Sg pr w au is the electron configuration for zn 2 and

Sg
Pr
W
Au
Is the electron configuration for Zn 2+ and Ni the same? Explain.
A transition metal ion has one electron removed from the 5s orbital. Giving it a completely empty
5s shell and a completely filled 4d orbital. What is the ion?
Based on what you know about electron configurations explain why Sb would form +3 and 5+
ions? Write out their electron configurations.

For the quantum number n=3. What is the possible l values? What orbitals do they correspond
with? How many total electrons can you have with the quantum number l =1?
Lewis Structures and VSEPR Model
Lewis Structures
• The electrons involved in bonding are the valence shell electrons
• Number of electrons in the valence shell is determine by row # excluding the transition metals
• Count the number of electron each atom brings in…..That is the total number of electrons you are
allowed to have in the molecule.
• Put the least electronegative element in the middle of the structure
• Nature likes symmetry
• Terminal atoms (atoms at the end of the Lewis structure) always satisfy the octet rule
•
Fluorine and Hydrogen (Hydrogen can only have 2 electrons) always only make one bond
•
N, O, and F always obey the octet rule
• Atom in the second row of the periodic table cannot have more than 8 electrons surrounding it
because no d prbitals are close enough in energy to use
Formal charge
1. Sum of all the formal charges is equal to the overall charge on the molecule
2. Minimize the number of atoms with a formal charge
3. Minimize the magnitude of the formal charge (we don’t like #’s >1)
4.
A more electronegative element is more likely to have a negative formal charge (there are
exceptions)
Problems
Draw the Lewis structures of the following compounds
SF
4
NO
2
NO
3
- IO
3
- PO
4
3-

Draw 3 possible Lewis structures for COS. Assign Formal charges. Which structure is the best
and why?
VSEPR Model
Basic
Geometry
0 lone pair
(shape)
1 lone pair
(shape)
2 lone pair
(shape)
3 lone pairs
(shape)
Hybridizatio
n
Trigonal
Planar
Trigonal Planar
bent
linear
Sp2
Tetrahedral
Tetrahedral
trigonal planar
bent
linear
Sp3
Trigonal
Bipyramid
Trigonal
Bipyramid
see-saw
T-
shape
linea
r
Sp3d
Octahedral
Octahedral square
pyramid
square planar
Sp3d2
Problem

Draw the VSEPR models of the following molecules. What are their geometries, shapes,
approximate bond angles, hybridization, and state whether they are polar or nonpolar?
a. SbF
4
-
b. BiBr
3
c. IOF
4
-
d. GeCl
4
e. SO
3
MO Theory
To the left of Nitrogen To the right of Nitrogen

Notes:
-The column containing nitrogen can use either MO structure
- for heteronuclear diatomic (two different atoms) use the side that the atoms lay on, if they lay
on opposite side of nitrogen use the structure for the right of nitrogen
-paramagnetic: magnetic, unpaired electrons
- diamagnetic: all the electrons are paired
-bonding orbitals: overlap of the electron density of the orbitals
-antibonding orbitals: no overlap, signified by a star (*)
- bond order = ½ (bonding electrons – antibonding electrons)