1. Chapter 7: Chemical Formulas and Chemical Compounds
Coach Kelsoe
Chemistry
Pages

2. Chapter 7-1: Chemical Names and Formulas
Coach Kelsoe
Chemistry
Pages

3. Section 7-1 Objectives Explain the significance of a chemical formula.
Determine the formula of an ionic compound formed between two given ions.
Name an ionic compound given its formula.
Using prefixes, name a binary molecular compound from its formula.
Write the formula of a binary molecular compound given its name.

4. Chemical Names and Formulas
The total number of natural and synthetic chemicals runs in the millions, so often times it is easier to give chemicals their own names:
Calcium carbonate –
Sodium chloride –
Dihydrogen monoxide –
Sodium bicarbonate –
Limestone
Table salt
Water
Baking soda

5. Chemical Names and Formulas
The only problem with common names is that you can’t tell about its chemical composition.
There is a systematic method for naming compounds and for writing chemical formulas.

6. Ionic Compounds vs. Molecular Compounds
Ionic compounds are compounds that are held together by ionic bonds.
Molecular compounds are compounds that are held together by covalent bonds.
So how do you know the difference? Electronegativity values, silly!

7. Significance of a Chemical Formula
A chemical formula indicates the relative number of atoms of each kind in a chemical compound.
For a molecular compound, the chemical formula reveals the number of atoms of each element contained in a single molecule of the compound.
C H

8. Significance of a Chemical Formula
The chemical formula for an ionic compound represents one formula unit–the simplest ratio of the compound’s cations and anions.
Al (SO )
Note the parentheses to identify the anion as a unit. The subscript 3 refers to the entire unit. With no subscript, assume one atom.

9. Monatomic Ions
By gaining or losing electrons, many main-group elements form ions with noble-gas configurations.
Group 1 elements tend to form 1+ cations, group 2 elements tend to form 2+, etc.
Ions formed from a single atom are known as monatomic ions.
Group 17 elements tend to form 1- anions.

10. Monatomic Ions
Not all main-group elements readily form ions. Rather than gaining or losing electrons, carbon and silicon atoms form covalent bonds. Tin and lead tend to lose the two electrons in their p orbitals, but retain the two in the s orbital. What charge would they have?
Elements from the d-block form 2+, 3+, or in a few cases 1+ or 4+ cations.

11. Naming Monatomic Ions
Monatomic cations are identified simply by the elements name, followed by “cation.”
Potassium cation
Magnesium cation
Naming monatomic anions requires dropping the ending of the element’s name and replacing it with the suffix –ide.
Chlorine  Chloride anion
Nitrogen  Nitride anion

12. Some Common Monatomic Ions
Main-group elements 1+ 2+ 3+
Lithium Li+
Sodium Na+
Magnesium Mg2+
Aluminum Al3+
Potassium K+
Calcium Ca2+
Rubidium Rb+
Strontium Sr2+
Cesium Cs+
Barium Ba2+ 1- 2- 3-
Fluoride F-
Oxide O2-
Nitride N3-
Chloride Cl-
Sulfide S2-
Bromide Br-
Iodide I-

13. Some Common Monatomic Ions
d-block elements 1+ 2+ 3+ 4+
Copper(I) Cu+
Cadmium Cd2+
Chromium(III) Cr3+
Lead(IV) Pb4+
Silver Ag+
Chromium(II) Cr2+
Iron(III) Fe3+
Vanadium(IV) V4+
Cobalt(II) Co2+
Lead(III) Pb3+
Tin(IV) Sn4+
Copper(II) Cu2+
Vanadium(III) V3+
Iron(II) Fe2+
Lead(II) Pb2+
Manganese(II) Mn2+
Mercury(II) Hg2+
Nickel (II) Ni2+
Tin(II) Sn2+
Vanadium(II) V2+
Zinc Zn2+

14. Binary Ionic Compounds
Compounds composed of two different elements are known as binary compounds.
In a binary compound, the total numbers of positive charges and negative charges must be equal! Therefore the formula for such a compound can be written given the identities of the compound’s ions. For example: magnesium bromide. We do NOT put the charges in the final formula!

