1. Section 6-3: Ionic Bonding and Ionic Compounds Coach Kelsoe Chemistry Pages 190-194

2. Section 6-3 Objectives Compare and contrast a chemical formula for a molecular compound with one for an ionic compound. Discuss the arrangement of ions in crystals. Define lattice energy and explain its significance.

3. Section 6-3 Objectives List and compare the distinctive properties of ionic and molecular compounds Write the Lewis structure for a polyatomic ion given the identity of the atoms combined and other appropriate information.

4. Intro to Ionic Compounds An ionic compound is composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal. Sodium chloride, or table salt, is composed of a sodium cation with a 1+ charge and a chloride anion with a 1– charge. Their charges balance out. It is an ionic compound.

5. Intro to Ionic Compounds Most ionic compounds exist as crystalline solids, like rocks and minerals. A crystal of any ionic compound is a three- dimensional network of positive and negative ions mutually attracted to one another. Because of this, an ionic compound is not made of independent, neutral units that can be isolated and examined, unlike covalent compounds.

6. Intro to Ionic Compounds The chemical formula of an ionic compound shows the ratio of the ions present in a sample of any size. A formula unit is the simplest collection of atoms from which an ionic compound’s formula can be established. In naming anions, the –ine ending of the element’s name is replaced with -ide.

7. Intro to Ionic Compounds The ratio of ions in a formula depends on the charges of the ions combined. For example, combining calcium and fluorine to form calcium fluoride: –Calcium has a charge of 2+ –Fluoride has a charge of 1– –Therefore there needs to be two fluoride anions to balance out the 2+ of calcium. –CaF 2

8. Formation of Ionic Compounds Electron-dot notation can be used to demonstrate the changes that take place in ionic bonding. Let’s consider sodium chloride again… –Sodium has 1 valence electron –Chlorine has 7 valence electrons –We know that alkali metals (Na) readily lose 1 electron to form a cation and halogens (Cl) readily gain 1 electron to form an anion. –See board; also Calcium fluoride

9. Characteristics of Ionic Bonding Nature favors arrangements where potential energy is minimized. In an ionic crystal, ions minimize their potential energy by combining in an orderly arrangement known as a crystal lattice.

10. Characteristics of Ionic Bonding The attractive forces at work within an ionic crystal include those between oppositely charged ions and those between the nuclei and electrons of adjacent ions. The repulsive forces include those between like-charged ions and those between electrons of adjacent ions.

11. Sodium Chloride

12. Characteristics of Ionic Bonding Each sodium cation (yellow) is surrounded by six chloride anions (green). In turn, each of those six chloride anions are surrounded by six sodium cations.

13. Crystal Lattice of NaCl

14. Characteristics of Ionic Bonding The 3-D arrangements of ions and the strengths of attraction between them vary with the sizes and charges of the ions. To compare bond strengths in ionic compounds, chemists compare the amounts of energy released when separated ions in a gas come together to form a crystalline solid.

15. Characteristics of Ionic Bonding Lattice energy is the energy released when one mole of an ionic crystalline compound is formed from gaseous ions. The energy values in your book are listed as negative to indicate that energy is released when the crystals are formed.

16. A Comparison of Ionic and Molecular Compounds The force that holds ions together is a very strong overall attraction between positive and negative charges. In a molecular compound, the covalent bonds of the atoms making up each molecule are also strong, but the forces of attraction between molecules are much weaker than the forces of ionic bonding. This gives rise to 2 types of compounds

17. A Comparison of Ionic and Molecular Compounds Ionic compounds consist of positive and negative ions bound together by electrical attraction. They have a high melting point and are harder to vaporize. Molecular compounds are groups of atoms held together by covalent bonding, or the sharing of electrons. They have a low melting point and are very easy to vaporize.

18. Polyatomic Ions Certain atoms bond covalently with each other to form a group of atoms that has both molecular and ionic characteristics. A charged group of covalently bonded atoms is known as a polyatomic ion. Polyatomic ions combine with ions of opposite charge to form ionic compounds

19. Polyatomic Ions The charge of a polyatomic ion results from either an excess (negative charge) or shortage (positive charge) of electrons. Examples: –Ammonium ion – [NH 4 ] + –Phosphate ion – [PO 4 ] 3– To draw a polyatomic ion Lewis structure, you will need to consider the total number of protons and electrons in the ion.

20. Vocabulary Formula unit Ionic compound Lattice energy Polyatomic ion