1. Chemical Names and Formulas
Chapter Two
Chemical Names and Formulas

2. *Introduction to Chemical Bonding*' '
*Introduction to Chemical Bonding*
Every substance is either an element or a compound
A Compound consists of more than one kind of atom
A compound is either molecular or ionic in nature
Characteristics of Molecular and Ionic Compounds:
Characteristic Molecular Compound Ionic Compound
Representative Unit Molecule Formula Unit
Type of Elements Nonmetallic Metal/Non metal
Physical State Solid, Liquid, Gas Solid
Melting Point Low(usually < 300 oC) High(>300 oC)

3. Molecules and Molecular Compound
Molecule- the smallest electrically neutral unit of a substance that still has the same properties of that substance
Molecular compound- Atoms of different elements can combine chemically to form compounds
Atoms combine to form molecules
Compounds are composed of molecules
                       

4. Representing Chemical Compounds
Molecular compounds are composed of two or more nonmetals
A molecular formula shows the number and kinds of atoms present in a molecule of a compound
Ionic Compounds are composed of oppositely charged ions combined in electrically neutral groupings
A formula unit gives the lowest whole
number ratio of ions in the compound.

5. Periodic Table Facts The # of the A Group = # of outer electrons
That is (1A,2A,3A-8A) OR (IUPAC 1,2,13-18)
Elements that: Lose electrons are positive
Elements that: Gain electrons are negative
Elements are most stable when they have 8 outer electrons—known as the Octet Rule
Example: Chlorine has 7 electrons/ gains 1/has a negative 1 oxidation number Cl is in Group 7A

6. Losing/Gaining Electrons
Atoms that have 1, 2 or 3 electrons in their outer levels will tend to lose them in interactions with atoms that have 5, 6 or 7 electrons in their outer levels. Atoms that have 5, 6 or 7 electrons in their outer levels will tend to gain electrons from atoms with 1, 2 or 3 electrons in their outer levels. Atoms that have 4 electrons in the outer most energy level will tend neither to totally lose nor totally gain electrons during interactions.

7. b Ionic Charges a
The charges of the ions of the representative elements can be determined by the position of these elements in the periodic table
Most transition metals have more than one common ionic charge
A polyatomic ion is a group of atoms that behaves as a unit and has a charge

8. Binary (two-element) ionic compounds are named by writing the name of the cation followed by the name of the anion.
When a cation can have more than one ionic charge, a Roman numeral is used in the name.
Ternary ionic compounds contain at least one polyatomic ion.

9. Criss-Cross Method Criss-Cross: write symbols
put oxidation # above each symbol
criss-cross # (not charge)
reduce #’s to get lowest possible ratio
do not need to write the # 1

10. A Group Oxidation # Short-cut
1A 2A 3A 4A 5A 6A 7A

11. EXAMPLES OF IONIC COMPOUNDS:2
ZnS
AlCl3
Ba3N2
CuBr2
Zinc sulfide
Aluminum Chloride
Barium Nitride
Copper (II) bromide

12. Ternary Ionic Compounds
Use the criss-cross method
Polyatomic ions are involved… “many atoms” that act together with a single charge
“treat” the polyatomic as if it is a single element regarding the criss-cross…you cannot change the subscripts for the polyatomic.
You might need to use parentheses when criss-crossing oxidation numbers

13. Ternary Ionic Compounds
Sodium Hydroxide…..NaOH
Calcium Nitrite……...Ca(NO2)2
Magnesium Sulfate…..MgSO4
Ammonium Nitrate…..NH4NO3
Calcium Phosphate…..Ca3(PO4)2

14. Molecular Compounds
Binary molecular compounds are composed of two nonmetallic elements.
Prefixes are used to show how many atoms of each element are present in a molecule of the compound.
DO NOT need to criss-cross for molecular compounds…Reason: prefix given

15. Summary of Naming and Formula Writing
Prefixes Used in Naming Binary Molecular Compounds
Prefix # Prefix #
Mono 1 Hexa
Di 2 Hepta
Tri 3 Octa
Tetra 4 Nona
Penta 5 Deca

16. Examples: 1. OF2 SO3 3. Nitrogen trifluoride 4. Dinitrogen tetroxide
Name these binary molecular
compounds:
1. OF2
SO3
Write formulas for the
following binary molecular
3. Nitrogen trifluoride
4. Dinitrogen tetroxide
Answers:
oxygen difluoride
sulfur trioxide
3. NF3
4. N2O4