23.1]
Two Fe(II) complexes are both low spin but have different ligands. A solution of one is green and a solution of the other is red. Which solution is likely to contain the complex that has the stronger-field ligand? [Section 23.6]
Explain the lanthanide contraction, and describe how it affects the properties of the transition-metal elements.
Sketch a plot of atomic radius versus number of valence d electrons for the period 5 transition metals, and explain the trend.
The oxidation state is common for almost all the transition metals. Suggest an explanation.
No compounds are known in which scandium is in the oxidation state. Suggest an explanation.
Write out the ground-state electron configurations of (a)Ti3+, (b) Ru2+ (c) Au3+, (d) Mn4+.
How many electrons are in the valence d orbitals in these transition-metal ions? (a) Co3+, (b) Cu+, (c) Cd2+, (d) Os3+,.
Explain the difference between a diamagnetic substance and a paramagnetic substance.
Distinguish among a ferromagnetic substance, an antiferromagnetic substance, and a ferrimagnetic substance.
What kind of magnetism is exhibited by this diagram:
(a) Draw the structure for Pt(en)Cl2. (b)What is the coordination number for platinum in this complex, and what is the coordination geometry? (c) What is the oxidation state of the platinum? [Section 23.2]
The most important oxides of iron are magnetite,Fe3O4,and hematite,Fe 3O4 (a) What are the oxidation states of iron in these compounds? (b) One of these iron oxides is ferrimagnetic, and the other is antiferromagnetic.Which iron oxide islikely to show which type of magnetism? Explain.
(a) What is the difference between Werner's concepts of primary valence and secondary valence? What terms do we now use for these concepts? (b) Why can the NH3 molecule serve as a ligand but the BH3 molecule cannot?
(a) What is the meaning of the term coordination number as it applies to metal complexes? (b) Give an example of a ligand that is neutral and one that is negatively charged. (c) Would you expect ligands that are positively charged to be common? = Explain. (d) What type of chemical bonding is
A complex is written as NiBr2.6NH3 (a) What is the oxidation state of the Ni atom in this complex? (b) What is the likely coordination number for the complex? (c) If the complex is treated with excess AgNO3(aq), how many moles of AgBr will precipitate per mole of complex?
A certain complex of metal M is formulated as MCl3.3H2O. The coordination number of the complex is not known but is expected to be 4 or 6. (a) Would conductivity measurements provide information about the coordination number? (b) In using conductivity measurements to test which ligands arebound
Indicate the coordination number of the metal and the oxidation number of the metal as well as the number and type of each donor atom of the ligands for each of the following complexes: (a) Na2[CdCl4] (b) K2[MoOCl4] (c) [Co(NH3) 4Cl2]Cl (d) [Ni(CN)5]3- (e) K3[V(C2O4)3] (f) [Zn(en)2]Br2
Indicate the coordination number of the metal and the oxidation number of the metal as well as the number and type of each donor atom of the ligands for each of the following complexes: (a) K3[Co(CN)6] (b) Na2[CdBr4] (c) [Pt(en)3](ClO4)4 (d) [Co(en)2(C2O4)+ (e) NH4[Cr(NH3)2(NCS)4] (f) [Cu(bipy)2 I]I
(a) What is the difference between a monodentate ligand and a bidentate ligand? (b) How many bidentate ligands are necessary to fill the coordination sphere of a six-coordinate complex? (c) You are told that a certain molecule can serve as a tridentate ligand. Based on this statement, what do you
For each of the following polydentate ligands, determine (i) the maximum number of coordination sites that the ligand can occupy on a single metal ion and (ii) the number and type of donor atoms in the ligand: (a) Ethylenediamine (en), (b) Bipyridine (bipy), (c) The oxalate anion (C2O4 2-) (d)
Polydentate ligands can vary in the number of coordination positions they occupy. In each of the following, identify the polydentate ligand present and indicate the probable number of coordination positions it occupies: (a) [Co(NH3)4 (o-phen)]Cl3 (b) [Cr (C2O4) (H2O)4]Br (c) [Cr[DATA)(H2O] (d)
Draw the Lewis structure for the ligand shown in the next column.Which atoms can serve as donor atoms? Classify this ligand as monodentate, bidentate, or tridentate.How many of these ligands are needed to fill the coordination sphere in an octahedral complex? [Section 23.2]NH2CH2CH2NHCH2CO2
(a) What is meant by the term chelate effect? (b)What thermodynamic factor is generally responsible for the chelate effect? (c) Why are polydentate ligands often called sequestering agents?
