Unit 6: Ionic Bonding & Nomenclature

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

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

Electron dot structures: diagrams showing valence e- as dots

Electron dot structures: diagrams showing valence e- as dots

Electron dot structures: diagrams showing valence e- as dots

Electron dot structures: diagrams showing valence e- as dots

Electron dot structures: diagrams showing valence e- as dots

Electron dot structures: diagrams showing valence e- as dots

Electron dot structures: diagrams showing valence e- as dots

Electron dot structures: diagrams showing valence e- as dots

Electron dot structures: diagrams showing valence e- as dots

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

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.

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.

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+.

Ionic Compounds Charges of Ions 1+ 2+ 3+

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

7.1 Formation of Anions Oxygen is in Group 6A.

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-

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

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

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+

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

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

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.

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

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-