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Problem 41
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and Se b. Ba and Cl c. Na and S d. Al and O
Problem 42
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Ca and N b. Mg and I c. Ca and S d. Cs and F
- What is the trend in the lattice energies of alkaline earth metal oxides? Here are the lattice energies (in kJ/mol): MgO -3795, CaO -3414, SrO -3217, BaO -3029.
Problem 43
Problem 44
Rubidium iodide has a lattice energy of -617 kJ/mol, while potassium bromide has a lattice energy of -671 kJ/mol. Why is the lattice energy of potassium bromide more exothermic than the lattice energy of rubidium iodide?
Problem 45
The lattice energy of CsF is -744 kJ/mol, whereas that of BaO is -3029 kJ/mol. Explain this large difference in lattice energy.
Problem 47
Use the Born–Haber cycle and data from Appendix IIB, Chapter 8 and this chapter to calculate the lattice energy of KCl. (ΔHsub for potassium is 89.0 kJ/mol.)
Problem 48
Use the Born–Haber cycle and data from Appendix IIB and Table 9.3 to calculate the lattice energy of CaO. (ΔHsub for calcium is 178 kJ/mol; IE1 and IE2 for calcium are 590 kJ/mol and 1145 kJ/mol, respectively; EA1 and EA2 for O are -141 kJ/mol and 744 kJ/mol, respectively.)
- Use covalent Lewis structures to explain why each element or family of elements occurs as diatomic molecules: a. hydrogen b. the halogens c. oxygen d. nitrogen.
Problem 49
Problem 51a,b,c
Write the Lewis structure for each molecule. a. PH3 b. SCl2 c. HI
Problem 51d
Write the Lewis structure for each molecule. d. CH4
Problem 52
Write the Lewis structure for each molecule. a. NF3 b. HBr c. SBr2 d. CCl4
Problem 53a
Write the Lewis structure for each molecule. a. SF2
Problem 53b
Write the Lewis structure for each molecule. b. SiH4
Problem 53c
Write the Lewis structure for each molecule. c. HCOOH (both O bonded to C)
Problem 53d
Write the Lewis structure for each molecule. d. CH3SH (C and S central)
Problem 54
Write the Lewis structure for each molecule. a. CH2O b. C2Cl4 c. CH3NH2 d. CFCl3 (C central)
Problem 55a
Determine if a bond between each pair of atoms would be pure covalent, polar covalent, or ionic. a. Br and Br
- Determine whether the bond between each of the following pairs of atoms would be pure covalent, polar covalent, or ionic: a. C and N b. N and S c. K and F d. N and N.
Problem 56
Problem 57
Refer to Figure 9.10 to estimate the percent ionic character of the CO bond.
Problem 58a
Draw the Lewis structure for BrF with an arrow representing the dipole moment. Refer to Figure 9.10 to estimate the percent ionic character of the BrF bond.
Problem 58b
Refer to Figure 9.10 to estimate the percent ionic character of the BrF bond.
Problem 59
Write the Lewis structure for each molecule or ion. a. CI4 b. N2O c. SiH4 d. Cl2CO
Problem 60b
Write the Lewis structure for each molecule or ion. b. OH-
Problem 60c
Write the Lewis structure for each molecule or ion. c. BrO-
Problem 61a,b,c
Write the Lewis structure for each molecule or ion. a. N2H2 b. N2H4 c. C2H2
Problem 61d
Write the Lewis structure for each molecule or ion. d. C2H4
Problem 62a
Write the Lewis structure for each molecule or ion. a. H3COCH3
Problem 63a
Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. a. SeO2
Problem 63b,c,d
Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. b. CO32– c. ClO– d. NO2–
Problem 64
Write a Lewis structure that obeys the octet rule for each ion. Include resonance structures if necessary and assign formal charges to each atom. a. ClO3- b. ClO4- c. NO3- d. NH4+