Compare the following molecules (CH4, NF3, SH2) and rank in
terms of decreasing bond angles (largest to smallest angle).
Justify your response by showing the Lewis structure, electron and
molecular geometry.
For each of the following molecules, predict the molecular
shape, give bond angles, hybridization and determine whether the
molecule will be polar or non-polar.
a. CF4
b. BeH2
c. SeF6
d. XeOF2
Predict all bond angles and the shape of the molecules and
ions. (draw Lewis structure first)
BF4-
HCO3-
CH3CHO
CH3COOH. 2.Indicate the polarity of the following
molecules. Draw Lewis structure and point out the polarity of each
chemical bond and then point our the polarity of the molecule.
CH2Cl2
HCN
H2O2
CH3CN
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
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
1. Predict which of the following molecules will have a stronger
ionic bond. (Think about charges and
bond lengths!)
a) MgBr2 or MgF2
b) Na2O or Rb2O
c) Ca3(PO4)2 or Li3PO4
2. Determine the number of valence electrons in each molecule
below.
a) C4H10O
b) CH3NO2
c) POCl2-1
d) HBrO3
3. Draw full Lewis structures for the following molecules. Indicate
formal charges and resonance
structures, as appropriate.
a) IO3-
b) SF4
c) SOCl2
d) dinitrogen monoxide (laughing gas), N –...
Of the following molecules, which is the strongest Lewis
Acid?
NH3, NF3, NCl, BH3, BF3, BCl3
Please include an explanation with the answer. I am having a
really hard time figuring this out.