Problem 1E: How do alkali metals differ from alkaline each metals in atomic structure and general properties? Problem 2E: Why does the reactivity of the alkali metals decrease from cesium to lithium? Problem 3E: Predict the formulas for the nine compounds that may form when each species in column 1 of Table... Problem 4E: Predict the best choice in each of the following. You may wish to review the Chapter on electronic... Problem 5E: Sodium chloride and strontium chloride are both white solids. How could you distinguish one from the... Problem 6E: The reaction of quicklime, CaO, with water produces slaked lime, Ca(OH)2, which is widely used in... Problem 7E: Write a balanced equation for the reaction of elemental strontium with each of the following: (a)... Problem 8E: How many moles of ionic species are present in 1.0 L of a solution marked 1.0 M mercury(I) nitrate? Problem 9E: What is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of... Problem 10E: The elements sodium, aluminum, and chlorine are in the same period.. (a) Which has the greatest... Problem 11E: Does metallic tin react with HCl? Problem 12E: What is tin pest, also Known as tin disease? Problem 13E: Compare the nature of the bonds in PbCl2 to that of the bonds in PbCl4. Problem 14E: Is the reaction of rubidium with water more or less Vigorous than that of sodium? How does the rate... Problem 15E: Write an equation for the reduction of cesium chloride by elemental calcium at high temperature. Problem 16E: Why is it necessary to keep the chlorine and sodium, resulting from the electrolysis of sodium... Problem 17E: Give balanced equations for the overall reaction in the electrolysis of molten lithium chloride and... Problem 18E: The electrolysis of molten sodium chloride or of aqueous sodium chloride produces chlorine.... Problem 19E: What mass, in grams, of hydrogen gas forms during the complete reaction of 10.01 g of calcium with... Problem 20E: How many grams of oxygen gas are necessary to react completely with 3.011021 atoms of magnesium to... Problem 21E: Magnesium is an active metal; it bums in the form of powder, ribbons, and filaments to provide... Problem 22E: Why is it possible for an active metal like aluminum to be useful as a structural metal? Problem 23E: Describe the production of metallic aluminum by electrolytic reduction. Problem 24E: What is the common are of tin and how is tin separated from it? Problem 25E: A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric... Problem 26E: Consider the production of 100 kg of sodium metal using a current of 50,000 A, assuming a 100%... Problem 27E: What mass of magnesium forms when 100,000 A is passed through a MgCl2 melt for 1.00 h if the yield... Problem 28E: Give the hybridization of the metalloid and the molecular geometry for each of the following... Problem 29E: Write a Lewis structure for each of the following molecules or ions. You may wish to review the... Problem 30E: Describe the hybridization of boron and the molecular structure about the boron in each of the... Problem 31E: Using only the periodic table, write the complete electron configuration for silicon, including any... Problem 32E: Write a Lewis structure for each of the following molecules and ions: (a) (CH3)3SiH (b) SiO44- (C)... Problem 33E: Describe the hybridization of silicon and the molecular structure of the following molecules and... Problem 34E: Describe the hybridization and the bonding of a silicon atom in elemental silicon. Problem 35E: Classify each of the following molecules as polar or nonpolar. You may wish to review the chapter on... Problem 36E: Silicon reacts with sulfur at elevated temperatures. If 0.0923 g of silicon reacts with sulfur to... Problem 37E: Name each of the fallowing compounds: (a) TeO2 (b) Sb2S3 (C) GeF4 (d) SiH4 (e) GeH4 Problem 38E: Write a balanced equation for the reaction of elemental boron with each of the following (most of... Problem 39E: Why is boron limited to a maximum coordination number of four in its compounds? Problem 40E: Write a formula for each of the following compounds: (a) silicon dioxide (b) silicon tetraiodide (c)... Problem 41E: From the data given in Appendix I, determine the standard enthalpy change and the standard free... Problem 42E: A hydride of silicon prepared by the reaction of Mg2Si with acid exerted a pressure of 306 torr at... Problem 43E: Suppose you discovered a diamond completely encased in a silicate rock. How would you chemically... Problem 44E: Carbon forms a number of allotropes, two of which are graphite and diamond. Silicon has a diamond... Problem 45E: Nitrogen in the atmosphere exists as very stable diatomic molecules. Why does phosphorus form less... Problem 46E: Write balanced chemical equations for the reaction of the following acid anhydrides with water: (a)... Problem 47E: Determine the oxidation number of each element in each of the following compounds: (a) HCN (b) OF2... Problem 48E: Determine the oxidation state of sulfur in each of the following: (a) SO3 (b) SO2 (C) SO32- Problem 49E: Arrange the following in order of increasing electronegativity: F; Cl; O; and S. Problem 50E: Why does white phosphorus consist of tetrahedral P4 molecules while nitrogen consists of diatomic N2... Problem 51E: Why does hydrogen- not exhibit an oxidation state of 1- when bonded to nonmetals? Problem 52E: The reaction of calcium hydride, CaH2, with water can be characterized as a Lewis acid-base... Problem 53E: In drawing Lewis structures, we learn that a hydrogen atom forms only one bond in a covalent... Problem 54E: What mass of CaH2 is necessary to react with water to provide enough hydrogen gas to fill a balloon... Problem 55E: What mass of hydrogen gas results from the reaction of 8.5 g of KH with water?. KH+H2OKOH+H2 Problem 56E: Carbon forms the CO32- ion, yet silicon does not form an analogous SiO3-2 ion. Why? Problem 57E: Complete and balance the following chemical equations: (a) hardening of plaster containing slaked... Problem 58E: Heating a sample