Describe each highlighted bond in terms of the overlap of atomic orbitals. (If the highlighted bond is not a pi bond, select the
blank option from the dropdown menu.) Compound 1: Molecular orbital type: _________ Atomic orbitals in the sigma bond: _________ Atomic orbitals in the pi bond: _________ Compound 2: Molecular orbital type: _________ Atomic orbitals in the sigma bond: _________ Atomic orbitals in the pi bond: _________
1 answer:
The image of the bonds are missing, so i have attached it.
Answer:
A) - Sigma bond
-Sp³ and Sp³
- None
B) - Sigma and pi bond
- Sp² of C and p of O
- p of C and P of O
Explanation:
A) For compound 1;
- the molecular orbital type is sigma bond due to the end-to-end overlapping.
- Atomic orbitals in the sigma bond will be Sp³ and Sp³
- Atomic orbitals in the pi bond would be nil because there is no pi bond.
B) For compound 2;
- the molecular orbital type is sigma and pi bond
-Atomic orbitals in the sigma bond would be Sp² of C and p of O
- The Atomic orbitals in the pi bond will be; p of C and p of O
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Answer:
a) The slope of the line of best fit plot = -12629.507
b) ΔH∘ = 105 kJ
c) Intercept of the line of best fit plot = 39.099
d) ΔS∘ = 325.1 J/K
e) Option A is correct.
Solubility will increase as temperature increases, because as T increases the (−ΔH∘/RT) term becomes smaller therefore K will get larger.
f) Option D is correct. All of the options are correct.
Explanation:
The complete question is presented in the first attached image to this question. This complete question has the data readings required to plot the graph.
The second attached image has the plotted graph and the regression analysis to obtain the line of best fit.
The equation of the line of best fit obtained is
y = -12629.507x + 39.099
Comparing the given expression for the question with the equation of a straight line
ln (K) = (−ΔH∘/RT) + (ΔS∘/R)
y = mx + c
y = In K
Slope = m = (−ΔH∘/R)
x = (1/T)
Intercept = c = (ΔS∘/R)
So, to answer the question now
a) The slope of the line of best fit plot = -12629.507
b) Slope = (−ΔH∘/R)
(−ΔH∘/R) = -12629.507
But R = molar gas constant = 8.314 J/mol.K
ΔH∘ = 12629.507 × 8.314 = 105,001.721198 J = 105,002 J = 105 kJ
c) Intercept of the line of best fit plot = 39.099
d) Intercept = (ΔS∘/R)
(ΔS∘/R) = 39.099
ΔS∘ = 39.099 × 8.314 = 325.069086 J/K = 325.1 J/K
e) Do you expect the solubility of Borax to increase or decrease as temperature increases?
Solubility will increase as temperature increases, because as T increases the (−ΔH∘/RT) term becomes smaller therefore K will get larger.
f) Why was it necessary to make sure that some solid was present in the main solution before taking the samples to measure Ksp? Select the option that best explains why.
A. To make sure no more sodium borate would dissolve in solution.
B. To ensure the dissolution process was at equilibrium.
C. To make sure the solution was saturated with sodium and borate ions.
D. All of the above
Hope this Helps!!!
