S3.1.1 The structure of the periodic table Notes

Periods, Groups, and Blocks in the Periodic Table

The Structure of the Periodic Table: Periods, Groups, and Blocks

The periodic table is divided into periods, groups, and blocks, each serving a specific role in organizing elements based on their electronic structure and properties.

Periods: Horizontal Rows

1. The horizontal rows of the periodic table are called periods.
2. Each period corresponds to the principal quantum number $n$, which represents the highest energy level occupied by electrons in an atom of an element in that row.
3. As you move across a period, the number of protons in the nucleus increases.
4. This stronger nuclear attraction pulls the electrons closer, leading to trends like decreasing atomic radius and increasing ionization energy.

Groups: Vertical Columns

1. The vertical columns of the periodic table are called groups.
2. Elements in the same group have the same number of valence electrons, which explains their similar chemical properties.
3. Group Numbers:
   1. Groups are numbered from 1 to 18.
   2. For groups 1 and 2, the group number equals the number of valence electrons.
   3. For groups 13–18, the last digit of the group number corresponds to the number of valence electrons.
4. Chemical Similarity:
   1. Elements within a group exhibit similar reactivity.
   2. For instance, all alkali metals react vigorously with water to produce hydrogen gas and a basic solution.

Blocks: s, p, d, and f

The periodic table is also divided into blocks, which correspond to the type of atomic orbital being filled with electrons.

1. s-block: Includes groups 1 and 2 (alkali and alkaline earth metals). The outermost electrons occupy the s sublevel.
2. p-block: Includes groups 13 to 18 (non-metals, metalloids, and some metals). The outermost electrons occupy the p sublevel.
3. d-block: Contains the transition metals (groups 3 to 12). The outermost electrons occupy the d sublevel.
4. f-block: Comprises the lanthanides and actinides (the two rows at the bottom). The outermost electrons occupy the f sublevel.

Metals, Metalloids, and Non-Metals: The Elemental Spectrum

The periodic table is also a map of elemental types, categorizing elements into metals, metalloids, and non-metals based on their properties.

Metals

1. Metals dominate the left and center of the periodic table (s-block, d-block, and parts of the p-block).
2. Properties:
   1. Metals are usually shiny, malleable, ductile, and excellent conductors of heat and electricity.
   2. They tend to lose electrons, forming positive ions ($cations$).
3. Examples: Sodium ($Na$), Iron ($Fe$), and Aluminum ($Al$).

Non-Metals

1. Non-metals are located on the right side of the periodic table (p-block).
2. Properties:
   1. Non-metals are often brittle (if solid), poor conductors of heat and electricity, and tend to gain or share electrons in reactions.
3. Examples: Oxygen ($O$), Chlorine ($Cl$), and Sulfur ($S$).

Metalloids

1. Metalloids form a zigzag line between metals and non-metals, exhibiting properties of both categories.
2. Properties:
   1. Metalloids can act as metals or non-metals depending on the chemical environment.
   2. For example, silicon ($Si$) conducts electricity like a metal but is brittle like a non-metal.
3. Examples: Boron ($B$), Silicon ($Si$), and Arsenic ($As$).