The reason for bond order of N 2 is greater than N 2 while that of O 2 is less than O 2 is to be explained. Concept Introduction: The combination of two atomic orbitals results in the formation of a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ molecular orbital, and orbitals parallel to each other combine to form π molecular orbitals. The molecular orbital formed by combination of 1s orbital forms bonding molecular orbital designated as σ 1 s , and antibonding molecular orbital as σ ∗ . The 2s orbital forms corresponding molecular orbitals. Bond order is determined by subtraction of the number of antibonding electrons from the number of bonding electrons and divide the obtained number by two.
The reason for bond order of N 2 is greater than N 2 while that of O 2 is less than O 2 is to be explained. Concept Introduction: The combination of two atomic orbitals results in the formation of a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ molecular orbital, and orbitals parallel to each other combine to form π molecular orbitals. The molecular orbital formed by combination of 1s orbital forms bonding molecular orbital designated as σ 1 s , and antibonding molecular orbital as σ ∗ . The 2s orbital forms corresponding molecular orbitals. Bond order is determined by subtraction of the number of antibonding electrons from the number of bonding electrons and divide the obtained number by two.
Solution Summary: The author explains that the bond order of N_Text2 is greater than the number of antibonding electrons in the nitrogen atom.
The reason for bond order of N2 is greater than N2 while that of O2 is less than O2 is to be explained.
Concept Introduction:
The combination of two atomic orbitals results in the formation of a bonding and an antibonding molecular orbital. Orbitals that lie on internuclear axis combine to form sigma σ molecular orbital, and orbitals parallel to each other combine to form π molecular orbitals.
The molecular orbital formed by combination of 1s orbital forms bonding molecular orbital designated as σ1s, and antibonding molecular orbital as σ∗. The 2s orbital forms corresponding molecular orbitals.
Bond order is determined by subtraction of the number of antibonding electrons from the number of bonding electrons and divide the obtained number by two.
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Question 59 of 70
The volume of
1
unit of plasma is 200.0 mL
If the recommended dosage
for adult patients is 10.0 mL per kg of body mass, how many units are needed for
a patient with a body mass of 80.0
kg ?
80.0
kg
10.0
DAL
1
units
X
X
4.00
units
1
1
Jeg
200.0
DAL
L
1 units
X
200.0 mL
= 4.00 units
ADD FACTOR
*( )
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ANSWER
RESET
D
200.0
2.00
1.60 × 10³
80.0
4.00
0.0400
0.250
10.0
8.00
&
mL
mL/kg
kg
units/mL
L
unit
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19
Identify the starting material in the following reaction. Click the "draw structure" button to launch the
drawing utility.
draw structure ...
[1] 0 3
C10H18
[2] CH3SCH3
H
In an equilibrium mixture of the formation of ammonia from nitrogen and hydrogen, it is found that
PNH3 = 0.147 atm, PN2 = 1.41 atm and Pн2 = 6.00 atm. Evaluate Kp and Kc at 500 °C.
2 NH3 (g) N2 (g) + 3 H₂ (g)
K₂ = (PN2)(PH2)³ = (1.41) (6.00)³ = 1.41 x 104
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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