1. Chemical Names and Formulas
Unit 4

2. Counting Atoms
The subscript tells how many of that element is present.
Eg: H2O2= 2 hydrogen, 2 oxygen
If there is no subscript next to the symbol, it counts as “1”.
Eg: NaCl = 1 sodium & 1 chlorine

3. Counting Atoms
If the subscripted number is outside of the parenthesis, it is distributed to all elements within the parenthesis.
Eg: Ca(NO3)2 = Ca + NO3 x 2.
A preceeding coefficient is multiplied to all atoms in the compound.
Eg: 2BaCl2 = 2 Barium & 4 chlorine

4. Counting Atoms Calcium Carbonate: CaCO3. Ca = Calcium = 1 C = Carbon =
Oxygen = 3 5
Total atoms =

5. Counting Atoms Magnesium Hydroxide: Mg(OH)2. Mg = Magnesium = 1 H =
Hydrogen = 2
O =
Oxygen = 2 5
Total atoms =

6. Counting Atoms Acetic Acid: 2HC2H3O2. H = Hydrogen = 2 + 6 = 8 C =
Carbon = 4
O =
Oxygen = 4 16
Total atoms =

7. Practice
WS #1 – Counting Atoms

8. Chemical Formulas: Ionic
The simplest ionic compounds contain 2 elements and are called Binary.
In ionic binary compounds, a cation and an anion join together to form a neutral compound.
Ionic compounds are made from a metal and a non-metal.
IMPORTANT: ALL COMPOUNDS ARE NEUTRAL!!! Therefore, the charges must balance out!!!
Cation +
Anion =
Compound

9. Example: Calcium Bromide
If the charges are not equal, “lasso” the number only (not the sign) to write the formula. 1
+ 2 2
- 1 Ca Br
CaBr2
NOT Balanced!

10. Example: Writing the Chemical Formula for Potassium Bromide
Write the two symbols for the ions in the compounds, placing the symbol for the cation first. +1 -1 K Br
KBr
Balanced!
Determine the charge of each ion from the oxidation state on the periodic table.
If the charges are equal, drop them and write the formula.

11. More examples… Potassium Bromide = KBr Calcium Bromide = CaBr2
Lithium Fluoride = LiF
Lithium Oxide = Li2O
Note: the subscript has nothing to do with the name of the ionic compound.

12. Writing the Name: Binary Ionic
Example: LiF
The element with the positive charge, cation (the metal) is written first.
This element is given its usual name, in this case, Lithium.
The second element is the anion. It’s name will be changed to end in “-ide”. Fluorine is changed to Fluoride.
The compound’s name = Lithium Fluoride.

13. Examples: Naming Binary Ionic
NaF
BaO
MgCl2
Sodium fluoride
Barium oxide
Magnesium chloride

14. Practice
WS #2 – Naming Binary Ionic Compounds

15. Naming Ionic Compounds with Polyatomic Ions
Same process as with binary compounds, but we don’t change the ending of the polyatomic to “ide.”
If the compound doesn’t end in “ide,” then it contains a polyatomic ion (look on your sheet).
Exception:
Hydroxide = OH-1

16. Naming Compounds w/ Polyatomic Ions
The cation keeps its name.
CaCO3
Carbonate
Calcium
Made of more than one element so it is a polyatomic ion.
The polyatomic ion also keeps its name, even though it is an anion.

17. Writing the Formula: Barium Phosphate
We recognize that Barium Phosphate contains a polyatomic ion because it ends in “ate”.
Get the charge of the polyatomic ion from the chart.
Use the periodic table for the charge on your element.