of Na2CO3xH2O weighing 4.640 g until the removal of the water of hydration leaves... Problem 59E: Write the Lewis structures for each of the following: (a) NH2- (b) N2F4 (c) NH2- (d) NF3 (e) N3- Problem 60E: For each of the following, indicate the hybridization of the nitrogen atom (for N3-. the central... Problem 61E: Explain how ammonia can function both as a Bronsted base and as a Lewis base. Problem 62E: Determine the oxidation state of nitrogen in each of the following. You may wish to review the... Problem 63E: For each of the following draw the Lewis structure, predict the ONO bond angle, and give the... Problem 64E: How many grams of gaseous ammonia will the reaction of 3.0 g hydrogen gas and 3.0 g of nitrogen gas... Problem 65E: Although PF5 and ASF5 are stable, nitrogen does not form NF5 molecules. Explain this difference... Problem 66E: The equivalence point for the titration of a 25.00-mL sample of CSOH solution with 0.1062 M HNO3 is... Problem 67E: Write the Lewis structure for each of the following. You may wish to review the chapter on chemical... Problem 68E: Describe the molecular structure of each of the following molecules or ions listed. You may Wish to... Problem 69E: Complete and balance each of the following chemical equations. (In some cases, there may be more... Problem 70E: Describe the hybridization of phosphorus in each of the following compounds: P4O10, P4O6, PH4l (an... Problem 71E: What volume of 0.200 M NaOH is necessary to neutralize the solution produced by dissolving 2.00 g of... Problem 72E: How much POCl3 can form from 25.0 g of PCl5 and the appropriate amount of H2O? Problem 73E: How many tons of Ca3(PO4)2 are necessary to prepare 5.0 tons of phosphorus if the yield is 90%? Problem 74E: Write equations showing the stepwise ionization of phosphorous acid. Problem 75E: Draw the Lewis structures and describe the geometry for the following: (a) PF4+ (b) FF5 (c) PF6- (d)... Problem 76E: Why does phosphorous acid form only two series of salts, even though the molecule contains three... Problem 77E: Assign an oxidation state to phosphorus in each of the following: (a) NaH2PO3 (b) PF5 (c) P4O6 (d)... Problem 78E: Phosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of... Problem 79E: Predict the product of burning francium in air. Problem 80E: Using equations, describe the reaction of water with potassium and with potassium oxide. Problem 81E: Write balanced chemical equations for the following reactions: (a) zinc metal heated in a stream of... Problem 82E: Write balanced chemical equations for the following reactions: (a) cadmium burned in air. (b)... Problem 83E: Illustrate the amphoteric nature of aluminum hydroxide by citing suitable equations. Problem 84E: Write balanced chemical equations for the following reactions: (a) metallic aluminum burned in air... Problem 85E: Write balanced chemical equations for the following reactions: (a) sodium oxide added to water (b)... Problem 86E: What volume of 0.250 M H2SO4 solution is required to neutralize a solution that contains 5.00 g of... Problem 87E: Which is the stronger acid, HClO4 or HBrO4? Why? Problem 88E: Write a balanced chemical equation for the reaction of an excess of oxygen with each of the... Problem 89E: Which is the stronger acid, H2SO4 or H2SeO4? Why? You may wish to review the Chapter on acid-base... Problem 90E: Explain why hydrogen sulfide is a gas at room temperature, whereas water, which has a lower... Problem 91E: Give the hybridization and oxidation state for sulfur in SO2, in SO3, and in H2SO4. Problem 92E: Which is the stronger acid, NaHSO3 or NaHSO4? Problem 93E: Determine the oxidation state of sulfur in SF6, SO2F2, and KHS. Problem 94E: Which is a stronger acid, sulfurous acid or sulfuric acid? Why? Problem 95E: Oxygen forms double bonds in O2, but sulfur forms single bonds in S8. Why? Problem 96E: Give the Lewis structure of each of the following: (a) SF4 (b) K2SO4 (c) SO2Cl2 (d) H2SO3 (e) SO3 Problem 97E: Write two balanced chemical equations in which sulfuric acid acts as an oxidizing agent. Problem 98E: Explain why sulfuric acid, H2SO4, which is a covalent molecule, dissolves in water and produces a... Problem 99E: How many grams of Epsom salts (MgSO47H2O) will form from 5.0 kg of magnesium? Problem 100E: What does it mean to say that mercury (II) halides are weak electrolytes? Problem 101E: Why is SnCl4 not classified as a salt? Problem 102E: The following reactions are all similar to those of the industrial chemicals. Complete and balance... Problem 103E: Which is the stronger acid, HClO3 or HBrO3? Why? Problem 104E: What is the hybridization of iodine in IF3 and IF5? Problem 105E: Predict the molecular geometries and draw Lewis structures for each of the following. You may wish... Problem 106E: Which halogen has the highest ionization energy? Is this what you would predict based on what you... Problem 107E: Name each of the following compounds: (a) BrF3. (b) NaBrO3. (c) PBr5. (d) NaClO4. (e) KClO Problem 108E: Explain why, at room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine... Problem 109E: What is the oxidation state of the halogen in each of the following?. (a) H5IO6. (b) IO4-. (c) ClO2.... Problem 110E: Physiological saline concentration—that is, the sodium chloride concentration in our bodies—is... Problem 111E: Give the hybridization of xenon in each of the following. You may wish to review the chapter on the... Problem 112E: What is the molecular structure of each of the following molecules? You may wish to review the... Problem 113E: Indicate whether each of the following molecules is polar or nonpolar. You may wish to review the... Problem 114E: What is the oxidation state of the noble gas in each of the following? You may wish to review the... Problem 115E: A mixture of xenon and ?uorine was heated. A sample of the white solid that formed reacted with... Problem 116E: Basic solutions of Na4XeO6, are powerful oxidants. What mass of Mn(NO3)26H2O reacts with 125.0 mL of... format_list_bulleted