1. The Periodic Table and Chemical Nomenclature
Chapter 4
The Periodic Table and Chemical Nomenclature
Malone and Dolter - Basic Concepts of Chemistry 9e

2. Setting the Stage – The Periodic Table
The periodic table is the map of chemical behavior of the elements
Chemical nomenclature is the vocabulary of chemistry – how we name compounds and write formulas
Malone and Dolter - Basic Concepts of Chemistry 9e

3. Malone and Dolter - Basic Concepts of Chemistry 9e
Setting a Goal - Part A Relationships Among the Elements and the Periodic Table
You will be able to explain the significance of the periodic table, its origins, and how different properties of an element can be predicted by its location on the table
Malone and Dolter - Basic Concepts of Chemistry 9e

4. Objective for Section 4-1
Describe the origins of the periodic table
Malone and Dolter - Basic Concepts of Chemistry 9e

5. 4-1 The Origin of the Periodic Table
The elements are grouped in several categories, according to properties and therefore according to position in the periodic table.
Two major groupings are metals and nonmetals
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6. Professor’s Little Joke
Malone and Dolter - Basic Concepts of Chemistry 9e

7. The Origin of the Periodic Table
John Newlands, Dmitri Mendeleev and Lothar Meyer were the main originators of the periodic table of elements
Malone and Dolter - Basic Concepts of Chemistry 9e

8. The Modern Periodic Table of Elements
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9. Malone and Dolter - Basic Concepts of Chemistry 9e
Metals
Tend to form cations in ionic compounds
Are ductile (can be drawn into wires)
Malleable (can be pounded into sheets)
Readily conduct electricity and heat
See Figure 4-1
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10. Malone and Dolter - Basic Concepts of Chemistry 9e
Nonmetals
Tend to form anions in ionic compounds
Are generally soft solids or gases
See Figure 4-2
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11. Malone and Dolter - Basic Concepts of Chemistry 9e
Classes of metals
Active metals
very reactive to air and water
include lithium, potassium and sodium
Noble metals
very unreactive
gold, silver and copper
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12. Malone and Dolter - Basic Concepts of Chemistry 9e
Metalloids
Have properties intermediate between metals and nonmetals
Their most important current use is as semiconductors
Malone and Dolter - Basic Concepts of Chemistry 9e

13. Objective for Section 4-2
Using the periodic table, identify a specific element as a metal or a nonmetal and give its period, group number, the name of the group if appropriate, and its physical state
Malone and Dolter - Basic Concepts of Chemistry 9e

14. 4.2 – Using the Periodic Table
Locating the main types of elements
Metals are found to the left of the periodic table
Nonmetals are found to the right of the periodic table
Metalloids are located along the metal-nonmetal dividing line
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15. Malone and Dolter - Basic Concepts of Chemistry 9e
The Periodic Table
Elements were originally arranged in columns by chemical properties, then atomic weight
The modern periodic table has the elements arranged by atomic number
The periodic law - the properties of the elements are periodic (cyclically repeating) functions of their atomic number
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16. Malone and Dolter - Basic Concepts of Chemistry 9e
Periodic Divisions
Period
Horizontal rows in the periodic table
Properties of elements across a period change dramatically
Each period ends with a member of the noble gas family
Group
Vertical columns in the periodic table
Properties of elements in the same group are similar
Malone and Dolter - Basic Concepts of Chemistry 9e

17. Malone and Dolter - Basic Concepts of Chemistry 9e
Main Group Elements
Group IA - alkali metals
Group IIA - alkaline earths
Group VIA - chalcogens
Group VIIA - halogens
Group VIIIA - noble gases
* These are the groups with specific names
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18. Malone and Dolter - Basic Concepts of Chemistry 9e
Transition Elements
Group B elements
Metals with multiple oxidation states
Includes noble or coinage metals (Cu, Ag, Au)
Platinum group metals (Ru, Rh, Pd, Os, Ir, Pt)
Structural metals such as Fe and Cr
Malone and Dolter - Basic Concepts of Chemistry 9e

19. Inner transition elements
Lanthanides
Often called rare earth elements due to the difficulty in isolating pure samples
Chemical properties almost identical
Actinides
Radioactive elements, many synthetic
Malone and Dolter - Basic Concepts of Chemistry 9e

20. Physical States of Elements
Reference condition is 1 atmosphere of pressure and 25 °C
Gaseous elements - H2, N2, O2, F2, Cl2, noble gases
Liquid elements - Hg, Br2 Others?
All other elements are solids
Other molecular nonmetals are not diatomic and may have several forms (allotropes)
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21. Periodic Table – Summary Chart
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22. Setting a Goal – Part B The Formulas and Names of Compounds
You will learn how to systematically name various types of molecular and ionic compounds and determine the formulas of compounds from the names
Malone and Dolter - Basic Concepts of Chemistry 9e

23. Objective for Section 4-3
Write and name ionic compounds involving a metal and a nonmetal using IUPAC conventions
Malone and Dolter - Basic Concepts of Chemistry 9e

