The periodic table:

• Is arranged by increasing atomic number. The atomic number tells us how many protons atoms of that element have. In atoms, there are an equal number of protons and electrons, so the atomic number also tells us how many electrons the atoms for that element has.

Metals, metalloids, non-metals:
         

• Metals are located on the left hand side of the periodic table.
• Non-metals are located on the right hand side of the periodic table
• Metals are located on the latter between metals and non-metals.
• Nonmetals have properties opposite those of the metals. The nonmetals are brittle, not malleable or ductile, poor conductors of both heat and electricity, and tend to gain electronsin chemical reactions. Some nonmetals are liquids.

Families:

• Families are a vertical column of elements that share
• Alkali Metals, Alkaline Earth Metals, Halogens and noble gasses are some common families in the periodic table.
• The vertical columnson the periodic table are called groups or families because of their similar chemical behavior. All the members of a family of elements have the same number of valence electrons and similar chemical properties.
• The electron arrangement is connected because in each family there is a certain amount of energy shells the atoms will have.

Periods:

• In each period (horizontal row), the atomic numbers increase from left to right. The periodsare numbered 1 through 7 on the left-hand side of the table. Elements that are in the same period have chemical properties that are not all that similar.
• All of the elements in a period havethe same number of atomic orbitals.

Ion charges:

• Chargesthat are negative are called anions. Elements in the same group have the same charge. A group in the periodic table is a term used to represent the vertical columns. The noble gases of the periodic table do not have a charge because they are nonreactive.
• This is because unpaired valence electrons are unstable and eager to bond with other chemical species. This means that the oxidation states would be the highest in the very middle of the transition metal periods due to the presence of the highest number of unpaired valence electrons.

Reactivity of elements:

• Caesiumand fluorine. Group I metals are the most reactive metals.
• They only have one electronin their outer shell which is easy to lose; they get more reactive as you go down the periodic table as the electron is further from the nucleus and shielded by the inner electrons
• At the top of the noble gasesis helium (He), with a shell that is full with only two electrons, is not reactive.
• Their outer shells are full means they are quite happy and don’t need to react with other elements. In fact, they rarely combine with other elements.