Configuración Electrónica y Tabla Periódica

The most stable and probable arrangement of electrons around an atomic nucleus.

The electron arrangement in an isolated atom at its lowest energy level.

No two electrons in an atom can have the same four quantum numbers.

Electrons fill orbitals individually before pairing up if orbitals have the same energy.

A region of space where an electron is most likely to be found.

The arrangement of electrons in the different energy levels and sublevels of an atom.

Elements in groups 1 and 2, and 13 through 18 of the periodic table; their electron configurations end in 's' or 'p' orbitals.

Elements in groups 3 through 12 of the periodic table; their electron configurations end in 'd' orbitals.

Elements within the transition elements group that have particular properties.

Elements in the f-block of the periodic table, including the lanthanides and actinides.

A horizontal row in the periodic table, related to the principal energy level of an electron.

A vertical column in the periodic table, elements within a group share similar chemical properties due to similar electron configurations.

The order in which atomic orbitals are filled with electrons, following Hund's rule and the Aufbau principle.

Elements in groups 1 and 2, and 13-18 of the periodic table. Their electron configurations end in 's' or 'p' orbitals.

Elements in groups 3-12 of the periodic table, located in the 'd' block. Their electron configurations end in 'd' orbitals.

Elements in groups 3-12 of the periodic table

Elements in the 'f' block of the periodic table, including lanthanides and actinides.

Arrangement of electrons in atomic orbitals, follows rules like Hund's rule and the Pauli exclusion principle

A visual way to show the distribution of electrons in each orbital

Gadolinium (Gd) has an electron configuration ending in 4f orbitals.

Elements of Group 1 (Alkali Metals) and Group 2 (Alkaline Earth Metals) are characterized by how their outermost electrons (and valence electrons) behave.

The arrangement of electrons in a Gadolinium atom.

Gadolinium's outer electron arrangement: 6s2 5d1 4f7

Shortened notation using noble gas symbols for inner electron shells

Elements with ns electrons.

Elements with ns2 np(1-6) electrons.

Elements with ns2 (n-1)d(1-10) electron arrangement.

Elements with ns2 (n-1)d1 (n-2)f(1-14) configuration.

Describes how electrons are arranged in atomic levels. This determines the atom's chemical behavior.

Electron arrangement of an element in the 4th period with three unpaired electrons in the p subshell, typically a nonmetal.

Electron arrangement in the 5th period and transition metal group, with two d electrons in the 4d subshell. Typically a transition metal.

Electron arrangement of a 6th period element with one single electron in the 6s subshell. Typically an alkali metal.

Electron arrangement of a 7th period element, typically a metal in the f-block.

Electron arrangement of a noble gas in the third period.

The element in the fourth period and the 13th group of the periodic table is Gallium (Ga).

Iron (Fe) is a transition metal in the 4th period with an electron configuration ending in 4s23d6.

Radon (Rn) is the noble gas located in the 6th period.