R. S. Mulliken proposed that the electronegativity (EN) of an atom is given by E N = k × ( E 1 − E e a ) where E 1 and E e a are the ionization energy and electron affinity of the atom, respectively. Using the electron affinities and ionization energy values for the halogen atoms up to iodine, estimate the value of k by employing the electronegativity values in Figure 10-6. Estimate the electron affinity of At.
R. S. Mulliken proposed that the electronegativity (EN) of an atom is given by E N = k × ( E 1 − E e a ) where E 1 and E e a are the ionization energy and electron affinity of the atom, respectively. Using the electron affinities and ionization energy values for the halogen atoms up to iodine, estimate the value of k by employing the electronegativity values in Figure 10-6. Estimate the electron affinity of At.
Solution Summary: The author explains how R.S.Mulliken proposed an equation for electronegativity of an atom.
R. S. Mulliken proposed that the electronegativity (EN) of an atom is given by
E
N
=
k
×
(
E
1
−
E
e
a
)
where
E
1
and
E
e
a
are the ionization energy and electron affinity of the atom, respectively. Using the electron affinities and ionization energy values for the halogen atoms up to iodine, estimate the value of k by employing the electronegativity values in Figure 10-6. Estimate the electron affinity of At.
Definition Definition Change in energy of a neutral gaseous atom when an electron is added to the atom to form a negative ion.
Use the periodic table to (i) predict electron configurations for the following species:
Arsenic ion, As3–
Magnesium ion, Mg2+
Vanadium(II) ion, V2+
(ii) Write the electron configurations of each species in the noble gas notation. (iii) Draw an orbital diagram to represent 1 c above.
Draw the Lewis electron dot structures of the following chemical species. In each case you must say whether or not the central atom obeys the Octet Rule.
CS2 and H2S
CF4 and SiH4
NH2Cl
CO32– and BF3
PCl5
ClF3, XeF2,
Calculate the formal charge on the Sulphur atom in the Sulphate anion structure shown below(picture attatched)
Give the electron-pair and molecular geometries for NF3 and XeF4.
Calculate the lattice energy of NaBr(s), given the following thermochemical
equations, where A/E and AEA are ionization energy and electron affinity,
respectively.
Na(s)Na(g) AH = +107 kJ
Na(g) Nat(g) + e A/E = +496 kJ
->
1/2 Br₂(g) → Br(g) AHf = +112 kJ
-
Br(g) + e¯ → Br¯(g) AEA = -325 kJ
Na(s) + 1/2 Br₂(g) → NaBr(s) AH = -361 kJ
->>
-
-1401 kJ
-751 kJ
+29 kJ
-29 kJ
+751 kJ
Given:
Enthalpy of atomisation of calcium =+ 178 kJ
First ionisation energy of calcium =+590 kJ
Second ionisation energy of calcium = +1145 kJ
Enthalpy of atomisation of chlorine =+ 121 kJ
Electron affinity of chlorine
Lattice energy of calcium chloride =- 2258 kJ
= - 346 kJ
Construct a Born-Haber cycle for calcium chloride, CaCl2 by using the data
given above. Hence, calculate the enthalpy of formation of calcium chloride.
b. The enthalpy of solution for calcium chloride crystal is -81.3 kJ mol'. Based on
the data from the above Born-Haber cycle, calculate the enthalpy change for the
reaction below:
Ca" (g) + 2CI (g)–→ Ca* (aq) + 2CI¯ (aq)
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Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY