Chemistry Question

Revised 6/21/17Name ____________________________ Station # _______ Date ______________
CHM 101 Chemical Nomenclature – Report Sheet
Name the following compounds:
1. ZnSO3
2. KI
3. Fe2O3
4. CaCl2
5. SnBr4
6. P2O5
7. AlPO4
8. (NH4)2S
9. H2SO4
10. CsOH
11. Mg(ClO3)2
12. HIO
13. Li4C
14. KMnO4
15. NaHCO3
16. SO2
17. TiO3
18. HCl (aq)
19. H2O2
20. N2O4
21. N2
22. Cu2SO4 • 5H2O
23. Fe(OH)2
24. HClO
25. PbO2
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Revised 6/21/17
Give the formula for the following compounds:
1. Vanadium (V) Oxide
2. Nitric Acid
3. Sulfur Hexachloride
4. Cesium Hydroxide
5. Dinitrogen Trioxide
6. Iron (III) Chloride
7. Molecular Oxygen
8. Silver Sulfide
9. Calcium Carbonate Trihydrate
10. Sodium Hypochlorite
11. Potassium hydrogen sulfite
12. Barium Iodide
13. Copper (I) Sulfate
14. Lead (II) Chromate
15. Phosphorus Trichloride
16. Aluminum Carbonate
17. Antimony (III) Sulfide
18. Ammonium Phosphate
19. Lithium Hydride
20. Beryllium Fluoride
21. Bismuth (III) Telluride
22. Phosphoric Acid
23. Sodium Cyanide
24. Potassium Dichromate
25. Hydrobromic Acid
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Revised 6/21/17
Name _________________________ Station # _______ Date _________________
CHM 101 Chemical Nomenclature
Pre-Lab Question
Balance the charge on the following ions and write the correct formula in each box
Ion
Cl-
K+
NH4+
Mg2+
Fe3+
Na+
Ca2+
Fe2+
Al3+
KCl
OHCO32PO43-
Ion
O2-
Na2O
NO3 SO42AsO43-
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Revised 6/7/17
CHM 101 – Chemical Nomenclature
A. Rules for naming
1. Compounds made up of a representative metal and non-metal: name the cation,
then name the anion using “ide” ending.
2. Compounds made up of a transition metal and a non-metal: name the cation, use
a Roman numeric to show charge on the cation. Name the anion using “ide”
ending.
3. Covalent compounds:
– Name the first non-metal by its element name.
– Name the second non-metal with an “ide” ending.
– Use prefix toindicate the number of atoms of each non-metal (mono is
usually omitted).
4. Acids: for Oxyacids (contain oxygen in a polyatomic ion), name the polyatomic
ion but change the “ate” ending to “ic”, or “ite” ending to “ous”, and add the word
acid. For example: HNO3 = Nitrate – ate + ic + acid = Nitric acid.
5. Exceptions: H3PO4 = phosphate – ate + oric + acid = Phosphoric acid.
H2SO4 = sulfate –ate + uric + acid = Sulfuric acid.
H2SO3 = sulfite – ite + urous + acid = Sulfurous acid.
6. Non-Oxy acids: Hydro + stem of the element + “ic” ending.
For example: HI = hydro + iod + ic acid = hydroiodic acid
HCl = hydro + chlor + ic acid = hydrochloric acid.
HCN = hydro + cyan + ic acid = hydrocyanic acid.
B. To create molecular formulas:
Use name, periodic table, and polyatomic ion list to determine charges (oxidation state)
of cation. For example: a representative metal element has a fixed charge, determine
charge on the anion (usually fixed charge); then combine cation and anion into a
molecule, using subscripts to exactly balance positive and negative charges.
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Revised 6/7/17
Anion
C2H3O2−
HCO3−
CO3 2−
CrO4 2−
Cr2O7 2−
CN−
HSO3−
NO3−
MnO4−
SO4 2−
Common Polyatomic Ions
Name
Anion
Acetate ion
OH−
Bicarbonate ion
ClO−
Carbonate ion
ClO2−
Chromate ion
ClO3−
Dichromate ion
ClO4−
Cyanide ion
O2 2−
Hydrogen sulfite ion
HSO4 −
Nitrate ion
NO2 −
Permanganate ion
PO4 3−
Sulfate ion
SO3 2−
Cation
NH4+
Name
Ammonium ion
Anion
Br−
Cl−
F−
I−
Common Monoatomic Anions
Name
Anion
Bromide ion
N 3−
Chloride ion
O 2−
Fluoride ion
P 3−
Iodide ion
S 2−
Name
Nitride ion
Oxide ion
Phosphide ion
Sulfide ion
Cation
Al 3+
Co 2+
Cu+
Cu 2+
Fe 2+
Fe 3+
Pb 2+
Sn 2+
Common Monoatomic Cations
Name
Cation
Aluminum ion
Zn 2+
Cobalt (II) ion
Co 3+
Copper (I) ion
Hg2 2+
Copper (II) ion
Hg 2+
Iron (II) ion
Mn 2+
Iron (III) ion
Ag+
Lead (II) ion
Pb 4+
Tin (II) ion
Sn 4+
Name
Zinc ion
Cobalt (III) ion
Mercury (I) ion
Mercury (II) ion
Manganese (II) ion
Silver ion
Lead (IV) ion
Tin (IV) ion
Name
Hydroxide ion
Hypochlorite ion
Chlorite ion
Chlorate ion
Perchlorate ion
Peroxide ion
Hydrogen sulfate ion
Nitrite ion
Phosphate ion
Sulfite ion
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