15. A Quick Math Review
Subscripts are the small numbers written to the right of an element’s symbol.
O2, H2O, CH4O
Coefficients are the large numbers written to the left of an element’s symbol.
2O2, 5H2O, 19CH4O
With polyatomic ions, the subscripts are multiplied:
(SO4)2, (HSO4)3, (H2PO4)4

16. “Crossing Over”
As an aid to determining subscripts in formulas for ionic compounds, the positive and negative charges can be “crossed over.”
Al3+ O2-
Al2O3
We can check to make sure this is correct by multiplying the original charge by the new subscripts to make sure the number is the same for both the atoms in the molecule.

17. Naming Binary Ionic Compounds
The nomenclature, or naming system, of binary ionic compounds involves combining the names of the compound’s positive and negative ions.
For most simple ionic compounds, the ratio of the ions is not indicated in the compound’s name because it is understood based on the relative charges of the compound’s ions.
Al2O3  Aluminum oxide

18. Sample Problem 1
Write the formula for the binary ionic compounds formed between zinc and iodine.
Zn2+ I-
ZnI2
Write the formula for the binary ionic compounds formed between zinc and sulfur.
Zn2+ S2-
ZnS

19. Sample Problems 1
Write formulas for the binary ionic compounds formed between the following elements:
Potassium and iodine
Magnesium and chlorine
Sodium and sulfur
Aluminum and sulfur
Aluminum and nitrogen

20. Sample Problems 1
Name the binary ionic compounds indicated by the following formulas:
AgCl
ZnO
CaBr2
SrF2
BaO
CaCl2

21. The Stock System of Nomenclature
Some elements, such as iron, form two or more cations with different charges. To distinguish the ions formed by such elements, the Stock system of nomenclature is used.
This system uses a Roman numeral to indicate an ion’s charge. The numeral is enclosed in parentheses and placed immediately after the metal name.
Fe2+  iron(II) Fe3+  iron(III)

22. The Stock System of Nomenclature
Names of metals that commonly form only one cation do not include a Roman numeral.
Na+  Sodium Ba2+  Barium
There is no element that commonly forms more than one monatomic anion.
Naming a binary ionic compound according to the Stock system is done as so:
CuCl2  copper(II) chloride
CuF3  copper(III) fluoride

23. Sample Problem 2
Write the formula and give the name for the compound formed by the ions Cr3+ and F-.
CrF3
Chromium(III) fluoride

24. Sample Problems 2
Write the formula and give the name for the following compounds formed between the following ions:
Cu2+ and Br-
Fe2+ and O2-
Pb2+ and Cl-
Hg2+ and S2-
Sn2+ and F-
Fe3+ and O2-
CuBr2; copper(II) bromide
FeO; iron(II) oxide
PbCl2; lead(II) chloride
HgS; mercury(II) sulfide
SnF2; tin(II) fluoride
Fe2O3; iron(III) oxide

25. Sample Problems 2 Give the names for the following compounds: CuO CoF3
SnI4
FeS
Copper(II) oxide
Cobalt(III) fluoride
Tin(IV) iodide
Iron(II) sulfide

26. Compounds Containing Polyatomic Ions
The list of polyatomic ions and their charges can be found on page 226 in your text.
All but the ammonium ion are negatively charged and most are oxyanions, polyatomic ions that contain oxygen.
It isn’t uncommon for two oxyanions to be formed from the same two elements:
Nitrogen and oxygen form nitrite and nitrate.