24. A Little Joke on Nomenclature
A research chemist walked into a pharmacy
and asks, “Do you have (5a,6a)-7,8-didehydro-4,5-
epoxy-3-methoxy-17-methylmorphinan-6-ol?”
The pharmacist scratched her head and
said, “Do you mean codeine?”
“That’s it!”, said the chemist, “I can
never remember that word!”
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25. 4-3 Naming and Writing Formulas of Metal-Nonmetal Binary Compounds
Binary compounds are composed of two different elements
Two types of metal-nonmetal binary compounds
Metals exhibiting only one oxidation state forming a compound with a nonmetal
Metals exhibiting two or more oxidation states forming a compound with a nonmetal
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26. Metals with only one Oxidation State
Groups of metals with only one common oxidation state
alkali metals +1
alkaline earths +2
Zn +2
Al +3
All other metals can exhibit more that one oxidation state
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27. Anions in Negative Oxidation States
Nonmetallic anions usually exhibit one negative oxidation state
Halogens -1
Chalcogens -2
N, P -3
C -4
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28. Forming Ionic Compounds
Metal and nonmetal combine to neutralize charge
Such compounds are often termed salts
Individual anions and cations do not exist separately – always found together
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29. Malone and Dolter - Basic Concepts of Chemistry 9e
Cross-Charge Method
Consider - Al3+, O2-
Cross multiply charges
2 Al O2- = Al2O3
Malone and Dolter - Basic Concepts of Chemistry 9e

30. Naming Binary Compounds
Use name of metal with no changes
Change the name of the anion by taking the “stem” and add the suffix -ide
Examples
NaCl - sodium chloride
MgCl2 - magnesium chloride
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31. Metals with Multiple Oxidation States
Two systems: Stock and “Classical”
Stock system
Metal name and the oxidation state in Roman numbers in parentheses
Fe2+ = iron(II)
Form compound by balancing charge of metal with correct number of nonmetals
CoCl3 = cobalt(III) chloride
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32. Classical Nomenclature
Metals in multiple oxidation states usually have one or two common oxidation states
First row transition metals are +2 and +3 (except Cu2+ and Cu+)
Use -ous suffix for lower common oxidation state
Use -ic suffix for higher common oxidation state
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33. Malone and Dolter - Basic Concepts of Chemistry 9e
Examples
CoCl3 - cobaltic chloride
NiCl2 - nickelous chloride
For metals with Latin names, use the Latin names
CuCl - cuprous chloride
FeBr3 - ferric bromide
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34. Objective for Section 4-4
Write and name compounds containing polyatomic ions using IUPAC conventions
Malone and Dolter - Basic Concepts of Chemistry 9e

35. 4-4 Naming and Writing Formulas of Compounds with Polyatomic Ions
Polyatomic ions (listed in Table 4-2) act as monoatomic ions in most circumstances
Most polyatomic ions are oxyanions, but some are simply polyatomic species with trivial names
Treat the polyatomic ion as a monoatomic ion in the cross-charge method for formula
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36. Malone and Dolter - Basic Concepts of Chemistry 9e
Oxyanions
Anions composed of oxygen and another element
Other elements can be a metal or a nonmetal
Examples
SO42-, NO2-, PO43-, MnO4-, CrO42-
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37. Malone and Dolter - Basic Concepts of Chemistry 9e
Naming Oxyanions
Need common oxidation states
most common oxidation state for nonmetals is the group number (except for the halogens)
next most common oxidation state is the group number minus one
Use -ate suffix for higher oxidation state and -ite suffix for next higher oxidation state
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38. Malone and Dolter - Basic Concepts of Chemistry 9e
Examples
SO42- - sulfate
SO32- - sulfite
NO3- - nitrate
NO2- - nitrite
Salts with these oxyanions
Na2SO4 - sodium sulfate
KNO3 - potassium nitrate
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39. Malone and Dolter - Basic Concepts of Chemistry 9e
Salts
Compounds formed by combining a cation and an anion in the proper ratio to yield a neutral species
Examples include NaCl, K2SO4, NH4I
Often formed by the reaction of a acid containing the anion and a hydroxide compound containing the cation
Malone and Dolter - Basic Concepts of Chemistry 9e

40. Examples of Salt Formation Occurring out of Water
2Na + Cl NaCl
NH3 + HCl NH4Cl
Malone and Dolter - Basic Concepts of Chemistry 9e

41. Objective for Section 4-5
Name binary molecular (nonmetal-nonmetal) compounds using proper Greek prefixes
Malone and Dolter - Basic Concepts of Chemistry 9e

42. 4-5 Naming Nonmetal-Nonmetal Binary Compounds
Name nonmetal further to the left of the periodic table first with no changes
Name nonmetal further to the right of the periodic table second with the -ide suffix
Use Greek prefixes to indicate the number of each one
Stock system is rarely used in this case since it can yield ambiguous results
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43. Malone and Dolter - Basic Concepts of Chemistry 9e
Greek Prefixes
Number
Prefixes 1
mono 2 di 3
tri 4
tetra 5
penta 6
hexa 7
hepta
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44. Malone and Dolter - Basic Concepts of Chemistry 9e
Examples
N2O3 – dinitrogen trioxide
N2O5 – dinitrogen pentoxide
CO2 – carbon dioxide
P2O5 – diphosphorus pentoxide
C3O2 – tricarbon dioxide (carbon suboxide)
CO – carbon monoxide
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45. Objective for Section 4-6
Name and write the formulas of acids
Malone and Dolter - Basic Concepts of Chemistry 9e

46. Malone and Dolter - Basic Concepts of Chemistry 9e
4-6 Naming Acids
Binary acids
Name begins with hydro
Then add stem of nonmetal plus -ic
End the name with acid
Examples
HCl - hydrochloric acid
H2S - hydrosulfuric acid
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47. Malone and Dolter - Basic Concepts of Chemistry 9e
Oxyacids (see Table 4-6)
Take oxyanion suffix and convert
Change -ate to -ic
Change -ite to -ous
Do not use hydro- in the beginning
Examples
H2SO4 - sulfuric acid
H2SO3 - sulfurous acid
Malone and Dolter - Basic Concepts of Chemistry 9e