Unit 12A - Bond Polarity - Intermolecular Forces

polar

anything with two opposite sides that are opposite with respect to something (ex. charge)

polar bond

an ionic or covalent bond that has opposite full or partial charges on each side (one side partially positive and one side partially negative), because of donation or unequal sharing of electrons

inter-

between

intra-

within

ionic bonds (metal + nonmetal, ΔEN >1.7)

e- donation, results in full charges forming on the e- donor and the e- recipient

coulombic force

the electrostatic charge attraction between ions, the force holding together ionic bonds (not true bonds)

polar covalent bonds (nonmetal + nonmetal, ΔEN = 0.35-1.7)

e- are shared unevenly between two atoms, results in partial charges forming on each atom involved

electron density maps

maps displaying uneven sharing of e- or partial charges by showing regions of high electron density (partial negative regions) in red and low electron density (partial positive regions) in blue

non polar covalent bonds (ΔEN=-0-0.35)

e- are shared evenly between the two atoms due to a really low difference in EN, resulting in no charges forming

metallic bonds

occurs between metal atoms in which valence electrons create a “sea of electrons” which are delocalized and not associated with any one atom/nucleus

conductors

delocalized electrons can “flow: in a certain direction through the matter, creating an electrical current

malleable

possible for the atoms to slide past each other when the metal is deformed instead of fracturing

bond character

what a bond ACTS like based on the difference in electronegativities between the two elements

large difference in electronegativity

points to electrons being associated with one element more than the other

ionic character of a bond formula

I = 1 - e ^(-Δx²/4)

bond type

how a chemical bond ACTUALLY behaves

affected by bond character (ΔEN) but also by nature of the materials themselves (EN values)

intramolecular forces

forces which hold a molecule together

strength of intramolecular forces

represented by bond dissociation energies