1. Chapter 7: Ionic Compounds & Metals
Chemistry

2. Section 7.1 Ion Formation Valence Electrons and Chemical Bonds…
A chemical bond is the force that holds two atoms together.
Chemical bonds form by the attraction between the positive nucleus of one atom and the negative electrons of another atom.

3. Atom’s try to form the octet—the stable arrangement of eight valence electrons in the outer energy level—by gaining or losing valence electrons.

4. Positive Ion Formation
A positively charged ion is called a cation.
Metals are reactive because they lose valence electrons easily.

5. Negative Ion Formation
An anion is a negatively charged ion.
Nonmetal ions gain the number of electrons required to fill an octet.

6. Section 7.2 Ionic Bonds and Ionic Compounds
The force that holds oppositely charged particles together in an ionic compound is called an ionic bond.

7. Compounds that contain ionic bonds are called ionic compounds.
Binary ionic compounds are made from a metal and a nonmetal. Ex: NaCl
Sodium Chloride Formation

8. Properties of Ionic Compounds
The repeating pattern of particle packing in an ionic compound is called an ionic crystal.
The strong attractions among the positive and negative ions result in the formation of the crystal lattice.

9. A crystal lattice is the three-dimensional geometric arrangement of particles, and is responsible for the structure of many minerals.
Calcite - CaCO3
Galena - PbS
Salesite - CuIO3OH

10. Ionic compounds have very high melting points and boiling points.

11. Solid ions are poor conductors of electricity because the ions are locked in place.
Liquid ions or aqueous solutions of ionic compounds are good conductors of electricity since their ions can move freely.
An ion in aqueous solution that conducts electricity is an electrolyte.

12. Crystals break apart when an external force is applied to form smaller crystals.

13. Energy and the Ionic Bond
Reactions that absorb energy are endothermic.
Ammonium thiocyante is mixed with barium hydroxide.
A drop of water is placed on a block of wood.
The bottom of the bottom becomes cold enough to freeze the water and stick to the wood.

14. Hindenberg Explosion, May 6, 1937
Reactions that release energy are exothermic.
Hindenberg Explosion, May 6, 1937
Hindenberg Explosion

15. Energy and the Ionic Bond
To break apart the crystal lattice of an ionic compound, much energy must be added – it is called lattice energy.
Smaller ions and ions with higher charges are more difficult to break apart and require more lattice energy.

17. Section 7.3 Names and Formulas for Ionic Compounds
Chemists around the world must communicate with one another, so a standardized system of naming compounds was developed.

18. Formulas for Ionic Compounds
A formula unit represents the simplest ratio of the ions involved.
Monatomic ions are one-atom ions.

19. Oxidation number, or oxidation state, is the charge of a monatomic ion.

20. The symbol for the cation is always written first, followed by the symbol of the anion.
Subscripts represent the number of ions of each element in an ionic compound.
NaCl H2O
LiNO Al2(CO3)3

21. The total charge must equal zero in an ionic compound.
If the charges do not add up to equal zero, use the Criss-Cross Method.

22. Polyatomic ions are ions made up of more than one atom.
Never change subscripts of polyatomic ions!!!
If more than one polyatomic ion is needed, place in parentheses and write the appropriate subscript outside the parentheses.

24. Names for Ions and Ionic Compounds
An oxyanion is a polyatomic ion composed of an element (usually a non-metal), bonded to one or more oxygen atoms.

26. Chemical nomenclature is a systematic way of naming compounds.
Name the cation followed by the anion.
For monatomic, cations use the element name.
For monatomic anions, use the root element name and the suffix –ide.
To distinguish between different oxidation states of the same element, the oxidation state is written in parentheses after the name of the cation.
When the compound contains a polyatomic ion, name the cation followed by the name of the polyatomic ion.