HW 5A The following electrostatic potential diagrams represent H2, HCL, or NaCl. Label each and explain your choices. Describe the type of bonding that exists in the F2(g) molecule. How does this type of bonding differ from that found in the HF(g) molecule? How is it similar? When comparing the size of different ions, the general radii trend is usually not very useful. What do you concentrate on when comparing sizes of ions to each other or when comparing the size of an ion to its neutral atom? In general, the higher the charge on the ions in an ionic compound, the more favorable the lattice energy. Why do some stable ionic compounds have +1 charged ions even though +4, +5, and +6 charged ions would have a more favorable lattice energy? Predict which bond in each of the following groups will be post polar. C-F, Si-F, Ge-F P-Cl or S-Cl S-F, S-Cl, S-Br Ti-Cl, Si-Cl, Ge-Cl Which of the following incorrectly shows the bond polarity? Show the correct bond polarity for those that are incorrect. δ+H-Clδ- δ+Cl-Iδ- δ+Si-Sδ- δ+Br-Brδ- δ+O-Pδ- Predict the type of bond one would expect to form between the following pairs of elements. Rb and Cl Ba and S S and S N and P C and F B and H Hydrogen has an electronegativity value between boron and carbon and identical to phosphorous. With this is mind, rank the following bonds in order of decreasing polarity: P-H, O-H, N-H, F-H, C-H Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answer. NaCl, KCl
HW 5A The following electrostatic potential diagrams represent H2, HCL, or NaCl. Label each and explain your choices. Describe the type of bonding that exists in the F2(g) molecule. How does this type of bonding differ from that found in the HF(g) molecule? How is it similar? When comparing the size of different ions, the general radii trend is usually not very useful. What do you concentrate on when comparing sizes of ions to each other or when comparing the size of an ion to its neutral atom? In general, the higher the charge on the ions in an ionic compound, the more favorable the lattice energy. Why do some stable ionic compounds have +1 charged ions even though +4, +5, and +6 charged ions would have a more favorable lattice energy? Predict which bond in each of the following groups will be post polar. C-F, Si-F, Ge-F P-Cl or S-Cl S-F, S-Cl, S-Br Ti-Cl, Si-Cl, Ge-Cl Which of the following incorrectly shows the bond polarity? Show the correct bond polarity for those that are incorrect. δ+H-Clδ- δ+Cl-Iδ- δ+Si-Sδ- δ+Br-Brδ- δ+O-Pδ- Predict the type of bond one would expect to form between the following pairs of elements. Rb and Cl S and S C and F Ba and S N and P B and H Hydrogen has an electronegativity value between boron and carbon and identical to phosphorous. With this is mind, rank the following bonds in order of decreasing polarity: P-H, O-H, N-H, F-H, C-H Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answer. NaCl, KCl
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