IB Chemistry Topic 2 & 12 Definitions

Two molecules bound together by a dative bond

A crystalline form of a compound

Metallic compounds (two metals mixed) that alter the properties of the components due to distortions in the lattice

A reaction that bonds monomers together to form a macromolecule

Non-metals that gain valence electrons to gain a negative charge

A reaction that breaks a macromolecule down into monomers

Positive ions. Commonly metals that lose valence electrons to gain a positive charge.

Ability of a material to conduct electricity 

A covalent bond formed when a single atom donates a shared pair of electrons. Also called dative covalent bond 

The electrostatic attraction of two nuclei to a shared pair of electrons

Temporary magnetism provoked by an external magnetic field aligning paired electrons in a transition metal complex

The attraction between oppositely charged dipoles of two polar molecules

A metal's ability to be drawn into a wire

The ability of a molecule to share electrons between multiple atoms due to aligned p-orbitals

The number of bonding and non-bonding pairs of electrons

Relative measure of the attraction an atom has for a shared pair of electrons when covalently bonded to another atom

Permanent magnetism due to parallel aligned unpaired electrons, exhibited in Fe, Ni, and Co

The mixing of bonding orbitals depending on the number of electron domains

A dipole-dipole force that occurs between compounds with a hydrogen atom, and a lone pair present on one of nitrogen, oxygen, or fluorine

A reaction that uses water to split a disaccharide into two monosaccharides

A dipole created by having a high concentration of electrons in a certain area at any point in time. Found in London dispersion forces 

The forces between molecules

The electrostatic attraction between oppositely charged ions

Atoms that have the same electron configuration 

A visual representation of covalent compounds, showing all valence electrons as dots, lines or Xs

A metal's ability to bend

The sum of all chemical reactions taking place within an organism

The electrostatic attraction between a lattice of positive ions and delocalized electrons

A small molecule

A bond formed when there is an electronegativity difference of <0.5, leading to no poles being formed

Temporary magnetism provoked by an external magnetic field aligning unpaired electrons in a transition metal complex

A bond formed when there is an electronegativity difference of 0.5-1.8, leading to one atom pulling electrons more towards itself to create a negative pole on its side and a positive pole on the other atom

Polymers formed when a diamine reacts with a dicarboxylic acid, releasing a water molecule for every amide link formed

Ions formed from more than one element, often when an acid loses one of more hydrogen ions

Polymers formed when a dialcohol reacts with a dicarboxylic acid, releasing a water molecule for every ester link formed

Atom with a lone electron, making it highly reactive

Atoms with a lone electron, making them highly reactive

A molecule that has more than one correct lewis structure

The directional sum of polarity when a molecule has multiple polar bonds

Outermost energy level of an atom 

Valence shell electron pair repulsion theory. Allows us to determine the correct 3D shape of a covalent compound

The sideways overlap of two p-orbitals resulting in an electron density lying above and below the internuclear axis

The direct head-on overlap of two orbitals resulting in an electron density lying along the internuclear axis that forms a single bond