1. Chapter 5
The Periodic Table

2. Section 5.1 In 1750, only 17 elements were known.
As the rate of discovery increased, so did the need to organize the elements
In 1789 Antoine Lavoisier grouped the known elements into metals, nonmetals, gases, and earths.

3. Mendeleev’s Periodic Table
 Medeleev made flash cards of the 63 known elements. (1863)
On each card he put the name of the element, mass, and properties.
When he lined the cards up in order of increasing mass, a pattern emerged.
Mendeleev arranged the elements into row in order of increasing mass so that elements with similar properties were in the same column.
A deck of cards can be divided into four suits—diamonds, spades, hearts, and clubs. In one version of solitaire, a player must produce an arrangement in which each suit is ordered from ace to king. This arrangement is a model for Mendeleev's periodic table.

4. Mendeleev’s Prediction
Periodic Table- Arrangement of elements in columns, based on a set of properties that repeat from row to row.
Mendeleev’s Prediction
He could not make a complete table because many of the elements had not yet been discovered. He had to leave spaces for those elements.
Eka-Aluminum – one space below Al. He predicted it would be a soft metal with a low m.p. and a density of 5.9 g/cm3
The close match between Mendeleev’s prediction and the actual properties of new elements showed how useful the periodic table could be.
Gallium was discovered in It’s a soft metal, m.p. is 29.7 ˚C, and has a density of 5.91 g/cm3
Heat from a person's hand can melt gallium. In some traffic signals, there are tiny light emitting diodes (LEDs) that contain a compound of gallium

6. Mendeleev’s Periodic Table
How is the table organized?
Elements are arranged in order of increasing mass.
What do the long dashes represent?
They represent undiscovered elements.
Why are masses listed with some of the dashes, but not with all of them?
He was able to predict properties for some unknown elements based on the properties of neighboring elements.

7. 5.2 The Modern Periodic Table
The sounds of musical notes that are separated by an octave are related, but they are not identical. In a similar way, elements in the same column of the periodic table are related because their properties repeat at regular intervals. But elements in different rows are not identical.

8. Periodic Law
Mendeleev developed his chart before the proton was discovered.
In the modern periodic table, elements are arranged by increasing atomic number. (# of protons)
Periods- Each row in the table of elements is a period.
Groups- Each column on the periodic table is called a group.
Properties of elements repeat in a predictable way when atomic numbers are used to arrange elements into groups.
Members of a group have similar chemical properties.
This pattern of repeating properties is called periodic law.

9. Periods Periods - the rows; represent energy levels.
Row 1 (energy level 1) 2 elements
Row 2 (energy level 2) 8 elements
Row 3 (energy level 3) 18 elements
Row 4(energy level 4) 32 elements
The number of available orbitals increases from energy level to energy level.
Elements change from metals to metalloids to nonmetals as you move from left to right across the period.

10. Groups Groups/Families - the columns.
Atomic masses increase from top to bottom.
Members of a group have similar electron configurations and therefore have similar chemical properties.
Tells how many valence electrons are in the last energy level of an element.***
Valence electrons increase from left to right on the periodic table.
Valence electrons – an electron that is in the highest occupied energy level of an atom.

11. Valence Electrons Group Valence Electrons 1A 1 2A 2 3A 3 4A 4 5A 5 6A7 8A 8
A valence electron is an electron that is in the highest occupied energy level of an atom.
They play a key role in chemical reactions.
The # of valence electrons increases from left to right.
Elements in a group have similar properties because they have the same number of valence electrons.

12. Valence Electrons
Electron configuration is the arrangement of electrons in an atom.
The most stable electron configuration is one in which the outermost electron shell is completely filled.
Atoms will gain or lose electrons in order to achieve the most stable electron configuration.

13. Atomic Mass Mass Number is the # protons plus the # neutrons.
Atomic mass is a value that depends on the distribution of an element’s isotopes in nature and the masses of those isotopes.
All atoms of the same element do not have the same atomic mass.
Average atomic mass of an element is a weighted average of the masses of an elements isotopes.
The unit for atomic mass is – AMU
The standard on which the atomic mass unit is based is the mass of a Carbon-12 atom.

14. Average Atomic Mass
Weighted Averages – some values are more important that other values
For isotopes, the one that occurs more in nature contributes more to the average atomic mass.

15. Solving for Average Atomic Mass
When solving,
Convert the % abundance to a decimal
Multiply by its mass
Add the products together
EX:
Chlorine % X =
Chlorine % X =
amu
You Try:
Isotope
Mass (amu)
% abundance
27X
27.977
92.23
28X
28.976
4.67
29X
29.974
3.10

16. Classes of Elements
1. Chemical symbols are color coded by solids, liquids, and gases.
The symbols for solids are black. The symbols for liquids are purple. The symbols for gases are red.
2. Elements are divided into those that occur naturally and those that do not
The symbols for elements that don’t occur naturally are white
3. They are also classified by their general properties.
METALS, NONMETALS, METALLOIDS
In the periodic table, metals are located on the left, nonmetals are on the right, and metalloids are in between.

17. METALS majority of elements good conductors of heat and electricity
most are solids at room temp. (except Hg)
most are malleable and ductile –ability to be drawn into wires
some are reactive, some are not.
Ex. Gold Ex. Mg
Magnesium and aluminum are typical metals

18. Transition Metals
The metals in groups 3-12 are called Transition Metals.
They form a bridge between the two sides of the table. They are well known for their ability to form compounds with distinctive colors.
A compound of erbium (Er) and oxygen is used to tint glass pink.

