Chem Chapter 7

Front 1

Standard quantum-mechanical orbitals of valence e'

Back 1

s,p,d,f and hybrids of those

Front 2

a chemical bond results from the overlap of

Back 2

two half-filled orbitals

Front 3

what determines the shape of the molecule

Back 3

the geometry of the overlapping orbitals

Front 4

why to atoms hybridize?

Back 4

to maximize bonding potential and stabilize the molecule. The more bonds=more full orbitals=more stability

Front 5

the number of standard atomic orbitals combined =

Back 5

the number or hybrid orbitals formed

Front 6

the number and type of standard atomic orbitals combined determines

Back 6

the shape of the hybrid orbitals

Front 7

the hybridization that occurs is the one that yields the ________ amount of energy for the molecule

Back 7

lowest

Front 8

which atom cannot hybridize and why

Back 8

Hydrogen because it only has one electon

Front 9

definition: mixing different types of orbitals in the valence shell to make a new set of degenrate orbitals

Back 9

hybridization

Front 10

what type of hybridization when an atom has four electron groups around it

Back 10

sp3

Front 11

what type of hybridization when at atom has three electron groups in it

Back 11

sp2

Front 12

definiton: results when the interacting atomic orbitals point along the axis connecting the two bonding nucleii

Back 12

sigma bond

Front 13

definition: results when the bonding atomic orbitals are parallel to each other and perpendicular to the axis connecting the two bonding nucleii

Back 13

pi bond

Front 14

which bonds are stronger, pi or sigma

Back 14

sigma

Front 15

single bonds consist of

Back 15

sigma bonds

Front 16

double bonds consist of

Back 16

1 sigma, 1 pi

Front 17

triple bonds consist of

Back 17

1 sigma, 2 pi

Front 18

sigma bonds overlap with

Back 18

hybrid orbital of one atom to a hybrid or non hybrid orbital of another atom

Front 19

pi bonds overlap between

Back 19

unhybridized p orbitals on bonded atoms

Front 20

which bond requires the breaking of the interaction between the orbitals to rotate

Back 20

pi bonds because its above and below

Front 21

which hybridization has two electon groups around it

Back 21

sp, and it is linear

Front 22

which hybridization has five electron groups around it

Back 22

sp3d

Front 23

which hybridization has six electron groups around it?

Back 23

sp3d2

Front 24

definition: occurs when the wave functions combine constructively and the resulting molecular orbital has less energy than the original atomic orbitals

Back 24

bonding molecular orbital

Front 25

definiton: occurs when the wave functions combine destructively and the resulting molecular orbital has more energy than the original atomic orbital

Back 25

antibonding molecular orbital

Front 26

bond order =

Back 26

1/2 difference between number of bonding and antibonding electrons. can be a fraction or a decimal

Front 27

the higher the bond order= the ___________ and _________ bonds

Back 27

stronger and shorter

Front 28

when molecular orbitals are occupied are ________ bands

Back 28

valence

Front 29

when molecular orbitals are unoccupied

Back 29

conduction bands