1. Chemical Names and Formulas
NC Competency Goal 2:
The learner will build an understanding of the structure and properties of matter
NC Competency Goal 3:
The learner will build an understanding of regularities in chemistry.
NC Competency Goal 2
NC Competency Goal 3

2. The Periodic Table The elements are arranged in rows and columns on
the periodic table, according to similarities in their
properties.
A column of elements in the periodic table is
known as a group.
The “Group A” elements in the periodic table are
known as the representative elements.
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3. Representative elements include both metals and nonmetals.
The Periodic Table
Representative elements include both metals and nonmetals.
The metallic elements or “metals” are elements that have a high luster when clean and a high electrical conductivity.
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4. Characteristics of Metals
The Periodic Table
Characteristics of Metals
Ductile – can be drawn into wires.
Malleable – can be hammered into thin sheets.
Most of the elements on the periodic chart are metals.
The “ Group-B” elements are known as transition metals.
Elements with atomic numbers and are known as the inner transition metals or “rare earth metals”.
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5. Characteristics of Nonmetals
The Periodic Table
Characteristics of Nonmetals
The elements grouped on the right side of the periodic table are called nonmetals.
Nonmetals are elements that are nonlustrous and are poor conductors of electricity.
Hydrogen is a nonmetal that is a special case. It’s a nonmetal grouped on the left side of the periodic chart.
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6. Characteristics of Semimetals
The Periodic Table
Characteristics of Semimetals
Elements that exhibit properties of both metals and nonmetals are called semimetals or metalloids.
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7. The Periodic Table Review Questions Identify the following as metals,
semimetals or nonmetals.
Potassium
_________
Boron
_________
Iodine
_________
metal
semimetal
nonmetal
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8. The Periodic Table Review Questions Which of the elements below are
representative elements?
Potassium
Boron
Uranium
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9. Atoms and Ions
Sometimes…to form a chemical compound an atom can gain or lose an electron.
When the number of electrons no longer equals the number of protons the “once electrically neutral” atom becomes a charged particle.
Ions are atoms (or groups of atoms) that have a positive or negative charge.
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10. Atoms and Ions
Sometimes…to form a chemical compound an atom can gain or lose an electron.
When the number of electrons no longer equals the number of protons the “once electrically neutral” atom becomes a charged particle.
Ions are atoms (or groups of atoms) that have a positive or negative charge. Ions are formed when
atoms gain or lose electrons.
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11. Li 3 2 3 Atoms and Ions Lithium ion atom
Metals tend to lose one or more electrons and
form positive ions. A cation is any atom or
group of atoms with a positive charge.
Protons Electrons Li
3 p+
4 no 3 2 3
Lithium
ion
atom
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12. F - 9 9 10 Atoms and Ions Fluorine atom Fluoride ion
Nonmetals tend to gain one or more electrons
And form negative ions. A anion is any atom or
group of atoms with a negative charge.
Protons Electrons - F
9 p+
10 no 9 9 10
Fluorine atom
Fluoride ion
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13. Strontium is a group IIA metal and forms a cation with at 2+ charge.
The Periodic Table
Review Question
3. Write the formula and name of the ion formed.
a.) A Strontium atom loses two electrons.
Sr2+
Strontium ion
Strontium is a group IIA metal and forms a cation with at 2+ charge.
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14. Iodine is a groupVIIA nonmetal and forms an anion with at 1- charge.
The Periodic Table
Review Question
3. Write the formula and name of the ion formed.
a.) An iodine atom gains one electron. I-
Iodide ion
Iodine is a groupVIIA nonmetal and forms an anion with at 1- charge.
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15. The Periodic Table Review Question 4. Complete this table:
Symbol Change in Formula Name of
of Element electrons of ion ion
Ca2+
Calcium ion
a. Ca electrons lost __________ ___________
F ____________ F ___________
c. _________ ____________ Al ___________
1 electron gained
Fluoride ion Al
3 electrons lost
Aluminum ion
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16. Compounds John Dalton proposed in his early “atomic
Atoms of “A” Atoms of “B” Mixture of Compound of “A” and “B” Molecules made
from “A” and “B”
Compounds
John Dalton proposed
in his early “atomic
theory” that atoms of
different elements could indeed join together to make brand new substances.
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17. A + B ---> AB Compounds
Compounds form when atoms or ions join together to form new substances.
A + B ---> AB
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18. A + Z ---> AZ Compounds Metals + Nonmetals ---> Ionic Compounds
Nonmetals + Nonmetals ---> Molecular Compounds
Metals + Nonmetals ---> Ionic Compounds
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19. A + Z ---> AZ Compounds A molecule is an electrically neutral
nonmetal nonmetal molecular compounds
A + Z ---> AZ
A molecule is an electrically neutral
group of atoms that act as a single unit.
Compounds that are composed of molecules are called molecular compounds
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20. A+ + Z- ---> A Z + - Compounds Ionic Compounds are composed of
metal nonmetal ionic compounds
A+ + Z- ---> A Z + -
Ionic Compounds are composed of
positive and negative ions.
The smallest representative unit of an ionic compound is called a formula unit.
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21. 1+ 2+ 3+ 3- 2- 1- Ionic Charges IA IIA IIIA IVA VA VIA VIIA VIIIA
Use the chart below to determine the
Ionic charges of the representative elements.
Metals that
Form Cations
Nonmetals that
Form Anions
IA IIA IIIA IVA VA VIA VIIA VIIIA 1+ 2+ 3+ 3- 2- 1- NO
Charges
Formed
Charges
Vary
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22. REVIEW Write the symbol for each ion. Be sure to include the charge.
Hydrogen ion __________
Phosphide ion __________
Barium ion _____________
Mercury (II) ion _________ H+
P3-
Ba2+
Hg2+
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23. REVIEW Name the following ions. Oxide ion Lithium ion Fluoride ion
Cu2+_____________________
Oxide ion
Lithium ion
Fluoride ion
Copper (II) ion
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24. FYI The smallest representative unit of an element is an atom.
molecular compound is a molecule.
The smallest representative unit of an ionic compound is a formula unit.
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25. Polyatomic ions are charged particles made up of many atoms.
Poly = “many”
Atomic = “atoms”
Ions = “charged particles”
Polyatomic ions are charged particles made up of many atoms.
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26. H2PO4 C2H3O2 HSO3 HSO4 - - - - Dihydrogen phosphate Acetate
Polyatomic Ions
1- Charge
Formula Name -
H2PO4
Dihydrogen phosphate -
C2H3O2
Acetate
Hydrogen sulfite
(bisulfite) -
HSO3 -
Hydrogen sulfate
(bisulfate)
HSO4
NC Competency Goals 2 and 3

