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For the following molecules, determine
a) the electronic geometry
b) the molecular geometry
c) whether it is polar or non-polar molecule
d) the formal charges on all the atoms
e) the hybridization of the central atom
(1) H2O (2)BrO3- bromate ion (3) SCl4 sulfur tetrachloride (4) PBr5 (5) XeF2 (6) NH4+
For the following molecules, determine
a) the electronic geometry
b) the molecular geometry
c) whether it is polar or non-polar molecule
d) the formal charges on all the atoms
e) the hybridization of the central atom
(1) H2O (2)BrO3- bromate ion (3) SCl4 sulfur tetrachloride (4) PBr5 (5) XeF2 (6) NH4+
Tod ThielLv2
19 Apr 2019
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Related questions
a. Draw Lewis structure for these molecules:
|
PCl3 |
ICl3 |
NO2 |
IF5 |
XeF2 |
IBr4- |
SF6 |
|
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|
|
|
|
|
|
b. Draw a 3-D Sketch
c. Do they have Resonance Structures?
d. Write they valence electrons
e. Does molecules have Bond Angles?
f. Write Bonding and non-bonding groups
g. Are they Polar or Non-Polar Molecules?
h. What is the Hybridization of Central Atom?
i. Write the Formal Charges
k. Electron Geometry
m. Molecular geometry
