18. When one electron is added to an oxygen molecule, a superoxide ion (O₂) is formed. The addition of two elec- trons gives a peroxide ion (O2). Removal of an electron from O₂ leads to O₂. (a) Construct the correlation diagram for O₂. (b) Give the valence electron configuration for each of the following species: O2, 0₂, 02, 02. (c) Give the bond order of each species. (d) Predict which species are paramagnetic. (e) Predict the order of increasing bond dissociation energy among the species.

18. When one electron is added to an oxygen molecule, a superoxide ion (O₂) is formed. The addition of two elec- trons gives a peroxide ion (O2). Removal of an electron from O₂ leads to O₂. (a) Construct the correlation diagram for O₂. (b) Give the valence electron configuration for each of the following species: O2, 0₂, 02, 02. (c) Give the bond order of each species. (d) Predict which species are paramagnetic. (e) Predict the order of increasing bond dissociation energy among the species.

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter3: Chemical Bonds

Section: Chapter Questions

Problem 3.95P

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(c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F. 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smalleor going down the halogen group from HF to HI Describe these observations
(a) Describe the molecule xenon trioxide, XeO3, usingfour possible Lewis structures, one each with zero, one,two, or three Xe¬O double bonds. (b) Do any of theseresonance structures satisfy the octet rule for every atomin the molecule? (c) Do any of the four Lewis structureshave multiple resonance structures? If so, how many resonancestructures do you find? (d) Which of the Lewisstructures in part (a) yields the most favorable formalcharges for the molecule?
In developing the concept of electronegativity, Pauling used the term excess bond energy for the difference between the actual bond energy of X¬Y and the average bond energies of X¬X and Y¬Y (see text discussion for the case of HF). Based on the values as shown, which of the following substances contains bonds with no excess bond energy?(a) PH3 (b) CS2 (c) BrCl (d) BH3 (e) Se8
Cyanogen (CN)2 is known as pseodohalogen because it has some properties like halogens. It is composed of two CN’s joined together.(i) Draw the Lewis structure for all the possible combination for (CN)2.(ii) Calculate the formal charge and determine which one of the structures that you have drawn is most stable.(iii) For the stable structure, determine the geometry around the two central atoms.(iv) For the stable structure, draw the dipole arrows for the bonds.(v) Base on the stable structure, determine the polarity of molecule and state your reason.
iv. Assign formal charges to the atoms in the following structures and decide which the more important contributor to the resonance hybrid is. (a) (b) H H C=N=N c-N=N H H v. What factor accounts for each of the following differences in bond length? (a) I, has a longer bond than Br,. (b) C-N bonds are shorter than C-C bonds. (c) H-C bonds are shorter than the C-O bond. (d) The C-O bond in formaldehyde, H,C=0, is longer than the bond in carbon monoxide, C=0.
32. Which term refers to how strongly an atom of an element attracts electrons in a chemical bond with another atom? (A) lonization energy (B) Atomic radius (C) Melting point (D) Electronegativity 33. Which of the following would have a trigonal pyramidal geometry? (A) NO2 (B) Оз (C) H2O (D) NH3 34. Calculate the molarity of a solution in which 360. grams of glucose, C6H12O6, are dissolved in enough water to make 250. mL of solution. (А) 1.0 М (В) 2.0 М (С) 4.0 М (D) 8.0 M 35. All of the following are ways to increase the rate of dissolving sugar except – (A) Increasing the mass of sugar (B) Crushing the sugar into a fine powder (C) Stirring with a spoon (D) Increasing the temperature of the water
Q.3 a) Write the chemical name and chemical formula of a compound formed between X (atomic number of X=56) and nitrate ion. (1 mark) b) Name and explain the type of chemical reaction that occurs in between two ionic compounds with the help of examples. (2 marks) c) Explain the bond formation with Lewis structure in a gas molecule that belongs to group 6A and exists as a diatomic molecule. (Mention the type of chemical bond) (2 marks)
In addition to ammonia, nitrogen forms three other hy-drides: hydrazine (N₂H₄), diazene (N₂H₂), and tetrazene (N₄H₄).(a) Use Lewis structures to compare the strength, length, and or-der of nitrogen-nitrogen bonds in hydrazine, diazene, and N₂.(b) Tetrazene (atom sequence H₂NNNNH₂) decomposes above 0°C to hydrazine and nitrogen gas. Draw a Lewis structure fortetrazene, and calculate ΔH°ᵣₓₙ for this decomposition.
For which of the following substances is the least energy required to convert one mole of the solid into separate ions? (a) MgO (b) SrO (c) KF (d) CsF (e) MgF2
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.
For which of the following substances is the least energy required to convert one mole of the solid into separate ions?(a) MgO(b) SrO(c) KF(d) CsF(e) MgF2
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.