1. Unit 5 “Chemical Names and Formulas”
H2O
Unit 5 “Chemical Names and Formulas”
Chemistry
Troy High School
Mr. Blake

2. Section 9.1 Naming Ions

3. Atoms and Ions are electrically neutral.
Same number of p+ and e-
- atoms with a charge (+ or -)
Made by gaining or losing
Only electrons can move

4. F1- O2- An Anion is… A negative ion = electrons.
Nonmetals gain electrons.
Charge is written as a superscript on the right.
F1-
Has gained electron (-ide is new ending = )
O2-
Gained electrons ( )

5. K1+ Ca2+ A Cation is… A positive ion = electrons. lose electrons
Has lost electron (no name change for positive ions)
More protons than electrons
Ca2+
Has lost electrons

6. Predicting Ionic Charges
Group 1A:
Lose electron to form ions
H1+
Li1+
Na1+
K1+
Rb1+

7. Predicting Ionic Charges
Group 2A:
Loses electrons to form ions
Be2+
Mg2+
Ca2+
Sr2+
Ba2+

8. Predicting Ionic Charges
Loses electrons to form
ions
Group 3A:
B3+
Al3+
Ga3+

9. Predicting Ionic Charges
! Group 4A elements rarely form ions (they tend to share)
Group 4A: Do they lose 4 electrons or gain 4 electrons?

10. Predicting Ionic Charges
Nitride
Gains _
electrons to form
ions
Group 5A:
P3-
Phosphide
As3-
Arsenide

11. Predicting Ionic Charges
Oxide
Gains electrons to form ions
Group 6A:
S2-
Sulfide
Se2-
Selenide

12. Predicting Ionic Charges
Gains _ electron to form ions
Group 7A:
F1-
Fluoride
Br1-
Bromide
Cl1-
Chloride
I1-
Iodide

13. Predicting Ionic Charges
Group 8A: Stable noble gases form ions!

14. Predicting Ionic Charges
Group B elements: Many transition elements
have possible charge.
Use of Roman numerals to show charges
Iron (II) =
Iron (III) =
Show roman numerals up to 5.

15. Naming Cations
system – use roman numerals in parenthesis to indicate the charge value
2. Classical method – uses root word with suffixes (-ous, -ic)
Does not give true value

16. Naming cations
If the charge is always the (like in the Group A metals) just write the of the metal.
Calcium = 𝐶𝑎 +2
metals can have more than one type of charge.
Indicate charge as roman numeral in after the name of the metal (Table 9.2, p.255)
Iron (IV) =

17. Predicting Ionic Charges
Some elements also
have more than one possible charge.
Tin (II) =
Lead ( ) = Pb2+
Tin (IV) =
Lead ( ) = Pb 4+

18. Predicting Ionic Charges
Group elements:
Some transition elements
have only one possible oxidation state, such as these three:
**Do not use roman numerals for these
Silver =
Zinc =
Cadmium =

19. Practice by naming these:
Ca2+
Al3+
Fe3+
Fe2+
Pb2+
Li+

20. Write symbols for these:
Potassium ion
Magnesium ion
Copper (II) ion
Chromium (IV) ion
Barium ion
Mercury (II) ion

21. Anions are the same charge Change the ending to _
Naming Anions
Anions are the same charge
Change the ending to _
F1- a Fluorine atom will become a ion.

22. Practice by naming these:
Cl-
N3-
Br-
O2-
Ga3+

23. Write symbols for these:
Sulfide ion
Iodide ion
Phosphide ion
Strontium ion

24. Polyatomic ions are…
Groups of atoms that together, have an charge, and one name.
Usually end in – or _
Acetate: C2H3O2-
Nitr : NO3-
Nitr : NO2-
Permanganate: MnO4-
Hydroxide: OH- and Cyanide: CN-?

25. Know Table 9.3 on page 257 Sulf : SO42- Phosph : PO43- Sulf : SO32-
Carbonate: CO32-
Chromate: CrO42-
Dichromate: Cr2O72-
Phosph : PO43-
Phosph : PO33-
Ammonium: NH41+
(One of the few positive polyatomic ions)

26. H + Polyatomic ion =….
If the polyatomic ion begins with H, then put “hydrogen” in front of the polyatomic ion: H CO32- → HCO31- hydrogen + carbonate → hydrogen carbonate ion
HSO3
HPO4
HCO3

27. Helpful Hints on Oxy-Anions
1. _________: smaller # of oxygen
2. _________: larger # of oxygen
Ex.
NO3- ____________________________
NO2- ____________________________
SO42- ____________________________
SO32- ____________________________

28. A Guide to Determine Whether the –ate Formula is –XO3 or –XO4:1 2 3 4 5 6 13 14 15 16 17 18
Transition Metals B C N Si P S Cl As Se Br I

29. Section 9.2 Naming and Writing Formulas for Ionic Compounds

30. Writing Ionic Compound Formulas
Example: Iron (III) chloride
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.

31. Writing Ionic Compound Formulas
Example: Aluminum sulfide
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.

32. Writing Ionic Compound Formulas
Example: Zinc hydroxide
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.

33. Writing Ionic Compound Formulas
Example: Magnesium carbonate (note the 2 word name)
1. Write the formulas for the cation and anion, including CHARGES!
Mg2+
CO32-
2. Check to see if charges are balanced.
They are balanced!

34. Writing Ionic Compound Formulas
Example: Barium nitrate (note the 2 word name)
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.

