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.
In Lewis theory, we use electron dot formulas and the VSEPR model to determine electron distributionand geometric structure of covalent particles. Two important basic forms are ??5 and ??6 as outlined here: SEE IMAGE.
A ) Iodine (?) often forms compounds with other halogens, such as fluorine (?), chlorine (??) and bromine(??). Compare valid Lewis electron structures and VSEPR geometries of the particles: see image
Write down the correct VSEPR classification (?????) for each particle and provide a valid geometry
What do you mean by the below statement ?
An inductive effect is the pull of electron density through σ bondscaused by electronegativity differences of atoms.
Can someone expain what it means when it says: draw a better resonance structure than the one shown below" does it mean it wants the highly electronegative atoms O and N to be nuetral? they are "happier neutral? do i draw lewis structure variations and then...?
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