Forming Compounds Lecture Review

A set of vocabulary flashcards covering the fundamental concepts of atomic stability, electron shell configurations, and different types of chemical bonding (covalent and ionic) based on the lecture notes.

Valence Shell

The outermost orbit of an atom; atoms seek stability by having all positions occupied in this shell.

Stable Octet

A configuration where an element's outer orbit (if it is more than one orbit) is fully occupied by 8 electrons, making it most stable.

$$2n^2$$

The formula used to determine the maximum number of electrons each shell can hold, where $n$ is the orbit number.

Covalent Bond

A bond formed when atoms share electrons, when a non-metal combines with another non-metal.

Molecules

Neutral particles built by covalent bonds.

Stable Duplex

A state of stability achieved when a valence shell (specifically the first orbit) is filled with 2 electrons, as seen in hydrogen molecules.

Triple Bond

The strongest type of covalent bond, formed when atoms share three pairs of electrons.

Non-polar Covalent Bond

A covalent bond where electrons are shared equally between two atoms, such as in $O_2$ or $N_2$.

Polar Covalent Bond

A covalent bond where electrons are not shared equally, resulting in one atom partially pulling the electrons toward itself, such as in $H_2O$.

Ion

An atom or group of atoms that carries an electrical charge.

Anion

A negatively charged atom that has gained one or more extra electrons.

Cation

A positively charged atom that has lost one or more electrons.

Ionic Compound

A substance composed of anions and cations, formed when a metal group atom combines with a non-metal group atom.

Ionic Bond

A bond resulting from the electrical attraction between a positive cation and a negative anion.

Coulomb's Law

In the context of chemistry, the law stating that shorter ionic bonds should be stronger than longer ones.

Lewis Dot Diagram

Also known as an Electron Dot Diagram, it is a representation used to show the valence electrons and bonding of atoms.