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WorksheetsMolecular Orbital Homework
Total questions: 20
Worksheet time: 42mins
The hybridization of the nitrogen atom in the cation NH2+ is:
sp2
sp3
dsp
sp
none of these
Atoms that are sp2 hybridized form ____ pi bond(s).
0
1
2
3
4
The hybridization of the central atom in XeF5+ is:
sp
sp2
sp3
dsp3
d2sp3
The hybridization of the central atom in ClF2+ is:
sp
sp2
sp3
dsp3
d2sp3
The hybridization of the central atom in O3 is:
sp
sp2
sp3
dsp3
d2sp3
The hybridization of Cl in ClF2+ is
sp
sp2
sp3
dsp3
d2sp3
A π (pi) bond is the result of the
overlap of two s orbitals
overlap of an s orbital and a p orbital
overlap of two p orbitals along their axes
sidewise overlap of two parallel p orbitals
sidewise overlap of two s orbitals
Which of the following statements is true?
Electrons are never found in an antibonding MO.
All antibonding MOs are higher in energy than the atomic orbitals of which they are composed.
Antibonding MOs have electron density mainly outside the space between the two nuclei.
None of the statements is true
Which of the following molecules contains the shortest C–C bond?
C2H2
C2H4
C2H6
C2Cl4
C2H4 and C2Cl4
The electron configuration of a particular diatomic species is (σ2s)2(σ*2s)2(σ2p)2(π2p)2(π*2p)4. What is the bond order for this species?
1.5
1
0.5
0
2
What is the bond order of He2+?
2
0
1/2
1
1 1/2
Which statement is false? A sigma molecular orbital
may result from overlap of p atomic orbitals perpendicular to the molecular axis (side-on).
may result from overlap of p atomic orbitals along the molecular axis (head-on).
may result from overlap of two s atomic orbitals.
may result from overlap of one s and one p atomic orbitals.
may be either bonding or antibonding.
If four orbitals on one atom overlap four orbitals on a second atom, how many molecular orbitals will form?
1
4
8
16
None of the answers are correct
When comparing Be2 and H2:
I.Be2 is more stable because it contains both bonding and antibonding valence electrons.
II.H2 has a higher bond order than Be2.
III.H2 is more stable because it only contains σ1s electrons.
IV.H2 is more stable because it is diamagnetic, whereas Be2 is paramagnetic.
I, II
III only
II, III
II, IV
III, IV
If a molecule demonstrates paramagnetism, then :
I.The substance can have both paired and unpaired electrons.
II.The bond order is not a whole number.
III.It can be determined by drawing a Lewis structure. IV.It must be an ion.
I, II
II,III
I, II, IV
I only
III only
For which of the following diatomic molecules would the bond order become greater if an electron is removed (i.e., if the molecule is converted to the positive ion in its ground state)?
B2
C2
P2
F2
Na2
How many of the following: F2, B2, O2, N2 , are paramagnetic?
0
1
2
3
4
Carbon monoxide has ten bonding electrons and four antibonding electrons. Therefore it has a bond order of
3
7
1/2
2
1.5
Which one of the following statements is false?
Valence bond theory and molecular orbital theory can be described as two different views of the same thing.
When one considers the molecular orbitals resulting from the overlap of any two specific atomic orbitals, the bonding orbitals are always lower in energy than the antibonding orbitals.
Molecular orbitals are generally described as being more delocalized than hybridized atomic orbitals.
One of the shortcomings of valence bond theory is its inability to account for the paramagnetism of the oxygen molecule, O2.
One of the shortcomings of molecular orbital theory is its inability to account for a triple bond in the nitrogen molecule, N2.
Which statement regarding stable heteronuclear diatomic molecules is false?
All have bond orders greater than zero.
The antibonding molecular orbitals have more of the character of the more electropositive element than of the more electronegative element.
Their molecular orbital diagrams are more symmetrical than those of homonuclear diatomic molecules.
The bonding molecular orbitals have more of the character of the more electronegative element than of the less electronegative element.
The greater is the difference in energy between two overlapping atomic orbitals, the more polar the resulting bond is, due to electrons occupying the resulting bonding molecular orbital.
