Ch 9 - Bonding Flashcards
ionic bonding
attraction of oppositely charged ions that arise through electron transfer
usually between metal and nonmetal
forms 3d array
lattice energy definition and trend
ΔH (positive) that accompanies seperation of 1 mol of a solid ionic compound into gaseous ions
measures strength of ionic interactions
increases up and left
affect of atomic size and charge on lattice energy
smaller ions attract each other more strongly, larger lattice energy
ions with higher charges attract each other more strongly, larger lattice energy
bond energy
breakage of a bond in 1 mol of gaseous molecules (+)
covalent bonding
bond through sharing of electrons that arises from balance between nuclei attracting the electrons and electrons repelling each other
results in greater electron density between nuclei
IE and EA of nonmetals
high IE and EA
potential energy diagram
no interaction, balance (well), too close (repulsion)
depth of well is bond energy
covalent bond strength and length
higher bond order, shorter bond length, higher bond energy
larger atom, longer bond, lower energy
ΔHrxn with bond strengths
ΔHrxn = ΣBE of reactant bond broken - Σ BE of product bond formed
metallic bonding
metals
electron sea model: cations and sea of electrons
high BP, conductive, malleable
EN trends
increases up and right
ionic EN
ΔEN > 1.7
larger ΔEN = increase % ionic character
polar covalent EN
o.4 < ΔEN < 1.7
pure covalent EN
ΔEN < 0.4
bond breaking
endothermic