35. Writing Ionic Compound Formulas
Example: Ammonium sulfate
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.

36. Writing Ionic Compound Formulas
Example: Aluminum phosphate
1. Write the formulas for the cation and anion, including CHARGES!
Al3+
PO43-
They ARE balanced!
2. Check to see if charges are balanced.

37. Naming Ionic Compounds
1. Cation , then anion
2. Monatomic cation = name of the element
Ca2+ = ion
3. Monatomic anion = root + -ide
Cl- =
CaCl2 =

38. Naming Ionic Compounds
(Metals with multiple oxidation states)
If the metal can have more than one charge ( ), use a Roman numeral in their name:
PbCl2  use the to find the charge on the cation (chloride is always 1-)
is the lead ( ) cation
PbCl2 = lead ( ) chloride

39. Things to look for:
If cations have ( ), the number in parenthesis is their .
If anions end in –ide, they are probably off the periodic table ( )
If anion ends in -ate or –ite, then it is

40. Practice by writing the formula or name as required…
Iron (II) Phosphate
Stannous Fluoride
Potassium Sulfide
Ammonium Chromate
MgSO4
FeCl3

41. Section 9.3 Naming and Writing Formulas for Molecular Compounds

42. Molecular compounds are…
Made of only
Smallest part is a
Can’t use charges to figure out how many of each atom (there are no charges present / they share electrons)

43. Molecular compounds are easier!
compounds use to determine how many of each.
Figure out charges and criss-cross numbers.
Molecular compounds: the name tells you the number of atoms.
Uses to tell you the exact number of each element present!

44. Prefixes (Table 9.4, p.269) 9 = nona- 10 = 1 = mono- 2 = di- 3 =
4 = tetra-
5 =
6 = hexa-
7 = hepta-
8 = octa-

45. Prefixes Prefix + name -ide
To write the name, include:
One exception is we don’t write if there is only of the element.
Normally, we do not have double vowels when writing names (oa oo)
Prefix + name -ide

46. Practice by naming these:
N2O
NO2
Cl2O7
CBr4
CO2
BaCl2

47. Write formulas for these:
diphosphorus pentoxide
tetraiodine nonoxide
sulfur hexafluoride
nitrogen trioxide
carbon tetrahydride
phosphorus trifluoride
aluminum chloride
(Ionic compound)

48. Section 9.4 Naming and Writing Formulas for Acids and Bases

49. Acids are…
Compounds that give off ions (H+) when dissolved in water (the Arrhenius definition)
Formula starts with .
Always be some Hydrogen next to an .
determines the name.

50. Rules for Naming acids: Name it as a normal compound first
If the anion attached to hydrogen ends in -ide, put the prefix and change -ide to - acid
In other words, if it’s just Hydrogen and one other nonmetal
HCl =
H2S =
acid
acid

51. Naming Acids
If the anion has oxygen in it, then it ends in -ate or -ite
Change -ate to -ic acid (use no prefix)
Example: HNO Hydrogen + nitrate =
Change -ite to -ous acid (use no prefix)
Example: HNO Hydrogen + nitrite =

52. Naming Acids ____-ide ____-ate ____-ite hydro-___-ic acid
Normal ending
____-ide
____-ate
____-ite
Acid name is…
hydro-___-ic acid
_____-ic acid
_____-ous acid

53. Practice by naming these:HF
H3P
H2SO4
H2SO3
HCN
H3PO4

54. Writing Acid Formulas – in reverse!
Hydrogen will be listed first
The name will tell you the
Be sure the charges cancel out.
Starts with hydro?
No hydro?
Anion is , ends in –ide
-ate anion comes from – ending
-ite anion comes from – ending

55. Write formulas for these:
hydroiodic acid
chloric acid
carbonic acid
phosphorous acid
hydrobromic acid

56. Names and Formulas for Bases
Base - an ionic compound that produces ions ( ) when dissolved in water (the Arrhenius definition)
Named the same way as other ionic compounds:
Name of cation ( ) followed by name of anion (which will be ).

57. Names and Formulas for Bases
NaOH =
Ca(OH)2 =
To write the formula:
Write symbol for metal cation
Followed by hydroxide ion (OH1-)
Use criss-cross method to balance the charges.

58. Practice by writing the formula for the following:
Magnesium hydroxide
Iron (III) hydroxide
Zinc hydroxide

59. Section 9.5 The Laws Governing Formulas and Names

60. Some Laws:
Law of Proportions- in a sample of a chemical compound, the of the are always in the proportions.
In every molecule of H2O (water), the mass ratio of H:O is 1:8

61. Some Laws:
Law of Proportions- Whenever two elements form than one compound, the masses of one element that combine with the mass of the other element are in the ratio of small
H2O (water) and H2O2 (hydrogen peroxide)
2: :2
2g:16g g:32g

62.
Law of Definite Proportions - Law of Multiple Proportions
by Brightstorm

63. Summary of Naming and Formula Writing
For naming, follow the flowchart- Figure 9.20, page 277
For writing formulas, follow the flowchart from Figure 9.22, page 278

64. Helpful to remember...
1. In ionic compounds, the net charge is _ (criss-cross method)
2. Put -ide at the end of monatomic
3. An -ite or -ate ending means there is a ion that has
4. Prefixes generally mean ; they show the number of each atom

65. Helpful to remember...
5. A Roman numeral after the name of a cation is the of the cation