1. Ionic Compounds & Metals
Chapter 7

2. Section 1
Ion Formation

3. Chemical Bond The force that holds two atoms together. Recall…
Valence Electrons – bonding occurs between the valence electrons of two atoms
Electron-Dot Structures – help us to determine where as chemical bond may form based on the octet rule.

4. Positive Ion Formation
Called a cation
A positive ion forms when an atoms loses on or more valance electrons in order to attain a noble gas configuration.
Write the electron configurations for Ne Na

5. Metal Ions – are reactive because they lose valence electrons easily.
Group 1 and 2 are the most reactive metals on the periodic table.
Transition Metal Ions – These metals tend to form ions with a +2 or +3 charge.
Pseudo-Noble Gas Configurations
The formation of an octet is the most stable electron configuration.
Elements in groups lose electrons to form an outer energy level containing full s, p, and d sublevels.

6. Negative Ion Formation
Called an anion
A negatively charge ion
Nonmetals form anions
Write the Electron Configurations Ar Cl

7. Ionic Bonds & Ionic Compounds
Section 2
Ionic Bonds & Ionic Compounds

8. Ionic Compounds – Are compounds that contain ionic bonds.
Ionic Bond - formed between a metal and a nonmetal; involves a complete transfer of electrons
Results in two ions with full positive and negative charges
These ions then attract each other due to electrostatic force
Ionic Compounds – Are compounds that contain ionic bonds.

9. Binary Ionic Compounds
Many ionic compounds are binary, which means that they contain only two different elements.
Binary ionic compounds contain a metallic cation and a nonmetallic anion.

10. Properties of Ionic Compounds
Physical Structure
Large numbers of cations and anions exist together in a specific ratio. These ions are packed tightly into a regular repeating pattern that balances the oppositely charged forces.

11. The strong attractions among the positive ions and the negative ion in an ionic compound result in the formation of a crystal lattice.
A crystal lattice is a three-dimensional geometric arrangement of particles.

12. Physical Properties Melting Point, boiling Point and hardness
These are all physical properties that depend on how strongly the particles that make up the matter are attracted to one another.
Electrolyte – An ionic compound whose aqueous solution conducts an electric current.

13. Energy & the Ionic Bond
During every chemical reaction, energy is either absorbed or released.
If energy is absorbed during a chemical reaction, the reaction is said to be endothermic.
If energy is released during a chemical reaction, the reaction is said to be exothermic.

14. The formation of ionic compounds from positive ions and negative ion is always exothermic.
If the amount of energy released during bond formation is reabsorbed, the bonds holding the positive ions and negative ions together will break apart.

15. Lattice Energy
Because the ions in an ionic compound are arranged in a crystal lattice, the energy required to separate 1 mol of the ions of an ionic compound is referred to as the lattice energy.
The strength of the forces holding ions in place is reflected by the lattice energy.

16. Names & Formulas for Ionic Compounds
Section 3
Names & Formulas for Ionic Compounds

17. Formula Unit – The chemical formula for an ionic compound.
Monatomic Ion – A one-atom ion.
Example:

18. Oxidation Number
The oxidation number of an element in an ionic compound equals the number of electrons transferred from the atom to form the ion.
Example:

19. Formulas for Binary Ionic Compounds
In the chemical formula for an ionic compound, the symbol of the cation is always written first, followed by the symbol of the anion.

20. Examples…

21. Polyatomic Ions
Polyatomic ions are ions made up of more than one atom.
A polyatomic ion acts as an individual ion in a compound and its charge applies to the entire group of atoms.
A polyatomic ion exists as a unit and because of that the subscripts of the atoms within the ion are NEVER changed.

22. Metallic Bonds & the Properties of Metals
Section 4
Metallic Bonds & the Properties of Metals

23. Metallic Bonds
Electron Sea Model – proposes that all the metal atoms in a metallic solid contribute their valence electrons to form a “sea” of electrons. This sea of electron surrounds the metal cations in the lattice.
The electrons present in the outer energy levels of the bonding metallic atoms are not held by any specific atoms and can move easily from one atom to the next, because of this they are often referred to as delocalized electrons.
A metallic bond is the attraction of metallic cation for delocalized electrons.

24. Properties of Metals Melting & Boiling Points
Malleability, ductility, & durability
Thermal conductivity & electrical conductivity
Hardness & strength