Chemistry Structure and Bonding

Flashcards covering key concepts on chemical bonding, molecular structure, and properties related to the chemistry lecture notes.

Dot-and-Cross Diagram

A representation of the arrangement of atoms and electrons in a molecule, where dots and crosses are used to show different electron contributions from different atoms.

Ionic Lattice

A regular arrangement of ions in a solid where strong electrostatic forces hold the oppositely charged ions together.

Covalent Bond

A chemical bond formed by the sharing of 1 or more pairs of electrons between 2 atoms.

Hydrogen Bonding

A strong type of dipole-dipole attraction between a hydrogen atom, bonded to a highly electronegative atom, and another electronegative atom.

Intermolecular Forces

Forces of attraction or repulsion which act between neighboring particles (atoms, molecules, or ions).

Polarity

A property of molecules that exhibit a separation of electric charge and results in the molecule having a negative end and a positive end.

Melting Point

The temperature at which a solid becomes a liquid, indicating the energy required to break the intermolecular forces.

Electrical Conductivity

The ability of a substance to conduct electric current, often dependent on the presence of charged particles.

Polar Covalent Bond

A type of covalent bond where electrons are shared unequally, resulting in a slight electrical dipole moment.

London Forces

Weak intermolecular forces arising from temporary changes in electron density in atoms or molecules, resulting in temporary dipoles.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons within a covalent bond.

Metallic Bonding

The electrostatic attraction between positive metal ions (cations) and a sea of delocalised electrons.

Dative Covalent Bond

Also known as a coordinate bond, this is a covalent bond in which both electrons in the shared pair come from the same atom.

Giant Covalent Structure

A large network of atoms held together by many strong covalent bonds, resulting in very high melting and boiling points.

Cation and Anion

A cation is a positively charged ion (X^{+}) and an anion is a negatively charged ion (X^{-}).

Simple Molecular Structure

Compounds consisting of small molecules held together by weak intermolecular forces, which typically have low melting points.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons within a covalent bond.

Metallic Bonding

The electrostatic attraction between positive metal ions (cations) and a sea of delocalised electrons.

Dative Covalent Bond

Also known as a coordinate bond, this is a covalent bond in which both electrons in the shared pair come from the same atom.

Giant Covalent Structure

A large network of atoms held together by many strong covalent bonds, resulting in very high melting and boiling points.

Cation and Anion

A cation is a positively charged ion (X^{+}) and an anion is a negatively charged ion (X^{-}).

Simple Molecular Structure

Compounds consisting of small molecules held together by weak intermolecular forces, which typically have low melting points.

Permanent Dipole-Dipole Interaction

An attractive force between the permanent dipoles in neighboring polar molecules.

Bond Enthalpy

The energy required to break 1 mole of a specified type of bond in a gaseous molecule.

VSEPR Theory

Valence Shell Electron Pair Repulsion theory; a model used to predict the geometry of molecules based on the repulsion between electron pairs.

Lone Pair

A pair of valence electrons that are not shared with another atom and exert greater repulsion than bonding pairs.

Bonding Pair

A pair of electrons shared between 2 atoms to form a covalent bond.

Allotrope

Different structural forms of the same element in the same physical state, such as diamond and graphite for carbon.