unit 8 Flashcards
three dimensional arrangement of atoms in space
molecular geometry
transfer of electrons from metal to a non metal
ionic bonding
share electrons between non metals and/or metalloids
covalent bonding
medium difference in electronegativites
ionic bonding- electrons not equally shared
small difference in electronegativity
non polar covalent bonding - electrons share equally
the repulsions between the valence shell electron pairs (both bonding and nonbonding electron pairs) is what controls the geometry
valence shell electron pair repulsion theory
3D arrangement of electron pairs
electronic geometry
2 pairs of electrons
linear- 180
3 pairs of electrons
trigonal planar- 120
4 pairs of electrons
tetrahedral- 109
5 pairs of electrons
trigonal pyramid- 120, 90, 180
6 pairs of electrons
octahedral- 90, 180
3D arrangement of atoms
molecular geometry
compounds with fewer than eight valence electrons around the central atom
incomplete octets
compounds with more than eight valence electrons around the central atom
expanded octets
compounds with an odd number of electrons around the central atom
free radicals
each orbital of a sub level must contain one electron before pairing can begin
hunds rule
when other atoms are present, an atom may combine its valent shell atomic orbitals to form a new set of orbitals
valence bond theory
combining orbitals
hybridization
new orbitals formed
hybrid orbitals
end to end orbital overlap
sigma bond
side to side orbital overlap
pie bond
angle between 2 covalent bonds
bond angles
length of a covalent bond; distance between the 2 nuclei of the atoms included in the covalent bond
bond lengths
