Which member of each pair of compounds forms intermol-ecular H bonds? Draw the H-bonded structures in each case:(a) (CH₃)₂NH or (CH₃)₃N (b) HOCH₂CH₂OH or FCH₂CH₂F
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Which member of each pair of compounds forms intermol-ecular H bonds? Draw the H-bonded structures in each case:(a) (CH₃)₂NH or (CH₃)₃N (b) HOCH₂CH₂OH or FCH₂CH₂F
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- The species is the simplest polyatomic ion. The geometry of the ion is that of an equilateral triangle. (a) Draw three resonance structures to represent the ion. (b) Given the following information 2 H+ + H+ ---> ∆H° = - 849 kJ/mol and H2 ---> 2H ∆H° = -436.4 kJ/mol calculate ∆H° for the reaction H+ + H2 --->A student investigates the physical and chemical properties of various carbon-containing compounds. Thr complete Lewis electron-dot diagrams and boiling points for two compounds, Q and Z, are shown in the following table: B) Any C — H bond in compound Q is shorter than the S — H bond in compound Z. Explain the reason for this difference using principles of atomic structure.2(a) Provide the Lewis structures for both CH3OH and C2H3Cl. 2(b) What is the largest bond angle among all the bond angles in CH3OH and C2H3Cl? Listthe three atoms making this largest bond angle, and estimate the value of the angle.2(c) What intermolecular forces are present(i) between CH3OH molecules?(ii) between C2H3Cl molecules?
- Which of the following is a resonance structure of compound X? N (A) OH NH (B) X NH O NH (C) N (D)Propylene, C3H6, is a gas that is used to form the importantpolymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylenemolecule? (b) How many valence electrons are usedto make s bonds in the molecule? (c) How many valenceelectrons are used to make p bonds in the molecule? (d) Howmany valence electrons remain in nonbonding pairs in themolecule? (e) What is the hybridization at each carbon atomin the molecule?19. :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.
- 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.Draw the Lewis structures for CO2 and CO, and predict the number of σ and π bonds for each molecule.(a) CO2(b) COWhich of the following bonds is most polar: S¬Cl, S¬Br, Se¬Cl,or Se¬Br?
- Identify the electron pair geometry and the molecular structure of each of the following molecules:(a) ClNO (N is the central atom)(b) CS2(c) Cl2CO (C is the central atom)(d) Cl2SO (S is the central atom)(e) SO2F2 (S is the central atom)(f) XeO2F2 (Xe is the central atom)(g) ClOF2+ (Cl is the central atom)Which of the following compounds does not follow the octet rule? (a) N2 (b) BeCl2 (c) CH4 (d) NH3Using the bond energy data from your text (or the internet), determine (show calculations for) the approximate enthalpy change , ∆H, for each of the following reactions: (a) Cl2 (g) + 3F2 (g) ⟶ 2ClF3 (g) (b) H2C=CH2 (g) + H2 (g) ⟶ H3CCH3 (g)