The document discusses naming rules for binary acids, oxyacids, and hydrated ionic compounds. It explains that binary acids contain hydrogen and a nonmetal and their names start with "hydro-", while oxyacids contain hydrogen and an oxyanion with the acid name based on the polyatomic ion. The document also outlines naming conventions for hydrated ionic compounds, which contain water molecules as part of their crystal structure.

1. Engage/Opening
Drag and drop to match the compound
name with its formula
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13. A binary acid is an acid that contains
only two different elements:
 The first element will always
be hydrogen!
 The second element will be a
nonmetal.
Start here

14. HF
HCl
H2S

15. Naming Binary Acids:
1. The name of the binary acid ALWAYS
begins with the prefix hydro—
2. The root of the second element’s name
follows the prefix.
3. The name ends with the suffix —ic.
Followed by the word acid.

16. HF
HCl
H2S
hydrofluoric acid
hydrochloric acid
hydrosulfuric acid

17. An oxyacid is an acid that contains
hydrogen and an oxyanion
An oxyanion is a polyatomic
anion that contains oxygen.
SO4
2-, NO3
-, PO4
3-, etc.

18. The name for the oxyacid is based
on the name of the polyatomic ion
contained in the acid.
The prefix hydro—
is NEVER used in naming oxyacids!!

19. Remember this:
—ate to —ic
—ite to —ous
If the polyatomic ion ends with the
suffix “—ate”,
change the “—ate” to “—ic”.

20. anion = nitrate (NO3)-
Change ate to ic
The acid is named
NITRIC ACID

21. anion = nitrite (NO2)-
Change ite to ous
The acid is named
NITROUS ACID

22.  The hydro- prefix tells us that this
is a binary acid.
 hydro—nonmetal root—ic acid
 So, the nonmetal is chlorine

23. Add the nonmetal: Cl-1
1. Write the symbols with their charges.
2. Cross over charges to subscript position
3. Need to reduce? No H Cl
1 -
+ 1
1 1
All acids begin with H+1

24. hydrobromic acid
hydroiodic acid
hydrosulfuric acid
HBr
HI
H2S

25.  No hydro- prefix tells us that this
is an oxyacid.
 Change the –ic back to -ate
 So, the polyatomic ion is acetate

26. Add the polyatomic ion: C2H3O2
-1
1. Write the symbols with their charges.
2. Cross over charges to subscript position
H C2H3O2
1 -
+ 1
1
All acids begin with H+1
1

27. Add the polyatomic ion: CO3
2-
1. Write the symbols with their charges.
2. Cross over charges to subscript position
H CO3
1 -
+ 2
2
All acids begin with H+
1

28. Acids are not ionic compounds. They
are molecules (covalently bonded).
Cl
H
However, when dissolved in water,
acids dissociate into ions. The
presence of the H+ makes it an acid.

29. sulfuric acid
phosphoric acid
nitrous acid
H2SO4
H3PO4
HNO2

31. Engage/Opening
Student Journal
Naming Rules for
Covalent Bonds
(handout)

33. MyBack Pack

37. Hydrated Ionic Compounds
 Hydrates contain a certain number
of water molecules with each
formula unit.
 Water molecules are a part of the
crystal structure of the ionic
compound.

38. Hydrated Ionic Compounds
CoCl2 6H2O
This portion of the formula is
the ionic compound.
cobalt (II) chloride
called the
water of
hydration

39. Hydrated Ionic Compounds
CoCl2 6H2O
Name the water molecules using
numerical prefixes with the root
“hydrate”.
cobalt (II) chloride
called the
water of
hydration
hexahydrate

40. Number Prefix Number Prefix
1 mono- 6 hexa-
2 di- 7 hepta-
3 tri- 8 octa-
4 tetra- 9 nona-
5 penta- 10 deca-

41. Hydrated Ionic Compounds
Barium hydroxide octahydrate
1. Write the formula for the ionic compound.
Ba(OH)28H2O
3. Write the prefix
number and add H2O.
2. Separate the hydrate
with a “dot”.

42. copper (II) sulfate
pentahydrate CuSO45H2O
Na2CO310H20
MgSO47H2O
sodium carbonate
decahydrate
magnesium sulfate
heptahydrate

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