1. THE PERIODIC TABLE OF ELEMENTS An Introduction

2. The Periodic Table By 1850, approximately 60 elements are known
Dmitri Mendeleev in 1869 publishes the first periodic table
Lists the physical and chemical properties of the known elements
Places elements with similar properties in families

3. First periodic table created by Dimitri Mendeleev in 1869.
                                

5. Mendeleev’s Periodic Table
Published in 1871, St. Petersburg, Russia by Dmitrii I. Mendeleev

6. The Modern Periodic Table

7. CURRENT PERIODIC TABLE
CONTAINS 113 ELEMENTS
ORGANIZED INTO 7 PERIODS
ORGANIZED INTO 18 FAMILIES/GROUPS

8. Why do we have those rows at the bottom?Tl Hg Au Hf Pt Ir Os Re W Ta He Rn At Po Bi Pb Cd Ag Zr Pd Rh Ru Tc Mo Nb Zn Cu Ti Ni Co Fe Mn Cr V In Xe I Te Sb Sn Ga Kr Br Se As Ge Al Ar Cl S P Si B Ne F O N C Li Be Na Mg K Ca Sc Rb Sr Y Cs Ba La Gd Cm Tb Bk Sm Pu Eu Am Nd U Pm Np Ce Th Pr Pa Yb No Lu Lr Er Fm Tm Md Dy Cf Ho Es Fr Ra Ac
This arrangement takes too
much space and is hard to read.

9. Atomic Symbols Each element is assigned a unique symbol.
hydrogen H arsenic As
uranium U radon Rn barium Ba gold Au
titanium Ti potassium K
Each symbol consists of 1 or 2 letters. The first is capitalized and the second is lower case.

11. The Periodic Table of the Elements
Alkali Metals
Alkali Earth Metals
Halogens
Nobel Gases
Lanthanide Series
Actinide Series
Metals
Non Metals
Semi metals
Representative Elements
Transition Elements
Periods
Family or Groups

12. Metals, Semimetals & Non MetalsH He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe * Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn + Fr Ra Lr * La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb + Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No

13. Common group names Alkali metals Alkaline earth metals Halogens
Noble gases
I A II A III A IV A V A VI A VIIA 0 H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar
III B IVB V B VIB VIIB VIII B IB IIB K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Lr Gd Tb Sm Eu Nd Pm Ce Pr Yb La Er Tm Dy Ho Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No

14. The Elements in the Human Body Biochemistry Percent dry weight
Carbon %
Hydrogen %
Oxygen 11%
Nitrogen 5.7%
Phosphorus 3.3%
Sulfur 1.0%
Calcium 5.0%
Potassium 1.3%
Sodium trace
Chlorine trace
Iron trace

15. THERE ARE 18 FAMILIES(GROUPS)
PERIODS AND FAMILIES
THERE ARE 18 FAMILIES(GROUPS)
THERE ARE 7 PERIODS

16. EXTENDED FAMILY: METALS
Have a high luster (are shiny) with most being silver/gray in color.
Good conductors (carriers) of heat and electricity.
Many have a high density
Many are ductile (can be drawn into a wire form)
Many are malleable (can be hammered into various shapes)
High melting points.
Majority of 113 elements are metals
Most have 1-2 valence electrons.
Metals hold onto electrons loosely—allows them to form metallic bonds.

17. METALS

18. FAMILY: ALKALI METALS (GROUP 1)
MOST REACTIVE OF METAL FAMILIES
Salt like in texture—can be cut with a knife
Low density
Good conductor of heat and electricity
They can harm the skin
They have 1 valence electron
Most reactive metals
Never found in the elemental form in nature. Always found as a compound with another element.
They corrode very rapidly in air.
Potassium and Sodium react very violently with water. They must be stored in kerosene or oil.

19. ALKALI METALS (Group 1)

20. Family: ALKALINE METALS EARTH METALS (GROUP 2)
SECOND MOST REACTIVE OF METAL FAMILIES
Harder and more dense than Alkali metals.
Never found in the elemental form in nature, always found as a compound.
Contain 2 valence electrons.
They react very easily, but not as active as alkali metals.
Have a higher melting point than alkali metals.

21. ALKALINE METALS (Group 2)
Earth Metals

22. EXTENDED FAMILY: TRANSITION METALS GROUPS 3-12
Most commonly used metals in everyday life.
Excellent conductors of heat and electricity
High melting points
High density
Most are very hard, some are brittle
Most have 2 valence electrons
Much less reactive than alkali and alkaline metals.
Many combine with oxygen to form oxides.
Many can be found in elemental form in nature as well as in compound form (colorful-gold,silver)
Iron,cobalt, nickel –can produce a magnetic field.

23. TRANSITION METALS
(Groups 3-12)
LANTHANOID
SERIES
ACTINOID
SERIES

24. EXTENDED FAMILY: RARE EARTH ELEMENTS
LANTHANOID SERIES
Metals are soft and malleable. Have a high luster and conductivity
Used to make various alloys (mixture of metals) and high quality glass
Contain 2 valence electrons.
ACTINOID SERIES
After Uranium the rest are synthetic/man made in the lab.
Contain 2 valence electrons
Uranium=fuel for nuclear reactions

25. EXTENDED FAMILY: METALLOIDS
Elements located along the dividing line between metals and non-metals.
They have properties of both metals and non-metals.
Metalloid means metal-like
They conduct heat + electricity better than non-metals-but not as good as metals
They are ductile and malleable.
They are all solids that can be shiny or dull.
Vary in valence electrons from 3 to 7.
Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium, Astatine

26. METALLOIDS

27. EXTENDED FAMILY: NON-METALS
Elements located to the right of the dividing line on the periodic table.
Can be solid, liquid, or gas
Physical and Chemical properties are opposite those of metals.
No luster, dull
Poor conductor of heat and electricity.
Not ductile or malleable—Many are brittle.
Lower densities + melting points than metals
Contain 4-8 valence electrons
Will share electrons—Not lose them. The positive nucleus will hold onto the electrons.

28. NONMETALS

29. FROM METALS TO NON-METALS
Four families compose them. They have metals, non-metals, and metalloids.
Families named after the first element in the group.
Boron Family (Group 13)—3 valence electrons (all metals except Boron) Aluminum—outstanding metal
Carbon Family (Group 14)——4 valence electrons—forms over 5million compounds. Carbon “basis of life compounds” Silicon—metalloid that makes glass, sand, computer chips
Nitrogen Family (Group 15)——5 valence electrons—they will not give them up only share them. Nitrogen=70% of air. Phosphorus—nonmetal makes match tips.
Oxygen Family (Group 16)——6 valence electrons—only share electrons

30. Carbon family
Nitrogen family
Oxygen family
Boron family

31. FAMILY: HALOGENS MOST REACTIVE FAMILY OF THE NON-METALS
Composed of 2 gases, 1 liquid + 2 solids
Halogen comes from 2 Greek words
Halos (salt) and Genos (to form)
Contains 7 valence electrons
Most active Non-metal family
Will gain or share 1 valence electron
When halogens react with metals they form salts
Sodium fluoride-used to fluoridate toothpaste + water (prevent cavities)
Calcium chloride—used to melt snow and ice
Fluorine-most reactive element

32. HALOGENS (Group 17)

33. FAMILY: NOBLE GASES LEAST REACTIVE FAMILY ON PERIODIC TABLE
All are gases and make up the last family.
All are present in various amounts in atmosphere
Used in colored lights (Neon=reddish orange)
Helium balloons
Called inert because they are not reactive
Contain 8 valence electrons.

34. NOBEL GASES (Group 18)