IB Chemistry S2.2 Definitions
This page contains our IB Chemistry definitions for S2.2. By learning each one of these definitions, you will fully cover the content for IB Chemistry 'Covalent bonding & forces'.
adduct
Two molecules bound together by a dative bond
allotrope
A crystalline form of a compound
coordinate covalent bond
A covalent bond formed when a single atom donates a shared pair of electrons. Also called dative covalent bond
covalent bond
The electrostatic attraction of two nuclei to a shared pair of electrons
dipole-dipole forces
The attraction between oppositely charged dipoles of two polar molecules
electron domain
The number of bonding and non-bonding pairs of electrons
electronegativity
Relative measure of the attraction an atom has for a shared pair of electrons when covalently bonded to another atom
hydrogen bonding
A dipole-dipole force that occurs between compounds with a hydrogen atom, and a lone pair present on one of nitrogen, oxygen, or fluorine
instantaneous dipole
A dipole created by having a high concentration of electrons in a certain area at any point in time. Found in London dispersion forces
intermolecular forces
The forces between molecules
Lewis structure
A visual representation of covalent compounds, showing all valence electrons as dots, lines or Xs
non-polar bond
A bond formed when there is an electronegativity difference of <0.5, leading to no poles being formed
polar bond
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
resonance hybrids
A molecule that has more than one correct lewis structure
resultant polarity
The directional sum of polarity when a molecule has multiple polar bonds
valence shell
Outermost energy level of an atom
VSEPR theory
Valence shell electron pair repulsion theory. Allows us to determine the correct 3D shape of a covalent compound
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