1. Ionic Compounds and Metals
Chapter 7
Ionic Compounds and Metals

2. Section 7.1
Ion formation

3. Chemical Bonds
A chemical bond is the force that holds two atoms together.
Can form by the attraction between the positive nucleus of one atom and the negative electrons of another
Can form between positive and negative ions

4. Valence Electrons Electrons in the outermost principal energy level
Shown in the electron dot structures
Octet rule – atoms will gain, lose or share electrons to obtain 8 valence electrons
The valence electrons determine the bonding properties of the atom

5. Positive Ion Formation
A positively charged ion is called a cation.
Positive ions are formed when an atom loses one or more valence electrons
Metals make positive ions

6. Negative Ion Formation
A negatively charged ion is called an anion.
Negative ions are formed when an atom gains one or more electrons in its valence shell.
Nonmetals make negative ions.

7. Ionic bonds and ionic compounds
Section 7.2
Ionic bonds and ionic compounds

8. Formation of an Ionic Bond
An ionic bond is the electrostatic force that holds oppositely charged particles together in an ionic compound
Compounds that contain ionic bonds are called ionic compounds.
Ionic compounds are formed between metals (+ charge) and nonmetals (- charge).

9. Binary Ionic Compounds
Contain a metallic cation and a nonmetallic anion.
Formation of Binary Ionic Compounds
Electron(s) is/are transferred from metal to nonmetal
Metal becomes positive, nonmetal becomes negative
Opposite charges attract

10. Properties of Ionic Compounds
Take the structure of a crystal lattice
Many units of positive and negative ions stick together in a three-dimensional geometric arrangement
Can conduct electricity when dissolved in water (they are electrolytes and break into ions when dissolved in water), but not in solid form
Melting point, boiling point and hardness depend upon how strongly the ions are attracted to each other

11. Names and formulas for ionic compounds
Section 7.3
Names and formulas for ionic compounds

12. Formulas for Ionic Compounds
Monatomic ions are one-atom ions
Examples: Mg2+ , Br-
Oxidation numbers are the charges on ions
Note: some elements have multiple oxidation states – you will have a periodic table to tell this
Binary ionic compounds are made of two monatomic ions (one positive, one negative)

13. Formulas for Binary Ionic Compounds
Symbol for cation is written first, anion second
Subscripts tell the number of atoms of each element
What are the following compounds made of?
CaF calcium, 2 fluorine
Na2S sodium, 1 sulfur
NaCl sodium, 1 chlorine

14. Naming Binary Ionic Compounds
Name the cation first
Name the anion second with –ide at the end
Examples
CaF2  calcium fluoride
Na2S  sodium sulfide
NaCl  sodium chloride

15. Try Naming a few more Binary Ionic Compounds
K2O potassium oxide
Al2S3 aluminum sulfide
Na3N sodium nitride

16. What if the cation has more than one oxidation state?
You tell which ion was used by putting a Roman Numeral after the name of the cation
Example:
CuS
We know S was -2 (that’s the only one it makes)
If there is only one atom of each element, the Cu must have been +2
So, the name is written as Copper (II) sulfide [the “II” indicates the charge]
Make sure, especially with transition elements, that you are checking the oxidation states

17. Writing Formulas for Binary Ionic Compounds
Look up the charges for each element
For a compound to form, the total charge must balance out to zero (positive charges must equal negative charges)
Example:
Sodium bromide
Na is +1, Br is -1
Only need one of each to balance
Formula is NaBr

18. Try writing some more formulas Binary Ionic Compounds
Potassium Iodide KI
Aluminum bromide AlBr3
Magnesium chloride MgCl2
Cesium nitride Cs3N

19. Formulas for Polyatomic Ionic Compounds
Polyatomic ions are ions that are made up of more than one atom
You will have a chart for these and do not have to memorize them.
Examples:
SO42- = sulfate
CN- = cyanide
NH4+ = ammonium

20. Naming Polyatomic Ionic Compounds
Name the cation first, anion second
Name the polyatomic as is – don’t change its name at all
Examples:
Ca3(PO4)2 calcium phosphate
Mg(CN)2 magnesium cyanide
NH4Cl ammonium chloride

21. Now you try naming Polyatomic Ionic Compounds
NaNO3 sodium nitrate
Ca(ClO3)2 calcium chlorate
Al2(CO3)3 aluminum carbonate

22. Writing formulas for Polyatomic Ionic Compounds
Same as binary ionic compounds EXCEPT you may not change anything in the polyatomic ion formula
Put them in a “bubble” and put subscripts outside that bubble
Example:
Calcium Nitrate
Ions are Ca2+ and NO3-
Formula will be Ca(NO3)2

23. Now you try writing formulas for Polyatomic Ionic Compounds
Sodium hydroxide NaOH
Copper (II) nitrate Cu(NO3)2
Silver chromate Ag2CrO4

24. Metallic bonds and the properties of metals
Section 7.4
Metallic bonds and the properties of metals

25. Metallic Bonds
The electron sea model proposes that all the metal atoms in a metallic solid contribute their valence electrons to form a “sea” of electrons
Since the electrons are free to move, they are called delocalized electrons
A metallic bond is the attraction of a metallic cation for delocalized electrons

26. Properties of Metals (revisited)
Moderately high melting points
High boiling points
Malleable, ductile, durable
Conduct heat and electricity well
Transition metals are harder/stronger than alkali metals because the transition metals have more delocalized electrons