Chapter 3 Unit Test Review

Molecular Compounds, Ionic Compounds,

NAME THE FOLLOWING COMPOUNDS:

1.  BaSO3

2.  (NH4)3PO4

3.  PBr5

4.  MgSO4

5.  CaO

6.  Na2Cr2O7

7.  MgO

8.  SO3

9.  Cu(NO3)2

10.  N2O

11.  MnO

12.  AgNO3

13.  As2O5

14.  Fe2O3

15.  N2O3

16.  NaHCO3

17.  SiBr4

18.  CuCl2

19.  SnO2

20.  BaCrO4

WRITE FORMULAS FOR THE FOLLOWING COMPOUNDS:

21.  chromium (III) carbonate

22.  magnesium sulfide

23.  iodine trichloride

24.  lithium hydroxide

25.  ammonium hydroxide

26.  calcium chloride

27.  iron(II) nitride

28.  aluminum hydroxide

29.  tin(II) fluoride

30.  sulfur tetrachloride

31.  mercury(II) iodide

32.  diphosphorus pentoxide

33.  lead(II) nitrate

34.  dihydrogen monoxide

35.  sodium oxalate

36.  silicon dioxide

37.  sodium chlorate

38.  xenon hexafluoride

39.  nickel nitrate

40.  potassium perchlorate

Draw the Lewis structures for the following:

CCl4

Na2O

SO3

SF6

Fe2S3

Determine the Molecular Geometry for the following. Determine the main intermolecular force takes place for each.

H2O

CH4

H2S

NOMENCLATURE REVIEW

Molecular Compounds, Ionic Compounds

ANSWER KEY

  1. barium sulfite
  2. ammonium phosphate
  3. phosphorus pentabromide
  4. magnesium sulfate
  5. calcium oxide
  6. sodium dichromate
  7. magnesium oxide
  8. sulfur trioxide
  9. copper(II) nitrate
  10. dinitrogen monoxide
  11. manganese(II) oxide
  12. silver nitrate
  13. diarsenic pentoxide
  14. iron(III) oxide
  15. dinitrogen trioxide
  16. sodium bicarbonate
  17. silicon tetrabromide
  18. copper(II) chloride
  19. tin(IV) oxide
  20. barium chromate
  1. Cr2(CO3)3
  2. MgS
  3. ICl3
  4. LiOH
  5. NH4OH
  6. CaCl2
  7. Fe3N2
  8. Al(OH)3
  9. SnF2
  10. SCl4
  11. HgI2
  12. P2O5
  13. Pb(NO3)2
  14. H2O
  15. Na2C2O4
  16. SiO2
  17. NaClO3
  18. XeF6
  19. the trick here is that Ni2+ is commonly referred to as just “nickel” = Ni(NO3)2
  20. KClO4