1. No category

Ionic Compounds Worksheet 1
Directions: Write the formula unit for the given ionic compound if the name is given. If the formula unit
is provided write the name of the ionic compound
1. Lithium oxide
21. CaO
2. Calcium fluoride
22. PI3
3. Aluminum sulfide
23. BaF2
4. Potassium nitride
24. MnO
5. Barium oxide
25. SnO2
6. Copper (I) oxide
26. CuF
7. Tin (IV) sulfide
27. MgS
8. Magnesium iodide
28. AlN
9. Iron (III) bromide
29. CaF2
10. Chromium (II) selenide
30. K2S
11. Tin (II) fluoride
31. SnO
12. Magnesium oxide
32. Ba3N2
13. Lead (IV) sulfide
33. K2S
14. Manganese (III) bromide
34. CoN
15. Copper (II) sulfide
35. PbS2
16. Chromium (III) iodide
36. RbF
17. Iron (II) nitride
37. NaCl
18. Rubidium phosphide
38. SnO
19. Mercury (II) nitride
39. CaS
20. Manganese (IV) nitride
40. Li2O
41. Why do metals lose electrons and nonmetals gain electrons?
42. What is the charge of an ionic compound?
43. List 3 properties of ionic compounds
Not an Ionic Compound… Why?
1. Circle the atom of the element that has a larger atomic radius
Magnesium
or
Fluorine
2. Circle the atom of the element that requires more energy to lose electrons (greater ionization
energy)
Magnesium
or
Fluorine
3. Show how Magnesium and Fluorine chemically combine to form Magnesium fluoride using
Lewis dot structures
4. Write the electron configuration for
Mg _____________________________________________________
Mg2+____________________________________________________
F_______________________________________________________
F-_______________________________________________________
1. Circle the atom of the element that has a larger atomic radius
Aluminum
or
Sulfur
2. Circle the atom of the element that requires very little energy to lose electrons (small ionization
energy)
Aluminum
or
Sulfur
3. Show how Aluminum and Sulfur chemically combine to form Aluminum sulfide using Lewis dot
structures
4. Write the electron configuration for
Al _____________________________________________________
Al3+____________________________________________________
S_______________________________________________________
S2-______________________________________________________
5. Why do transition metals, when becoming ions, need a roman numeral after the name when
Group 1,2 and 3 metals do not when becoming ions?