Identify the electron pair geometry and the molecular structure
of each of the following molecules or ion. For the molecules (not
the ions), determine if the molecule is polar or nonpolar. IF6+,
CF4, BF3, SiF5-, BeCl2, H3O+, PCl4-, BrCl4-, ICl3, XeF4, SF2
Determine the electron geometry, molecular geometry, and
idealized bond angles for each of the following molecules. In which
cases do you expect deviations from the idealized bond angle?
CF4
NF3
OF2
H2S
Repulsion of electrons within two interacting molecules produces
changes in electron distribution. This change in electron
distribution creates temporary dipole moments. Which of the
following does this explain?
Choose one or more:
A. This explains why the dipole-dipole attractive force between
dimethyl ether and acetone does not entirely account for the
attractive force between these molecules. B. This explains why
ammonia and nitrogen gas exhibit an attractive force between them.
C. This explains how the molecules hydrogen fluoride and methanol...
indicate the electron pair geometry and the molecular geometry
for each of the six compounds listed below by completing the
following table ( bent , trigonal planar, linear, tetrahedral,
trigonal pyramidal)
compound electron pair geometry molecular
geometry
O3
OF2
CO2
PF3
SO3
HCL4
In the following molecules, predict the geometry, hybridization,
and bond angle for the central atom. Give your answer using
drawings.
a)
H3O
b)
BeCl2
c) BCl3