CHEMICAL BONDING
Name________________________________________
The force of attraction that holds two atoms together is a ___________________ _________________.

________________________ electrons , or electrons in the outer energy level, hold the key to bonding.

An atom has a tendency to fill its outer energy level. An atom becomes more stable when its outermost energy level is
____________________________.

Atoms will _____________,________________________, or _________________ electrons to bond with other atoms.

In order to become stable every atom needs a completely full valence electron shell. Most atoms need __________
electrons in order to become stable. Remember the ____________________ rule.
IONIC BONDS are bonds between _____________________________ and __________________________________.









Ionic bonds form when atoms ______________ or ______________________ valence electrons.
Metals tend to lose valence electrons (Cations) while nonmetals tend to gain valence electrons (Anions).
Most ionic compounds are salts.
The two charged ions form a neutral compound
Ionic compounds have high boiling point/melting point
Oppositely charge ions are held together by the attraction of oppositely charges called _________________________
________________________________.
LEWIS DOT DIAGRAMS
o Magnesium and Oxygen
o Sodium and Sulfur
o Barium and Chlorine
o Calcium and Bromine
Naming Ionic Compounds
o The cation in the first part, then the anion.
o Most cations have the _______________ _____________ as their element.
o The anions change the last part of the original element’s name to the suffix ____________________.
 Example: F fluorine and the ion, F- is fluoride.
 Practice:
 KBr
 LiF
 MgS
 CaO
Writing the formula for an ionic compound
o The electrical charge must equal ____________.
o The correct formula contains the ____________ positive and negative ions that are needed to make the total
electrical charge zero.
o __________________________ are used to indicate more than one of that ion.
o Use the _________________________________ method of determining these subscripts.
o Move the number of the charge on the ion down to the subscript of the opposite ion.
 Al3+ + S2Al2 S3
o Don’t use criss cross method when the positive and negative charges add up to ______________.
 Lithium iodide
Calcium fluoride
 Sodium oxide
Magnesium phosphide
COVALENT BONDS are bonds formed between __________________________ and _______________________________.




Atoms _____________________________ valence electrons.
Low melting point/boiling point.
When covalent bonds form, the electron clouds overlap and the atoms actually merge or overlap to form a _________
Naming Covalent Bonds
o Prefixes
MonoDiTriTetraPentaHexaHeptaOctaNonaDeca Write the element which appears to the left and lower FIRST. (Add prefix if more than one.)
 Write the next element and change the ending to –ide. (Drop the “o” & “a” from prefix before a vowel)
 Use prefixes to tell how many of each kind of atom are in the molecule.
o Practice : Write the correct formula for
Practice: Write the correct name for each of these
each of these molecules:
covalent molecules:
1. Carbon tetrachloride
1. SiO2
2. Iodine heptafluoride
2. SO2
3. Dinitrogen monoxide
3. PBr5
4. Sulfur dioxide
4. CF4
5. Carbon monoxide
5. N2F3
6. Carbon dioxide
6. N2O4
7. Carbon disulfide
7. NF3
8. Phosphorous pentoxide
8. SF4
9. Diphosphorus trioxide
9. XeF4
10. Phosphorus trichloride
10. As2O5
IDENTIFYING AND NAMING BONDS
a. Tell whether the bond is ionic or covalent
b. Name the compound
a. CCl4
e. NaF
b. AlP
f. PF5
c. CO2
g. MgS
d. KCl
h. BaI
CHEMICAL FORMULAS
 Subscript- tells you the number of atoms of an element that are present in the formula.
 Coefficient- tells you the number of molecules that are present in the formula.
CHEMICAL EQUATION -A statement that uses symbols, chemical formulas and numbers to stand for a __________ __________
 Reactants (substances that go through a chemical reaction) to form a product.
 C + O2
C O2
 The letters in parentheses show the physical state of the substance: gas (g), liguid (l), solid (s), aqueous (aq)
BALANCING EQUATIONS
 Due to the law of conservation of mass, each equation must be balanced. You must have the same number of each
atom of each element on both sides of the equation.
 Take inventory of each element of both sides of the equation.
 Use coefficients to balance the equation.
 NEVER change the subscript!
LAW OF CONSERVATION OF MASS -- mass cannot be _________ nor ____________in chemical reactions.
 The mass of the products is equal to the mass of the reactants.
TYPES OF CHEMICAL EQUATIONS---Synthesis, Decomposition, Single Replacement, Double Replacement