Pyridine (C5H5N), abbreviated py, is the molecule(a) Why is pyridine referred to as a monodentate ligand? (b) For the equilibrium reaction what would you predict for the magnitude of the equilibrium constant? Explain your answer.
Is the following ligand a chelating one? Explain.
What is the geometry about the metal center in this complex? Would you expect this complex to have counterions? Explain.
Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) Hexaamminechromium (III) nitrate (b) Tetraamminecarbonatocobalt (III) sulfate (c) Dichlorobis (ethylenediamine) platinum(IV) bromide (d) Potassium diaquatetrabromovanadate
Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) Tetraaquadibromomanganese(III) perchlorate (b) Bis(bipyridyl)cadmium(II) chloride (c) Potassium tetrabromo(ortho-phenanthroline)- cobaltate (III) (d) Cesium
Write the names of the following compounds, using the standardnomenclature rules for coordination complexes: (a) [Rh(NH3)4Cl2]Cl (b) K2[TiCl6] (c) MoOCl4 (d) [Pt(H2O)4(C2O4)]Br2
Write names for the following coordination compounds: (a) [Cd(en)Cl2] (b) K4[Mn(CN)6] (c) [Cr(NH3)5CO3]Cl (d) [Ir(NH3)4(H2O)2](NO3)3
By writing formulas or drawing structures related to any one of these three complexes, [Co(NH3) 4Br2]Cl [Pd(NH3)2(ONO)2] cis- [V(en)2C12]+, illustrate (a) Geometric isomerism, (b) Linkage isomerism, (c) Optical isomerism, (d) Coordination-sphere isomerism.
The complex ion shown here has a charge. Name the complex ion. [Section 23.4]
(a) Draw the two linkage isomers of [Co (NH3)5SCN]2+ (b) Draw the two geometric isomers of [Co (NH3)5IC3]2+ (c) Two compounds with the formula Co(NH3)5ClBr can be prepared. Use structural formulas to show how they differ. What kind of isomerism does this illustrate?
A four-coordinate complex MA2B2 is prepared and found to have two different isomers. Is it possible to determine from this information whether the complex is square planar or tetrahedral? If so, which is it?
Consider an octahedral complex MA3B3. How many geometric isomers are expected for this compound? Will any of the isomers be optically active? If so, which ones?
Sketch all the possible stereoisomers of (a) Tetrahedral [Cd(H2O)2Cl2], (b) Square-planar [IrCI2(PH3)2]- , (c) Octahedral [Fe(o-phen) 2CI2]+,
Sketch all the possible stereoisomers of (a) [Rh(bipy)(o-phen)2]3+, (b) [Co(NH3)3 (bipy)Br]2+ (c) square-planar [Pd(en)(CN)2].
(a) Can we see light that is 300 nm in wavelength? 500 nm in wavelength? (b) What is meant by the term complementary color? (c)What is the significance of complementary colors in understanding the colors of metal complexes? (d) If a complex absorbs light at 610 nm, what is the energy of this
(a) A complex absorbs light in the range of 200-300 nm. Do you expect it to have visible color?
A compound whose empirical formula is XF3 consists of 65% F by mass.What is the atomic mass of X?
The compound XCl4 contains 75.0% Cl by mass.What is the element X?
What is the molecular formula of each of the following compounds? (a) Empirical formula CH2,molsr mass = 84g/mol (b) Empirical formula NH2Cl,molar mass = 51.5 g /mol
There are two geometric isomers of octahedral complexes of the type MA3X3 , where M is a metal and A and X are monodentate ligands. Of the complexes shown here, which are identical to (1) and which are the geometric isomers of (1)? [Section 23.4]
What is the molecular formula of each of the following compounds? (a) Empirical formula HCO2, molar mass = 90.0g / mol (b) Empirical formula C2H4O, molar mass = 88g / mol
Determine the empirical and molecular formulas of each of the following substances:(a) Styrene, a compound substance used to make Styrofoam® cups and insulation, contains 92.3% C and 7.7% H by mass and has a molar mass of 104 g>mol.(b) Caffeine, a stimulant found in coffee, contains 49.5% C,

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