19. Nonmetals properties are opposite of metals. poor conductors
many are gases at room temp.
the solids tend to be brittle
Some are very reactive, some don’t react at all.
Ex. F is most reactive element. Ex. Ne is not reactive.
Toothpaste contains a compound that helps to protect teeth from tooth decay. The compound is formed from the nonmetal fluorine and the metal sodium

20. Metalloids
elements with properties that fall between those of metals and nonmetals.
Ex. A metalloid’s ability to conduct electricity can vary with temperature. Si and Ge are insulators at low temps. and conductors at high temps.
Variation Across a Period
Across a period from left to right, the elements become less metallic.
From left to right across Period 3, there are three metals (Na, Mg, and Al), one metalloid (Si), and four nonmetals (P, S, Cl, and Ar). Many light bulbs are filled with argon gas.

21. 5.3 Representative Groups
“A” groups are #1-8
The number of the group is equal to the number of valence electrons in an atom of that element.
Valence electrons- An electron that is in the highest occupied energy level of an atom. 
Elements in a group have similar properties because they have the same number of valence electrons.
(This is why H is grouped with metals)

22. Alkali Metals Element Symbol Hyperlink Lithium Li Sodium Na Potassium
Rubidium Rb
Cesium Cs
Francium Fr
Group 1A
Most reactive metals
Reactivity increases from the top to the bottom.
So reactive many are kept under oil to prevent reacting with water or oxygen.
One Valence Electron
Found in nature only in a compound.
Form +1 ions because they will easily give up 1 electron for stability.

23. Alkaline Earth Metals Element Symbol Hyperlink Beryllium Be Magnesium
Group 2A
Have 2 Valence Electrons
Harder than the metals in 1A.
Form +2 Ions because they easily give up 2 electrons for stability.
Magnesium used in photosynthesis within the chlorophyll.
Calcium used in teeth and bone.
Element
Symbol
Hyperlink
Beryllium Be
Magnesium Mg
Calcium Ca
Strontium Sr
Barium Ba
Radium Ra

24. Boron Family Element Symbol Hyperlink Boron B Aluminum Al Gallium Ga
Group 3A
Have 3 Valence electrons
Form +3 Ions because they easily give up 3 electrons for stability.
1 metalloid (Boron)
Six metals
Aluminum is the most abundant metal in the Earth’s crust.
People are encouraged to recycle aluminum because it doesn’t take that much energy to do so.
Element
Symbol
Hyperlink
Boron B
Aluminum Al
Gallium Ga
Indium In
Thallium Tl
Ununtrium
Uut

25. Carbon Family Element Symbol Hyperlink Carbon C Silicon Si Germanium
Group 4A
Have 4 Valence Electrons
Form +/- 4 Ions because it will easily lose or gain 4 electrons for stability.
1 Nonmetal (Carbon)
2 Metalloids
3 Metals
Metallic nature increases from top to bottom.
With the exception of water, most of the compounds in your body contain carbon.
Silicon is the second most abundant metal in the earth’s crust.
Element
Symbol
Hyperlink
Carbon C
Silicon Si
Germanium Ge
Tin Sn
Lead Pb
Ununquadium
Uuq

26. Nitrogen Family Element Symbol Hyperlink Nitrogen N Phosphorus P
Group 5A
Have 5 Valence Electrons
Forms -3 Ions because it will easily gain 3 electrons for stability.
2 nonmetals
2 metalloids
2 Metals
Nitrogen and Phosphorus are used in fertilizers.
Element
Symbol
Hyperlink
Nitrogen N
Phosphorus P
Arsenic As
Antimony Sb
Bismuth Bi
Ununpentium
Uup

27. Oxygen Family Element Symbol Hyperlink Oxygen O Sulfur S Selenium Se
Group 6A
Have 6 Valence Electrons
Forms -2 Ions because it will easily gain 2 electrons for stability.
3 nonmetals
2 metalloids
1 metal
Oxygen is the most abundant element in the Earth’s Crust.
Ozone is another from of oxygen. At ground level it can irritate your eyes and lungs. At higher levels it absorbs harmful radiation from the sun.
Element
Symbol
Hyperlink
Oxygen O
Sulfur S
Selenium Se
Tellurium Te
Polonium Po
Ununhexium
Uuh

28. Halogens Element Symbol Hyperlink Fluorine F Chlorine Cl Bromine Br
Group 7A
Have 7 Valence electrons
Form -1 Ions because it will easily gain 1 electron for stability.
Most reactive nonmetals increase from bottom to top.
Known as “Salt Formers”
5 nonmetals
1 Unknown
Fluorine is the most reactive.
React easily with most metals.
Element
Symbol Hyperlink
Fluorine F
Chlorine Cl
Bromine Br
Iodine I
Astatine At
Ununspetium
Uus

29. Noble Gases Element Symbol Hyperlink Helium He Neon Ne Argon Ar
Krypton Kr
Xenon Xe
Radon Rn
Ununoctium
Uuo
Group 8A
8 Valence Electrons
Helium is the exception with only 2 valence electrons.
Extremely Un-reactive (Do not form Ions)
Odorless and colorless.
Used in light bulbs.
All are used in neon lights except argon.
Have the most stable electron configuration.

30. Patterns on the Periodic Table
Atomic # L to R.
Atomic mass L to R.
Energy level and orbitals in rows from T to B.
(Physical Properties) metals metalloids nonmetals from L to R.
Columns atomic mass from T to B.
Columns are based on chemical properties (reactivity).
Valence Electrons from L to R.
Most reactive metals are on the left side.
Most reactive non-metals are on the right side.