Kössel-Lewis Approach to Chemical Bonding

Flashcards summarizing the vocabulary and key concepts of the Kössel-Lewis approach to chemical bonding, including the octet rule, valence electrons, and ion formation.

Kössel and Lewis ($1916$)

The two scientists who independently provided a logical explanation of valence based on the inertness of noble gases.

Kernel

Lewis's description of an atom consisting of the positively charged nucleus and the inner electrons.

The Octet

A particularly stable electronic arrangement where eight electrons occupy the corners of a cube surrounding the Kernel.

Valence Electrons

The outer shell electrons that take part in chemical combination, while inner shell electrons remain protected.

Lewis Symbols

Simple notations introduced by American chemist G.N. Lewis to represent the valence electrons in an atom using dots.

Group Valence

A value calculated as either the number of dots in a Lewis symbol or $8$ minus the number of dots.

Halogens and Alkali Metals

Highly electronegative and highly electropositive elements, respectively, which are separated by noble gases in the periodic table.

Noble Gases

Elements (except helium) that possess a particularly stable outer shell configuration of eight electrons, denoted as $ns^{2} np^{6}$.

Electrostatic Attraction

The force that stabilizes positive and negative ions formed by the loss and gain of electrons during chemical bonding.

Bonding in Sodium and Chlorine

The formation of $Na^{+}$ and $Cl^{-}$ ions through the transfer of an electron, allowing each to attain a stable outer octet.

Bonding in $Cl_{2}$, $H_{2}$, and $F_{2}$

The process where chemical bonds are formed by the sharing of a pair of electrons between atoms to achieve a stable outer octet.