1. Warm-Up
What is an ion?
How is it formed?

2. NOMENCLATURE Naming and Writing Compounds

3. Three categories of compounds
Acids – begin with a hydrogen (HCl)
Ionic – metal bonded with a non-metal or polyatomic ion
Covalent – non-metal bonded with non-metal
FIRST DETERMINE WHAT TYPE OF COMPOUND YOU ARE DEALING WITH

4. Identify the compounds below as ionic compounds, covalent compounds, or as acids
NaBr
SO2 HF
P3O8
HC2H3O2
REMINDER
Acids – begin with a hydrogen (HCl)
Covalent – non-metal bonded with non-metal
Ionic – metal bonded with a non-metal or polyatomic ion

5. Identify the compounds below as ionic compounds, covalent compounds, or as acids
NaBr
SO2 HF
P3O8
HC2H3O2
REMINDER
Acids – begin with a hydrogen (HCl)
Covalent – non-metal bonded with non-metal
Ionic – metal bonded with a non-metal or polyatomic ion

6. Identify the compounds below as ionic compounds, covalent compounds, or as acids
WP2
NaCN
HNO3
BeF2
CO2
REMINDER
Acids – begin with a hydrogen (HCl)
Covalent – non-metal bonded with non-metal
Ionic – metal bonded with a non-metal or polyatomic ion

7. Identify the compounds below as ionic compounds, covalent compounds, or as acids
WP2
NaCN
HNO3
BeF2
CO2
REMINDER
Acids – begin with a hydrogen (HCl)
Covalent – non-metal bonded with non-metal
Ionic – metal bonded with a non-metal or polyatomic ion

8. Identify the compounds below as ionic compounds, covalent compounds, or as acids
HClO4
Cu2O
ZnCl2
Ca(IO3)2
H2O
REMINDER
Acids – begin with a hydrogen (HCl)
Covalent – non-metal bonded with non-metal
Ionic – metal bonded with a non-metal or polyatomic ion

9. Identify the compounds below as ionic compounds, covalent compounds, or as acids
HClO4
Cu2O
ZnCl2
Ca(IO3)2
H2O
REMINDER
Acids – begin with a hydrogen (HCl)
Covalent – non-metal bonded with non-metal
Ionic – metal bonded with a non-metal or polyatomic ion

10. Naming Acids Chemical formula starts with HYDROGEN (H)
Water (H2O) is NOT AN ACID
Examples:
HCl HF
H2CO3
HClO

11. Naming Acids
Look at the negative (anion) part of the acid to determine if it is:
An element
A polyatomic ion ending in –ate (from page 7 of your chemistry reference table)
A polyatomic ion ending in –ite (from page 7 of your chemistry reference table)

12. Naming Acids If is is an element: Hydro (element) ic acid
HCl  Hydro ic acid
2) HF  Hydro ic acid

13. Naming Acids If is is an element: Hydro (element) ic acid
HCl  Hydrochloric acid
2) HF  Hydrofluoric acid

14. Naming Acids A polyatomic ion ending in –ate
(name of polyatomic ion, minus –ate)ic acid
H2CO3  (name of CO32-) ic acid

15. Naming Acids A polyatomic ion ending in –ate
(name of polyatomic ion, minus –ate)ic acid
H2CO3  Carbonic acid

16. Naming Acids A polyatomic ion ending in –ite
(name of polyatomic ion, minus –ite)ous acid
HClO  (name of ClO-) ous acid

17. Naming Acids A polyatomic ion ending in –ite
(name of polyatomic ion, minus –ite)ous acid
HClO  Hypochlorous acid

18. Naming Acids
Try a few on your own!
HClO4
HClO3
H2S
HNO2
HCN HI
H2SO4

19. Naming Acids Try a few on your own! HClO4  perchloric acid
HClO3  chloric acid
H2S  hydrosulfuric acid
HNO2  nitrous acid
HCN  hydrocyanic acid
HI  hydroiodic acid
H2SO4  sulfuric acid

20. Writing ACID formulas
Write the symbol(s) for the negative part. Find the charge for the negative part (anion).
After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript) to make the compound neutral.

