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jadeshark113Lv1
20 Mar 2020
Calculate the formal charge on the indicated atom in each of the following molecules or ions: (a) the central oxygen atom in O3, (b) phosphorus in PF6–, (c) nitrogen in NO2, (d) iodine in ICl3, (e) chlorine in HClO4 (hydrogen is bonded to O).
Calculate the formal charge on the indicated atom in each of the following molecules or ions: (a) the central oxygen atom in O3, (b) phosphorus in PF6–, (c) nitrogen in NO2, (d) iodine in ICl3, (e) chlorine in HClO4 (hydrogen is bonded to O).
Reid WolffLv2
25 May 2020
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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
