Molecule A has hydrogen bonds; Molecule B is non -
polar. Which of the molecular liquids will have the higher boiling
point? Why? Also, which of the molecular liquids will have the
lower vapor pressure? Why?
valence electrons, lewis structure, electron geometry, molecular
geometry, bond angles, polar or non polar
IF4^+
ICl4^-
part b
lewis structure electron geometry, sketch of molecule, polar or
non polar
SCl3F3
CBr2F2
IO3^-
PO3^3-
BH3
TeF5^-
XeF2O2
What determines the electron-group geometry of a molecule? What
determines the molecular geometry of a molecule? Why can-electron
group geometry differ from molecular geometry? sidenote:please
answer every part of the question
a) number of valence electrons, lewis structure, electron
geometry, molecular geometry, bond angles, polar or non polar :
ICl4^-
B) lewis structure, electron geometry, molecular geometry, polar
or non polar, sketch or molecule: IO3^1, SCN^-, BH3
For each molecule, determine a.) the electron domain geometry,
b.) the molecular geometry and c.) whether the molecule is polar or
non-polar:
PH3
ICl5
H2CO
SO3
TeCl4
What is the molecular geometry around an atom in a molecule or
ion which is surrounded by one lone pair of electrons and four
single bonds.
Select one:
a. linear
b. T-shaped
c. See-saw
d. trigonal bipyramidal
e. trigonal planar
Which of the following concerning electron pair space
requirements and bond angles is/are incorrect?
1.
Lone pairs of electrons require more space than bonding
pairs.
2.
Multiple bonds require the same amount of space as single
bonds.
3.
The HOH...