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EBK GENERAL CHEMISTRY
- Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardUsing the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulfur double bond in CS2.arrow_forwardNitrosyl azide, N4O, is a pale yellow solid first synthesized in 1993. Write the Lewis structure for nitrosyl azide.arrow_forward
- Consider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?arrow_forwardA new element, Bw, has been identified to be part of Period 10 Group VIIA. Draw the proper structure of the polyatomic ion, BwCl2S3 ^ - . According to VSEPR theory, this ion has a molecular shape of [1]. (Type the shape exactly as written on the table provided to you on the exam data sheet) The formal charge of the Bw atom must be [2]. (Type in the charge including a sign and numberi.e. +1, -1, -2, +2, 0, etc.)arrow_forwardDraw the Lewis structure for the N H 4 + ion.arrow_forward
- Hydrazine, N2H4, burns in oxygen as follows: N2H4 + O2 → N2 + 2H2O [The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496] Draw the chemical structures of the reactants and products and give the formula to calculate enthalpy change in a reaction, ΔH.arrow_forwardThe azide ion, N, is a symmetrical ion, in which all of the possible Lewis structures have formal charge on one or more atoms. Draw three possible Lewis structures for this ion. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all nonbonding electrons. Show the formal charges of all atoms. Q NNNITY ¤•• Q Submit Q NENN N=N-N² N²NN с H O N S P F Br CI X Type the new charge. Press ENTER to finish editing. Press TAB to go through atoms in the structure. Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining Morearrow_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_forward
- Write all resonance structures for NCO− ion. Use formal charges to predict the most stable one (i.e. the one that has the lowest energy configuration) and the least stable. Briefly explain.arrow_forward2arrow_forward1a)Rank the following ionic compounds in order of lattice energy, from the least exothermic (least negative lattice enthalpy) to the most exothermic (most negative lattice enthalpy): KCI, SrO, RbBr, CaO 1b)Rank the following elements in order of decreasing metallic character (from most metallic to least metallic): S, CI, K, Cs, Se 1c) by using the table of bond enthalpies, predict ?rH of the following reaction in kJ/mol H2C=CH2 + Cl2 ---> Cl-CH2-CH2-Clarrow_forward
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