1. BONDING
Chapters 4 & 12

2. Ionic vs. Covalent Bonds
result from the attraction between opposite charges of ions
Covalent
result from sharing of electrons between atoms

3. The Octet Rule
Atoms will gain, lose, or share electrons to achieve a noble gas configuration
If the atom has 1-3 valence electrons, it will LOSE those electrons and become a positive ion (CATION).
If the atom has 5-7 valence electrons, it will GAIN electrons until it has EIGHT, becoming a negative ion (ANION).

4. Practice Forming Ions Complete the table below for each of the atoms:
# of Valence Electrons
GAIN or LOSE electrons?
ION
CATION or ANION?
Magnesium
Chlorine
Potassium
Nitrogen
Oxygen
Lithium

5. What are Ionic Compounds?
Compound made of only ions
Formed by the gaining or losing of electrons
Typically between a metal and a non-metal
Ionic Bonding
A positively charged ion (anion) will be attracted to and will form a bond with a negatively charged ion (cation)
The ions will exchange electrons to achieve their charge (and reach the noble gas configuration)

6. Ionic Attraction?

7. Properties of Ionic Compounds
Overall neutral
High melting points
Generally brittle solids
Dissolve in water to form electrolytes

11. Types of Ions
Monoatomic cations
Monoatomic anions
Polyatomic ions

12. Monoatomic cations Positively charged, ions formed from ONE atom
To name the cation, simply add the word “ion” after the element’s name
Li+ Lithium ion
Mg+2 Magnesium ion
Some atoms have the ability to form multiple ions (most of these are “transition” metals)
To name, simply name the element, indicate the charge in roman numerals and then add the word “ion”
Fe Iron (II) ion
Fe Iron (III) ion

13. Monoatomic anion Negatively charged, ions formed from ONE atom
To name the anion, replace the ending of the element’s name with “-ide”
F - Fluorine  Fluoride
O -2 Oxygen  Oxide

14. Monoatomic ion Practice
Complete the table below for each of the atoms:
ATOM
ION
CATION or
ANION?
NAME of ION
Magnesium
Chlorine
Potassium
Nitrogen
Oxygen
Lithium

15. Polyatomic ions
Multiple atoms that, TOGETHER, carry a charge.

16. IONIC COMPOUNDS WRITING FORMULAS
Write the symbol for the cation first.
Write the symbol for the anion second.
Add subscripts so the charges equal zero when added.
NAMING COMPOUNDS
Write the name of the cation unchanged first.
Write the root of the anion with the –ide ending.

17. How do I write a formula for an ionic compound?
Use the CRISS-CROSS METHOD:
Write the ions in order of metal then nonmetal
Take the ionic charge number (written as the superscript) of each element and criss cross it to the subscript of the other element +2 -1 Ca Cl
Ca_Cl_ 1 2

18. Ionic Compound Formula Practice
Write the ionic formula for the following ions
Mg+2 with P-3
B+3 with S-2
Li+1 with S-2
Ga+3 with Se-2
B+3 with At-1

19. How do I name ionic compounds?
Compounds are named from the ions that form them…
The first element (metal) keeps its name
If it’s a transition metal, you must use a roman numeral to indicate its charge
The second element (nonmetal) keeps the first syllable of its name and the ending is changed to “-ide”
NaCl
Sodium Chloride
Fe2O3
Since Fe is a transition
metal, you must find its
charge… UNCRISS CROSS
Fe2O3
Iron (III)
Oxide +3 -2 Fe O

20. Ionic Compound Naming Practice
Write the ionic compound name for the following…
BaCl2
NaF
Ag2O
CuBr
CuBr2

21. Binary Ionic Compounds
Binary Compound
Ionic compound composed of two atoms
Formula Unit
Smallest representative unit
ATOMS
FORMULA
NAME of COMPOUND
Magnesium & Chlorine
IONS:
Potassium & Nitrogen
Lithium & Oxygen

22. Tertiary Ionic Compounds
Tertiary Compound
Ionic compound composed of three atoms
IONS
FORMULA
NAME of COMPOUND
K+ and NO3-
Mg+2 and OH-
Cu+2 and PO4-3

23. Copper Sulfate Pentahydrate
Hydrates
PREFIX
NUMBER
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10
Ionic compounds that absorb water into their solid structures
CuSO4 ● 5H2O
Copper Sulfate Pentahydrate

25. Covalent Compounds Covalent Bond Molecule Molecular Compound
Formed by the sharing of electrons
Molecule
Smallest representative unit
Molecular Compound
Compounds composed of molecules
Molecular Formula
Shows the kind and numbers of atoms present in a molecule

26. Properties of Covalent Compounds
made of two nonmetals
low melting and boiling points
solid, liquid, or gas at room temp.
do not dissociate in water

27. Naming Covalent Compounds
Write the less electronegative element first.
Write the root of the more electronegative element with the -ide ending second.
REVIEW: Electronegativity
- the attraction to electrons involved in a chemical bond
Add prefixes to both indicating the number of atoms of each element

28. Exceptions when Naming Covalent Compounds
Do not use mono-with the first element in the compound
Prefixes are sometimes shortened.
CO (Carbon Monoxide)
Chemist use common names for some compounds other than the formal names.
NH3 (Ammonia)

29. Naming Covalent Compounds
FORMULA
NAME of COMPOUND CO
CO2
CO3-2
C2O4-2

30. Types of Covalent Bonds
Polar Covalent Bond
one atom in a molecule is significantly more electronegative
causes a slight positive and negative charge on a molecule.
Nonpolar Covalent Bond
electrons are shared equally
Electronegativity Differences Bond Type
 nonpolar
polar
 ionic

31. Covalent Bonds Single Covalent Bond Double Covalent Bond
two atoms share 1 pair of electrons
Double Covalent Bond
two atoms share 2 pair of electrons
Triple Covalent Bond
two atoms share 3 pair of electrons

32. Acid
A molecular substance that dissolves in water to produce a hydrogen ion
Acts like an ionic compound because they break down into cations and anions in water
Produces a characteristic anion for which it is named.
If the anion ends with
-ide (i.e. chloride or fluoride)
Add the prefix hydro- and change the ending to –ic and add the word acid
-ate (i.e. phosphate or sulfate)
Change the ending to –ic and add the word acid
-ite (i.e. sulfite and phosphite)
Change the ending to –ous and add the word acid