periodic table review 1

Periodic Law

The elements on the periodic table are arranged according to their ATOMIC NUMBERS.

Atomic Number

Determines the ELEMENT.

Henry Moseley

Proposed the arrangement of the periodic table by atomic numbers in 1915.

Period

A HORIZONTAL row on the Periodic Table. (Left to right)

Group

A VERTICAL column on the Periodic Table. (Top to bottom)

Ionization Energy

The amount of energy required to remove the most loosely bound electron from an atom.

Electronegativity

The ability to gain or attract electrons, or the affinity for electrons.

Malleable

The ability to be hammered into sheets. (e.g., aluminum foil)

Ductile

The ability to be made into wires. (e.g., copper wires)

Metals

Make up 2/3 of the Periodic Table and are located to the left of the metalloid staircase.

Metal Properties

Tend to lose electrons easily and form positive ions.

Metal Atom vs Ion Size

In metals, the atom is larger than the ion. (e.g., Na is larger than Na+)

Conductivity of Metals

Metals are good conductors of heat and electricity.

Reactivity of Metals

The most reactive metals are found in the lower left region of the Periodic Table. (Fr, Ra area)

Nonmetals

Located to the right of the staircase on the Periodic Table.

Nonmetal Properties

Tend to gain electrons and form negative ions.

Nonmetal Atom vs Ion Size

In a nonmetal, the ion is larger than the atom. (e.g., Cl- is larger than Cl)

Reactivity of Nonmetals

The most reactive nonmetals are found in the upper right region of the Periodic Table. (F, O area)

Metalloids

Are located on the staircase of the Periodic Table.

Metalloid Properties

Have some metallic and non-metallic properties.

Examples of Metalloids

Boron (B), silicon (Si), germanium (Ge), arsenic (As), antimony (Sb), tellurium (Te).