Draw the Lewis Dot Structure for the following compounds and
then determine
a) the hybridization of the central atom
b) the electron group arrangement
c) the bond angle around the central atom
d) the molecular geometry.
a)
H3O+
b)
NO3-
c) O3
`
d)
HCN
e) CH3CH3
Draw Lewis structures for each of the following compounds. In
each case, specify the number of valence electrons surrounding the
central atom.
a) bromine dioxide (BrO2) (Assume the central atom
does not contain an expanded octet.)
There are ___ valence electrons surrounding the central
atom.
b) beryllium fluoride (BeF2)
There are___ valence electrons surrounding the central atom.
c) phosphorus pentabromide (PBr5)
There are ___ valence electrons surrounding the central
atom.
draw the best lewis structure for SF42- and calculate the formal charge on sulfur Draw the best Lewis structure for CH6N+ and calculate the formal charge on nitrogen.
Draw the condensed and Lewis structures for each of the
following compounds (include lone pairs where appropriate in the
Lewis structure). You should use a search engine to find the
structures for each of the names.
Name
Condensed Structure
Lewis Structure
Propan-1-ol
Ethanoic acid.
Butane
Diethyl ether
Ethylamine
a.) Draw Lewis dot structures for each molecule, b.) Identify
the geometric shape of each molecule, c.) Predict whether the bonds
in the molecule are polar or non polar and d.) predict whether the
molecule would be considered polar molecules: a. BeF2 b. SI6 c.
CCl4 d. BH2- e.SF5- f. NI3 g. BCl3 h. ClF3 i. ClO4- j. NO2
Draw a Lewis structure for each of the following compounds:(a) C_22H_66 \hspace{.2cm} (b) C_22H_44 \hspace{.2cm} (c) C_22H_22 \hspace{.2cm} (d) C_33H_88 \hspace{.2cm} (e) C_33H_66 \hspace{.2cm} (f) CH_33OH
Draw a Lewis structure for each of the following compounds:(a) C_22H_66 \hspace{.2cm} (b) C_22H_44 \hspace{.2cm} (c) C_22H_22 \hspace{.2cm} (d) C_33H_88 \hspace{.2cm} (e) C_33H_66 \hspace{.2cm} (f) CH_33OH