1. HISTORY OF THE PERIODIC TABLE NOTES

3. Organization of the Periodic Table
The _periodic_ _table_ is defined as an organization of the _elements_ in order of increasing _atomic_ _number_ and grouped according to similar _chemical___ properties and similar _electron_ arrangements.
Organization of the Periodic Table

4. Dmitri Mendeleev was a _Russian____ scientist who set up the first periodic table in the __19th____century.
Using Mendeleev’s system elements with similar _physical_ and _chemical_ properties fell into families or groups.
In the beginning…

5. Mendeleev’s Period Table
Organized by mass number
Mendeleev’s Period Table

6. Periodic table is made up of _families_, which are the _vertical_ columns.
_Families_ are a group of elements that share the same _chemical_ properties and the same number of _valence_ electrons.
Groups or Families

7. The _horizontal_ rows on the periodic table are called _periods_.
Elements found on the same _period_, share the same number of _energy_ levels found in the electron cloud.
Elements on the periodic table are identified by three things _chemical symbol_, _atomic_ number, and _atomic_ mass.
Periods

10. Metals Example: Al Metals lose electrons and have a positive charge
Most metals are solids except for Mercury (Hg) is a liquid
Properties of Metals
luster (are shiny)
malleable (bendable)
ductile (can be stretched into a wire)
conduct electricity
Francium (bottom left corner) is the most reactive metal
Metals Example: Al

12. Metalloids Example: Si
Lose or gain electrons to become stable
All solids
Some metalloids like Silicon have luster but others like arsenic do not
Some are malleable and ductile
Some conduct electricity
Metalloids are not very reactive because they need to gain or lose a lot of electrons
Metalloids Example: Si

14. Nonmetals Example: S Gain electrons and have a negative charge
All states of matter are represented
Bromine- liquid
Iodine- solid
Xenon- gas
No luster, malleability, or ductility
Poor conductors of heat and electricity
Fluorine (top right) is the most reactive nonmetal
Noble Gases are completely unreactive
Nonmetals Example: S

15. Families / Groups Alkali Metals Noble Gases Boron Group Oxygen Group
1 1
18 8
Group
Valence e-
Period 2 1 2 3 4 5 6 7
Alkaline Earth Metals
Alkali Metals
Noble Gases
Boron Group
Nitrogen Group
Oxygen Group
Halogens
Carbon Group
Transition Metals
Lanthanide Series
Actinide Series 6 7
Families / Groups

16. Groups are vertical columns
Periods represent horizontal rows
Elements in the same family share the same number of valence electrons.
Families

17. Families Hydrogen belongs to
NO family: ***It is in group one because it has one valence electron but it is not a metal and is not basic. Alkali means basic.
Be and Sr belong to the
Alkaline Earth Metals family.
Circle the element that belongs to the transition metal family: Rn, W, U, Ne, Sn
Families

18. Charges

19. Charges Ions: atoms that form a CHARGE by losing or gaining electrons
Oxidation Number/Charge: the number of electrons GAINED or LOST in an atom.
Positive Ions: are called CATIONS; they lose their valence electrons
Negative Ions: are called ANIONS; they gain e- in order to have a total of 8 valence electrons.
Charges

20. When ions are formed, atoms can only become stable by GIVING or RECEIVING electrons with other atoms.
Compounds: two or more atoms BONDED together by the VALENCE SHELL of their atoms.
Charges

21. Ionic Bonds: a bond that TRANSFER electrons; a bond between METAL and NON- METAL.
Covalent Bonds: a bond that SHARE electrons; a bond formed between NON- METAL and NON-METAL.
Metallic Bonds: a sea of ELECTRONS in the metals atoms that gives metals its luster, malleability, ductility, and conductivity. This is not a TRUE bond, but it allows molten metal to form ALLOY (metal solutions), like brass.
Charges

22. Reactivity F Metal Reactivity Decreases Non-Metal Reactivity Increases
Non-Metal Reactivity Decreas
Metal Reactivity Increases Fr
Reactivity

23. Arrange the following elements to increasing metal reactivity: Ca, Sr, Ba
Arrange the following elements to increasing non-metal reactivity: As, P, N
Arrange the following elements to increasing metal reactivity: Ni, Co, Fe
Arrange the following elements to increasing non-metal reactivity: C, O, F
Arrange the following element to decreasing metal reactivity: K, Na, Li
Reactivity

24. Atomic Radii

25. Atomic Radii The size of the atom
The atomic radii increases down a group because it is adding extra energy levels
The atomic radii decreases across a period because the atom does not want to lose electrons so it attracts them close to the positive nucleus (the force of attraction increases)
Atomic Radii

26. Ionization Energy

27. Ionization Energy The energy needed to remove an electron
As you move down a group the ionization energy decreases because the electrons are so far from the nucleus they are not held tightly to the atom and it takes little energy to remove them
As you move across a period ionization energy increases because the atom does not want to lose electrons so it holds the electrons tighter which takes more energy to remove them
Ionization Energy

28. Electronegativity

29. Electronegativity The ability of an atom to attract electrons
Electronegativity decreases down a group because the levels of electrons shield the positive nucleus from being able to attract additional electrons
Electronegativity increases across a period because the atoms need to gain electrons to become stable
Electronegativity