G10 Chemistry Bonding Booklet Practice Flashcards

A comprehensive set of vocabulary flashcards covering chemical bonding concepts including ionic, covalent, and metallic bonding, as well as molecular shapes, electronegativity, and intermolecular forces.

Ion

An atom that has an overall charge because it has either lost or gained electrons.

Cation

A positively charged atom formed when an atom loses electrons, resulting in more protons than electrons.

Anion

A negatively charged atom formed when an atom gains electrons, resulting in more electrons than protons.

Octet Rule

The tendency of atoms to react by losing, gaining, or sharing electrons so that there are $8$ electrons in their outermost shell to achieve stability.

Monatomic Anion

An anion consisting of only one atom present, typically ending with the suffix -ide.

Polyatomic Ion

An ion that contains more than one atom bonded together, such as sulfate ($SO_4^{2-}$), which carries an overall charge.

Ionic Bond

The strong electrostatic attraction between positively charged cations and negatively charged anions that holds the ions together.

Lattice Structure

A giant, regular repeating three-dimensional arrangement of ions or atoms, such as the arrangement found in ionic compounds or metals.

Chemical Formula (Ionic)

A representation showing the ratio of cations to anions required to form a neutral ionic compound with no net electrical charge.

Subscript

A notation in a chemical formula used to show the ratio of elements containing $2$ or more atoms.

Covalent Bond

A bond formed when the orbitals of nonmetal atoms overlap and electrons are shared to fulfill the octet rule.

Single Bond

A covalent bond formed by one pair of shared electrons.

Lone Pair

A pair of valence electrons that is not bonded to another atom.

Double Bond

A covalent bond formed when four electrons (two pairs) are shared between atoms, as seen in oxygen.

Triple Bond

A covalent bond formed when six electrons (three pairs) are shared between atoms, as seen in nitrogen.

Lewis Symbol

The chemical symbol of an element surrounded by dots, where each dot represents one valence electron.

Lewis Structure

A diagram showing the arrangement of atoms in a molecule, including the number of covalent bonds and lone pairs of electrons.

Delocalized Electrons

Valence electrons in a metallic lattice that are not tied to a specific nucleus and are free to move throughout the structure, also called a "sea of electrons."

Metallic Bond

The electrostatic attraction between positively charged metal ions (cations) and the delocalized sea of electrons.

Malleable

The property of metals that allows them to be bent or hammered into different shapes because layers of atoms can slide past each other without breaking bonds.

Giant Covalent Structure

Large extended structures of atoms, such as diamond or graphite, joined together by strong covalent bonds.

Simple Covalent Molecule

A substance made of a set number of atoms joined by covalent bonds, characterized by weak forces between molecules and low melting/boiling points.

Brittle

A physical property describing materials that shatter when hit, caused by like-charges repelling each other (in ions) or covalent bonds breaking (in giant structures).

Electron Pair Repulsion Theory

A theory stating that electron pairs (bonding and lone pairs) repel each other and arrange themselves to be as far apart as possible to minimize repulsion, determining molecular shape.

Electronegativity

A relative measurement of the ability of an atom to attract electrons in a chemical bond, with Fluorine assigned a value of $4.0$.

Nonpolar Covalent Bond

A bond formed when atoms have very similar electronegativities, resulting in electrons being shared equally and charge distributed evenly.

Polar Covalent Bond

A bond formed when the difference in electronegativity is between $0.4$ and $1.8$, causing electrons to be shared unequally.

Dipole Moment

The separation of charge within a molecule that creates a partial positive charge ($δ+$) on one end and a partial negative charge ($δ-$) on the other.

Polar Molecule

A molecule with an uneven distribution of electrons resulting in a dipole, where polar bonds are arranged asymmetrically.

London Dispersion Forces

Weak intermolecular forces that exist between all atoms and molecules caused by temporary and induced dipoles.

Permanent Dipole-Permanent Dipole Interaction

An intermolecular force occurring between polar molecules where the slightly positive side of one molecule is attracted to the slightly negative side of another.

Hydrogen Bonding

A specific strong dipole-dipole force occurring when hydrogen is bonded to highly electronegative atoms like oxygen ($O$), nitrogen ($N$), or fluorine ($F$).