Module 8: The Periodic Table and Its Periodic Trends

Periodic Table

is an arrangement of the atoms in increasing order of their atomic numbers.

Period or Series

The arrangement of elements in horizontal rows

Family or Group

The vertical arrangement of elements in the Periodic Table and is identified by Roman Numerals and letters at the top of the column.

1. H to He

2. Li to Ne

3. Na to Ar

4. K to Kr (within Sc to Cu; 1^st transition series)

5. Rb to Xe (within Y to Ag; 2^nd transition series)

6. Cs to Rn (Lantanide series; 3^rd transition series)

7. Fr to Uu (Actinide series, 4^th trans, series)

There are seven periods on the basis of the seven energy levels.  The periods are in order of:

Representation - Family A

The kinds of elements of the different family in the Periodic Table are determined by the electronic configuration that ends with s and p are called _______ and fall under

Transition - Family B

Those electronic configuration ending with f and d are called and fall under

Same

Elements having the highest configuration with the same number of energy level based on electrons, fall under the _____ period.

Hydrogen

• Component of hydrochloric acid or most commonly known as muriatic acid

• Used as fuel to launch a rocket

• An ingredient in making cleaning chemicals, fiber textile, and glass.

Helium

• Most commonly used for inflating decorative balloons

• Used for scanning barcodes at checkouts

• Also used to inflate airbags. It can diffuse quicker than most unreactive gases

Lithium

• Used for mental illnesses including bipolar disorder, depression, and schizophrenia.

• Used in making rechargeable batteries

Periodic trends

The Periodic Table is a very valuable tool for predicting the ________ of atoms of elements. It summarizes the relationships of elements as to atomic size, electronegativity, electron affinity, and ionization energy.

Decreases

Atomic size ______ from left to read (period)

Ionization energy

is the energy required to remove the most loosely held electron from a gaseous atom.

Decreases

From top to bottom, Ionization energy

Increases

From left to right, Ionization energy

Electron Affinity

is a measure of the energy involved when an electron is added to a gaseous atom to form a negative ion. It is a measure of the attraction between the incoming electron and the nucleus - the stronger the attraction, the more energy is released.

Increases

Electron affinity _____ from left to right

Decreases

From top to bottom, electron affinity _____ on the basis of the # of energy levels

Nonmetals

• ____ have a greater electron affinity than metals because their atomic structure allows them to gain electrons rather than lose them.

• Atoms with a low electron affinity want to give up their valence electrons because they are further from the nucleus; as a result, they do not have a strong pull on the valence electrons.

Electron negativity

is the ability of an atom in compound to attract electrons to itself.

Increases

Electron negativity from left to right _____

Decreases

Electron negativity from top to bottom _____