1. Naming Compounds
Ionic Compounds
Covalent Compounds
Acids

2. Look at the first element. Is it a metal, nonmetal, or hydrogen?
Metal = Ionic Bond
Nonmetal = Covalent Bond
Hydrogen = Acid

3. Ionic Compounds Writing Formulas (Binary)
Binary Compounds have only two types of elements
Determine the ions’ charges using the periodic table or compound’s name.
Balance charges in the compound.

4. Ionic Bonds – Naming Binary Compounds
Check to see if the element has more than one oxidation number.
If the metal has more than one oxidation number, the compound will be named using the Cation - Roman Numeral – Anion
The anion’s ending is changed to ide for all binary compounds.

5. Ionic Compounds with Polyatomic Ions
Ionic compounds that contain more than two types of atoms are called polyatomic.
Examples of Polyatomic Ions
Sulfate – SO4-2
Carbonate – CO3-2
Phosphate – PO4-3
Ammonium – NH4+

6. Polyatomic Ions Cont. These compounds are named in three ways:
Polyatomic Ion – Polyatomic Ion
Ex. Ex. (NH4)3PO4
Ammonium Carbonate
Cation – Polyatomic Ion
Ex. Lithium Nitrate
Ex. Ca(NO3)2
Polyatomic Ion – Anion (with ide ending)
Ex. Ammonium nitride

7. Covalent Compounds To name covalent compounds: prefix-first element
prefix-root of second element - ide
Prefixes
1 = mono 6=hexa = di 7=hepta 3=tri 8=octa 4=tetra 9=nona 5=penta 10=deca

8. Naming Acids Does the acid contain oxygen?
YES
Oxyacid
Change polyatomic ending from:
ate to ic
ite to ous
Add the word Acid NO
Binary Acid
Hydro-root of nonmetal - ic
Add the word Acid

9. If water molecules are attached= Hydrate
Add numerical prefix and the word hydrate
Ex. MgSO4 • 7H2O
magnesium sulfate pentahydrate

10. Chemical Bonds
Ionic Bonding
Covalent Bonding
Acids

11. Ionic Bonding
Positively charged ions are attracted to negatively charged ions, making a neutral compound.

12. The Octet Rule
Atoms tend to gain or lose electrons in order to acquire a full set of valence electrons.
Therefore, atoms will transfer electrons to each other in order to have a full set of valence electrons.
When electrons are transferred, ionic bonds are formed.
Ionic Bonding

14. Energy Changes in Bond Formation
Energy is absorbed when an element loses an electron.
Energy is released when an element gains an electron.
Lattice energy is the energy released when ionic bonds are formed.

15. Properties of Ionic Compounds
high melting points
dissolve in water: which makes solutions good conductors of electricity
have large electronegativity difference between elements
usually form between metals and nonmetals
Lattice crystal: the regular pattern in which a crystal is arranged.

16. Types of Ions 1) Monoatomic Ions - have one element
2) Polyatomic Ions - consist of more than one atom and have an overall charge
Atoms in polyatomic ions are held together by covalent bonds.
Ex. Sulfate ion, ammonium ion, etc.
See polyatomic sheet

17. Covalent Bonding
Covalent Bonds are formed by SHARING pairs of electrons between 2 atoms.
Usually formed between two nonmetals
Molecules
a group of atoms held together by covalent bonds
molecular substance - contains molecules

19. Types of formulas for covalent bonding
Molecular formula - tells you how many atoms make up a compound ex. C6H12O H2O
Structural formula - shows how the atoms are bonded to each other

20. Multiple Bonds Single Covalent Bonds -share one pair of electrons
Double bonds - share 2 pairs of electrons
Triple Bonds - share 3 pairs of electrons (STRONGEST BOND)
Use dashes to represent covalent bonds in a structural formula.

21. :N = N:

22. Exceptions to the Octet Rule
Atoms with less than an octet Boron BF3
Atoms with more than an octet Phosphorus and Sulfur PCl5
Molecules with an odd number of electrons ex. NO

23. Properties of Covalent Bonds
-Low melting points, brittle, strong odor, poor conductors of electricity
Shared electrons are attracted to more electronegative element
Polar bonds - form between elements with big differences in electronegativity ex. H2O
Nonpolar bonds - exert equal pull on electrons ex. F-F or O=O

26. How can you tell if a compound has ionic or covalent bonds?
Use electronegativity difference between the elements
non polar covalent less than 0.4
polar covalent
ionic bonds greater than 2.0
See electronegativity chart for values.

27. Acids
A molecular compound that dissolves in water to produce hydrogen ions and a characteristic ion.
In water, acids behave like ionic compounds

28. Types of Acids Organic Acids contain the carboxylic group, -COOH.
Binary Acids: contain hydrogen and another element
Oxo Acids: contains oxygen and another element