1. Naming Ionic CompoundsCl
Cl -
sodium
sodium
chlorine
chloride
sodium chloride
Photo by Ra’ike

2. When metals lose electrons they become ions.
Remember…
When metals lose electrons they become ions.
When nonmetals gain electrons they become ions.
Let’s learn how to name ions…

3. chlor- + -ide = chloride
Rules for Naming Ions
1. The names of metals do not change.
2. The names of nonmetals do change:
root of element name ide = name of ion
Examples of nonmetals:
The name of chlorine’s ion:
chlor ide = chloride
The name of nitrogen’s ion:
nitr ide = nitride

4. Examples of naming ions:
The name of calcium’s ion:
calcium
(The names of metals don’t change!)
The name of oxygen’s ion:
ox ide = oxide
The name of aluminum’s ion:
aluminum
(The names of metals don’t change!)

5. Write the name of each of the ions on your notes.
sulfide
lithium
nitride
bromide
potassium
chloride
oxide
hydrogen (+), hydride (-)

6. It is also important that you can identify the names of polyatomic ions. Polyatomic ions are covalently bonded elements that have a charge!

7. Write the name of each of the polyatomic ions on your notes using your reference sheet as a guide.
sulfate
carbonate
permanganate
sulfite
hydroxide
nitrate

8. Steps for Naming Ionic Compounds YOU ARE DONE! It is that easy.
CaBr2
calcium
bromide
Step 1: Write the name of the metal ion.
Step 2: Write the name of the nonmetal ion.
YOU ARE DONE! It is that easy.

9. 1. NaF
2. MgO
sodium
fluoride
magnesium
oxide
3. SrCl2
4. Li2S
strontium
chloride
lithium
sulfide
5. CaO
6. KI
calcium
oxide
potassium
iodide

10. When polyatomic ions are used, simply use the name of the polyatomic ion in the compound.
1. NH4F
2. CaSO4
ammonium
fluoride
calcium
sulfate
3. Mg(NO3)2
4. NaOH
magnesium
nitrate
sodium
hydroxide

11. Mg I +2 - MgI2 magnesium iodide
You can also determine the formula of an ionic compound from its name. To do this, you will need to use what you already know about the Periodic Table.
magnesium iodide Mg I +2 -
MgI2
Step 1: Write the symbol and charge of the metal ion using the Periodic Table.
Step 2: Write the symbol and charge of the nonmetal ion using the Periodic Table.
Step 3: Determine the formula from the ions.

12. Sr NO3 +2 - Sr(NO3)2 strontium nitrate
This is just as easy to do with polyatomic ions. You just need to use the table of polyatomic ions found on the naming compounds reference sheet.
strontium nitrate Sr
NO3 +2 -
Sr(NO3)2
Step 1: Write the symbol and charge of the metal ion.
Step 2: Write the formula and charge of the polyatomic ion using your STAAR Reference Sheet.
Step 4: Determine the formula from the ions.

13. N-3 NO3- S-2 SO3-2 P-3 PO4-3 nitrate nitride sulfide sulfite phosphate
Be very careful that you do not mix up the names of ions. This is very common for beginners to naming.
Decide which name goes with each ion.
nitrate
N-3
NO3-
nitride
sulfide
S-2
SO3-2
sulfite
phosphate
P-3
PO4-3
phosphide

14. SO4-2 S-2 SO3-2 N-3 NO2- NO3- Helpful Hint:
If the ion ends in –ide, it is probably from the periodic table. If the ion ends in –ate or –ite, it is a polyatomic ion. If you’re not sure, just check the list to see if it is there!
Examples:
sulfate
sulfide
sulfite
SO4-2
S-2
SO3-2
nitride
nitrite
nitrate
N-3
NO2-
NO3-

15. We know they are positive because metals are always positive.
Remember that the names of transition metals includes their charge because their charges are less predictable.
What are the charges of the transition metals below:
Iron (II) _______ Iron (III) _______
Copper (II) _______ Copper (I) _______
Tin (IV) _______ Tin (II) _______
Lead (II) _______ Lead (IV) _______ +2 +3 +2 +1 +4 +2 +2 +4
We know they are positive because metals are always positive.

