Elements in the same group possess the same number of valence electrons, which determines their chemical properties.

Sodium belongs to Group 1 of the periodic table, known as the alkali metals.

Group 17 elements are collectively known as halogens.

Noble gases occupy Group 18 and are characterized by their complete valence shells.

The transition metals are found in the d-block, located between groups 3 and 12.

Atomic radius decreases across a period because the effective nuclear charge increases, pulling electrons closer to the nucleus.

Silicon exhibits properties of both metals and non-metals, classifying it as a metalloid.

Group 2 elements are designated as alkaline earth metals.

The f-block elements (lanthanides and actinides) are commonly called inner transition metals.

The modern periodic table is organized by the increasing atomic number (number of protons) of the elements.

Metalloids, or semi-metals, possess intermediate properties between those of typical metals and non-metals.

Vertical columns in the periodic table are known as groups, which usually contain elements with similar chemical properties.

Group 18 elements are known as noble gases; they have a full outer shell of electrons and are largely unreactive.

Sulfur is a non-metal that is solid at room temperature, while Bromine is a liquid and Neon is a gas.

The d-block elements (Groups 3-12) are widely known as the transition metals.

As you move down a group, the atomic size increases and the valence electrons are further from the nucleus, causing electronegativity to decrease.

Hydrogen (Atomic number 1) is the lightest and simplest element in the periodic table.

The f-block elements consist of the lanthanide and actinide series, commonly known as inner transition metals.

Horizontal rows are called periods, representing the principal energy level being filled by electrons.