1. Do Now: What are ionic compounds and what do they consist of?
Define cations and anions.
How do you determine the charge of ions formed from representative elements?

2. Ionic Compounds
Ions formed from transfer of electrons (to satisfy octet rule)
Consist of cations(+) and anions(-) held together by ionic bond (electrostatic force of attraction)
Typically, metals(+) and nonmetals(-)
Let’s work on nomenclature, rules for naming

3. What is the charge and symbol for the following Cations Anions
Nitride?
Sulfide?
Chloride?
Iodide?
Oxide?
Magnesium?
Copper (II)?
Sodium?
Zinc?
Aluminum?
Iron (III)
Talk about transition metals

4. Formulas: Ionic Compounds
are electrically neutral
Write the symbol and charge for each ion
Balance it! The total positive charge must equal the total negative charge.
1. Potassium chloride
2. Barium iodide
3. Aluminum oxide
4. Nickel (II) fluoride

5. Write formulas for Lithium oxide Iron (III) bromide
Nickel (II) fluoride
Aluminum sulfide
Magnesium chloride
Strontium phosphide

6. What are polyatomic ions?

7. Polyatomic Ions
Ions that are made up of more than one atom. Examples are SO42- or OH- or NO3-
Use as you would any part of a compound

8. Write balanced formulas for
Barium nitrate
Sodium permanganate
Ammonium chromate
Copper (II) hydroxide
When do you need parentheses?

9. Name these compounds
NaCl
K2S
(NH4)2O

10. NaCl 1st …Cation 2nd … Anion Naming binary ionic compounds …
Monatomic Monatomic-
same name as atom ends in “ide”
*For transition metals
Indicate charge of the ion
After the name using
Roman numeral in
parentheses
Cation always written first, then anion
NaCl

11. Try to name these ionic compounds
BaCl2
Na2S
Ca3P2
Cu2O

12. Cation Anion Name: KClO3 (NH4)2S Al(OH)3 FeSO4
Naming ionic compounds …
Cation Anion
Polyatomic – use the ion sheet!!!
Name:
KClO3
(NH4)2S
Al(OH)3
FeSO4
Cation always written first, then anion

13. Do Now… Name the following:
CaF2
Al2O3
NaClO4
(NH4)3PO4
PbCrO4
LiClO
NaCN
Cu(NO3)2
What are the rules for naming
Ionic compounds?

14. Rules for Monatomic positive ion …. If it’s a transition metal ….
Monatomic negative ion …
Polyatomic ion (positive ion or negative ion)
Get ready to put problems on board from HW

15. What are molecular compounds?
What do they consist of?
What type of bonding is involved?

16. Molecular Compounds No charges … no balancing All nonmetals
Share electrons(covalent bond) to satisfy octet rule
No charges … no balancing

17. Write the formula for Carbon dioxide Carbon monoxide
Dicarbon hexahydride
Prefix tells how many atoms are in the compound

18. Formula ---> Name Carbon dioxide Molecular (binary compound only)
Second atom - ends in “ide”.
Also, always add a prefix
indicating how many atoms
First atom - retains
the name of the element
Add a prefix if there
is more than one of the
atom
Carbon
dioxide

19. Name
PH3 PCl3 SiI4 NH3 XeF4

20. DO NOW! When do you use parentheses? When do you use roman numerals?
When do you use prefixes?
Air is mainly composed of nitrogen and oxygen gases. What are the formulas of these compounds?

21. Jill was handed an assortment of index cards
Jill was handed an assortment of index cards. Each index card had the chemical symbol for an ion
Na+
Zn2+
Cl-
Ni2+
O2-
PO43-
Al3+
Jill formed ionic compounds using index cards. She combined sodium and zinc to from the compound Na2Zn. Is this a possible ionic compound? Why or why not?
2. Jill then wrote the formulas for all the possible ionic comounds that can be formed. What formulas did she write? Name each compound.
3. Jill wrote the following compounds. Identify whether each formula is correct or incorrect. If the formula is incorrect, change it to make it correct.
ZnCl3 Al3O2 Ca3(PO4)2

22. DO Now… What are the prefixes for the numbers 1-10?
How do you name a binary molecular compound? for the first atom … for the second atom …
What are diatomic molecules? List the 7 examples.

23. Write balanced chemical formulas for Magnesium hydroxide )
Write balanced chemical formulas for
Magnesium hydroxide
Calcium acetate
Barium phosphide
Ammonium sulfate
Copper (II) fluoride
Sodium sulfide
Lead (III) dichromate