The electronic configurations of CO and O 2 , on the basis of the molecular orbital model are to be stated. Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the H 2 + molecular ion. The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as, Bond order = [ ( Electrons in bonding orbitals ) − ( Electrons in anti-bonding orbitals ) ] 2 As the bond order increases, the stability also increases. The bond order is directly proportional to the bond energy and inversely proportional to the bond length. To determine: The electronic configuration of O 2 on the basis of the molecular orbital model. The electronic configuration of CO on the basis of the molecular orbital model. Two points of difference between CO and O 2 .
The electronic configurations of CO and O 2 , on the basis of the molecular orbital model are to be stated. Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the H 2 + molecular ion. The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as, Bond order = [ ( Electrons in bonding orbitals ) − ( Electrons in anti-bonding orbitals ) ] 2 As the bond order increases, the stability also increases. The bond order is directly proportional to the bond energy and inversely proportional to the bond length. To determine: The electronic configuration of O 2 on the basis of the molecular orbital model. The electronic configuration of CO on the basis of the molecular orbital model. Two points of difference between CO and O 2 .
Solution Summary: The author explains how the electronic configurations of CO and
Interpretation: The electronic configurations of
CO and
O2, on the basis of the molecular orbital model are to be stated.
Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the
H2+ molecular ion.
The bond order is calculated by difference between the anti-bonding electrons and the bonding electrons by two. This can be stated as,
As the bond order increases, the stability also increases. The bond order is directly proportional to the bond energy and inversely proportional to the bond length.
To determine: The electronic configuration of
O2 on the basis of the molecular orbital model.
The electronic configuration of
CO on the basis of the molecular orbital model. Two points of difference between
CO and
O2.
Experiment 1
Data Table 1: Conservation of Mass - Initial Mass
Data Table 1
Data Table 2
Data Table 3
Data Table 4
Panel 1
Photo 1
Data Table 5
Reaction Mass of test tube and 5.0% HC₂H₂O2 (g)
#
(A)
(B)
Mass of NaHCO, (g) Mass of balloon and NaHCO, (g)
(C)
0.10
1
0829
14.38g
0.20
2
0.929
14.29g
0.35
1.00g
3
14.25g
0.50
1.14g
14.29
Experiment 1
Data Table 2: Moles of HC2H3O2
Reaction Volume of Mass of
Moles of HC₂H₂O₂
5.0%
Vinegar
(g)
(ML)
5.0
0.25
0042 mol
2
5.0
0.25
0042 mol
3
5.0
0.25
0042 mol
5.0
0.25
0042 mol
Experiment 1
Data Table 3: Moles of NaHCO3
Reaction Mass of NaHCO (g)
10g
20g
35g
50g
Experiment 1
Data Table 4: Theoretical Yield of CO₂
Reaction #
1
2
3
Experiment 1
Total mass before reaction (g)
(D=A+C)
15.29
15.21g
15.25g
15.349
Exercise 1
Data Table 1
Data Table 2
Data Table 3
Data Table 4
Panel 1
Photo 1
Data Table 5
Exercise 1-
Data Table 1
Data Table 2
DataTable 3
Data Table 4
Panel 1
Photo 1
Data Table 5
Exercise 1-
Moles of NaHCO
0012 mol
0025 mol
0044 mol
0062 mol…
The chemical reaction you investigated is a two-step reaction. What type of reaction occurs in each step? How did you determine your answer?
Chapter 4 Solutions
Bundle: Chemistry: An Atoms First Approach, Loose-leaf Version, 2nd + OWLv2 with Student Solutions Manual, 4 terms (24 months) Printed Access Card
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Quantum Molecular Orbital Theory (PChem Lecture: LCAO and gerade ungerade orbitals); Author: Prof Melko;https://www.youtube.com/watch?v=l59CGEstSGU;License: Standard YouTube License, CC-BY