Atomization energy diagram

Abstract Atomization energy diagram is proposed for analyzing the chemical bond in... 

Figure 12.2 Atomization energy diagram for binary hydrides.

For any perovskite-type hydrides, M1M2H3/ (e.g., KMgH3, as shown in Figure 12.3), it is known that the Ml-H and M2-H interactions are rather ionic in character, even though covalent character still remains to some extent in the M2-H bond because of the shorter M2-H distance than the Ml-H distance. The covalent character further increases in case when M2 is a transition metal. As shown in Figure 12.4, the atomization energy diagram for perovskite-type... 

Figure 12.4 Atomization energy diagram for perovskite-type hydrides and binary hydrides.

For comparison, the atomization energy diagram is shown in Figure 12.6 for the binary oxides and the perovskite-type oxides, M1M203, where M2 are the... 

Figure 12.9 Atomization energy diagram for metal hydrides.

Figure 12.12 Atomization energy diagram for complex hydrides.

To date there is no evidence that sodium forms any chloride other than NaCl indeed the electronic theory of valency predicts that Na" and CU, with their noble gas configurations, are likely to be the most stable ionic species. However, since some noble gas atoms can lose electrons to form cations (p. 354) we cannot rely fully on this theory. We therefore need to examine the evidence provided by energetic data. Let us consider the formation of a number of possible ionic compounds and first, the formation of sodium dichloride , NaCl2. The energy diagram for the formation of this hypothetical compound follows the pattern of that for NaCl but an additional endothermic step is added for the second ionisation energy of sodium. The lattice energy is calculated on the assumption that the compound is ionic and that Na is comparable in size with Mg ". The data are summarised below (standard enthalpies in kJ) ... 

K. L. Komarek, ed.. Hafnium Physico-Chemical Properties of Its Compounds andEUhys, International Atomic Energy Agency, Vieima, 1981, pp. 11,13,14, 16. Covers tbermocbemical properties, phase diagrams, crystal stmcture, and density data on hafnium, hafnium compounds, and alloys. 

Fig. 1.18. Molecular orbital energy diagram for methane. Energies are in atomic units. ...

Strategy Determine the number of electrons in the atom from its atomic number. Using the energy diagram in Figure 6.8, fill the appropriate sublevels. 

At this point we might recast the hydrogen atom energy level diagram to express what we know... 

The energy level diagrams resemble the hydrogen atom level diagram except that the ri levels with the same value of n no longer all have the same energy. 

Amplitude of a process, 114. Andrew s diagram, 173 Anisotropic bodies, 193 Aphorism of Clausius, 83, 92 Arrhenius theory of electrolytic dissociation, 301 Aschistic process, 31, 36, 51 Atmosphere, 39 Atomic energy, 26 Availability, 65, 66 Available energy, 66, 77, 80, 98, 101... 

Figure 2.14. The molecular orbitals of gas phase carbon monoxide, (a) Energy diagram indicating how the molecular orbitals arise from the combination of atomic orbitals of carbon (C) and oxygen (O). Conventional arrows are used to indicate the spin orientations of electrons in the occupied orbitals. Asterisks denote antibonding molecular orbitals, (b) Spatial distributions of key orbitals involved in the chemisorption of carbon monoxide. Barring indicates empty orbitals.5 (c) Electronic configurations of CO and NO in vacuum as compared to the density of states of a Pt(lll) cluster.11 Reprinted from ref. 11 with permission from Elsevier Science.

In Fig. 1 there is indicated the division of the nine outer orbitals into these two classes. It is assumed that electrons occupying orbitals of the first class (weak interatomic interactions) in an atom tend to remain unpaired (Hund s rule of maximum multiplicity), and that electrons occupying orbitals of the second class pair with similar electrons of adjacent atoms. Let us call these orbitals atomic orbitals and bond orbitals, respectively. In copper all of the atomic orbitals are occupied by pairs. In nickel, with ou = 0.61, there are 0.61 unpaired electrons in atomic orbitals, and in cobalt 1.71. (The deviation from unity of the difference between the values for cobalt and nickel may be the result of experimental error in the cobalt value, which is uncertain because of the magnetic hardness of this element.) This indicates that the energy diagram of Fig. 1 does not change very much from metal to metal. Substantiation of this is provided by the values of cra for copper-nickel alloys,12 which decrease linearly with mole fraction of copper from mole fraction 0.6 of copper, and by the related values for zinc-nickel and other alloys.13 The value a a = 2.61 would accordingly be expected for iron, if there were 2.61 or more d orbitals in the atomic orbital class. We conclude from the observed value [Pg.347]

Scheme 30 represents the energy diagram for the photorearrangement shown in Scheme 29. Quenching of the triplet state of the sensitizer by the cis allyl phosphate, c/s-1, generates the triplet state, T , of the 1,2-biradical 2. The 1,2-biradical is trapped by the phosphorus atom to afford the triplet state, TP, of the spirophosphoranyl 1,3-biradical 3. Then, inter-system crossing generates the...

An atomic energy level diagram showing the relationships among atomic energy levels and photon absorption and emission. 

C07-0032. Describe an atomic energy ievei diagram and the information it incorporates. 

C07-0123. An atomic energy level diagram, shown to scale, follows ... 

C08-0110. The figure below shows four proposed electron energy diagrams for a phosphorus atom. Which are... 

C08-0111. None of the four proposed electron energy diagrams shown below describes the ground state of a sulfur atom. For each, state the reason why it is not correct ... 

Figure 6.11. Schematic energy diagram of an atom approaching a free electron metal with an sp band. Notice that the vacuum level is the...

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