Ionic Bonding Flashcards
Ionic bonds
bonding due to electrostatic attraction between cations and anions
covalent bonds
bonding due to electrostatic attraction between atomic nuclei and a shared pair of electrons
Metallic bonds
bonding due to electrostatic attraction between metallic cations and a sea of delocalized electrons
molecular covalent
compounds contain atoms held together by covalent bonds.
covalent network
formed by networks or chains of atoms or molecules held together by covalent bonds. (ex: diamond)
electrostatic attraction
when two particle types have opposite charge and there is mutual attraction.
Melting point
temperature at which the solid and liquid forms of a substance can exist in equilibrium. (ionic compounds have ones)
boiling point
temperature at which the gas and liquid forms of a substance can exist in equilibrium (ionic compounds have high ones)
volatility
a material quality which describes how readily a substance vaporizes. (ionic compounds are not this)
Electrical conductivity
ability to carry and electrical charge. Ionic compounds can do this when they are molten or dissolved in solution.
Thermal conductivity
ability to transfer heat. Ionic compounds do not do this.
Brittle
hard but liable to break or shatter easily. Ionic compounds are this.
corrosion
a process by which metals deteriorate through oxidation. Some ionic compounds can do this.
Electronegativity
a chemical property that describes the tendency of an atom or a functional group to attract electrons toward itself
Cation
positively charged species due to a loss of electrons.
oxidation
the loss of electrons
reduction
the gain of electrons
anion
negatively charged species due to a gain of electrons.
redox reaction
the coupling of a loss of electrons from one chemical to the gain of electrons by another.
OIL RIG
oxidation is loss and reduction is gain (of electrons)
hydride
H3O+, the ion formed when hydrogen ions are in aqueous solution
octet rule
the tendency of atoms to prefer to have eight electrons in the valence shell.
transition elements
elements with an incomplete d orbitals
Exothermic
a process that releases energy
Endothermic
a process that absorbs energy
Polyatomic ions
an ion composed of more than one atom.
Nitrate
NO3 -1
ammonium
NH4 +
hydroxide
OH -
hydrogencarbonate
HCO3 -
carbonate
CO3 2-
Sulfate
SO4 2-
Phosphate
PO4 3-
Pauling scale
the most commonly used scale to measure relative electronegativity
Ionic crystals
solids consisting of ions bound together by their electrostatic attraction into a regular lattice.
lattice structure
the symmetrical three-dimensional structural arrangements of atoms, ions or molecules
non-directional bonding
due to ionic charges being uniform in all directions, An ion is surrounded by other ion from all the directions.
lattice enthalpy
a measure of the strength of the forces between the ions in an ionic solid.
solubility
a measure of the strength of the forces between the ions in an ionic solid. If the attraction between the solvent and the solute is higher than the lattice enthalpy of the compound then it will dissolve.
Polar solvent
can dissolve polar and ionic compounds
Non polar solvent
can dissolve non-polar compounds
How ionic radius affects lattice enthalpy
the higher the ionic radius the lower the lattice enthalpy
how ionic charge affects lattice enthalpy
the higher the ionic charge the higher the lattice enthalpy
