Concept explainers
Volcanoes and deep sea hydrothermal vents are both associated with sulfur-rich environments. Mount Etna is classed as a continuously degassing volcano and emissions of
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Inorganic Chemistry
Additional Science Textbook Solutions
Basic Chemistry
Organic Chemistry
Inorganic Chemistry
Chemistry In Context
Thermodynamics, Statistical Thermodynamics, & Kinetics
- In which of the following molecules does the sulfur have an expanded octet? For those that do, write the Lewis structure. (a) SO2 (b) SF4 (c) SO2Cl2 (d) SF6arrow_forwardAcetylene (C2H2) and nitrogen (N2) both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) By referring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O5(g) and of acetylene to formCO2(g) and H2O(g). (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O5(g) is 11.30 kJ/mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forwardWith reference to the “Chemistry Put to Work” box on explosives, (a) use bond enthalpies to estimate the enthalpy change for the explosion of 1.00 g of nitroglycerin. (b) Write a balanced equation for the decomposition of TNT. Assume that, upon explosion, TNT decomposes into N2(g), CO2(g), H2O(g), and C(s).arrow_forward
- An ionic compound of formula XY2 (X = cation with two positive charges, Y = anion with one negative charge) has the following mass composition: Mg 10.9%, Cl 31.8%, O57.3%. (a) What is the chemical formula and name of the compound? (b) Give the most probable Lewis structure for the ions contained in the compound.arrow_forwardUse principles of atomic structure to answer each of the following: (1] (a) The radius of the Ca atom is 197 pm; the radius of the Ca2* ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is –3460 kJ/mol; the lattice energy of K20 is –2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First lonization Energy (kJ/mol) Second lonization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.arrow_forwardWhich of the following bonds are polar: (a) P—O; (b) S—F; (c) Br—Br; (d) O—Cl? Which is the more electronegative atom in each polar bond?arrow_forward
- An important starting material for the manufacture ofpolyphosphazenes is the cyclic molecule (NPCl₂)₃. The mol-ecule has a symmetrical six-membered ring of alternating N and P atoms, with the Cl atoms bonded to the P atoms. The nitrogen-phosphorus bond length is significantly less than that expectedfor an N−P single bond.(a) Draw a likely Lewis structure for the molecule.(b) How many lone pairs of electrons do the ring atoms have?(c) What is the order of the nitrogen-phosphorus bond?arrow_forwardAnswer the following questions that relate to the chemistry of nitrogen. (a) Two nitrogen atoms combine to form a nitrogen molecule, as represented by the following equation. 2 N(g) ® N2(g) Using the table of average bond energies below, determine the enthalpy change, AH, for the reaction. Average Bond Energy (k) mol-1) Bond N-N 160 N=N 420 N°N 950 (b) The reaction between nitrogen and hydrogen to form ammonia is represented below. N2(g) + 3 H2(g)® 2 NH3(g) AH° = -92.2 kJ Predict the sign of the standard entropy change, AS', for the reaction. Justify your answer. (C) The value of AG° for the reaction represented in part (b) is negative at low temperatures but positive at high temperatures. Explain.arrow_forwardWhich compound in each of the following pairs has the larger lattice energy? Note: Ba2+ and K+ have similar radii; S2– and Cl– have similar radii. Explain your choices.(a) K2O or Na2O(b) K2S or BaS(c) KCl or BaS(d) BaS or BaCl2arrow_forward
- Acetylene 1C2H22 and nitrogen 1N22 both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) Byreferring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O51g2 and of acetylene to formCO21g2 and H2O1g2. (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O51g2 is 11.30 kJ>mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forwardCommon exceptions to the octet rule are compounds and polyatomic ions with central atoms having more than 8 electrons around them. Phosphorus pentafluoride, PF5; sulfur tetrafluoride, SF4; xenon tetrafluoride, XeF4; and tri-iodide ion, I3, are all examples of exceptions to the octet rule. (a) Draw the Lewis structures of these substances.(b) For which elements in these substances can theatoms have more than 8 electrons around them?(c) How can the atoms of the elements youidentified in Part (b) be surrounded by morethan 8 electrons?arrow_forward19. :O: || :0-N- O: Which of the following statements, if true, would support the claim that the NO3 ion, represented above, has three resonance structures? (A) The NO3 ion is not a polar species. (B) The oxygen-to-nitrogen-to-oxygen bond angles are 90°. (C) One of the bonds in NO3 is longer than the other two. (D) One of the bonds in NO3¯ is shorter than the other two.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning