Bonding and Chemical Interactions Flashcards
one or more electrons from an atom with a low ionization energy (typically a metal) are transferred to an atom with a high electron affinity (typically a nonmetal), resulting electrostatic attraction between opposite charges holds ions together
ionic bonding
an electron pair is shared between two atoms (typically nonmetals) with relatively similar values of electronegativity; degree to which electron pair is shared determines degree of polarity
covalent bonding
electron pair is shared equally
nonpolar covalent bonding
electron pair is shared unequally
polar covalent bonding
if both of the shared electrons are contributed by only one of the two atoms
coordinate covalent bonding
form between atoms that have significantly different electronegativities, electrons are not shared, very high boiling and melting points
ionic bonds
formed by atom that loses electrons
cation
formed by atom that gains electrons
anion
structure formed by ionic constituents in a solid state, consists of repeating positive and negative ions
crystalline lattice
form between atoms with similar electronegativities, share electrons, lower boiling and melting points
covalent bonds
bond with nearly identical electronegativities, equal distribution of electrons, no separation of charges
nonpolar covalent bond
bond with atoms that differ moderately in electronegativities, share electrons unevenly, have separation of charges
polar covalent bond
a vector quantity of polar bond or molecule
dipole moment (p)
dipole moment (p)
p = qd
where:
q = magnitude of charge
d = displacement vector separating partial charges
bond where both of shared electrons originated on same atom, such as when lone pair of one atom attacks another atom with an unhybridized p-orbital to form a bond, typically found in Lewis acid-base reactions
coordinate covalent bond
resonance structure stability is greater when:
1) less or smaller formal charges are present
2) there is less separation between opposite formal charges
3) negative formal charges are placed on more electronegative atoms
spatial arrangement of all pairs of electrons around central atom, including bonding and lone pairs of electrons
electronic geometry
spatial arrangement of only bonding pairs of electrons
molecular geometry
weak electrostatic interactions between atoms and compounds, can impact boiling and melting points
intermolecular forces
attractive or repulsive forces of short lived and rapidly shifting dipoles, a type of van der Waals force, weakest type of intermolecular forces
London dispersion forces
attractive electrostatic force between positive region of one molecule close to the negative region of another, denoted by dashed lines between molecules, present in solid and liquid phases, polar species tend to have higher boiling and melting points, middle strength of intermolecular forces
dipole-dipole interactions
unusually strong dipole-dipole interaction formed when hydrogen molecules bond to very electronegative N, O, or F; H atom carries very small amount of electron density in covalent bonds allowing it to essentially act as a naked proton interacting with partial negative charges of nearby molecules; very high boiling point, strongest type of intermolecular forces
hydrogen bonds
