1. The Composition of Chemical Compounds

2. Formation of Simple Ions (Monatomic Ions)
Metals have a tendency to lose electrons to become positively charged ions. (cations)
Eg - Na -- loses one e- --> Na+
Ca -- loses two e- --> Ca2+
Al -- loses three e- --> Al3+
Metals have a tendency to lose their valence electrons.

3. Formation of Simple Ions (Monatomic Ions)
Non-metals with 5, 6, or 7 valence electrons have a tendency to gain electrons to become negatively charged ions (anions)
Eg - Cl -- gains one e- --> Cl-
S -- gains two e- --> S2-
N -- gains three e- --> N3-

4. Ions of Multi-Valent Metals
Some metals, such as iron and copper can form more than one ion each with its own charge.
Eg. Fe iron (II) ion
Fe iron (III) ion
Cu copper (II) ion
Cu copper (I) ion
Note: on the periodic table the more common one is listed first.

5. Formation of Complex Ions (Polyatomic Ions)
Groups of atoms will sometimes behave as a single unit. They will usually accept electrons to become negatively charged ions.
PO43- - the phosphate ion
SO42- - the sulfate ion
Cr2O72- - the dichromate ion

6. Formation of Complex Ions (Polyatomic Ions)
One exception is the ammonium ion which loses an electron to become positively charged.
NH4+
Note: See examples of other polyatomic ions on the periodic table of the ions

7. Formation of Binary Ionic Compounds
Binary ionic compounds contain two different kinds of simple ions.
Electrons are transferred from the metal atom to the non-metal atom. The attraction of positive(+) and negative(-) charges forms an ionic bond

8. Formation of Binary Ionic Compounds
Eg. Na transfers an electron to an atom of Cl to form NaCl
Note: the net electric charge of a compound is zero.
(1-) (1-)
Na+Cl Ca2+Cl Al3+Cl3-
Charges are not shown in the chemical formula
NaCl CaCl2 AlCl3

9. Formation of Binary Ionic Compounds
Binary ionic compounds contain a metal(which is listed first) and a nonmetal.
The combination of a metal and a nonmetal must be yield a net charge of zero.
Ionic compounds are written with the simplest whole number ratio of ions

10. Formation of Compounds of Multi-Valent Ions
Eg - in the reaction between iron and oxygen two products are possible
Fe3+O2- Fe2+O2-
Fe2O3(s) FeO(s)
iron(III) oxide iron(II) oxide

11. Formation of Compounds of Polyatomic Ions
The charge on the polyatomic ion is the charge on the unit.
Na+ with NO3- forms NaNO3
Ca2+ with NO3- forms Ca(NO3)2
Note: in the second example two nitrate ions are required to combine with one calcium ion so the ion is in brackets before doubling

12. Steps in Writing Chemical Formulas for Ionic Compounds
1. Predict the chemical symbol for each ion in the name.
2. Predict the simplest whole number ratio of the ions to obtain a total charge of zero.
3.Subscripts indicate the relative number of ions present.
4. Charges are not shown.

13. Naming Binary Ionic Compounds
1. Name the positive ion with its metal name.
2. The negative ion has a shortened name with an “ide” ending.
Eg - NaCl is sodium chloride
CaCl2 is calcium chloride
Al2S3 is aluminum sulfide

14. Naming Ionic Compounds with Polyatomic ions
1. Name the positive ion with its metal name (or the ammonium ion NH4).
2. The negative ion is named by the name of the polyatomic ion.
Eg - Na2SO4 - sodium sulfate
NH4NO3 - ammonium nitrate

15. Ionic Hydrates
Hydrates produce water when they decompose upon heating.
When the formula of a hydrated compound is written, the number of water molecules is also included
eg.copper (II) sulfate pentahydrate is written as CuSO4•5H2O.

16. Naming Ionic Hydrates
Classical Method - the number of water molecules is indicated with a prefix in front of the word hydrate
Use the following prefixes to indicate the number of water molecules.
mono = 1 hexa = 6
di = 2 hepta = 7
tri = 3 octa = 8
tetra = 4 nona = 9
penta = 5 deca = 10

17. Naming Ionic Hydrates cont.
IUPAC method - the number of water molecules in the hydrate is indicated with -X-water, where X represents the number of water molecules
eg. the name for CuSO4•5H2O is copper II sulfate-5-water

18. Do to the end of Page 32.

19. Properties of Acids Acids have a pH below 7
Are soluble in water to some degree.
Acidic solutions conduct electricity.
Turn blue litmus paper red.
Turn bromothymol blue to yellow.
Turn phenolphthalein colorless

20. Properties of Acids React with active metals to produce H2
Acids come in any physical state.
Acids taste sour.
Acids neutralize bases

21. Naming Acids - Classic System
Ionic Name Acid Name
hydrogen ____ ide hydro___ ic acid
hydrogen ____ ate _______ ic acid
hydrogen ____ ite ______ous acid

22. Naming Acids - IUPAC System
Ionic Name Acid Name
hydrogen ____ ide aqueous hydrogen _____ ide
hydrogen ____ ate aqueous hydrogen _____ ate
hydrogen ____ ite aqueous hydrogen _____ ite.

23. Properties of Bases Bases do not react with metals to produce hydrogen
Bases are usually solids
Bases neutralize acids
Bases have a pH above 7
Bases are usually soluble in water
Bases feel slippery to the touch.

24. Chemical Bonding Covalent Bonds
An attraction between non-metallic atoms.
Atoms share electrons to become noble - gas - like.
Simultaneous attraction

25. Covalent Compounds Molecular Formulas
Non-metallic atoms bond to form molecules and a molecular formula is the chemical formula of a molecule. Molecular substances contain only non-metallic atoms bonded covalently.

26. Molecular Elements 1) Non-molecular, non-metallic elements
C or Cn Si or Sin
2) Molecular monatomic elements
- noble gases - He, Ne, Ar, Kr, Xe, and Rn

27. Molecular Elements 3) Molecular diatomic elements - the “gens”
- the halogens
F2, Cl2, Br2, I2, and At2
- along with H2, N2, and O2
4) Polyatomic molecular elements
P4 and S8

28. Binary Molecular Compounds
Binary - 2 kinds of atoms
Molecular - contain non-metals
Nomenclature (naming)
- 1st element named in full
- 2nd element shortened with “ide” ending.

29. The Prefix System
the same prefixes as were used for hydrated ionic compounds are used to indicate the number of each type of atom
CO carbon monoxide
N2O dinitrogen monoxide

30. Memorized Molecular Compounds
many compounds have historical names that have stuck.
Eg. H2O is water, not dihydrogen oxide
a list of these compounds that must be memorized is found on page 34 of Nelson Chemistry

31. Binary Molecular Compounds
Eg. - CO - carbon monoxide
- SF6 - sulfur hexafluoride
- CCl4 - carbon tetrachloride
Some compound formula need to be memorized because they do not follow IUPAC rules

32. Do the end of #24 on Page 41.
That would mean ALL of pages 36 and 37
And Then 1-24 on pages 39-41