Name __________________________________ period _______
CE Chemistry Chapter 4 Review: Forces Between Particles
4.1 Noble Gas Configurations Draw correct Lewis structures for atoms of representative elements.
Write the abbreviated electron configuration and draw the Lewis Structure for each of the following:
1. Iodine [Kr]5s24d105p5
3. As [Ar]4s23d104p3
2. Element number 38 [Kr]5s2
4. Phosphorus [Ne]3s23p3
4.2 Ionic Bonding: Predict the number of electrons that will be lost or gained by the following. Write the
equation to represent each change. Example: Cesium: 1 electron lost Cs → Cs+ + e5. Oxygen
6. Element #7
7. Al
8. Fluorine
2 e added
2 e added
3e lost
1e- added
233+
O+2e →O
N+3e →N
Al → Al + 3e
F + e- →F-
4.3 Ionic Compounds: Write the formula for the ionic compound formed from Ba2+ and the following anions, then
write the name of the compound.
9. Se210. P311. PO3312. PO43- Ba3(PO4)2
BaSe
Ba3P2
Ba3(PO3)2
Barium phosphate
Barium selenide
Barium phosphide
Barium phosphite
4.4 Naming Binary Ionic Compounds Correctly name binary ionic compounds.
Name the following compounds
13. CrCl2
14. CrCl3
15. FeO
Chromium (II)
Chromium (III)
Iron (II) oxide
chloride
chloride
16. Fe2O3
Iron (III) oxide
4.5 The Smallest Unit of Ionic Compounds Determine formula weights for ionic compounds.
Determine the formula weight for each of the following:
17. Fe2O3 159.6
18. H3PO3 82
19. Ca3(PO3)2 278
20. Mg(OH)2 58.3
4.6 Covalent Bonding: Draw the Lewis Structures for each of the following:
21. CH4
22. CO2
23. ClO3-
24. NH3
4.7 Polyatomic Ions Draw correct Lewis structures for polyatomic ions and name the shape.
25. NH4+
26. PO4327. SO32-
4.8 Shapes of Molecules and Polyatomic Ions : Use VSEPR theory to predict the shapes of molecules and determine
polar or nonpolar.
28. O3 polar, bent
29. CS2 nonpolar, linear
30. C2H4 both C trigonal
31. SO42- tetrahedral,
planar,
nonpolar
nonpolar
1
4.9 The Polarity of Covalent Molecules Classify as ionic, nonpolar covalent or polar covalent bonds.
32. LiBr ionic
33. HCl polar
34. PH3 polar
35. SO2 polar
36. CsF ionic
covalent
covalent
covalent
37. What type of bond would form between A and B if their electronegativity difference is 0.8? polar covalent
38. Arrange the following in order of increasing bond polarity:
C—F , C—O , C—N
C—N < C—O < C—F
4.10 More about Naming Compounds: Write correct formulas.
39. Calcium nitrate
42. Potassium sulfite
45. Carbon tetrachloride
Ca(NO3)2
K2SO3
CCl4
40. Magnesium hypochlorite
43. Chlorine dioxide
46. Boron trifluoride
Mg(ClO)2
ClO2
BF3
41. Cesium dichromate
44. Dinitrogen pentoxide
47. Carbon disulfide
Cs2Cr2O7
N2O5
CS2
Write the correct names
48. SiO2 silicon dioxide
53. NaI sodium iodide
49. P2F5 diphosphorus pentafluoride
54. CuSO4 copper (II) sulfate
50. CBr4 carbon tetrabromide
55. Fe2(SO3)3 iron (III) sulfite
51. Li2CO3 lithium carbonate
56. SnO tin (II) oxide
52. Mg(OH)2 magnesium hydroxide
57. SnO2 tin (IV) oxide
4.11 Other Interparticle Forces: Relate melting and boiling points of pure substances to the strength and type of
interparticle forces present in the substances.
58. List the following interparticle forces in order of increasing strength: dispersion forces, hydrogen bonds, &
dipolar forces
Dispersion forces (weakest), dipolar forces, hydrogen bonds (strongest of these)
59. How do interparticle forces relate to melting and boiling points of substances?
The stronger the interparticle force, the higher the melting and boiling points of the substances.
60. Which interparticle forces leads to compounds with the lowest melting points? If a compound only has
dispersion forces, they will have the lowest melting points. (they are usually gases)