1. Basics of Bonding

2. Types of Bonding Bonds: how atoms are held together
3 main bonding types
Ionic (strong)
Covalent (weak)
Metallic (strong)

3. Ionic Between metals and nonmetals Both form ions
Ions are attracted to each other
By nuclear charge
Metals form cations
lose electrons
Nonmetals form anions
gain electrons

4. Ions formed Main group elements typically have set charges.
There are exceptions to this guideline

5. Transition Metal Mainly D-block metals/ groups 3-12
There are exceptions
Change oxidation states / charges from to 4 +
Depending on what they are bonded with
To determine charge
Find the charge of the NON-METAL
Transition metals form cations

6. Polyatomic Ions
Nonmetals, covalently, bonded together that have an overall charge
Poly: many
Atomic: atoms
Ions: charged
they form both cations and anions
Must memorized grouping and charge
Have a different naming system
DON’T FORGET THE QUIZLET

7. Why do compounds form ? STABILITY!!!!
All ions either lose or gain electrons
Octet Rule: To have a FULL (2 or 8) outer shell
Nonmetals gain electrons
Metals lose electrons
Oppositely charged ions attract to form bonds

8. Creating Ionic Compounds
Find the metal on the periodic table
Determine type of atom
Metal, nonmetal, transition metal
Determine charge of atom
How many electrons does it gain/lose
Metals lose (cation)
Nonmetals gain(anion)
Equalize the charge
By using subscripts which tell number

9. Let's form some “normal” ionic compounds!
Sodium Fluoride
Na F1-
(1+)+(1-) = 0
NaF
Calcium Oxide
Ca O2-
(2+)+(2-) = 0
CaO
Calcium Fluoride
Ca F1-
(2+)+(1-) = 1+
(2+)+ ___ (1-) = 0
CaF2
Sodium Oxide Na1+ O2- (1+) + (2-) = 1- ___ (1+) + (2-) = 0 Na2O 2 2

10. How to determine a Transition Metal Charge
From the Name
The roman numeral is the charge of the transition metal
From the formula
Determine the NON- METAL’S or Polyatomic ions’ charge
Equalize the compound to neutral
Make charges equal and opposite
Use subscripts

11. Lets Determine Charge! FeO Fe: ? O: 2- _____ + 2- = 0 Fe2S3 Fe: ?
Manganese (II) Oxide
Mn:
O: 2- 2 3

12. Naming Ionic Compounds
The cation keeps its full name
Anion take the root of the word
Change the ending to “ide”
Exception: polyatomic ions always keep their full name
Put them together

13. Lets name some compounds!
CuCl2
Li(C2H3O2)  
V2Se3  
Mn3N4
BeO
Na2(SO4)
copper (II) chloride
lithium acetate  
vanadium (III) selenide  
manganese (IV) nitride
beryllium oxide
sodium sulfate

14. Properties of Ionic Bonds
Strong
Form Crystalline solids
Network solids
Can conduct electricity when
molten
Aqueous
High melting points
Hard
Brittle
Electronegativity Difference > 1.9

15. Covalent When atoms share electrons Between non-metals
Not all sharing is equal

16. Why do the form ? Valence shell/ orbitals over lap to share electrons
Covalent compounds can share
One pair
Two pairs 
Three pairs 
Stability
Share electrons so valence shell is full
Duet (Hydrogen and Helium only) or Octet
Lowest possible energy

17. Steps to making covalent compounds
NO CHARGES ARE INVOVOLED 
Amount is indicated by number prefix in the name

18. Naming Covalent Compounds
First element keeps it full name
If there is more then one of the element
Gets a number prefix
Second element keeps the root of the name
Ends in “ide”
Always gets a number prefix

19. Lets make some Covalent Compounds
carbon tetrafluoride
silicon dioxide
dinitrogen trisulfide
phosphorus mononitride
hydrogen gas
carbon disulfide
CF4
SiO2
N2S3 PN H2
CS2

20. Lets Name Covalent Compounds
Carbon Monoxide
Carbon Dioxide
Dinitrogen Trioxide
Nitrogen gas
Nitrogen MonoPhosphide
6. Sulfide Dichloride CO
CO2
N2O3 N2 NP
SCl2

21. Properties of Covalent Bonds
Weak
Liquids
Gases
Nonconductive
Low melting points
Flows easily
Electronegativity difference of 0.3 < EN < 1.9

22. Metallic Bonding Force that keeps metal atoms together
Delocalization of electrons
Sea of electrons flowing between metal cations
Leads to metallic properties
Ductility
Pulled into wires
Malleability
Hammered into sheets
Conductivity
Can move electricity

23. Properties of Metallic Bonds
Strong
Solids
Extremely conductive
High melting points
Hard
Malleable
Ductile
Electronegativity Difference < 0.3