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Electron Configuration

The arrangement of valence electrons around the nucleus that determines an element's chemical and physical properties.

Periodic Table Structure

A framework that helps predict the properties of elements based on their electron configurations and patterns in valence electrons.

s-block

The section of the periodic table that includes Groups 1 and 2, where elements have 1 or 2 electrons in their outer s subshell.

p-block

The section of the periodic table that includes Groups 13–18, where elements have electrons in the p subshell.

d-block

The section of the periodic table that includes transition metals (Groups 3–12), characterized by filled or partially filled d subshells.

f-block

The section of the periodic table that includes lanthanides and actinides, where f subshells are being filled.

Alkali Metals

Elements in Group 1 with one electron in the outer s subshell, known for their high reactivity.

Alkaline Earth Metals

Elements in Group 2 with two electrons in the outer s subshell, less reactive than alkali metals.

Halogens

Elements in Group 17 that are one electron short of a full octet, making them very reactive.

Noble Gases

Elements in Group 18 with a full valence shell, characterized by their relative nonreactivity.

Transition Metals

Elements in Groups 3–12 that contain filled or partially filled d subshells and are generally less reactive than Groups 1 and 2.

Core Electrons

Electrons in the inner energy levels of an atom that do not participate in chemical reactions.

Valence Electrons

Electrons in the outermost energy level that participate in chemical reactions.

Coulomb’s Law

A principle that describes the force between two charged particles based on their charges and the distance between them.

Effective Nuclear Charge (Zeff)

The net positive charge experienced by valence electrons, calculated as Zeff = Z - S, where Z is the nuclear charge and S is the shielding constant.

Shielding Effect

The phenomenon where core electrons reduce the effective nuclear charge felt by valence electrons due to their repulsive forces.

Periodic Trends

Observations about how properties such as Zeff change across periods and down groups in the periodic table.

Comparative Models

Analyzing elements in the same group, like silicon and germanium, to understand variations in effective nuclear charge due to differences in shielding and nuclear charge.