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Chemistry Set 3

bonding

TermDefinition
boiling point The temperature at which a substance changes from a liquid to a gas, usually under standard atmospheric pressure.
covalent bond A chemical bond formed by the sharing of electron pairs between atoms.
ionic bond A chemical bond formed by the transfer of electrons from one atom to another, resulting in the formation of ions with opposite charges that attract each other.
melting point The temperature at which a substance changes from a solid to a liquid under standard atmospheric pressure.
molecule A group of atoms bonded together, representing the smallest fundamental unit of a chemical compound.
single, double, triple bond(s) Different levels of bonding in covalent compounds where one, two, or three pairs of electrons are shared between atoms, respectively.
Coulomb’s law A law describing the electrostatic interaction between charged particles. It states that the force between two charged objects is directly proportional to the product of their charges and inversely proportional to the square of the distance between their centers.
dipole A molecule or a part of a molecule that possesses both positively and negatively charged regions due to an uneven distribution of electrons.
dipole-dipole A type of intermolecular force where the positive end of one polar molecule interacts with the negative end of another polar molecule.
dissolve The process in which a solute mixes uniformly with a solvent to form a solution.
electrical conductivity The ability of a material to conduct an electric current, often related to the presence of ions or free electrons.
electrostatic force The force of attraction or repulsion between charged particles due to their electric charges.
hydrogen bond A special type of dipole-dipole interaction where a hydrogen atom is bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine), creating a strong attraction between molecules.
intermolecular force Forces of attraction or repulsion between molecules.
intramolecular force Forces that hold atoms together within a molecule, such as covalent bonds.
lattice energy The energy required to completely separate one mole of a solid ionic compound into its ions in the gas phase.
London dispersion forces Weaker intermolecular forces that arise from temporary fluctuations in electron distribution, leading to temporary dipoles.
metallic bonding A type of bonding where electrons are shared among a lattice of metal atoms, leading to properties such as electrical conductivity and malleability.
permanent polarity The property of a molecule having a permanent dipole moment due to differences in electronegativity between atoms.
polarity A measure of the separation of charge in a molecule, leading to a dipole moment.
surface area The total area of the exposed surface of an object.
surface tension The tendency of a liquid surface to minimize its area, resulting in a force that acts to reduce the surface area.
momentary dipole A temporary uneven distribution of electrons in a molecule, leading to a temporary dipole moment.
van der Waals forces Intermolecular forces including London dispersion forces and dipole-dipole interactions.
vapor pressure The pressure exerted by a vapor when it is in equilibrium with its liquid phase.
electrostatic attraction The force of attraction between charged particles due to their electric charges.
immiscible Incapable of being mixed or blended together.
induced dipole A temporary dipole moment induced in a molecule by the presence of a nearby charge or dipole.
insoluble Incapable of being dissolved in a particular solvent.
metallic bond The bonding in metals where electrons are delocalized and move freely throughout the metal lattice.
miscible Capable of being mixed or blended together.
nonpolar A molecule or bond that has an even distribution of electrons, resulting in no permanent dipole moment.
polar A molecule or bond that has an uneven distribution of electrons, resulting in a permanent dipole moment.
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