2. The Lewis structure for the acetate ion [C₂H₂O₂] ¹ is given below: a. Read section 1.9. What is the geometry (shape) around each of the carbon atoms in the acetate ion - tetrahedral, trigonal planar or linear? b. Each of the oxygen atoms in the acetate ion have an octet. Draw all lone pairs of electrons in the acetate ion given above. c. Read section 1.7. Use electron pushing to generate a resonance structure of the acetate Lewis structure given above.

2. The Lewis structure for the acetate ion [C₂H₂O₂] ¹ is given below: a. Read section 1.9. What is the geometry (shape) around each of the carbon atoms in the acetate ion - tetrahedral, trigonal planar or linear? b. Each of the oxygen atoms in the acetate ion have an octet. Draw all lone pairs of electrons in the acetate ion given above. c. Read section 1.7. Use electron pushing to generate a resonance structure of the acetate Lewis structure given above.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 37CR

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a. How many sticks did you need to make the skeleton structure?____________ b. How many sticks are left over? ____________ If your model is to obey the octet rule, each ball must have four sticks in it except for hydrogen atom balls, which need and can only have one. Each atom in an octet rule species is surrounded by four pairs of electrons. c. How many holes remain to be filled? ____________ Fill them with the remaining sticks, which represent nonbonding electron pairs. Draw the complete Lewis structure for NH2Cl using lines for bonds and pairs of dots for nonbonding electrons.
Draw a curve that describes the energy of a system with H and Cl atoms at varying distances. Then, find the minimum energy of this curve two ways. (a) Use the bond energy found in Table 8.1 to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?) (b) Use the enthalpy of reaction and the bond energies for H2 and Cl2 to solve for the energy of one mole of HCl bonds. H2(g)+Cl2(g)2HCl(g)Hrxn=184.7kJ/mol
Bond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?
Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?
Compare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?
The chemistry of the nitrite ion and HNO2: (a) Two resonance structures are possible for NO2. Draw these structures, and then find the formal charge on each atom in each resonance structure. (b) In forming the acid HNO2 an H+ ion attaches to the O atom and not the N atom of NO2. Explain why you would predict this result. (c) Two resonance structures are possible for HNO2. Draw these structures, and then find the formal charge on each atom in each resonance structure. Is either of these structures strongly preferred over the other?
How does the bond energy of HCl(g) differ from the standard enthalpy of formation of HCl(g)?
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A common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called methyl cyanoacrylate, the main ingredient in Super Glue. Draw a complete Lewis structure for methyl cyanoacrylate in which all atoms have a formal charge of zero.
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