In this problem, we examine the basis of three different electronegativity scales and work through the same types of calculations as those performed by the people who initially suggested these scales. The scale developed by Robert Mulliken employs ionization energies (E) and electron amenities E e a whereas the scale developed by Linus Pauling is based on bond dissociation energies (D). The scale developed by A. Louis Aired and Eugene G. Rochow employs effective nuclear charges ( Z e a ) and covalent radii The key equations for each scale are given below. In devising his scale, Pauling observed that the bond energy, D a − z for the A − B bond is greater than the average of A − A the and B − B bond energies, 1 2 ( D A − A + D B − B ) , and he attributed the increase in bond strength to the partial ionic character of the A − B bond. Mulliken argued that the ionization energy ( E 1 ) and electron affinity ( E e a ) are of equal importance for the electronegativity Of an atom. Therefore, he suggested that the average of these two quantities, ( E 1 + E e a ) / 2 be used to define the electronegativity of an atom. Alred and Rochow focused on the attractive Coulombic force between an electron near the surface of an atom and the nucleus of that atom. They argued that the magnitude of this force is proportional to where ( e ) ( Z a r e ) / r 2 e a v } = e 2 Z a m / r 2 e a v where e = 1.602 × 10 12 C is the magnitude of the charge of an electron, Z e a e is the nuclear charge experienced by an electron near the atom's surface, and r is the covalent radius and a realistic measure of the size of an atom. The values of D , Z e a and r given below are the actual values used by Pauling and by Alfred and Rochow in their original papers. use the data below and the equations above to calculate the electronegativities of F, CI, Br, and l. Summarize your results in a table having four columns: Atom, EN(Pauling), EN(MuIliken), (Hint: The Pauling values you calculate will not be exactly equal to those in Figure 10-6. The values in Figure 10-6 are based on bond dissociation energies from a wider range of molecules than we are considering in this problem.
In this problem, we examine the basis of three different electronegativity scales and work through the same types of calculations as those performed by the people who initially suggested these scales. The scale developed by Robert Mulliken employs ionization energies (E) and electron amenities E e a whereas the scale developed by Linus Pauling is based on bond dissociation energies (D). The scale developed by A. Louis Aired and Eugene G. Rochow employs effective nuclear charges ( Z e a ) and covalent radii The key equations for each scale are given below. In devising his scale, Pauling observed that the bond energy, D a − z for the A − B bond is greater than the average of A − A the and B − B bond energies, 1 2 ( D A − A + D B − B ) , and he attributed the increase in bond strength to the partial ionic character of the A − B bond. Mulliken argued that the ionization energy ( E 1 ) and electron affinity ( E e a ) are of equal importance for the electronegativity Of an atom. Therefore, he suggested that the average of these two quantities, ( E 1 + E e a ) / 2 be used to define the electronegativity of an atom. Alred and Rochow focused on the attractive Coulombic force between an electron near the surface of an atom and the nucleus of that atom. They argued that the magnitude of this force is proportional to where ( e ) ( Z a r e ) / r 2 e a v } = e 2 Z a m / r 2 e a v where e = 1.602 × 10 12 C is the magnitude of the charge of an electron, Z e a e is the nuclear charge experienced by an electron near the atom's surface, and r is the covalent radius and a realistic measure of the size of an atom. The values of D , Z e a and r given below are the actual values used by Pauling and by Alfred and Rochow in their original papers. use the data below and the equations above to calculate the electronegativities of F, CI, Br, and l. Summarize your results in a table having four columns: Atom, EN(Pauling), EN(MuIliken), (Hint: The Pauling values you calculate will not be exactly equal to those in Figure 10-6. The values in Figure 10-6 are based on bond dissociation energies from a wider range of molecules than we are considering in this problem.
Solution Summary: The author explains that Pauling, Mulliken and Allred-Rochow have proposed three different scales for electronegativity.
In this problem, we examine the basis of three different electronegativity scales and work through the same types of calculations as those performed by the people who initially suggested these scales. The scale developed by Robert Mulliken employs ionization energies (E) and electron amenities
E
e
a
whereas the scale developed by Linus Pauling is based on bond dissociation energies (D). The scale developed by A. Louis Aired and Eugene G. Rochow employs effective nuclear charges
(
Z
e
a
)
and covalent radii The key equations for each scale are given below.
In devising his scale, Pauling observed that the bond energy,
D
a
−
z
for the
A
−
B
bond is greater than the average of
A
−
A
the and
B
−
B
bond energies,
1
2
(
D
A
−
A
+
D
B
−
B
)
, and he attributed the increase in bond strength to the partial ionic character of the
A
−
B
bond. Mulliken argued that the ionization energy
(
E
1
)
and electron affinity
(
E
e
a
)
are of equal importance for the electronegativity Of an atom. Therefore, he suggested that the average of these two quantities,
(
E
1
+
E
e
a
)
/
2
be used to define the electronegativity of an atom. Alred and Rochow focused on the attractive Coulombic force between an electron near the surface of an atom and the nucleus of that atom.
They argued that the magnitude of this force is proportional to where
(
e
)
(
Z
a
r
e
)
/
r
2
e
a
v
}
=
e
2
Z
a
m
/
r
2
e
a
v
where
e
=
1.602
×
10
12
C
is the magnitude of the charge of an electron,
Z
e
a
e
is the nuclear charge experienced by an electron near the atom's surface, and r is the covalent radius and a realistic measure of the size of an atom. The values of
D
,
Z
e
a
and r given below are the actual values used by Pauling and by Alfred and Rochow in their original papers. use the data below and the equations above to calculate the electronegativities of F, CI, Br, and l. Summarize your results in a table having four columns: Atom, EN(Pauling), EN(MuIliken), (Hint: The Pauling values you calculate will not be exactly equal to those in Figure 10-6. The values in Figure 10-6 are based on bond dissociation energies from a wider range of molecules than we are considering in this problem.
Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.
Use the literature Ka value of the acetic acid, and the data below to answer these questions. Note: You will not use the experimental titration graphs to answer the questions that follow.
Group #1:
Buffer pH = 4.35
Group #2:
Buffer pH = 4.70
Group #3:
Buffer pH = 5.00
Group #4:
Buffer pH = 5.30
Use the Henderson-Hasselbalch equation, the buffer pH provided and the literature pKa value of acetic acid to perform the following:
a) calculate the ratios of [acetate]/[acetic acid] for each of the 4 groups buffer solutions above.
b) using the calculated ratios, which group solution will provide the best optimal buffer (Hint: what [acetate]/[acetic acid] ratio value is expected for an optimal buffer?)
c) explain your choice
How would you prepare 1 liter of a 50 mM Phosphate buffer at pH 7.5 beginning with K3PO4 and 1 M HCl or 1 M NaOH? Please help and show calculations. Thank you
Draw the four most importantcontributing structures of the cation intermediate thatforms in the electrophilic chlorination of phenol,(C6H5OH) to form p-chlorophenol. Put a circle aroundthe best one. Can you please each step and also how you would approach a similar problem. Thank you!
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