27. HCO3 NO2 NO3 - - - Hydrogen carbonate (bicarbonate) Nitrite Nitrate
Polyatomic Ions
1- Charge
Formula Name -
HCO3
Hydrogen carbonate
(bicarbonate) -
NO2
Nitrite -
Nitrate
NO3
NC Competency Goals 2 and 3

28. CN OH MnO4 - - - Cyanide Hydroxide Permanganate 1- Charge
Polyatomic Ions
1- Charge
Formula Name - CN
Cyanide - OH
Hydroxide -
Permanganate
MnO4
NC Competency Goals 2 and 3

29. ClO ClO2 ClO3 ClO4 - - - - Hypochlorite Chlorite Chlorate Perchlorate
Polyatomic Ions
1- Charge
Formula Name -
ClO
Hypochlorite
ClO2 -
Chlorite
ClO3 -
Chlorate
ClO4 -
Perchlorate
NC Competency Goals 2 and 3

30. HPO4 C2O4 SO4 CO3 Hydrogen Phosphate Oxalate Sulfate Carbonate
Polyatomic Ions
2- Charge
Formula Name 2-
HPO4
Hydrogen Phosphate
C2O4 2-
Oxalate
SO4 2-
Sulfate
CO3 2-
Carbonate
NC Competency Goals 2 and 3

31. CrO4 Cr2O7 SiO3 Chromate Dichromate Silicate 2- Charge Polyatomic Ions
Formula Name 2-
CrO4
Chromate
Cr2O7 2-
Dichromate
SiO3 2-
Silicate
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32. PO4 PO3 Phosphate Phosphite 3- Charge Polyatomic Ions Formula Name 3-
NC Competency Goals 2 and 3