21. Writing ACID formulas Practice! Hydrochloric acid Nitrous acid
Write the symbol(s) for the negative part. Find the charge for the negative part (anion).
After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript)
Practice!
Hydrochloric acid
Nitrous acid
Acetic acid
Hydroselenic acid
Permanganic acid

22. Writing ACID formulas Practice! Hydrochloric acid  HCl
Write the symbol(s) for the negative part. Find the charge for the negative part (anion).
After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript)
Practice!
Hydrochloric acid  HCl
Nitrous acid  HNO2
Acetic acid  HC2H3O2
Hydroselenic acid  H2Se
Permanganic acid  HMnO4

23. Writing ACID formulas Practice! 6. Hypochlorous acid
Write the symbol(s) for the negative part. Find the charge for the negative part (anion).
After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript)
Practice!
6. Hypochlorous acid
7. Hydrocyanic acid
8. Chromic acid
9. Phosphoric acid
10. Hydrosulfuric acid

24. Writing ACID formulas Practice! 6. Hypochlorous acid  HClO
Write the symbol(s) for the negative part. Find the charge for the negative part (anion).
After you find the charge on the negative part (anion), ADD that many HYDROGENS to the front (with a subscript)
Practice!
6. Hypochlorous acid  HClO
7. Hydrocyanic acid  HCN
8. Chromic acid  H2CrO4
9. Phosphoric acid  H3PO4
10. Hydrosulfuric acid  H2S

25. Ionic Compounds
This is a bond between a metal and non-metal OR involving a polyatomic ion (ex.  NH4+)

26. Ionic Compounds
This is a bond between a metal and non-metal OR involving a polyatomic ion (ex.  NH4+)
Write the name of the first element or polyatomic ion
Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide
Add a roman numeral if the metal is a transition or inner transition metal (in the middle block) to identify the metals charge!
Exceptions: Ag1+, Zn2+, Cd2+, Al3+

27. Ionic Compounds NaCl K2S MgSO4 Mn(OH)2 Li2S
Write the name of the first element or polyatomic ion
Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide
Add a roman numeral if the metal is a transition or inner transition metal (not in group 1A or 2A)
Exceptions: Ag1+, Zn2+, Cd2+, Al3+

28. Ionic Compounds NaCl  sodium chloride K2S  potassium sulfide
MgSO4  magnesium sulfate
Mn(OH)2  manganese (II) hydroxide
Li2S  lithium sulfide
Write the name of the first element or polyatomic ion
Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide
Add a roman numeral if the metal is a transition or inner transition metal (not in group 1A or 2A)
Exceptions: Ag1+, Zn2+, Cd2+, Al3+

29. Ionic Compounds CaBr2 Ni(CN)2 HgI2 Fe2(SO4)3 TiCl3
Write the name of the first element or polyatomic ion
Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide
Add a roman numeral if the metal is a transition or inner transition metal (not in group 1A or 2A)
Exceptions: Ag1+, Zn2+, Cd2+, Al3+

30. Ionic Compounds CaBr2  calcium bromide Ni(CN)2  nickel (II) cyanide
HgI2  mercury (II) iodide
Fe2(SO4)3  iron (III) sulfate
TiCl3  titanium (III) chloride
Write the name of the first element or polyatomic ion
Write the name of the second element or polyatomic ion. If it is an element change the ending to –ide
Add a roman numeral if the metal is a transition or inner transition metal (not in group 1A or 2A)
Exceptions: Ag1+, Zn2+, Cd2+, Al3+

31. Writing IONIC formulas
Write the symbol and find the charge of the positive side (cation)
Write the symbol and write the charge of the negative side (anion)
Determine how many of each ion are needed to make a neutral compound.
Erase the charges of each ion and add subscripts to show the number of each ion needed.
Write the cation first!
If a polyatomic ion needs a subscript, put parentheses around the ion formula!

