Periodic Table With Names 1

How to study periodic table with names?

The modern periodic table was discovered by Dmitriv Mendeleev and it is the arrangement of elements according to their atomic numbers. So, the periodic law states that the property of an element is a periodic function of its atomic number. This table is one of the foundations of chemistry, providing a wealth of information about the elements, their properties, and their relationships with one another. In this blog post, we will explore the periodic table’s structure, the significance of its arrangement, and some interesting facts about the elements it contains. The study of periodic table and periodicity is very essential in learning chemistry as it serves as one of the foundations in building a solid chemistry knowledge..

The Structure of the Periodic Table

The periodic table is organized into rows called periods which is determined by the number of periods while the columns are called groups which is determined by the number of valence electrons.

Periodic Table With Names 3
Periodic Table With Names 3
  • Rows (Periods): These represent the energy levels or shells of the atoms. As you move from left to right across a period, the atomic number increases, indicating a rise in the number of protons in the nucleus.
  • Columns (Groups or Families): These indicate the number of valence electrons in the outer shell of an atom. Elements within the same group typically share similar chemical properties.

Also the periodic table is further divided into blocks based on electron configuration:

  • s-block: Groups 1 and 2, and Helium, contain elements with their outermost electrons in the s orbital.
  • p-block: Groups 13 to 18 contain elements with their outermost electrons in the p orbital.
  • d-block: Transition metals, in-between Groups 2 and 3 in small abridged periodic table, have electrons in the d orbital.
  • f-block: The lanthanides and actinides, which are usually shown separately at the bottom, have electrons in the f orbital.

studying periodic table with names

Alkali Metals (Group 1)

The group 1 elements are called alkali metals because of their quick tendency to form alkali when dissolved in water.

Na + 2H20 ==== 2NaOH + H2O

The alkali metals, including lithium, sodium, and potassium, are highly reactive and not found in nature as free elements. They have one valence electron and are known for their ability to react with cold water.

Alkaline Earth Metals (Group 2)

These elements, including magnesium and calcium, are less reactive than alkali metals but still exhibit reactivity. They have two valence electrons and form alkaline oxides.

Transition Metals (Groups 2-3 in the abridged version)

Transition metals, such as Scandium, titanium, vanadium, manganese are very special because of the special properties which they possess for example ability to form colorful compounds and ions, serve as catalyst, variable oxidation states etc.

Halogens (Group 17)

Halogens are called salt formers because they can easily form salts with metals.

2Na + Cl2 ====2NaCl

Other examples include fluorine, iodine, and astatine are highly reactive nonmetals with seven valence electrons. .

Noble Gases (Group 18)

Noble gases are stable because of the octet configuration or duplet configuration. They rarely participate in bonding as a result and examples are, helium, neon, and argon, are inert gases with full valence electron shells. This makes them non-reactive and ideal for use in lighting and cryogenics.

The periodic table remains a fundamental tool for chemists and scientists across various fields and understanding the periodic table with names makes it easier for learners to easily grasp the full content of the periodic table. .

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