27. Compounds Containing Polyatomic Ions
When naming compounds containing oxyanions, the most common ion is given the ending –ate. The ion with one less oxygen atom is given the ending –ite.
NO2  Nitrite NO3  Nitrate
If two elements form more than two different oxyanions, an anion with one less oxygen than the –ite anion is given the prefix hypo-.
ClO2  Chlorite ClO  Hypochlorite

28. Compounds Containing Polyatomic Ions
An anion with more oxygen than the –ate anion is given the prefix per-.
Compounds containing polyatomic ions are named in the same manner as binary ionic compounds.
AgNO3  Silver nitrate; AgNO2  Silver nitrite
When more than one polyatomic ion is present in a compound, use parentheses.
Al2(SO4)3  Aluminum sulfate

29. Sample Problems 3 Write the formula for tin(IV) sulfate.
Sn4+ SO42-
Sn(SO4)2
Write the formulas for the following ionic compounds:
Sodium iodide
Calcium chloride
Potassium sulfide
Lithium nitrate
Copper(II) sulfate
NaI
CaCl2
K2S
LiNO3
CuSO4

30. Sample Problems 3 Give the name for the following compounds: Ag2O
Ca(OH)2
KClO3
NH4OH
FeCrO4
KClO
Silver oxide
Calcium hydroxide
Potassium chlorate
Ammonium hydroxide
Iron(II) chromate
Potassium hypochlorite

31. Naming Binary Molecular Compounds
Unlike ionic compounds, molecular compounds are composed of individual covalently bonded units, or molecules.
Chemists use two nomenclature systems to name binary molecules: the Stock system and the prefix system.
The prefix system uses numerical prefixes to identify the number of atoms in the molecule.

32. Naming Binary Molecular Compounds
For example, CCl4 is called carbon tetrachloride. The prefix tetra- means “four.”
The prefix will come before both molecules. The prefix mono- can sometimes be left off. 1
mono- 6
hexa- 2
di- 7
hepta- 3
tri- 8
octa- 4
tetra- 9
nona- 5
penta- 10
deca-

33. Rules for Naming Binary Molecular Compounds
The less-electronegative element is given first. It is given a prefix only if it contributes more than one atom to a molecule of the compound.
The second element is named by combining (a) a prefix indicating the number of atoms contributed by the element, (b) the root of the name of the second element, and (c) the ending –ide. With few exceptions, the ending –ide indicates that a compound contains only two elements.

34. Rules for Naming Binary Molecular Compounds
The o or a at the end of a prefix is usually dropped when the word following the prefix begins with another vowel, e.g., monoxide or pentoxide.
Tetraphosphorus decoxide
P4O10
Phosphorus comes first because it is less electronegative than oxygen.
The order of nonmetals in binary compound names and formulas- C, P, N, H, S, I, Br, Cl, O, F.

35. Sample Problem 4 Give the name for As2O5.
Diarsenic pentoxide
Name the following binary molecular compounds:
SO3
ICl3
PBr5
Sulfur trioxide
Iodine trichloride
Phosphorus pentabromide

36. Sample Problem 4 Write the formula for oxygen difluoride.
OF2
Write formulas for the following compounds:
Carbon tetraiodide
Phosphorus trichloride
Dinitrogen trioxide
CI4
PCl3
N2O3

37. Acids and Salts
Most acids used in the laboratory can be classified as either binary acids or oxyacids.
Binary acids are acids that consist of two elements, usually a hydrogen and one of the halogens – F, Cl, Br, or I.
Oxyacids are acids that contain hydrogen, oxygen, and a third element, usually a nonmetal.

38. Acids and Salts
Acids were first recognized as a specific class of compounds based on their properties in solutions of water. Consequently, in chemical nomenclature, the term acid usually refers to a solution in water of one of these special compounds rather than to the compound itself.
For example, hydrochloric acid refers to a water solution of the molecular compound hydrogen chloride, HCl.

39. Acids and Salts
Many polyatomic ions are produced by the loss of hydrogen ions from oxyacids.
An ionic compound composed of a cation and the anion from an acid is often referred to as a salt.
Table salt, NaCl, contains the anion from hydrochloric acid. Calcium sulfate, CaSO4, is a salt containing an anion from sulfuric acid.

40. Acids and Salts
Some salts contain anions in which one or more hydrogen atoms from the acid are retained. Such anions are named by adding the word hydrogen or the prefix bi- to the anion name.
The best known such anion comes from carbonic acid, H2CO3.