32. Writing IONIC formulas
Write the symbol and find the charge of the positive side (cation)
Write the symbol and write the charge of the negative side (anion)
Determine how many of each ion are needed to make a neutral compound.
Erase the charges of each ion and add subscripts to show the number of each ion needed.
Write the cation first!
If a polyatomic ion needs a subscript, put parentheses around the ion formula!
Practice!
Sodium bromide
Lithium sulfide
Potassium iodide
Copper (II) chloride
Beryllium phosphide

33. Writing IONIC formulas
Write the symbol and find the charge of the positive side (cation)
Write the symbol and write the charge of the negative side (anion)
Determine how many of each ion are needed to make a neutral compound.
Erase the charges of each ion and add subscripts to show the number of each ion needed.
Write the cation first!
If a polyatomic ion needs a subscript, put parentheses around the ion formula!
Practice!
Sodium bromide = NaBr
Lithium sulfide = Li2S
Potassium iodide = KI
Copper (II) chloride = CuCl2
Beryllium phosphide = Be3P2

34. Writing IONIC formulas
Write the symbol and find the charge of the positive side (cation)
Write the symbol and write the charge of the negative side (anion)
Determine how many of each ion are needed to make a neutral compound.
Erase the charges of each ion and add subscripts to show the number of each ion needed.
Write the cation first!
If a polyatomic ion needs a subscript, put parentheses around the ion formula!
Practice!
Lead (II) nitrate
Calcium carbonate
Magnesium hydroxide
Sodium phosphate
Magnesium acetate

35. Writing IONIC formulas
Practice!
Lead (II) nitrate = Pb(NO3)2
Calcium carbonate = CaCO3
Magnesium hydroxide = Mg(OH)2
Sodium phosphate = Na3PO4
Magnesium acetate = Mg(C2H3O2)2
Write the symbol and find the charge of the positive side (cation)
Write the symbol and write the charge of the negative side (anion)
Determine how many of each ion are needed to make a neutral compound.
Erase the charges of each ion and add subscripts to show the number of each ion needed.
Write the cation first!
If a polyatomic ion needs a subscript, put parentheses around the ion formula!

36. Covalent Compounds
A non-metal bonded to another non-metal

37. Covalent Compounds A non-metal bonded to another non-metal
Name first element (add a prefix if there is more than one of that element)
Add a prefix and write the name of the second element. Change the suffix to -ide

38. Covalent Compounds
Name first element (add a prefix if there is more than one of that element)
Add a prefix and write the name of the second element. Change the suffix to –ide
Practice!
SO2
N2O4
P4O10
NO2
N2Cl4

39. Covalent Compounds
1. Name first element (add a prefix if there is more than one of that element)
2. Add a prefix and write the name of the second element. Change the suffix to -ide
SO2  sulfur dioxide
N2O4  dinitrogen tetroxide
P4O10  tetraphosphorous decoxide
NO2  nitrogen dioxide
N2Cl4  dinitrogen tetrachloride

40. Covalent Compounds
Name the first element (add a prefix if there is more than one of that element)
Add a prefix and write the name of the second element. Change the suffix to -ide
Practice!
SO3
ClO2
CS2
XeF2
S2Cl2

41. Covalent Compounds
Name first element (add a prefix if there is more than one of that element)
Add a prefix and write the name of the second element. Change the suffix to -ide
Practice!
SO3  sulfur trioxide
ClO2  chlorine dioxide
CS2  carbon disulfide
XeF2  xenon difluoride
S2Cl2  disulfur dichloride

42. Writing COVALENT formulas
Write the symbol for the first element. If there is a prefix add that number as the subscript.
Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono).

43. Writing COVALENT formulas
Write the symbol for the first element. If there is a prefix add that number as the subscript.
Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono)
Practice!
Boron trichloride
Dinitrogen monoxide
Dihydrogen monoxide
Carbon monoxide
Carbon dioxide

44. Writing COVALENT formulas
Write the symbol for the first element. If there is a prefix add that number as the subscript.
Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono)
Practice!
Boron trichloride  BCl3
Dinitrogen monoxide  N2O
Dihydrogen monoxide  H2O
Carbon monoxide  CO
Carbon dioxide  CO2

45. Writing COVALENT formulas
Write the symbol for the first element. If there is a prefix add that number as the subscript.
Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono)
Practice!
Sulfur trioxide
Phosphorus trihydride
Diphosphorus tetrabromide
Silicon dioxide
Sulfur hexafluoride

46. Writing COVALENT formulas
Write the symbol for the first element. If there is a prefix add that number as the subscript.
Write the symbol for the second element. Add the prefix number as the subscript (if it’s not mono)
Practice!
Sulfur trioxide  SO3
Phosphorus trihydride  PH3
Diphosphorus tetrabromide  P2Br4
Silicon dioxide  SiO2
Sulfur hexafluoride  SF6