1. Formula Writing

2. TYPES OF COMPOUNDS Molecular: composed of molecules.
Contains two nonmetals and a covalent bond. (sharing electrons)
Ionic: composed of ions.
Contains metal-nonmetal and ionic bond. (transfer of electrons.)

3. Chemical Formula Composition Qualitative-which elements
Are in the compound
Quantitative-how many of each element
Molecule: group of 2 or more atoms of the same element or group of atoms of different elements sharing electrons to form a compound.

4. MEMORIZE THESE!! Structural formula: shows how the atoms are joined.
Empirical formula-smallest representative unit.(molecular formula in its lowest terms)Ex. C6H12O6 empirical formula is CH2O
Formula unit-the lowest whole number ratio of ions in an ionic compound
Monatomic vs Diatomic Elements:
MEMORIZE THESE!!
H2 N2 O2 F2 Cl2 Br2 I2

5. Ionic bonding
Octet Rule: Atoms react by changing the number of electrons so as to acquire the stable electron configuration of a noble gas.
Depends on the number of valence electrons.
Lewis Dot Diagrams are helpful

6. Ions- atom or group of atoms that have a positive or negative charge.
Cation: positively charged ion. Has lost electrons.
Anion: negatively charged ion. Has gained electrons.
Ionic bond is the force of attraction between oppositely charge ions.

7. IONIC CHARGES OF THE ELEMENTS
Location on the periodic table.
Transition metals can have multiple charges.
Polyatomic ions are a tightly bond groups that behave as a unit and carry a charge.

9. ION CHARGES TO BE MEMORIZED Fe+2, Fe+3 iron(II), iron(III)
ION CHARGES TO BE MEMORIZED Fe+2, Fe+3 iron(II), iron(III) ferrous ferric Cu+1, Cu+2 copper(I), copper(II) cuprous cupric Hg+1, Hg+2 mercury(I), mercury(II) mercurous mercuric

10. Sn+2, Sn+4 tin(II), tin(IV)
Sn+2, Sn+4 tin(II), tin(IV) stannous, stannic Pb+2, Pb+4 lead(II), lead (IV) plumbous, plumbic

11. POLYATOMIC IONS TO BE MEMORIZED
ammonium NH hydroxide OH-1 nitrate NO3-1 chlorate ClO3-1 sulfate SO4-2 phosphate PO4-3 carbonate CO3-2

12. Rules For Writing Ionic Compounds
Write symbols of elements. Cation is first.
Determine charge on ions.
Select subscripts so the formula has zero total charge.
Polyatomic ions do not break down under ordinary chemical reactions.
When using subscripts with polyatomic ions, place formula ion in parentheses.

14. Criss Cross Method Numerical charge of each ion is crossed over and used as a subscript for the other ion. Signs of the number are dropped. Check for lowest whole number ratio.

15. NAMING IONIC COMPOUNDS
Cation named first.
Binary compounds: Two elements. Change the nonmetal ending to –ide.
Ternary compound: name polyatomic ion.
Some metals have more than one charge. Use –ous for lower charge. Use –ic for higher charge.
Stock naming system uses Roman numerals to show charge on ion.

16. Molecular Compounds Covalent Bond
sharing electrons
between two nonmetals
Use prefixes to designate number of atoms.
Write the element name first.
Change the ending of the second element to -ide.

17. PREFIXES FOR MOLECULAR COMPOUNDS
mono 1
di 2
tri 3
tetra 4
penta 5
hexa 6
hepta 7
octa 8
nona 9
deca 10

18. Naming Acids Acids are ionic compounds that starts with H.
Binary Acids
The acid name begins with the prefix hydro-.
The root of the anion is used and the –ide is changed to –ic.
The word “acid” is used as the second word in the name.

19. Ternary Acids or Oxyacids
Acids involving hydrogen and a polyatomic ion.
When the anion ends in –ite, change the –ite ending on the stem to –ous.
When the anion ends in –ate, change the –ate ending on the stem to –ic.
The word “acid” is used as the second word in the name.

20. Relation of polyatomic ions
Name depends on the number of oxygens.
-ate is the higher number of oxygens.
-ite is the lower number of oxygens.
Per- is one oxygen more than –ate.
Hypo- is one oxygen less than –ite.

22. Hydrates Hydrates are ionic compounds that contain water.
Name the ionic compound.
Using the greek prefixes, indicate the number of water molecules present.
Ex. Zn(NO3)2 • 6 H2O
zinc nitrate hexahydrate.