1. Unit 6: Ionic Bonding & Nomenclature

2. Section 1: Ions
Pyrite (FeS2) is a common mineral that is often mistaken for gold—hence its nickname, “fool’s gold.” Pyrite is an example of a crystalline solid. In this chapter, you will learn about crystalline solids composed of ions that are bonded together. But first you need to understand how ions form from neutral atoms.
1-2,11-13,15,19-21

3. Valence Electrons: Group # = Valence #
electrons in the highest occupied energy level
9-Fluorine (F)
10-Neon (Ne)
11-Sodium (Na)
- determines chemical properties
- only e- involved in chemical reactions

4. Electron dot structures:
diagrams showing valence e- as dots

5. Electron dot structures:
diagrams showing valence e- as dots

6. Electron dot structures:
diagrams showing valence e- as dots

7. Electron dot structures:
diagrams showing valence e- as dots

8. Electron dot structures:
diagrams showing valence e- as dots

9. Electron dot structures:
diagrams showing valence e- as dots

10. Electron dot structures:
diagrams showing valence e- as dots

11. Electron dot structures:
diagrams showing valence e- as dots

12. Electron dot structures:
diagrams showing valence e- as dots

13. Ne The Octet Rule most atoms form bonds to have 8 valence e-
full outer energy level
like the Noble Gases Ne
Lewis dot structure

14. Cations Anions metals lose electrons to form positive ions
leaving a complete octet in the next-lowest energy level.
Anions
nonmetals gain electrons to form negative ions
to achieve a complete octet in its valence level.

15. The electron configuration of the sodium ion is the same as that of a neon atom.
Use egg with 10 marbles inside, and 1 outside for Na valence electron.

16. Na Mg Na+ Mg2+ Group 1 always 1+ charge Group 2 always 2+ charge 7.1
Cations of Group 1A elements have a charge of 1+. Cations of Group 2A elements have a charge of 2+.

17. Ionic Compounds
Charges of Ions 1+ 2+ 3+

18. 7.1
Formation of Anions
The electron configuration of the chloride ion is the same as that of argon.

19. 7.1
Formation of Anions
Oxygen is in Group 6A.

20. F F - O O 2- N N 3- Group 17 (7A) always 1- charge Group 16 (6A)
7.1
Group 17 (7A)
always 1- charge F F -
Group 16 (6A)
always 2- charge O O 2-
Atoms of nonmetals and metalloids form anions by gaining enough valence electrons to attain the electron configuration of the nearest noble gas. Interpreting Diagrams In which group of the periodic table do the elements bromine and iodine belong?
Group 15 (5A)
always 3- charge N N 3-

21. Anions names typically end in -ide Nonmetal Monatomic Anions Ion Name
7.1
Anions names typically end in -ide
Nonmetal
Monatomic Anions
Ion Name
Fluorine F-
Fluoride
Chlorine
Cl-
Chloride
Bromine
Br-
Bromide
Iodine I-
Iodide
Oxygen
O2-
Oxide
Sulfur
S2-
Sulfide
Nitrogen
N3-
Nitride
Phosphorus
P3-
Phosphide

22. charges vary but always +
Charges of Ions 1+ 2+ 3+ 3- 2- 1-
charges vary but always +

23. Iodine gains __ e- to form ___ Magnesium loses __ e- to form ___
7.1
Conceptual Problem 7.1
Fill in the blanks.
Iodine gains __ e- to form ___
Magnesium loses __ e- to form ___
Sulfur _____ __ e- to form ___
Aluminum _____ __ e- to form ___ 1 I-
Mg2+ 2
gains 2
S2-
loses 3
Al3+

24. Quick Quiz!
1. How many valence electrons are in an atom of oxygen? 2 4 6 8

25. Quick Quiz.
2. Atoms that tend to gain a noble gas electron configuration by losing valence electrons are
metals.
nonmetals.
halogens.
anions.

26. Quick Quiz.
3. When a magnesium atom forms a cation, it does so by
losing two electrons.
gaining two electrons.
losing one electron.
gaining one electron.

27. Quick Quiz.
4. When a bromine atom forms an anion, it does so by
losing two electrons.
gaining two electrons.
losing one electron.
gaining one electron

28. Quick Quiz.
5. Write the name and the symbol of the ion formed from a nitrogen atom.
nitrogen ion, N3+
nitride, N-
nitride, N3-
nitrogen ion, N2-