Thionyl chloride (SOCl₂) is a sulfur oxohalide used indus-trially to dehydrate metal halide hydrates. (a) Write a balancedequation for its reaction with magnesium chloride hexahydrate,in which SO₂ and HCl form along with the metal halide. (b) Drawa Lewis structure of SOCl₂ with minimal formal charges.

Thionyl chloride (SOCl₂) is a sulfur oxohalide used indus-trially to dehydrate metal halide hydrates. (a) Write a balancedequation for its reaction with magnesium chloride hexahydrate,in which SO₂ and HCl form along with the metal halide. (b) Drawa Lewis structure of SOCl₂ with minimal formal charges.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 6.ACP

See similar textbooks

Similar questions

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.
Three main group elements, X, Y and Z, from three different groups inthe Periodic Table, each form a neutral trifluoride, i.e. XF3, YF3 andZF3. (a) To which three groups of the Periodic Table could the elementsX, Y and Z belong? Are any of these atoms X, Y or Zhypervalent in the trifluorides formed? (b) Use VSEPR theory to deduce the shapes of the molecules XF3,YF3 and ZF3, showing full working, and sketch these shapes (c) Only two of the three trifluorides have a non-zero dipole moment.For these molecules to which groups of the Periodic Table do thecentral atoms belong?
By referring only to the periodic table, select (a) the most electronegativeelement in group 6A; (b) the least electronegativeelement in the group Al, Si, P; (c) the most electronegative elementin the group Ga, P, Cl, Na; (d) the element in the group K,C, Zn, F that is most likely to form an ionic compound with Ba.
Use 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.
Acetylene (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.
Which of these statements about resonance is true?(a) When you draw resonance structures, it is permissibleto alter the way atoms are connected.(b) The nitrate ion has one long N¬O bond and two shortN¬O bonds.(c) “Resonance” refers to the idea that molecules areresonating rapidly between different bonding patterns.(d) The cyanide ion has only one dominant resonancestructure.(e) All of the above are true.
The hypochlorite ion, ClO-, is the active ingredient inbleach. The perchlorate ion, ClO4-, is a main componentof rocket propellants. Draw Lewis structures for both ions. (a) What is the formal charge of Cl in the hypochlorite ion?(b) What is the formal charge of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (c) What is theoxidation number of Cl in the hypochlorite ion? (d) Whatis the oxidation number of Cl in the perchlorate ion, assumingthe Cl—O bonds are all single bonds? (e) In a redox reaction,which ion would you expect to be more easily reduced?
Sulfur tetrafluoride (SF4) reacts slowly with O2 to form sulfurtetrafluoride monoxide (OSF4) according to the followingunbalanced reaction: SF4(g) + O2(g)---->OSF4(g)The O atom and the four F atoms in OSF4 are bonded to acentral S atom. (a) Balance the equation. (b) Write a Lewisstructure of OSF4 in which the formal charges of all atomsare zero. (c) Use average bond enthalpies (Table 8.3) to estimatethe enthalpy of the reaction. Is it endothermic or exothermic?(d) Determine the electron-domain geometry ofOSF4, and write two possible molecular geometries for themolecule based on this electron-domain geometry. (e) Foreach of the molecules you drew in part (d), state how manyfluorines are equatorial and how many are axial.
Formic acid has the chemical formula HCOOH. It is a colorlessliquid that has a density of 1.220 g/mL. (a) The carbonatom in formic acid is bound to one H and both O’s. Drawthe Lewis structure for formic acid, showing resonance ifpresent. (b) Formic acid can react with NaOH in aqueoussolution to produce the formate ion, HCOO-. Write thebalanced chemical equation for this reaction. (c) Draw theLewis structure of the formate ion, showing resonance ifpresent. (d) How many milliliters of a 0.100 M solution ofNaOH would it take to completely react with 0.785 mL offormic acid?
(a) Compare the bond enthalpies (Table 8.3) of the carbon–carbon single, double, and triple bonds to deduce an averageπ -bond contribution to the enthalpy. What fraction ofa single bond does this quantity represent? (b) Make a similarcomparison of nitrogen–nitrogen bonds. What do youobserve? (c) Write Lewis structures of N2H4, N2H2, and N2,and determine the hybridization around nitrogen in eachcase. (d) Propose a reason for the large difference in yourobservations of parts (a) and (b).
In addition to ammonia, nitrogen forms three other hydrides: hydrazine (N2H4), diazene (N2H2), and tetrazene (N4H4).(a) Use Lewis structures to compare the strength, length, and order of the nitrogen-nitrogen bonds in hydrazine, diazene, and N2.(b) Tetrazene (atom sequence H2NNNNH2) decomposes above 08C to hydrazine and nitrogen gas. Draw a Lewis structure for tetrazene, and calculate ΔH°rxn for this decomposition.
The cyanate ion, NCO-, has three possible Lewis structures.(a) Draw these three structures and assign formal charges ineach. (b) Which Lewis structure is dominant?