33. Ammonium NH4 1+ Charge Polyatomic Ions Formula Name 1+
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34. (even though it’s originally formed from two charged particles) !
Writing Formulas for
Binary Ionic Compounds
A binary ionic compound is an ionic compound composed of two elements (metal and nonmetal).
When writing a formula for a binary ionic compound you must remember that the compound formed is electrically neutral
(even though it’s originally formed
from two charged particles) !
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35. Binary Ionic Compounds
Writing Formulas for
Binary Ionic Compounds
A binary ionic compound is an ionic compound composed of two elements.
metal nonmetal ionic compound
A+ + Z- ---> A Z + -
…..But, what if one of the ions above has a charge greater than 1+ or 1- ……then what do you do?
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36. A+ + Z2----> A Z + 2- 2 Writing Formulas for Binary Ionic Compounds
A binary ionic compound is an ionic compound composed of two elements.
metal nonmetal ionic compounds
A+ + Z2----> A Z + 2- 2
…Since the compound formed from two ions has to be electrically neutral….YOU have to balance the compound formula by adding subscripts where they’re needed.
…That means YOU have to add the subscript “2”
onto element “A” to show 2 atoms of this element
are needed to electrically “neutralize” each atom
of “Z” it combines with.
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37. Binary Ionic Compounds
Writing Formulas for
Binary Ionic Compounds
A binary ionic compound is an ionic compound composed of two elements.
Write the formula for a compound composed of the following pair of ions:
Answer Box
Li+ and S2-
Li2S
Lithium Sulfide
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38. Binary Ionic Compounds
Writing Formulas for
Binary Ionic Compounds
A binary ionic compound is an ionic compound composed of two elements.
Write the formula for a compound composed of the following pair of ions:
Answer Box
Mg2+ and N3-
Mg3N2
Magnesium Nitride
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39. Naming Ternary Ionic Compounds
Chemical Names
And Formulas
Naming Ternary Ionic Compounds
Ternary compounds contain atoms of three different elements.
Example: What is the formula for Potassium Nitrate?
Step 1: Write the formula for the cation. K+
NO3 -
Step 2: Write the formula for the anion.
Step 3: Balance the charges using
subscripts, if necessary.
NC Competency Goal 2
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40. Naming Ternary Ionic Compounds
Chemical Names
And Formulas
Naming Ternary Ionic Compounds
Ternary compounds contain atoms of three different elements.
Example: What is the formula for Lithium Sulfate?
Step 1: Write the formula for the cation.
Li+
SO4 2-
Step 2: Write the formula for the anion.
Step 3: Balance the charges using
subscripts, if necessary. 2
NC Competency Goal 2
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41. Naming Ternary Ionic Compounds
Chemical Names
And Formulas
Naming Ternary Ionic Compounds
Remember: Subscripts are numbers you add to balance the charges in the compound formula, however, the subscript itself is NOT a cation or anion!
Example: What is the formula for Lithium Sulfate?
Step 1: Write the formula for the cation.
Li+
SO4 2-
Step 2: Write the formula for the anion.
Step 3: Balance the charges using
subscripts, if necessary. 2
NC Competency Goal 2
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42. Naming Ternary Ionic Compounds
Chemical Names
And Formulas
Naming Ternary Ionic Compounds
Ternary compounds contain atoms of three different elements.
Example: What is the formula for Calcium Nitrate?
Step 1: Write the formula for the cation.
Step 2: Write the formula for the anion.
Ca2+
NO3 -
Step 3: Balance the charges using
subscripts, if necessary.
NC Competency Goal 2
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43. Naming Ternary Ionic Compounds
Chemical Names
And Formulas
Naming Ternary Ionic Compounds
When adding a subscript to polyatomic ion, first place parenthesis around the polyatomic ion. Then add the subscript needed to balance the charges on the OUTSIDE of the parenthesis
Example: What is the formula for Calcium Nitrate?
Step 1: Write the formula for the cation.
Step 2: Write the formula for the anion.
Ca2+
(NO3) -
Step 3: Balance the charges using
subscripts, if necessary. 2
NC Competency Goal 2
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44. 1+ 2+ 3+ 3- 2- 1- Ionic Charges IA IIA IIIA IVA VA VIA VIIA VIIIA
You may recall that an ionic charge formed
from a representative element can be determined
based on it’s location within the periodic chart.
Metals that
Form Cations
Nonmetals that
Form Anions
IA IIA IIIA IVA VA VIA VIIA VIIIA 1+ 2+ 3+ 3- 2- 1- NO
Charges
Formed
Charges
Vary
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45. Chemical Names
And Formulas
Naming cations that are formed from
transition elements (and group IVA metals)
Some transition elements (and group IVA metals) form cations that have multiple charges.
Cu1+
Cu2+
Copper (I) ion
Copper (II) ion
When naming these cations, indicate their ionic charge using a roman numeral within parenthesis.
NC Competency Goal 2
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46. Naming Ternary Ionic Compounds
Chemical Names
And Formulas
Naming Ternary Ionic Compounds
Example: What is the formula for Copper (II) Nitrate?
Step 1: Write the formula for the cation.
Cu2+
NO3 -
Step 2: Write the formula for the anion.
Step 3: Balance the charges using
subscripts, if necessary.
NC Competency Goal 2
NC Competency Goal 3