18. Barium Phosphate Ba PO4 Let’s Lasso! Add each ion’s charge. NO!!
Write the chemical symbols.
Are the charges balanced?
- 3 3
+ 2 2 Ba
PO4
We have 2 “PO4” ions so we need parentheses to separate the ion from the extra subscript.
Warning: only use parentheses if there is more than one polyatomic ion!!
Ba3(PO4)2

19. Let’s Try Again Mg OH Write the formula for Magnesium Hydroxide. + 2 2
- 1 1 Mg OH
We have 2 “OH” ions so we need parentheses to separate the ion from the subscript.
Mg(OH)2

20. Practice
WS #3 – Naming Ionic Compounds (no Transition Metals)

21. Transition Elements and Roman Numerals
Some metals can form more than one type of ion and therefore, have more than one possible charge.
To tell which charge is used, the chemical name contains a Roman numeral.
The Roman numeral tells the charge of the cation.

22. Transition Elements and Roman Numerals
WARNING
Roman numerals are NEVER used in the chemical formula!!

23. Rules to Write a Chemical Formula when Roman Numerals are Present
To write the chemical formula for Iron (III) Sulfide:
Write the two symbols for the ions in the compounds, placing the symbol for the cation first.
Get the charge of the metal from the Roman numeral in ( ) after the metal and look up the anion’s charge.
- 2 2
Fe2S3
+ 3 3 Fe S

24. Rules to Write a Chemical Name when Roman Numerals are Needed
If the metal has more than one oxidation state, the chemical name will contain a Roman numeral.
Oxygen has a charge of -2 and there are 3 for a total charge of -6.
Mn must have a charge of +6 to neutralize the -6 charge.
Mn can have a charge of +7, 6, 4, 2 or 3
Now write the chemical name using a roman numeral to represent the charge of the Manganese.
Start with the anion to determine its overall negative charge.
You CANNOT lasso up to determine the Roman numeral.
Manganese (VI) Oxide
MnO3

25. Let’s Try Again Fe2O3 Write the chemical name of Fe2O3. Rust
The 2 Fe ions must have an overall charge of +6. So 6/2 = +3.
Fe can have a charge of +2 or 3
Oxygen has a charge of -2 and there are 3 for a total charge of -6.
Rust
Fe2O3
Iron (III) Oxide
Now write the chemical name.
Now do part C of your worksheet.

26. Practice WS #4 – Naming Ionic Compounds with Transition Metals
WS #5 – Mixed Ionic Naming Review
WS #6 – Ionic Naming Quiz Review
Ionic Naming Quiz

27. Covalent Compounds
Covalent compounds are made from 2 non-metals and are binary.
Since there are no ions involved, we don’t look at charges.
And because we don’t look at charges, we must use numbering prefixes!!
The subscript to the right of the element tells the prefix to use for that element.
We change the ending of the second element to –ide.
SO2 = Sulfur Dioxide

28. Covalent Compounds
One caveat: If there is only one beginning element, we DO NOT use the prefix mono
However, if there is only one second element, we DO USE the prefix mono
SO2 = Sulfur Dioxide
Not:
SO2 = Monosulfur Dioxide
But:
CO = carbon monoxide

29. Covalent Compound Prefixes
Mono = one
Di = two
Tri = three
Tetra = four
Penta = five
Hexa = six
Hepta = seven
Octa = eight
Nona = nine
Deca = ten
Triangle
Hexagon

30. Some Covalent Compounds
NF3
nitrogen trifluoride
N2Cl4
dinitrogen tetrachloride
NO2
nitrogen dioxide
TOXIC!
N2O
dinitrogen monoxide
Laughing Gas

31. Practice WS #7 – Naming Covalent Compounds
WS #8 – Ionic/Covalent Naming Review

32. Naming Acids
Acids are compounds that give off hydrogen ions when dissolved in water.
Acids begin with H followed by an anion.
The anion determines the name.

