1. Periodic Table of Elements
By: Suad, Khadija & Sahra

2. Reviewing the Atom...
The first official discovery of the atom was by Dalton who came up with a atomic theory which stated:
All elements are composed of tiny indivisible particles
Atoms of the same element are identical. The atoms of any one element are different
from those of any other element
Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratios to form compounds
Chemical reactions occur when atoms are separated from each other, joined, or rearranged in a different combination. Atoms of one element, however, are never changed into atoms of another element as a result of a chemical reaction

3. After Dalton a new explosion of studies around this area of chemistry erupted
Schrodinger devised the quantum mechanical model
Thomson discovered the electron, as well as isotopes.
Rutherford discovered that there was a nucleus in atoms
Bohr proposed that electrons had energy levels and that they revolved around the atomic nucleus but electrons can jump from one energy level (or orbit) to another.
Dobereiner organized elements into triads
Mendeleev was known for creating the first version of the periodic table

4. Reviewing Atomic Make-up...
The atom is divided up into three parts which vary from element to element. The neutrons added to the protons is called the mass number.
Protons
a subatomic particle in an atom's nucleus, with a positive electric charge
They also determine an atom's atomic number
Mass is that of 1 mass unit
Neutrons
a subatomic particle found in the nucleus like proton but without an electric charge
They help determine an atom's isotope
Mass is that of 1 mass unit
Electrons
a subatomic particle with a negative electric charge
They help determine an atom's ability to bond and location on the periodic table
Mass is 1/1840 relative to the mass of proton

5. Organizing the Periodic Table
There are many ways to organize the periodic table;
You can divide it up into Metals, Non Metals
and Metalloids (shown below)
You can divide up the elements on the table
by Alkali Metals, Alkaline Earth Metal, Transitional
Metals, Inner Transitional Metals, Halogens, Metals, Non Metals,
Metalloids and Noble gases (shown right)

6. What Makes NOBLE GASES special
The noble gases are located in the far right of the periodic table and were previously referred to as the "inert gases" due to the fact that their filled valence shells, making them extremely unreactive. The elements in this group are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).

7. The ACTINIDE Period...
They are all radioactive and some are not found in nature. Some of the elements with higher atomic numbers have only been made in labs. This atoms that are made in lab usually have short life-spans. The elements from are synthetic, and are occur naturally from different circumstances. The elements in this period include actinium (Ac), thorium (Th), protactinium (Pa), uranium (U), neptunium (Np), plutonium (Pu) americium (Am), curium(Cm), berkelium (Bk), californium (Ca), einsteinium (Es), fermium (Fm), mendelevium (Md), nobelium (No), lawrencium (Lr).

8. The LANTHANIDE Period...
Unlike Actinides, all the Lanthanides occur naturally in nature. The elements of this section of the period table are lanthanum (La), Cerium (Ce), Praseodymium (Pr), Neodymium (Nd), Promethium (Pm), Samarium (Sm), Europium (Eu), Gadolinium (Gd), Terbium (Tb), Dysprosium (Dy), Holmium (Ho), Erbium (Er), Thulium (Tm), Ytterbium (Yb), and Lutetium (Lu)

9. What Make HALOGENS special
The halogens are located on the left of the noble gases on the periodic table. These five toxic, non-metallic elements make up Group 17 of the periodic table and consist of: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). Although astatine is radioactive it is often included in the halogen group. Because the halogen elements have seven valence electrons, they only require one additional electron to become “happy” atoms. This characteristic makes them more reactive than other non-metal groups.

10. ALKALINE EARTH METAL Family
They are all shiny, silvery-white, somewhat reactive metals and are most likely gonna lose their two outermost electrons to form cations with a positive charge. The alkaline earth metals are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). They are in the second group and therefore have 2 valence electrons. All the discovered alkaline earth metals occur in nature.

11. ALKALI METALS Family
Alkali metals are among the most reactive metals. This is due in part to their larger atomic radii and low ionization energies. They tend to donate their electrons in reactions a become positive cation. The alkali metals include: lithium (Li), sodium (Na), potassium (K), rubidium (RB), cesium (Cs), and francium (Fr), hydrogen (H)

12. Metals, Nonmetals & Metalloids
When you divide the Periodic Table into three general groups you come up with Metals, Nonmetals and Metalloids
Metals
Makes up 80% of the table. It includes areas like the transition metals and alkali metals
Some notable qualities are their sheen, conductibility, that their ductile and malleable, metals are also solid at room temp.
Nonmetals
Is mostly found in the upper-right corner except for hydrogen which is on the left. Includes noble gases
Some notable qualities are that they the are poor conductors and most gases at room temp.
Metalloids
The metalloids part of the periodic table is the stepping stair between the metals and nonmetals
Share qualities of both metals and nonmetals

13. Important Terms to Know!
Octet Rule- That when forming compounds, elements like to have similar electron configurations to noble gases, which is to have eight electrons in their highest occupied shell
Valence Electrons- Are the electrons in the highest occupied shell of an atom
Cations- An ion with a positive charge
Anion- An ion with a negative charge
Ion- Is an atom or group of atoms that has a positive or negative charge. This is dependant on if the electrons in an atom is equal to the protons in an atom
Ionization Energy- The energy required an electron from an atom
Electronegativity- Is the ability of an atom of an element to attract electrons when the atom is in a compound

14. JOKES/RIDDLES What do you do with a sick chemist?
Anyone know any jokes about sodium?

15. Answers
If you can't helium, and you can't curium, then you might as well barium. NA