Bonding & Moles & Energy Flashcards
ion
positively or negatively charged atom
ionic bond
strong connection between two oppositely charged ions; formed by the transfer of electron(s) from one to another
cation
positive ion (metal)
anion
negative ion (non-metal)
ionic compound physical properties
high melting & boiling points due to strong electrostatic forces of attraction between oppositely charged ions
not conductive in solid state due to fixed ions (not free to move) in the lattice
conductive in molten or aqueous state due to free-moving ions
brittle as like charges repel each other
soluble in polar liquids
metallic bond
attraction between a lattice of positive ions and a sea of delocalized electrons
metal physical properties
high melting & boiling points due to strong attractions between positive metal ions and delocalized electrons
conductive due to delocalized free-moving electrons which carry the charge
malleable & ductile due to layers of positive metal ions sliding over each other
shiny & lustrous
high density due to tightly packed atoms
covalent bond
sharing of electron pair(s) between two atoms
dative bond
covalent bond where one atom donates both electrons (lone pair / non-bonding electrons) to the bond
represented by an arrow instead of a line
covalent molecular structure physical properties
low melting & boiling points due to weak intermolecular bonds
soft & brittle
not conductive due to no charge
insoluble in polar liquids (water)
soluble in non-polar liquids (hexane)
network covalent structure physical properties
high melting points due to many strong covalent bonds
not conductive due to no free electrons
insoluble in water
hard
valence shell electron pair repulsion theory
shapes & bond angles
electron pairs repel each other as far away as possible
linear : 180°
bent : 104.5°
pyramidal : 107°
trigonal planar : 120°
tetrahedral : 109°
intermolecular force
force of attraction between separate molecules
dispersion force (instantaneous / temporary dipole attraction)
dipole-dipole attraction (permanent dipole attraction)
hydrogen bonding
dispersion force (instantaneous / temporary dipole attraction)
force of attraction between molecules due to temporary dipoles created by random movement of electrons
dipole-dipole attraction (permanent dipole attraction)
force of attraction between polar molecules due to positive and negative ends of polar molecules
