NOMENCLATURE REVIEW
Molecular Compounds, Ionic Compounds, & Acids
NAME THE FOLLOWING COMPOUNDS:
1.
BaSO3
14. AgNO3
2.
(NH4)3PO4
15. As2O5
3.
PBr5
16. Fe2O3
4.
MgSO4
17. HClO
5.
CaO
18. N2O3
6.
H3PO4
19. HF
7.
Na2Cr2O7
20. H2C2O4
8.
MgO
21. NaHCO3
9.
SO3
22. SiBr4
10. Cu(NO3)2
23. CuCl2
11. HI
24. HNO2
12. N2O
25. SnO2
13. MnO
26. BaCrO4
WRITE FORMULAS FOR THE FOLLOWING COMPOUNDS:
27. hydrobromic acid
40. diphosphorus pentoxide
28. chromium (III) carbonate
41. sulfurous acid
29. magnesium sulfide
42. lead (II) nitrate
30. iodine trichloride
43. dihydrogen monoxide
31. lithium hydride
44. sodium oxalate
32. ammonium hydroxide
45. perchloric acid
33. calcium chloride
46. chlorous acid
34. hydroselenic acid
47. silicon dioxide
35. iron (II) nitride
48. carbonic acid
36. aluminum hydroxide
49. sodium chlorate
37. tin (II) fluoride
50. xenon hexafluoride
38. sulfur tetrachloride
51. nickel (II) nitrate
39. mercury (II) iodide
52. potassium perchlorate
NOMENCLATURE REVIEW
CHEMISTRY TEST STUDY GUIDE
Chemical Bonding
Molecular Compounds, Ionic Compounds, & Acids
ANSWER KEY
1.
2.
3.
4.
5.
barium sulfite
ammonium phosphate
phosphorus pentabromide
magnesium sulfate
calcium oxide
6. phosphoric acid
7. sodium dichromate
8. magnesium oxide
9. sulfur trioxide
10. copper(II) nitrate
11. hydroiodic acid
12. dinitrogen monoxide
13. manganese(II) oxide
14. silver nitrate
15. diarsenic pentoxide
16. iron(III) oxide
17. hypochlorous acid
18. dinitrogen trioxide
19. hydrofluoric acid
20. oxalic acid
21. sodium bicarbonate
22. silicon tetrabromide
23. copper(II) chloride
24. nitrous acid
25. tin(IV) oxide
26. barium chromate
27. HBr
28. Cr2(CO3)3
29. MgS
30. ICl3
31. LiH
32. NH4OH
33. CaCl2
34. H2Se
35. Fe3N2
36. Al(OH)3
37. SnF2
38. SCl4
39. HgI2
40. P2O5
41. H2SO3
42. Pb(NO3)2
43. H2O
44. Na2C2O4
45. HClO4
46. HClO2
47. SiO2
48. H2CO3
49. NaClO3
50. XeF6
51. Ni(NO3)2
52. KClO4
Read over your notes, and rework your homework assignments and
quizzes (especially those you didn’t do well on). You will be provided
with the periodic table reference sheet as well as necessary
electronegativity values. You will do AWESOME on this test if you
can do the following things.
INTRODUCTION TO BONDING





Explain what chemical bonds are and why they form.
Identify characteristics of covalent, ionic, and metallic bonding.
Compare and contrast nonpolar, polar, and ionic bonds.
Determine bond type using electronegativity values.
Define the following terms:
 binary/ternary compound
 monatomic/polyatomic ion
MOLECULAR, IONIC, & ACIDS
 Use Lewis structures to show the formation of molecular and ionic
substances from individual atoms. Label partial charges (/) if
polar and full charges (+/) if ionic.
 Name and write formulas for molecular compounds, ionic
compounds, and acids.
 Define the following terms:
 potential energy
 dipole
 bond energy
 electronegativity
 lattice energy
 Explain the following concepts:
 the relationship between potential energy and stability.
 the effect of attractive and repulsive forces on stability as two
atoms approach each other (PE diagram).
 the relationship between bond length & bond energy.