Chemistry by OpenStax (2015-05-04) 1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
1 Essential Ideas 2 Atoms, Molecules, And Ions 3 Composition Of Substances And Solutions 4 Stoichiometry Of Chemical Reactions 5 Thermochemistry 6 Electronic Structure And Periodic Properties Of Elements 7 Chemical Bonding And Molecular Geometry 8 Advanced Theories Of Covalent Bonding 9 Gases 10 Liquids And Solids 11 Solutions And Colloids 12 Kinetics 13 Fundamental Equilibrium Concepts 14 Acid-base Equilibria 15 Equilibria Of Other Reaction Classes 16 Thermodynamics 17 Electrochemistry 18 Representative Metals, Metalloids, And Nonmetals 19 Transition Metals And Coordination Chemistry 20 Organic Chemistry 21 Nuclear Chemistry Chapter18: Representative Metals, Metalloids, And Nonmetals
Chapter Questions Section: Chapter Questions
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... Problem 81E: Write balanced chemical equations for the following reactions: (a) zinc metal heated in a stream of...
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Write a balanced equation describing each of the following chemical reactions. 3 , decomposes to form solid potassium chloride and diatomic oxygen gas.2 I6 .
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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