뒤로
- Use covalent Lewis structures to explain why the compound that forms between nitrogen and hydrogen has the formula NH3 and why NH2 and NH4 are not stable.
문제 5
문제 35
Write the electron configuration for oxygen. Then write the Lewis symbol for oxygen and show which electrons from the electron configuration are included in the Lewis symbol.
문제 37b
Write the Lewis symbol for each atom or ion. b. K+
문제 37c
Write the Lewis symbol for each atom or ion. c. S
문제 37d
Write the Lewis symbol for each atom or ion. d. S2-
문제 39d
Write the Lewis symbols for the ions in each ionic compound. d. K2O
문제 40a,d
Write the Lewis symbols for the ions in each ionic compound. a. SrO d. RbF
문제 40b
Write the Lewis symbols for the ions in each ionic compound. b. Li2S
문제 40c
Write the Lewis symbols for the ions in each ionic compound. c. CaI2
문제 41
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Mg and S b. Sr and Br c. K and Se d. Al and S
문제 42
Use Lewis symbols to determine the formula for the compound that forms between each pair of elements. a. Sr and P b. Ba and S c. Sr and Se d. Rb and I
문제 45
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?
문제 47
The lattice energy of CsF is -744 kJ/mol, whereas that of BaO is -3029 kJ/mol. Explain this large difference in lattice energy.
문제 48
Arrange these compounds in order of increasing magnitude of lattice energy: CaO, NaBr, CsI, BaS.
문제 49
Use the Born–Haber cycle and data from Appendix IIB, Chapter 9 and this chapter to calculate the lattice energy of LiBr. (ΔHsub for lithium is 138 kJ>mol.)
문제 50
Use the Born–Haber cycle and data from Appendix IIB and Table 10.3 to calculate the lattice energy of MgO. (ΔHsub for magnesium is 137 kJ/mol; IE1 and IE2 for magnesium are 738 kJ/mol and 1450 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.
문제 51
문제 55a,b,c
Write the Lewis structure for each molecule. a. PH3 b. SCl2 c. HI
문제 55d
Write the Lewis structure for each molecule. d. CH4
문제 57a
Write the Lewis structure for each molecule. a. SF2
문제 57b
Write the Lewis structure for each molecule. b. SiH4
문제 57d
Write the Lewis structure for each molecule. d. CH3SH (C and S central)
문제 58
Write the Lewis structure for each molecule. a. CH2O b. C2Cl4 c. CH3NH2 d. CFCl3 (C central)
문제 59a
Determine if a bond between each pair of atoms would be pure covalent, polar covalent, or ionic. a. Ba and O
문제 61
Refer to Figure 10.10 to estimate the percent ionic character of the Hbr bond.
문제 62a
Draw the Lewis structure for ClF with an arrow representing the dipole moment.
문제 62b
Refer to Figure 10.10 to estimate the percent ionic character of the ClF bond.
문제 64b
Write the Lewis structure for each molecule or ion. b. OH-
문제 64c
Write the Lewis structure for each molecule or ion. c. BrO-
문제 65d
Write the Lewis structure for each molecule or ion. d. C2H4