Show:
Geometries
Polarity and Ions
Hybrid Orbitals
Multiple Bonds
Molecular Orbitals
100
Name the five types of electron domain geometry
linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral (R.T)
100
Define polarity.
Uneven distribution of electrons in a molecule. (C.W.)
100
What does VSEPR stand for?
Valence Shell Electron Pair Repulsion model (MY.L)
100
In a sigma bond, electrons are centered around the what axis?
Internuclear (A.W.)
100
How does MO differ from VSEPR?
MO is theoretical, it has anti-bonding orbitals, and it involves the entire molecule instead of single atoms (A.W.)
200
What are the bond angles of a tetrahedral molecule?
109.5 (A.W.)
200
Is H2O polar? Give the bond angles, and explain your answer.
Yes. Angles are less than 109.5. The un-bonded electrons are free to move around more than the bonded electrons, so they push the bonded electrons and decrease the angles (MY.L)
200
If there is one s- atomic orbital and one p- atomic orbital, how many sp- hybrid orbitals are created?
2 (C.W.)
200
Sigma bonds usually occur (first/second). Pi bonds occur (first/second).
....first....second.... (R.T.)
200
Which takes a higher energy to fill? Bonding or anti-bonding orbitals?
Anti-bonding (C.W.)
300
What is the molecular geometry of a BF3 molecule?
Trigonal Planar (C.W.)
300
Can a molecule have two dipole moments and still be nonpolar? Explain.
Yes. The dipoles can be opposite in direction, and we can say that they cancel out. Take CO2 for example (R.T.)
300
What is the hybridization is present in linear molecules?
sp (A.W.)
300
(Sigma/Pi) bonds create rigidity in a molecule. Explain.
Pi. The pi bonds can only form if they are in the same axis. Since there are three dimensions that a pi bond can occur in, and bonds can only form if they are in the same axis, it restricts movement of the molecule's components. (MY.L)
300
Calculate the bond order of the following molecules. H2^-, H2.
H2^-: 1/2 H2: 1 (MY.L.)
400
What is the molecular geometry of an octahedral molecule with four bonding regions and one non-bonding region? Are there geometric isomers of this molecule? Explain why one is more probable than the others.
MG: Square Planar Yes, there are isomers, and one is more probable because of electron repulsion (UU>US>SS) (MY.L.)
400
Predict whether the following molecules are polar or non-polar. IF, CS2, SO3.
IF:polar CS2:non-polar SO3:non-polar (A.W.)
400
In a PF5 molecule, what is the hybridization of the central molecule?
sp3d (R.T.)
400
How many sigma and how many pi bonds are present in an N2 molecule?
One sigma, two pi (C.W.)
400
Define and give an example of each: diamagnetism and paramagnetism.
Diamagnetism: no unpaired electrons, weakly repelled in a magnetic field. ex: F2 Paramagnetism: unpaired electron, the more unpaired electrons means the stronger the attraction in a magnetic field. ex: O2 (R.T.)
500
Draw a Lewis structure for NH3. Give the EDG and MG for the molecule, and determine if it is polar or non-polar. What are the bond angles? What is the hybridization?
EDG:tetrahedral MG:trigonal pyramidal It is polar angles less than 109.5 Hybridization: sp3 (A.W.)
500
Draw the Lewis structure for the CO_3^2- molecule.
(Ask group 5 to draw it on the board). (C.W.)
500
Give the hybridization of the central atom in a IF4^- molecule.
sp3d2 (MY.L.)
500
What is delocalization? Explain using benzene as an example.
It is where pi bonds give a special stability, but due to resonance, the pi bonds are constantly changing. This results with a hexagon base with a circle in the middle, denoting delocalization. It means that the bonds are not restricted to one place. (R.T.)
500
Draw the MO diagram for Ne2. What is the bond order? What does it imply?
Ask group five to draw on board. 0 It does not exist in nature naturally. (C.W.)