Unit 5 - Ionic Bonding Study Guide
Name: ______KEY______________________________________________ Period: _____ Date: _________
Review Ionic Bonds
1. What two types of elements will transfer electrons to form an ionic bond?
Metal & nonmetal
2. What is an ionic bond?
An electrostatic force that holds together a cation and anion
3. How can you describe the electrical charge of an ionic compound?
Neutral
4. Metals will lose all of their valence electrons to form a positively charged cation. The oxidation number
will be equal to the number of valence electrons.
5. Nonmetals will gain valence electrons to form a negatively charged anion. The oxidation number will
be equal to 8 – the # of valence electrons.
6. Which elements are least likely to undergo bonding? Noble Gases
7. Write the oxidation number for the
following elements.
a. Cesium
___+1____
b. Potassium
___+1____
c. Aluminum
___+3____
d. Iron (III)
___+3____
e.
f.
g.
h.
i.
j.
Magnesium
Barium
Nitrogen
Iodine
Oxygen
Selenium
8. Which alkali metal has the highest ionization energy? Hydrogen
9. Which alkaline earth metal has the lowest ionization energy? Radium
10. What properties characterize ionic compounds?
 High melting point & boiling point
 Solid at room temperature
 Brittle
 Ionic solids can’t conduct electricity
 Molten ionic compounds can conduct electricity
Transferring of Electrons
11. Please draw the transfer of electrons for the following:
a. NaBr
___+2____
___+2____
___-3____
___-1____
___-2____
___-2____
b. MgO
c.
CaF2
d. K2S
12. How do the following atoms fulfill the octet rule when they form ionic bonds? What valence or
oxidation number does each of these have?
a. Lithium
Loses 1 e-; valence 1+
b. Beryllium
Loses 2 e-; valence 2+
c. Boron
Loses 3 e-; valence 3+
d. Carbon
Loses 4 e-; valence 4-
e. Nitrogen
Gains 3 e-; valence 3f. Oxygen
Gains 2 e-; valence 2g. Fluorine
Gains 1 e-; valence 1h. Neon
Full shell – no change
13. Define the indicators (what you look for) that identify each type of compound based on their names and
their formulas:
a. Simple Binary Ionic –
i. Name – Group 1A/2A metal or Aluminum & Nonmetal with “ide” ending
ii. Formula – Group 1A/2A metal or Aluminum & Nonmetal
b. Polyvalent Binary Ionic –
i. Name – Roman Numerals!
ii. Formula – Transition Metal & Nonmetal
c. Polyatomic Ionic –
i. Name – Metals & anions with “ate” or “ite” endings
ii. Formula – Parentheses!
Writing Formulas for Ionic Compounds
Write the formula for the following ionic compounds:
14. Barium oxide
15. Lithium nitride
16. Magnesium fluoride
17. Lithium phosphate
18. Calcium iodide
19. Copper (II) nitrite
20. Beryllium chloride
21. Gold (III) carbonate
22. Potassium sulfate
23. Calcium hydroxide
24. Barium chloride
25. Lithium oxide
26. Magnesium oxide
27. Calcium fluoride
28. Iron (II) chloride
29. Silver bromide
BaO
Li3N
MgF2
Li3PO4
CaI2
Cu(NO2)2
BeCl2
Au2(CO3)3
K2SO4
Ca(OH)2
BaCl2
Li2O
MgO
CaF2
FeCl2
AgBr
Naming Ionic Compounds
Write the name for the following ionic compounds. Be sure to include parenthesis with Roman numeral for
the transition metals:
30. AlBr3
31. Fe2(SO3)3
32. MgCl2
33. K3PO4
34. TiCl2
35. Cr2O3
36. Ag2S
37. Cu(OH)2
38. Zn3N2
39. AgNO3
40. PbF2
41. Cu2S
42. CaF2
43. FeCl3
44. Li3P
45. Au(C2H3O2)3
aluminum bromide
iron (III) sulfite
magnesium chloride
potassium phosphate
titanium (II) chloride
chromium (III) oxide
silver (I) sulfide
copper (II) hydroxide
zinc (II) nitride
silver (I) nitrate
lead (II) fluoride
copper (I) sulfide
calcium fluoride
iron (III) chloride
lithium phosphide
Gold (III) acetate