1. The Structure Of Matter
Compounds, ionic bonds, covalent bonds, and naming compounds
The Structure Of Matter

2. What is a compound?
A compound is made of two or more elements that are chemically combined
The forces that hold the atoms together are called chemical bonds

3. Why do elements form compounds?
To make themselves stable
- How do atoms make themselves stable?
By filling their outer most energy level (orbital)
- 1st energy level – 2 electrons to be filled
-2nd energy level – 8 electrons to be filled
- 3rd energy level – 8 electrons to be filled
By filling their outer shell, each atom will have a similar structure to a noble gas

4. C would like to
N would like to
O would like to

5. Chemical Bonds hold electrons together
There are two types of chemical bonds:
Ionic Bonds – strong bonds
Covalent Bonds – not as strong

6. Ionic Bonds
Bond formed by the Transfer of electrons from one atom to another
Occurs between a metal and a nonmetal
Metals lose electrons and are electron donors
Nonmetals gain an electron and are electron acceptors

7. Ionic Bonds transfer e-

8. What is an Ion?
An Ion is an atom that has gained or lost an electron which gives the atom as a whole a positive or negative charge

9. Cation and Anion
When an atom gains or loses an electron when they bond we give it a new name
Cations - are atoms that lose an election so they become more positive(+)
- Metals
Anions- are atoms that gain an electron so they become more negative(-)
- Non-meals

11. Ionic Bonds

13. 1). Ionic bond – electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions.

14. Covalent Bonds Bond formed by the sharing of electrons
Occurs between nonmetals and other nonmentals
Not as strong of a bond as ionic bond

16. Covalent Bonds

17. In Covalent Bonds, atoms may share more than one electron
Single Bond
Double Bond
Triple Bond

18. Naming Ionic Compounds
Ionic Compounds – named for the cations(+ metal) and anion(- nonmetal)) they are made of
Cation ion comes first
Anion comes second + -ide on the end of the element

19. Steps to name ionic compounds
Identify the cation (metal)
Identify the anion (nonmetal)
Change the anion (nonmetal) by adding –ide to the end
Ex: NaCl - Sodium Chloride
KBr
CaO

20. Writing the Formulas of Ionic Compounds
Ionic compounds must have a total charge of zero
Ex: Calcium has a +2 charge (Ca2+)
Fluoride has a – 1 charge (F1-)
To make Calcium Fluoride equal 0 you need:
1 Calcium and 2 Fluorine atoms
So the formula for calcium fluoride would be CaF2

21. Steps to writing Ionic formulas
Identify the charge of the cation (+1, +2, +3)
Identify the charge of the anion (-1, -2, -3)
Balance the charges so they equal zero
The charge of the cation and anion becomes a subscript (little number at the bottom)

22. Steps to writing Ionic formulas
Example: Zinc Chloride 1. Zinc Chlorine Balance: 1 Zinc and 2 Chlorine = 0 4.ZnCl2

23. Steps to writing Ionic formulas
Example:
Sodium Nitride
1. Na +1
2. N -3
3. Balance: Need 3 Na for every 1 N
4. Na3N

24. Naming Covalent Compounds
Covalent compounds use prefixes for the number of atoms in the compound

25. Steps to Naming Covalent Compounds
Both are nonmetals
Use prefixes to indicate how many atoms are present
Name the first element: prefix + full name
Name second element: prefix+ full name+ ide at the end
Don’t use “mono” with the first element
Example:
BF3 – Boron Trifluoride
SO3 – Sulfur Trioxide

26. Steps to writing Covalent Compounds
Identify the elements
Identify the prefixes of the element
Charges don’t matter for these formulas
Examples:
Carbon dioxide = 1 carbon, 2 oxygen = CO2
Hydrogen Monoxide =1 Hydrogen, 1 Oxygen = HO
Dihydrogen monoxide = H2O
Phosphorus Hexabromide = PBr6