33. Naming Rules When the anion DOES NOT contain Oxygen:
Use the prefix hydro + root of the anion’s name + ic + the word acid
Examples: HCl - hydrochloric acid HBr- hydrobromic acid
When the anion contains Oxygen:
The name will depend on the name of the polyatomic anion. DO NOT use the prefix hydro.
Examples:
H2SO4 the anion is sulfate, therefore the acid name will end in ic
H2SO4 = Sulfuric acid.
H2SO3 the anion is sulfite, therefore the name of the acid will end in ous
H2SO3 = sulfurous acid.
ATE → IC
ITE → OUS

34. Name these Acids HF H3P H3PO4 H3PO3 HCN H2CrO4 Hydrofluoric Acid
Hydrophosphoric Acid
Phosphoric Acid
Phosphorous Acid
Hydrocyanic Acid
Chromic Acid

35. Practice WS #9 – Naming Acids
WS # 10 – Mixed Naming Review (Ionic, Covalent, Acids)

36. Binary Acids
Binary Acids contain only 2 elements, and the cation is hydrogen. Add the prefix hydro-, take the anion name and change the suffix to –ic.
HCl(aq) Hydrochloric Acid
HF(aq) Hydrofluoric Acid
HI(aq) Hydroiodic Acid

37. Binary Acids Exceptions: HCN = Hydrocyanic Acid CN = Cyanide
HN3 = Hydroazoic Acid azo = Nitrogen

38. Oxyacids
Ternary Acids contain 3 elements, hydrogen and a polyatomic ion containing oxygen.
The acid suffix is determined by the polyatomic ion suffix.
If the anion ends in -ate, change the suffix to –ic acid.
Nitric Acid
HNO3 =
Hydrogen & Nitrate =

39. More Oxyacids H2SO4 = Hydrogen & Sulfate = Sulfuric Acid Chloric Acid
HClO3 =
Hydrogen & Chlorate =

40. More Oxyacids
If the anion has one less oxygen & ends in -ite, change the suffix to –ous acid.
Hydrogen & Nitrite =
HNO2 =
Nitrous Acid
H2SO3 =
Hydrogen & Sulfite =
Sulfurous Acid
HClO2 =
Hydrogen & Chlorite =
Chlorous Acid

41. Oxyacids
If a third acid is formed with 1 less oxygen than -ite, it keeps the prefix hypo- and adds the suffix –ous.
E.g. HClO = Hydrogen & hypochlorite = Hypochlorous Acid
If it has one more oxygen than -ate, it keeps the prefix per- and adds the suffix –ic.
E.g. HClO4 = hydrogen & perchlorate = Perchloric Acid.

42. Writing Formulas for Acids
Hydrogen will always be first.
The name tells you the anion.
Make sure the molecule is neutral.
If the name starts with the prefix hydro- and ends with -ic, there is no oxygen in the formula.
If there is no prefix, the suffix –ate comes from –ic and –ite comes from –ous.

43. Write Formulas for these Acids
hydroiodic acid
acetic acid
carbonic acid
phosphorous acid
hydrobromic acid HI
HC2H3O2
H2CO3
H3PO3
HBr

44. Naming Organic Compounds
Hydrocarbons are compounds made of only carbon and hydrogen linked in long chains.
Alkanes – have single bonded carbons so they are saturated.

45. Naming Organic Compounds
Alkenes – have double bonded carbons so they are unsaturated.
Alkynes – have triple bonded carbons
We’ll work with alkanes so hydrocarbons will have the suffix –ane.

46. Organic Stems 1 carbon = meth- 6 carbons = hex- 2 carbons = eth-
7 carbons = hept-
3 carbons = prop-
8 carbons = oct-
4 carbons = but-
9 carbons = non-
5 carbons = pent-
10 carbons = dec-

48. Organic Compounds
If the atoms are linked in a ring rather than in a chain, the prefix cyclo- is added.
Hexane in a chain CH3-CH2- CH2- CH2- CH2- CH3.
Cyclohexane has 6 carbons in a ring.
Each point represents a carbon.

49. Organic Compounds If the chain is straight: CnH2n+2 n=#carbons
E.g. C3H(2×3)+2 = C3H8 = Propane
CH3-CH2-CH3
If the chain is cyclic: CnH2n
E.g. C3H6 = cyclopropane