Chapter 6 Flashcards
How is a molecule polar?
when two atoms have different electronegativities, this creates a polar bond
Dipole moments
the extent to which the molecules align in an electric field
Bond length
the internuclear separation distance where the molecule is most stable
Bond energy
the stability of a chemical bond, energy required to break the bond
How is a molecule non-polar?
The molecular symmetry cancel out the vectors.
How many ligands and lone pairs are in the following molecules? What about their steric number?
a) CH4
b) NH3
c) H20
ligands lone pairs
a) 4 0
b) 3 1
c) 2 2
steric number is all the same = 4
Draw the Lewis structure for HCN.
see cahier
Draw the Lewis structure for ketene, C2H2O
see cahier
Draw the Lewis structure for ClBr3, identify if its polar or non-polar, the approximate bond angles, and its molecular geometry.
see cahier
polar
90 degrees, 180 degrees
t-shaped
Draw the Lewis structure for ClF4-
see cahier
Draw the resonance structures for NO3-
see cahier
Arrange the following set of bonds according to length, from longest to shortest. N triple bonded to N , N=N,
N-N
N-N , N=N, N triple bonded to N
What are the bond angles for the following:
a) O-S-O angle of SO2
b) O-S-O angle of SO3
c) F-O-F angle of OF2
d) O-C-O angle of CO2
e) F-P-F angle of PF3
f) Cl-Si-Cl angle of SiCl4
a) 120
b) 120
c) 109.5
d) 180
e) 109.5
f) 109.5
Predict the approximate bond angles of the following molecules:
a) CH3
b) SiCl4
a) 120
b) 109.5
Which of these are polar?
a) SO2
b) CO2
c) CH2Cl2
d) PCl3
a) SO2
c) CH2Cl2
d) PCl3
Draw the Lewis structure for BF3, show all lone pairs, optimize formal charges, but do not show them.
see cahier
Draw the Lewis structure for ICl2+, show all lone pairs, optimize formal charges, but do not show them.
see cahier
Draw the Lewis structure for NO2-, show all lone pairs, optimize formal charges, but do not show them.
see cahier
Draw the Lewis structure for CH3CH2CO2-, show all lone pairs, optimize formal charges, but do not show them.
see cahier
Draw the Lewis structure for SbCl5, show all lone pairs, optimize formal charges, but do not show them.
see cahier
Consider the following: CO2, SO2, NO2- Which of the statements is correct? a) all three have a trigonal planar electron group geometry b) all three are polar c) NO2- is the only polar one d) SO2 and NO2- are the only polar ones e) CO2 and SO2 are polar while NO2- is non polar
d) SO2 and NO2- are the only polar ones
What is the arrangement of the bonds surrounding a carbon atom in an alkene?
a) linear
b) tetrahedral
c) trigonal planar
d) trigonal bipyramidal
e) octahedral
b) tetrahedral
Based on the VSPER Theory the ClF3 molecule is:
a) T-shaped
b) seesaw shaped
c) trigonal bipyramidal
d) linear
e) has 3 lone pairs
a) T-shaped
* always assume molecular shape if not specified*
According to the Lewis Theory, what are the formal charges on the atoms of HOOH?
HOOH
0 0 0 0
Despite many attempts the perbromate ion (BrO4-) was not prepared in the laboratory until about 1970. What is the formal charge on the bromine atom in this ion?
0
What is the molecular shape of IF5?
a) square pyramidal
b) tetrahedral
c) seesaw
d) trigonal bipyramidal
e) octahedral
a) square pyramidal
What are the ideal bond angles in SF4?
a) 109.5
b) <120
c) <90 and<120
d) >120 and >90
e) 120 and 90
c) <90 and <120
Draw the best lewis structure for IBrCl-
see binder
Draw the best lewis structure for GaI3
see binder