47. Naming Ternary Ionic Compounds
Chemical Names
And Formulas
Naming Ternary Ionic Compounds
When adding a subscript to polyatomic ion, first place parenthesis around the polyatomic ion. Then add the subscript needed to balance the charges on the OUTSIDE of the parenthesis
Example: What is the formula for Copper (II) Nitrate?
Step 1: Write the formula for the cation.
Step 2: Write the formula for the anion.
Cu2+
(NO3) -
Step 3: Balance the charges using
subscripts, if necessary. 2
NC Competency Goal 2
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48. Cu2 O Cu O Chemical Names And Formulas Naming compounds that contain
transition elements or group IVA metals.
Example: Write the name for the for compounds below?
Cu2 O Cu O
Copper (I) Oxide
Copper (II) Oxide
REMEMBER: Copper is a transition element, therefore you have to indicate the charge of copper (using a roman numeral within parenthesis) when writing the name for a “copper compound”.
NC Competency Goal 2
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49. Naming Binary Molecular Compounds
Chemical Names
And Formulas
Naming Binary Molecular Compounds
Binary Molecular Compounds are composed of two nonmetals.
Example:
CO2
Prefixes are used to name binary molecular compounds.
Carbon Dioxide

50. Prefixes Used to Name Binary Molecular Compounds
Number
Example CO
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10
Name
Carbon Monoxide

51. Prefixes Used to Name Binary Molecular Compounds
Number
Example
CCl4
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10
Name
Carbon Tetrachloride
Note: If one of the elements in the compound is a single atom, the prefix is normally omitted.

52. Prefixes Used to Name Binary Molecular Compounds
Number
Example
N2O5
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10
Name
Dinitrogen Pentoxide

53. P2O3 Prefixes Used to Name Binary Molecular Compounds Prefix Number
Example
P2O3
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10
Name
Diphosphorous Trioxide
Final Rule to Remember: Binary Compounds end in
the suffix –ide.

54. Chemical Names
And Formulas
Naming Acids
Acids are compounds that give off H+ (Hydrogen ions) when dissolved in water.
The symbol (aq) represents “aqueous”.
This symbol is an indication that HCl has been dissolved in water.
HCl(aq)
Hydrochloric Acid
NC Competency Goal 2
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55. Apply the rules in the chart below to name acids.
Chemical Names
And Formulas
Naming Acids
Apply the rules in the chart below to name acids.
Anion Suffix Example Acid Name Example
-ide Cl hydro-(stem)-ic acid hydrochloric acid
chloride
-ite SO (stem)-ous acid sulfurous acid 3
sulfite
-ate NO- (stem)-ic acid nitric acid 3
nitrate

56. HC2H3O2(aq) Acetic Acid Name the following acids Chemical Names
Anion Suffix Anion Name Acid Name Example
-ide hydro-(stem)-ic acid
-ite (stem)-ous acid
-ate C2H3O (stem)-ic acid acetic acid
Acetate ion -
Chemical Names
And Formulas
Name the following acids
HC2H3O2(aq)
Acetic Acid
(Press spacebar for answer)
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57. HF(aq) Hydrofluoric Acid Name the following acids Chemical Names
Anion Suffix Anion Name Acid Name Example
-ide F hydro-(stem)-ic acid hydrofluoric acid
-ite (stem)-ous acid
-ate (stem)-ic acid
fluoride ion
Chemical Names
And Formulas
Name the following acids
HF(aq)
Hydrofluoric Acid
(Press spacebar for answer)
NC Competency Goal 2
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58. HNO2(aq) Nitrous Acid Name the following acids Chemical Names
Anion Suffix Anion Name Acid Name Example
-ide hydro-(stem)-ic acid
-ite NO (stem)-ous acid Nitrous Acid
-ate (stem)-ic acid
nitrite ion -
Chemical Names
And Formulas
Name the following acids
HNO2(aq)
Nitrous Acid
(Press spacebar for answer)
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59. Summary: Chemical Names And Formulas
In an ionic compound, the net ionic charge is zero.
An –ide ending indicates a binary compound when (working with two elements).
An – ite or –ate ending means the formula has a polyatomic ion (when working with a compound).
Prefixes in the name indicate a molecular compound.
They show the number of each atom in a formula.
A roman numeral shows the ionic charge of the cation.
NC Competency Goal 2
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