16. Fe O +3 -2 Fe2O3 iron (III) oxide
The charges of the transition metals are important when you are determining the formula of an ionic compound.
iron (III) oxide Fe O +3 -2
Fe2O3
Step 1: Write the symbol and charge of the metal ion using the roman numeral given.
Step 2: Write the symbol and charge of the anion.
Step 4: Determine the formula from the ions.

17. Write the formula of each of the ionic compounds named on your notes.KI
SnCl4
BaSO4
NaCl
SrS
CuCO3
AlBr3
Li3N

18. Now let’s talk about naming
Covalent Compounds

19. So why do atoms share electrons?
Atoms share electrons so that they can both be in the most stable configuration!
So when are atoms the most stable?
Atoms are the most stable when they have 8 valence electrons in their outer energy level.
(Hydrogen and Helium only need 2 valence electrons.)

20. Chemical reactions occur when atoms gain, lose, or share electrons.
Nonmetals
Chemical reactions occur when atoms gain, lose, or share electrons.
Sharing electrons creates a covalent bond
Nonmetals can _______ electrons to form a covalent bond.
This creates a ___________.
share
molecule

21. There are 7 elements that exist in nature as diatomic molecules.
What elements exist as diatomic molecules?
H2, N2, O2, F2, Cl2, Br2, I2 21

22. Binary Covalent Compounds
There are millions of covalent compounds. These can be classified into many different types of compounds. Each type of compound has a different set of rules for naming. You will be learning about the easiest type of covalent compound to name:
Binary Covalent Compounds
What does binary mean?
Binary means 2.
Binary covalent compounds are between 2 different nonmetals.

23. phosphorous and chlorine
Nonmetals can share electrons in many different ways. This means that two nonmetals can create multiple compounds together.
carbon and oxygen
phosphorous and chlorine CO
CO2
PCl3
PCl5
nitrogen and oxygen
N2O4
N2O3
Each of these contains a different ratio of elements. Because of this, we have to make sure that the name of the compound explains the correct ratio.

24. To show the correct ratio of elements, we use prefixes.

25. Binary Covalent Compounds
Steps for Naming
Binary Covalent Compounds
N2O4
dinitrogen
nitrogen
tetroxide
oxide
Step 1: Write the name of the first nonmetal.
Step 2: Write the name of the second nonmetal changing its ending to -ide.
Step 3: Add prefixes to specify how many of each element are present.

26. Rules for Using Prefixes
Rule 1: Prefixes are only for COVALENT compounds.
Rule 2: The prefix mono- is never used on the first element of a binary covalent compound. Without a prefix it is assumed that there is only 1.
Example: CO2 is carbon dioxide, not monocarbon dioxide.
Rule 3: Remove the -o or -a from a prefix before adding it to oxide.
Example: CO is carbon monoxide, and not carbon monooxide.

27. How would you write each of the prefixes in front of oxide?
Remember: Remove the -o or -a from a prefix before adding it to oxide. Leave -i alone.
mono- ____________ di- ____________
tri- ____________ tetra- ____________
penta- ____________ hexa- ____________
hepta- ____________ octa- ____________
nona- ____________ deca- ____________
monoxide
dioxide
trioxide
tetroxide
pentoxide
hexoxide
heptoxide
octoxide
nonoxide
decoxide

28. Name the binary covalent compounds that are found on your notes.
carbon dioxide
carbon disulfide
phosphorous tribromide
phosphorous pentabromide
diphosphorous pentasulfide
dinitrogen monosulfide
silicon disulfide
nitrogen tribromide
dinitrogen tetrachloride

29. dinitrogen tetrafluoride
Because of the prefixes, it is very easy to go from the name of a binary covalent compound to its formula.
dinitrogen tetrafluoride N2 F4
Step 1: Write the symbol of the first nonmetal and the subscript that matches the prefix.
Step 2: Write the symbol of the second nonmetal and the subscript that matches the prefix.

30. Write the formulas of the binary covalent compounds in your notes.
CCl4
IF7
PCl5
N2O4
N2O
PCl3 CS CO
BH3
ICl
S2Br6
S4N4
SiS2
H2O
PI3
ClF5
NCl3
NO2