Representative elements
Representative elements
They follow a pattern for valence electrons.
They follow a pattern for valence electrons.
They follow a pattern for valence electrons.
The tall columns in the periodic table are called groups or families. Elements in the same group share similar chemical properties and have the same number of valence electrons. For example, Group 1 contains alkali metals, while Group 17 consists of halogens. Each group typically exhibits trends in reactivity and other characteristics down the column.
They follow a pattern for valence electrons.
Elements in the tall columns of the periodic table, known as representative elements, are called so because they exhibit a wide range of chemical and physical properties that are representative of the broader trends in the periodic table. These elements include groups 1, 2, and 13-18, which display predictable patterns in their valence electron configurations and reactivity. Their behavior and characteristics make them ideal for illustrating the principles of periodicity and element classification.
Representative elements
Conventionally representative elements are called the chemical elements from the groups 1,2, 13-18. These elements haven't generally variable valencies. The transitions metals are not representative elements.
elements from group1-2 ,13-18 are called representative elements. Those from 3-12 form the transition elements!
The two rows at the bottom of the periodic table are taken out to make the table more compact and easier to read. These two rows are known as the lanthanides and actinides series. They are removed and placed below the main table to avoid making the entire table wider than it is tall.
Elements in the tall columns of the periodic table are called representative elements because they exhibit a wide range of physical and chemical properties that are representative of the overall characteristics of the elements in their respective groups. These elements include groups 1, 2, and 13-18, which display predictable behaviors in bonding and reactivity due to their valence electron configurations. Their diverse properties make them key examples for understanding the trends and patterns within the periodic table.