1. Elements and The Periodic Table

2. Classification of Matter

3. “I Have No Bright Or Clever Friends”
The 7 Diatomic Elements
“I Have No Bright Or Clever Friends”
Or… HOFBrINCl

4. Dimitri Mendeleev 1869 Credited as the Father of the Periodic Table
Periodic Law: When arranged by atomic number, the properties of the elements repeat at regular intervals.

5. Mendeleev heard about atomic masses
He placed the name of each known element on a card, together with the atomic mass of the element and a list of observed chemical and physical properties.
He then arranged the cards according to various properties and looked for trends or patterns.

6. Mendeleev noticed that when the elements were arranged in order of increasing atomic mass, certain similarities in their chemical properties appeared in regular intervals. Such a repeating pattern is referred to as periodic.
Mendeleev created a table in which elements with similar properties were grouped together – a periodic table of elements! His procedure of organizing according to atomic mass left several empty spaces in his table and he was able to predict the properties of the elements that would fill these spaces!

8. Henry Mosely
In 1911, Henry Mosely discovered that the elements in the periodic table fit into patterns better when they were arranged in order of increasing atomic number.
Periodic Law states that the physical and chemical properties of the elements are periodic functions of the atomic numbers.

9. The periodic table has undergone extensive changes since Mendeleev’s time. Chemists have discovered new elements and, in more recent years, have synthesized new elements.
The periodic table is an arrangement of the elements in order of their atomic numbers so that the elements with similar properties fall into the same column, or group.

11. Long Form of the Periodic Table

12. and the same number of valence electrons

14. Metals, Non-metals, and Metalloids
There are two basic divisions on the periodic table. A thick zigzag line on the right-hand side on the periodic table designates the division.
Elements to the right of the line are non-metals, while the elements to the left are the metals (including the lanthanide and actinide series).
Elements along the border between metals and no-metals are called the metalloids. These exhibit properties of both metals and non-metals.

15. Metals, Non-metals, and Metalloids

16. Metaloids Contains properties of both metals and non-metals Silicon
Physical Properties
Shiny or Dull
Malleable
Ductile
Solid at room temperature
Properties
Better conductor than non-metals but worse than metals
Better conductors at high temperatures
Polonium is radioactive
Silicon
Arsenic
Germanium

17. Hydrogen (A class of it’s own)
Sometimes it behaves like an alkali metal, sometimes like a halogen, and sometimes in its own unique way.

18. Group 1: Alkali Metals
1 valence electron (electrons in their outermost shell)
Soft, shiny, easily cut with a knife
The most reactive metals
React violently with water (stored in oil or a vacuum)
React with halogens to form salts
Never found as free elements in nature, always bonded with other elements
Braniac: alkali metals
Disposal of sodium 1947

19. Group 2: Alkaline Earth Metals
2 valence electrons
Light, reactive metals
Form oxides when exposed to air. React with oxygen to from oxides, react with hydrogen to form hydrides (except beryllium). React with water to liberate hydrogen

20. Groups 3-12: Transition Metals
1 or 2 valence electrons
Strong, hard metals
Good conductors of heat and electricity
Wide range of chemical and physical properties

21. Group 17: Halogens 7 valence electrons Extremely reactive nonmetals
Not lustrous, nonconductors of electricity

22. Group 18: Noble Gases
Full outer shell
Extremely unreactive (inert)

23. Lanthanides (Rare Earth Metals)
Elements 57-70

24. Actinides Elements 89-102 Transuranic Elements: Synthetic elements