Chapter 09 – Chemical Bonding I: Basic Concepts
Chapter 09
Chemical Bonding I: Basic Concepts
1. Which one of the following is most likely to be an ionic compound?
2. Which one of the following is most likely to be an ionic compound?
Chapter 09 – Chemical Bonding I: Basic Concepts
3. Which one of the following is most likely to be an ionic compound?
4. Which one of the following is most likely to be a covalent compound?
Chapter 09 – Chemical Bonding I: Basic Concepts
5. Which one of the following is most likely to be a covalent compound?
6. Which one of the following is most likely to be a covalent compound?
Chapter 09 – Chemical Bonding I: Basic Concepts
7. Which one of the following compounds utilizes both ionic and covalent bonding?
8. Which one of the following compounds utilizes both ionic and covalent bonding?
Chapter 09 – Chemical Bonding I: Basic Concepts
9. Which one of the following compounds utilizes both ionic and covalent bonding?
10. Complete this statement: Coulomb’s law states that the magnitude of the force of
interaction between two charged bodies is
Chapter 09 – Chemical Bonding I: Basic Concepts
11. The Lewis dot symbol for the S 2– ion is
Chapter 09 – Chemical Bonding I: Basic Concepts
12. The Lewis dot symbol for the chloride ion is
Chapter 09 – Chemical Bonding I: Basic Concepts
13.
The Lewis dot symbol for the calcium ion is
14. Which one of the following ionic solids would have the largest lattice energy?
Chapter 09 – Chemical Bonding I: Basic Concepts
15. Which of the following ionic solids would have the largest lattice energy?
16. Which of the following ionic solids would have the largest lattice energy?
17. Which of the following solids would have the highest melting point?
Chapter 09 – Chemical Bonding I: Basic Concepts
18. Which of the following solids would have the highest melting point?
19. Which of the following solids would have the lowest melting point?
Chapter 09 – Chemical Bonding I: Basic Concepts
20.
Calculate the energy change for the reaction
K(g) + Br(g) → K+(g) + Br– (g)
given the following ionization energy (IE) and electron affinity (EA) values.
Chapter 09 – Chemical Bonding I: Basic Concepts
21.
Calculate the energy change for the reaction
K(g) + I(g) → K+(g) + I – (g)
given the following ionization energy (IE) and electron affinity (EA) values.
22.
Use the Born-Haber cycle to calculate the lattice energy of KCl(s) given the following data:
H(sublimation) K = 79.2 kJ/mol
I1 (K) = 418.7 kJ/mol
Bond energy (Cl–Cl) = 242.8 kJ/mol
EA (Cl) = 348 kJ/mol
H (KCl(s)) = –435.7 kJ/mol
Chapter 09 – Chemical Bonding I: Basic Concepts
23.
Use the Born-Haber cycle to calculate the lattice energy of MgO (s) given the following data:
H(sublimation) Mg = 130 kJ/mol
I1 (Mg) = 738.1 kJ/mol
I2 (Mg) = 1450 kJ/mol
Bond energy (O=O) = 498.7 kJ/mol
EA (O) = 141 kJ/mol
EA (O–) = –780 kJ/mol
H (MgO(s)) = –601.8 kJ/mol
24.
Use the Born-Haber cycle to calculate the standard enthalpy of formation (H) for LiCl(s) given the following data:
H(sublimation) Li = 155.2 kJ/mol
I1 (Li) = 520 kJ/mol
Bond energy (Cl–Cl) = 242.7 kJ/mol
EA (Cl) = 349 kJ/mol
Lattice energy (LiCl(s)) = 828 kJ/mol
Chapter 09 – Chemical Bonding I: Basic Concepts
25. Which of the elements listed below would most likely form a polar covalent bond when
bonded to oxygen?
26. Which of the elements listed below would most likely form an ionic bond when bonded to
oxygen?
Chapter 09 – Chemical Bonding I: Basic Concepts
27. Which of the elements listed below would most likely form a nonpolar covalent bond
when bonded to bromine?
28. Which of the elements listed below would most likely form an ionic bond when bonded to
chlorine?
Chapter 09 – Chemical Bonding I: Basic Concepts
29. Define electronegativity:
30. Arrange the elements F, P, and Cl in order of increasing electronegativity.
31. Arrange the elements C, O, and H in order of increasing electronegativity.
Chapter 09 – Chemical Bonding I: Basic Concepts
32. Arrange the elements Ba, Br, and Ga in order of increasing electronegativity.
33. A polar covalent bond would form in which one of the following pairs of atoms?
Chapter 09 – Chemical Bonding I: Basic Concepts
34. Which one of these polar covalent bonds would have the greatest percent ionic
character?
35. What type of chemical bond holds the atoms together within a water molecule?
Chapter 09 – Chemical Bonding I: Basic Concepts
36. A nonpolar covalent bond (i.e., pure covalent) would form in which one of the following
pairs of atoms?
37. Which of the bonds below would have the greatest polarity (i.e., highest percent ionic
character)?
Chapter 09 – Chemical Bonding I: Basic Concepts
38. Which of the following covalent bonds is the most polar (i.e., highest percent ionic
character)?
39. The covalent bond with the greatest polarity would form in which of the atom pairs
below?